JP2012505810A - Heterogeneous hydrogen catalyst reactor - Google Patents

Abstract

  Power source consisting of a reaction cell for the catalytic reaction of atomic hydrogen to form hydrinos, a source of atomic hydrogen, and a source of hydrogen catalyst consisting of a solid, liquid, or heterogeneous-catalytic reaction mixture And a hydride reactor is provided. Catalytic reactions were activated or initiated and propagated by one or more other chemical reactions. These reactions maintained on an electrically conductive support can consist of several classes. For example, (i) an exothermic reaction that provides activation energy for a hydrino catalysis reaction, (ii) a coupling that supplies for at least one of a catalyst or a source of atomic hydrogen to support the hydrino catalysis reaction. (Iii) a free radical reaction that functions as an acceptor of electrons from the catalyst during the hydrino catalysis reaction, and (iv) an acceptor of electrons from the catalyst during the hydrino catalysis reaction. An oxidation-reduction reaction in (v) an exchange reaction, such as anion exchange, which facilitates the action of an ionizing catalyst upon receipt of energy from atomic hydrogen to form hydrino, and (vi) Kinetics for supplying electrons in at least one of the chemical environments for the hydrino reaction and for transferring electrons to facilitate the H catalyst function. Through a convertible phase or other physical change or change in its electronic state, and binding a lower energy hydrogen product to increase at least one of the extent or rate of the hydrino reaction, Getter, support, or matrix-assisted hydrino reaction. Power and chemical plants that can be operated continuously using electrolysis or thermal regeneration reactions were maintained in synchrony with at least one of power and lower energy hydrogen chemical production.

Description

(Cross-reference of related patents)
This application is filed on US Provisional Application No. 61/084923, filed July 30, 2008, US Provisional Application No. 61 / 086,316, filed August 5, 2008, August 13, 2008. US Provisional Application No. 61 / 088,492, filed September 5, 2008, US Provisional Application No. 61 / 094,513, filed September 19, 2008, US Provisional Application No. 61 / 088,492, filed September 19, 2008 61 / 098,514, U.S. Provisional Application No. 61 / 102,465, filed October 3, 2008, U.S. Provisional Application No. 61 / 104,534, filed Oct. 10, 2008, 2008 US Provisional Application No. 61 / 105,660, filed October 15, 2008, US Provisional Application No. 61 / 106,932, filed October 20, 2008, filed October 28, 2008 US provisional application number 61 / 109,088, US Provisional Application No. 61 / 110,253, filed October 31, 2008, US Provisional Application No. 61 / 112,491, filed November 7, 2008, 2008 US Provisional Application No. 61 / 114,735, filed November 14, 2014, US Provisional Application No. 61 / 116,966, filed November 21, 2008, filed December 5, 2008 U.S. Provisional Application No. 61 / 193,543, U.S. Provisional Application No. 61 / 139,293, filed Dec. 19, 2008, U.S. Provisional Application No. 61/145, filed Jan. 15, 2009. , 022, US provisional application number 61 / 146,962 filed on January 23, 2009, US provisional application number 61 / 150,571 filed February 6, 2009, February 2009. On the 13th U.S. Provisional Application No. 61 / 152,500, U.S. Provisional Application No. 61 / 156,328, filed Feb. 27, 2009, U.S. Provisional Application No. 61, filed Mar. 6, 2009. No./158,252, US Provisional Application No. 61 / 160,145, filed March 13, 2009, US Provisional Application No. 61 / 164,151, filed March 27, 2009, 2009 US Provisional Application No. 61 / 166,495 filed April 3, US Provisional Application No. 61 / 170,418 filed April 17, 2009, United States Application filed April 30, 2009 Provisional Application No. 61 / 174,346, U.S. Provisional Application No. 61 / 176,675, filed May 8, 2009, U.S. Provisional Application No. 61/178, filed May 15, 2009, 796, May 2, 2009 US Provisional Application No. 61 / 180,456 filed on 2nd, US Provisional Application No. 61 / 182,468 filed on 29th May 2009, US Provisional Application filed on 12th June 2009 No. 61 / 186,660, US Provisional Application No. 61 / 218,771, filed June 19, 2009, US Provisional Application No. 61 / 220,911, filed June 26, 2009 Claims the benefit of US Provisional Application No. 61 / 222,721, filed July 2, 2009, and US Provisional Application No. 61 / 226,541, filed July 17, 2009, All these contents are incorporated herein by reference.

(Summary of disclosed embodiments)
The present disclosure relates to a hydrogen catalyst capable of forming an atomic hydrogen source in a low energy state in an atom H in a state of n = 1, and other catalysts capable of initiating and propagating the reaction to form low energy hydrogen. The aim is a catalyst system consisting of seeds. In certain embodiments, the present disclosure is directed to a reaction mixture comprising at least one source material of atomic hydrogen and a catalyst or catalyst source to support hydrogen catalysis to form hydrinos. The reactants and reactions disclosed herein for solid and liquid fuels are also heterogeneous fuel reactants and reactions including a mixture of phases. The reaction mixture consists of at least two components selected from a hydrogen catalyst or a hydrogen catalyst source and an atomic hydrogen source, and at least one of the atomic hydrogen and the hydrogen catalyst may be formed by the reaction of the reaction mixture. In other embodiments, the reaction mixture further includes a support that is conductive in certain embodiments, a solvent such as an organic or inorganic solvent that includes a molten salt, a getter (residual gas adsorbent), and its At least one reactant that activates catalysis by potency.

  Reactions that form hydrinos are activated, initiated, and propagated by one or more chemical reactions. These reactions include (i) an exothermic reaction that provides activation energy for the hydrino reaction, (ii) a conjugation reaction that provides at least one catalyst source or atomic hydrogen to support the hydrino reaction, (iii) certain In embodiments, a free radical reaction that acts as an electron acceptor from the catalyst during the hydrino reaction, (iv) a redox reaction that acts as an electron acceptor from the catalyst during the hydrino reaction in certain embodiments, (v) In embodiments, when the catalyst receives energy from atomic hydrogen and forms hydrinos, the halide, sulfide, hydride, arsenide, oxide, phosphide, and nitride exchanges that facilitate the action of the catalyst to ionize. Provide at least one chemical environment for exchange reactions, including anion exchange, and (vi) hydrino reactions Acts to move electrons to promote H catalyst function, causes a reversible phase or other physical or electronic state change, and low to increase at least one of the extent or rate of hydrino reactions It is possible to select from getters, supports or matrix-assisted hydrino reactions that bind to energetic hydrogen products. In certain embodiments, the conductive support allows for an activation reaction.

In another embodiment, the disclosure provides a catalyst source or catalyst; an atomic hydrogen source or atomic hydrogen; a catalytic source or catalyst and an reactant that forms an atomic hydrogen source or atomic hydrogen; one or more that initiates the catalytic action of atomic hydrogen. And a power system comprising at least two components selected from a support that enables the catalyst,
Here, the power system further includes a reaction vessel, a vacuum pump, a separation system for reversing the exchange reaction, a power converter and system such as an electrolytic cell, a thermal system, and a chemical synthesis that regenerates fuel from the reaction product. Any of the reactors can be included.

In a further embodiment, the present disclosure provides a catalyst source or catalyst; an atomic hydrogen source or atomic hydrogen; a catalyst source or catalyst and an reactant that forms an atomic hydrogen source or atomic hydrogen; one or more initiators that initiate atomic hydrogen catalysis A system for forming a compound having hydrogen in a low energy state comprising a reactant; and at least two components selected from a support that enables the catalyst;
Here, the system that forms the compound with hydrogen in the low energy state further regenerates the fuel from the reaction vessel, vacuum pump, separation system to reverse the exchange reaction, electrolyzer, thermal system, and reaction product Any of the chemical synthesis reactors can be included.

Other embodiments of the present disclosure include a catalyst source or catalyst; an atomic hydrogen source or atomic hydrogen; a catalyst source or catalyst and an reactant that forms an atomic hydrogen source or atomic hydrogen; one or more initiators that initiate atomic hydrogen catalysis A battery or fuel cell system for forming a compound having hydrogen in a low energy state comprising a reactant; and at least two components selected from a support that enables a catalyst;
Here, a battery system or fuel cell system that forms a compound having hydrogen in a low energy state further includes a reaction vessel, a vacuum pump, a separation system for reversing the exchange reaction, an electrolyzer, a system such as a thermal system, and the like Any of the chemical synthesis reactors that regenerate the fuel from the reaction products can be included.

FIG. 1 is a schematic diagram of an energy reactor and power plant according to the present disclosure. FIG. 2 is a schematic diagram of an energy reactor and power plant for reusing or regenerating fuel according to the present disclosure. FIG. 3 is a schematic diagram of a power reactor according to the present disclosure. FIG. 4 is a schematic diagram of a system for reusing or recycling fuel according to the present disclosure. FIG. 5 is a schematic diagram of a discharge power and plasma cell and reactor according to the present disclosure. FIG. 6 is a schematic diagram of a battery and a fuel cell according to the present disclosure.

  The present disclosure is directed to a catalyst system that releases energy from atomic hydrogen and forms a low energy state in which the electron shell is close to the nucleus. The released power is used for power generation, and new hydrogen species and compounds are the desired products. These energy states are predicted by conventional physical laws and require a catalyst that receives energy from hydrogen to make the corresponding energy release transition.

Classical physics gives closed-form solutions of hydrogen atoms, hydrogen ions, hydrogen molecular ions, and hydrogen molecules, and predicts corresponding species with fractional principal quantum numbers. Using Maxwell's equations, the electron is constrained that the constrained n = 1 state electron cannot release energy and includes a time-varying electromagnetic field source current between transitions, and the structure of the electron is a boundary value problem. Led. The reaction predicted by the solution of H atoms leads to the formation of hydrogen at lower energy states than previously thought possible, from otherwise stable atomic hydrogen to a catalyst that can accept energy, Includes non-radiative energy transfer. Specifically, classical physics provides a reaction with a net enthalpy of integer multiples of the atomic hydrogen potential energy, where E _h = 27.2 eV, when E _h is 1 Hartley. Predict that atomic hydrogen may experience catalytic reactions with atoms, excimers, ions, and diatomic hydrides. Certain species (eg, He ⁺ , Ar ⁺ , Sr ⁺ , K, Li, HCl, and NaH) that are identifiable on the basis of their known electron energy levels can be used to catalyze the process of atomic hydrogen. Presentation is required. The reaction involves the transfer of q · 13.6 eV to H to form a hydrogen atom that is lower in energy than the unreacted atomic hydrogen corresponding to the principal quantum number of fractions, and especially hot, excited H Includes non-radiative energy transfer following q · 13.6eV continuous emission. That is, in the formula for the main energy level of the hydrogen atom,

n = 1, 2, 3,. . . (2)
Where a _H is the Bohr radius of a hydrogen atom (52.947 pm), e is the magnitude of the charge of the electron, ε ₀ is the dielectric constant of the vacuum, and the fractional quantum number is It becomes like this.

Here, p is an integer such that p ≦ 137, but replaces the well-known parameter of n = integer in the Rydberg equation for excited hydrogen, and in a lower energy state (low energy state) called “hydrino” Represents a hydrogen atom. The n = 1 state of hydrogen and the n = 1 / integer state of hydrogen are non-radioactive, but between two non-radioactive states, for example n = 1 to n = 1/2 Transition is possible by non-radioactive energy transfer. Hydrogen is a special case of the steady state where the corresponding radius of the hydrogen or hydrino atom is given by the following equations and is given by equations (1) and (3).
r = а _H / p (4)
Here, p = 1, 2, 3,... For energy conservation, there must be an energy transfer from the hydrogen atom to the catalyst in the integer unit of the hydrogen atom potential energy in the radial transition to a _H / (m + p) and the normal n = 1 state. Hydrino is formed by the reaction of a normal hydrogen atom with a suitable catalyst having the net enthalpy of reaction of the following formula where m is an integer.
m · 27.2eV (5)
It is believed that the rate of catalysis increases as the net enthalpy of reaction more closely matches m · 27.2 eV. Catalysts with a net enthalpy of reaction within ± 10%, preferably within ± 5% of the energy m · 27.2 eV have been found to be suitable for most applications.

  Catalytic reactions include two steps of energy release: non-radiative energy transfer to the catalyst, followed by additional energy release as the radius decreases to the corresponding stable final state. The general reaction is represented by the following formula:

Cat ^{(q + r) +} + re ⁻ → Cat ^{q +} + m · 27.2 eV (8)
Further, here, the total reaction is as follows:

Here, q, r, m, and p are integers. H * [a _H / (m + p)] has a central field of view equal to the radius of a hydrogen atom (corresponding to 1 in the denominator) and (m + p) times that of a proton, and H * [a _H / (m + p)] Is the corresponding stable state at a radius 1 / (m + p) times that of H. When an electron undergoes radial acceleration from the radius of a hydrogen atom to a radius of 1 / (m + p) times this distance, energy is released as characteristic light emission or as kinetic energy of the third body. The The emission may be in the form of extreme ultraviolet continuous radiation with an edge at [(p + m) ² −p ² −2 m] · 13.6 eV (91.2 / [(p + m) ² −p ² −2 m] nm). Absent. In addition to radiation, resonant kinetic energy transfer may occur that forms a fast H. Subsequent excitation of these fast Hs (n = 1) by collisions with background H ₂ with the corresponding fast atom emission of H (n = 3) results in broadened Balmer alpha radiation. It can be seen that the extreme Balmer alpha broadening (> 100 eV) is consistent with the prediction.

Preferred catalysts can therefore provide the net enthalpy of reaction of m · 27.2 eV. That is, the catalyst undergoes non-radiative energy transfer from hydrogen atoms in resonance and releases energy to the surroundings to affect electronic transitions to fractional quantum energy levels. As a result of the non-radiative energy transfer, the hydrogen atom is unstable and has additional energy until it achieves a lower energy non-radiative state with the main energy level given by equations (1) and (3). Release. In this way, for n given by equation (3), energy is catalytically released from the hydrogen atom with a corresponding decrease in the size of the hydrogen atom with r _n = na _H. For example, 204EV by the catalytic action of the H (n = 1) to H (n = 1/4) is released, hydrogen radius decreases from _{a H} (1/4) to * _{a H.} The catalyst product H (1 / p) may react again with electrons to form the hydrino hydride ion H ⁻ (1 / p), or two H (1 / p) May react to form the corresponding molecule hydrino H ₂ (1 / p).

In particular, the catalyst product H (1 / p) is also a novel hydride ion H with binding energy E _B (1 / p) ^- might react with electrons to form. here,

And a, p = an integer> 1, s = 1/2 , h ( Eichiba) is Planck's constant (in terms of Planck constant), mu ₀ is the permittivity of vacuum, _{m e} is the electron mass, mu _e is the converted electron mass

Where m _p is the proton mass, a ₀ is the Bohr radius, and the ionic radius r ₁ is

From equation (10), the calculated ionization energy of the hydride ions is 0.75418 eV, and the experimental value is 6082.999 ± 0.15 cm ⁻¹ (0.75418 eV).

The NMR peak shifted to the high magnetic field side is a direct proof of the presence of lower energy hydrogen with a reduced radius compared to normal hydride ions, and has an increase in the diamagnetic shield of the proton. There is direct evidence of the presence of low energy hydrogen. The shift is given by the sum of the factors due to the lower energy state and the normal hydride ion H ⁻ .

Here, p = 0 with respect to H ⁻ , p = integer> 1 with respect to H ⁻ (1 / p), and α is a fine structure constant.

H (1 / p) may react with protons and two H (1 / p) may react, producing H ₂ (1 / p) ⁺ and H ₂ (1 / p), respectively. Will. Hydrogen molecular ions and molecular charge and current density functions, bond distances, and energies are solved from Laplacian in ellipsoidal coordinates with non-radiative constraints.

The total energy E _T of a hydrogen molecular ion having a central field of + pe at each focal point of the molecular orbit of the long sphere is as follows.

Here, p is an integer, c is the speed of light in vacuum, and μ is the reduced nuclear mass. The total energy of a hydrogen molecule with a central field of + pe at each focal point of the long spherical orbital is

The bond dissociation energy E _D of the hydrogen molecule H ₂ (1 / p) is the difference between the total energy of the corresponding hydrogen atom and E _T.
E _D = E (2H (1 / p)) − E _T (15)
here,
E (2H (1 / p)) = − p ² 27.20 eV (16)
And
E _D is given by Equation (15-16) and (14).
E _D = −p ² 27.20 eV-E _T
= -P ² 27.20 eV
− (− P ² 31.351 eV-p ³ 0.326469 eV)
= P ² 4.151 eV-p ³ 0.326469 eV (17)
The calculated and experimental parameters for H ₂ , D ₂ , H ₂ ⁺ , and D ₂ ⁺ are given in Table 1.

NMR of the catalytic product gas provides a definitive test of the theoretically predicted chemical shift of H ₂ (1/4). In general, the ¹ H NMR resonance of H ₂ (1 / p) is predicted to be higher than that of H ₂ due to the fractional radius in elliptical coordinates where the electrons are very close to the nucleus. Shift .DELTA.B _T / B predicted for H ₂ (1 / p) is that of _{H 2,} and _is given by the sum of the dependent terms p = an integer> 1 for H 2 (1 / p).

Here, for H ₂ , p = 0. The experimental absolute H ₂ gas phase resonance shift of −28.0 ppm agrees very well with the predicted absolute gas phase shift of −28.01 ppm (Equation (19)).

The vibrational energy E _vib for the transition from υ = 0 to υ = 1 of the hydrogen type molecule H ₂ (1 / p) is as follows.
E _vib = p ² 0.515902 eV (20)
Here, p is an integer. The rotational energy E _rot for the transition from J to J + 1 of the hydrogen type molecule H ₂ (1 / p) is as follows.

Here, p is an integer and I is the moment of inertia.

The p ² dependence of the rotational energy arises from the reciprocal dependence of the internuclear distance p and the corresponding effect on the moment of inertia I. The predicted internuclear distance 2c ′ for H ₂ (1 / p) is as follows:

  Data from a broad spectrum of research technology shows strongly and consistently that hydrogen can exist in lower energy states than previously thought possible. This data supports the existence of these lower energy states, called “hydrinos” as “small hydrogens”, and the corresponding hydride ions and molecular hydrinos. Some of these related previous studies supporting the possibility of a novel reaction of atomic hydrogen that produces hydrogen in a fractional quantum state, an energy lower than the traditional “ground” (n = 1) state. Includes extreme ultraviolet (EUV) spectroscopy, characteristic emission from catalysts and hydride ion products, lower energy hydrogen emission, chemically formed plasma, ballmer alpha broadening, H-line inversion distribution High electron temperature, abnormal plasma afterglow time, power generation, and analysis of new compounds.

The catalytic low energy hydrogen transition of the present disclosure takes the energy that causes the transition from atomic H and is in the form of an endothermic chemical reaction of integer m of 27.2 eV, which is the potential energy of atomic hydrogen that does not depend on the catalyst. Requires a catalyst that can be. The endothermic catalytic reaction may be one or more ionizations from species such as atoms or ions (eg, m = 3 for Li → Li ²⁺ ) and the first bond (eg, for NaH → Na ²⁺ + H). It may further comprise a concerted reaction of bond breakage by ionization of one or more electrons from one or more of the partners of m = 2). He ⁺ meets the catalytic criteria of a chemical or physical process with an enthalpy change equal to an integer multiple of 27.2 eV because it ionizes at 54.417 eV, 2 × 27.2 eV. Two hydrogen atoms may also function as a catalyst of the same enthalpy. Hydrogen atom H (1 / p) p = 1, 2, 3,. . . 137 can experience further transitions to lower energy states given by equations (1) and (2). Here, the transition of one atom is catalyzed by a second one that receives m · 27.2 eV resonantly and non-radiatively, with a concomitant reverse change in its potential energy. The general formula for the transition from H (1 / p) to H (1 / (p + m)) induced by the resonance transfer of m · 27.2 eV to H (1 / p ′) is expressed.

H (1 / p ') + H (1 / p)
→ H + H (1 / (p + m)) + [2 pm+m ² −p ′ ² +1] · 13.6 eV (23)

The hydrogen atoms may act as a catalyst where one is a catalyst for the other and m = 3 and m = 2 for one and two atoms, respectively. When a very fast H collides with one molecule so that two atoms receive 54.4 eV from the third hydrogen atom of the collision partner both resonantly and non-radiatively to form 2H, two atoms The rate for catalyst 2H may be high.

The product of catalyst He ⁺ and 2H at m = 2 is H (1/3) which reacts fast to form H (1/4) and, as a preferred state, to form molecular hydrinos. In particular, in the case of high hydrogen atom concentration, H (1/3) · (p = 3) to H (1/4) · (p + m = 4) with respect to (p ′ = 1; m = 1) H as a catalyst. The further transition given by equation (23) can be fast.

The corresponding molecular hydrino H ₂ (1/4) and hydrino hydride ion H ⁻ (1/4) show that the quantum state with p = 4 has a long theoretical lifetime for further catalysis, H (1 Since it has a multipole many times larger than that of the quadrupole given to / 4), it is the final product consistent with the observation result.

Non-radiative energy transfer to He ⁺ and 2H is expected to increase the He ⁺ ion energy level and increase the electronic excitation temperature of H in helium hydrogen and hydrogen plasmas. For both catalysts, the intermediate H * [а _H / (2 + 1)] (equation (6) with m = 2) has the radius of the hydrogen atom (corresponding to 1 in the denominator) and 3 of that of the proton. doubles have equal central field, [а _{H /} 3] is equivalent to a stable state having the same radius of 1/3 of the H. As electrons undergo a radial acceleration from the radius of the hydrogen atom to a radius of 1/3 of this distance, the energy is released as characteristic luminescence or as third body kinetic energy. The emission may be in the form of extreme ultraviolet continuous radiation with an emission edge at 54.4 eV (22.8 nm) and extending to longer wavelengths. Instead, fast H is predicted for resonant kinetic energy transfer. The second continuum band, atomic hydrogen is subjected to 27.2eV from [а _H / 3], catalysis product [а _H / 3] from (equation (4-7) and (23)) Expected to result from a subsequent rapid transition to the [а _H / 4] state. Extreme ultraviolet (EUV) spectroscopy and high resolution visible spectroscopy were recorded in pulsed emission, emission, and microwaves of helium and hydrogen alone with hydrogen supplying catalysts He ⁺ and 2H, respectively. He ⁺ ion beam pumping occurred with the addition of hydrogen and the excitation temperature of the hydrogen plasma under certain conditions was very high. At both 22.8 nm and 40.8 nm, EUV continuum was observed, and extraordinary (> 50 eV) Balmer alpha broadening was observed. H ₂ (1/4) was dissolved in CDCl ₃ and observed by solution NMR at 1.25 ppm in a gas collected from helium-hydrogen, hydrogen, water-steam-assisted hydrogen plasma.

Similarly, the reaction from Ar ⁺ to Ar ²⁺ has a net reaction enthalpy of 27.63 eV, corresponding to m = 1 in formula (4-7). When Ar ⁺ functions as a catalyst, its expected 91.2 nm and 45.6 nm continuum is observed by solution NMR at 1.25 ppm, as well as the expected gas phase hydrino product H ₂ (1 / 4), fast H, catalytically excited pumping, and other characteristic traces of the hydrino transition were also observed. Considering these results and those of the helium plasma, a q 13.6 eV continuum with thresholds at 54.4 eV (q = 4) and 40.8 eV (q = 3) for the He ⁺ catalyst is observed. It had been. For hydrino transitions to lower states that cause high energy continuous radiation in a broad spectral range, very large values of q are possible.

In recent power generation and product characterization studies, atomic lithium and molecular NaH functioned as catalysts. Because they have enthalpy changes equal to an integer multiple m of the atomic hydrogen potential energy of 27.2 eV (eg, m = 3 for Li and m = 2 for NaH). Alternatively, it satisfies the catalyst standard of physical process. Corresponding hydrino hydride ions H ⁻ (1/4) of the new alkali-halide-hydrino hydride compounds (MH * X; M = Li or Na, X = halogen compounds) and molecular hydrino H ₂ (1 / Specific predictions based on a closed form equation for the energy level of 4) were tested using chemically generated catalytic reactants.

First, the Li catalyst was tested. Li and LiNH ₂ were used as a source of atomic lithium and hydrogen atoms. Using water batch calorimetry, the measured power from 1 g of Li, 0.5 g of LiNH ₂ , 10 g of LiBr, and 15 g of Pd / Al ₂ O ₃ is ΔH = −19.1 kJ The energy balance was about 160W. The observed energy balance was 4.4 times the maximum theoretical value based on known chemistry. Next, LiBr functions as a getter for the catalytic product H (1/4) to form LiH * X, as well as trapping H ₂ (1/4) in the crystal, and power in chemical synthesis. When the reaction mixture was used, Raney nickel (R-Ni) functioned as a dissociator. ToF-SIM showed a LiH * X peak. ¹ H MAS NMR LiH * Br and Li * I showed a large and distinguishable high field resonance at about −2.5 ppm matching H ⁻ (1/4) in the LiX matrix. NMR peak of 1.13ppm corresponds to interstitial _H 2 (1/4), its ^{4 double} _H 2 (1/4) rotational vibration of the usual _{H 2} is at 1989cm ^-1 in FTIR spectra Observed. Although the XPS spectrum recorded in the Li * Br crystal showed peaks of about 9.5 eV and 12.3 eV that were not assigned to any known element based on the absence of any other major element. It matched the binding energy of H ⁻ (1/4) in two chemical environments. A further trace of the energy process is that when atomic Li is present with atomic hydrogen, a very low field strength of about 1-2 V / cm and rt− at low temperature (eg, about 10 ³ K). It was an observation of plasma formation called plasma or resonance transfer. It was observed that the time-dependent linewidth expansion of H-balmer alpha rays corresponds to an unusually fast H (> 40 eV).

Compounds of the present disclosure, such as MH consisting of hydrogen and at least one element M other than hydrogen, function as a source of hydrogen and a source of catalyst for forming hydrinos. In addition to the ionization of t electrons from the atom M to each successive energy level, the catalytic reaction is such that the sum of the ionization energy and binding energy of t electrons is approximately m · 27.2 eV, where m is an integer. , Provided by the breaking of MH bonds. Such a catalyst system includes sodium. The binding energy of NaH is 1.9245 eV. The first and second ionization energies of Na are 5.13908 eV and 47.2864 eV, respectively. Based on these energies, NaH molecules can function as a catalyst and a source of H. This is because the binding energy of NaH and double ionization (t = 2) from Na to Na ²⁺ is 54.35 eV (2 · 27.2 eV). The catalytic reaction is given by:

Na ²⁺ + 2e ⁻ + H → NaH + 54.35 eV (26)
The total reaction is expressed as follows.

The product H (1/3) reacts immediately to form H (1/4) and, in a preferred state, the molecular hydrino H ₂ (1/4) (formula (24)). NaH catalytic reaction is emphasized because the sum of NaH binding energy, Na double ionization to Na ²⁺ (t = 2) and H potential energy is 81.56 eV (3.27.22 eV) Maybe.

Na ²⁺ + 2e ⁻ + H + H _fast ⁺ + e ⁻ → NaH + H + 81.56 eV (29)
The total reaction is represented by the following formula.

Here, H _fast ⁺ is a fast hydrogen atom having a kinetic energy of at least 13.6 eV. H ⁻ (1/4) forms a stable hydride, and 2H (1/2) → H ² (1/4) and H ⁻ (1/4) + H ⁺ → H ₂ (1 / 4) is the preferred product with the corresponding molecule formed by the reaction.

Sodium hydride is typically in the form of an ionic crystalline compound formed by the reaction of metallic sodium with gaseous hydrogen. And in the gas phase, sodium contains covalently bound Na ₂ molecules with a binding energy of 74.8048 kJ / mole. When NsH (s) is heated at a very slow rate of temperature increase (0.1 ° C./min) under a helium atmosphere to produce NaH (g), the prediction given by equation (25-27) It was discovered that the exothermic reaction was observed at high temperatures by differential scanning calorimetry (DSC). In order to achieve high power, the chemical system was designed to greatly increase the rate and amount of NaH (g) formation. Reaction of NaOH and Na to Na ₂ O and NaH (s), calculated from the heat of formation, releases ΔH = −44.7 kJ / NaOH mole of heat.
NaOH + 2Na → Na ₂ O + NaH (s)
ΔH = −44.7 kJ / mole NaOH (31)
This exothermic reaction can promote the formation of NaH (g) and was utilized to promote the exothermic reaction given by equations (25-27).
Na ₂ O + H → NaOH + Na
ΔH = −11.6 kJ / mole NaOH (32)
NaH → Na + H (1/3)
ΔH = −10,500 kJ / mole H (33)
NaH → Na + H (1/4)
ΔH = −19,700 kJ / mole H (34)

NaH is highly kinetic because the catalytic reaction relies on the intrinsic release of H through concomitant transitions that form H (1/3), which further reacts to form H (1/4). Achieve energy uniquely. Differential scanning calorimetry (DSC) was performed on ionized NaH in a helium atmosphere at an extremely slow rate of temperature rise (0.1 ° C./min) to increase the amount of molecular NaH formation. A novel exothermic effect of −177 kJ / mole NaH was observed in the temperature range of 640 ° C. to 825 ° C. To achieve high power, R—Ni with an area of about 100 m ² / g was surface coated with NaOH and reacted with Na metal to form NaH. Using a water flow batch calorimeter, from 15 g R-Ni, the measured power is ΔH≈0 kJ of the change from R-Ni to R-NiAl alloy as starting material when reacted with Na metal The energy balance of ΔH = −36 kJ was about 0.5 kW. Observed energy balance of Nah ^reaction was the -1.6X10 4 kJ / mole H _2, was -241.8kJ / mole H ₂ of 66 times or more combustion enthalpy. By increasing to 0.5 wt% in NaOH doping, the R-Ni alloy Al functioned to replace Na metal as a reductant to produce the NaH catalyst. When heated to 60 ° C., 15 g of composite catalyst material released 11.7 kJ of excess energy and required no additives to obtain 0.25 kW of power. When solution NMR was performed on the product gas dissolved in DMF-d7, H ₂ (1/4) was shown at 1.2 ppm.

ToF-SIM exhibited sodium hydrino hydride, NaH _x, peaks. The ¹ H MAS NMR spectra of NaH * Br and NaH * Cl show large distinguishable magnetic field resonances at −3.6 ppm and −4 ppm, respectively, matching H ⁻ (1/4), and H ₂ (1/4 ) Showed an NMR peak at 1.1 ppm that matched. NaH * Cl from the reaction of solid acid KHSO ₄ as the only source of hydrogen and NaCl contained two fractional hydrogen states. The H ⁻ (1/4) NMR peak was observed at −3.97 ppm. And the H ⁻ (1/3) peak was also present at −3.15 ppm. Corresponding H ₂ (1/4) and H ₂ (1/3) peaks were observed at 1.15 ppm and 1.7 ppm, respectively. ¹ H NMR of NaH * F dissolved in DMF-d7 showed separated H ₂ (1/4) and H ⁻ (1/4) at 1.2 ppm and −3.86 ppm, respectively. Here, a solid NMR assignment was confirmed since there was no possibility of any solid matrix effect or alternative peak assignment. The XPS spectrum recorded for NaH * Br showed H ⁻ (1/4) peaks at about 9.5 eV and 12.3 eV that matched the results from LiH * Br and KH * I. On the other hand, sodium hydrino hydride, in the absence of halides peak, H at 6 eV ^- showed (1/3) two fractional hydrogen states, further with XPS peaks of. Rotational transitions were predicted with ^{4 2} times the energy of the normal of _{H 2} energy has also been observed from _H 2 (1/4) excited using electron beam 12.5KeV.

  These data, such as NMR changes, ToF-SIMs mass, XPS binding energy, FTIR and emission spectra, characterize and identify the hydrino products of catalytic systems including aspects of the present disclosure.

I. Hydrino A hydrogen atom having a binding energy given by the following formula is a product of the H-catalyzed reaction of the present disclosure, where p is an integer greater than 1, and preferably 2 to 137.
Binding energy = 13.6 / (1 / p) ² eV (35)
The binding energy of an atom, ion, or molecule (also known as ionization energy) is the energy required to remove one electron from the atom, ion, or molecule. The hydrogen atom having the binding energy given by the formula (35) is hereinafter referred to as “hydrino atom” or “hydrino”. When the radius of a normal hydrogen atom is a _H and p is an integer, the code designating a hydrino having a radius а _H / p is H [а _H / p]. The hydrogen atom having the radius a _H is hereinafter referred to as “ordinary hydrogen atom” or “ordinary hydrogen atom”. Normal atomic hydrogen is characterized by a 13.6 eV binding energy.

Hydrino is formed by reacting ordinary hydrogen atoms with a suitable catalyst having the following net reaction product enthalpy.
m · 27.2eV (36)
Here, m is an integer. It is believed that the rate of catalysis increases when the net reaction enthalpy more closely matches m · 27.2 eV. Catalysts with a net reaction enthalpy within ± 10% (preferably ± 5%) of m · 27.2 eV have been found to be suitable for most applications.

This catalysis releases energy from hydrogen atoms with a corresponding decrease in the size of the hydrogen atoms with r _n = na _H. For example, the catalytic action of the H (n = 1) to H (n = 1/2) releases a 40.8 eV, and the hydrogen radius decreases from _{a H} in (1/2) а _H. The catalyst system is provided by ionization of each t electron from each atom to a continuum energy level such that the total ionization energy of the t electron is approximately m · 27.2 eV. Here, m is an integer.

According to the above given equations (6-9), a further example to a catalyst system includes lithium metal. The first and second ionization energies of lithium are 5.39172 eV and 75.64018 eV. The double ionization (t = 2) reaction from Li to Li ²⁺ has a net reaction enthalpy of 81.0319 eV (equal to m = 3 in equation (36)).

Li ²⁺ + 2e ⁻ → Li (m) +81.0319 eV (38)
The overall reaction is as follows.

In another embodiment, the catalyst system includes cesium. The first and second ionization energies of cesium are 3.89390 eV and 23.15745 eV. The double ionization (t = 2) reaction from Cs to Cs ²⁺ then has a net reaction enthalpy of 27.05135 eV (equal to m = 1 in equation (36)).

Cs ²⁺ + 2e ⁻ → Cs (m) +27.05135 eV (41)
The overall reaction is as follows.

A further catalyst system includes potassium metal. The first, second, and third ionization energies of potassium are 4.334066 eV, 31.63 eV, 45.806 eV. The triple ionization (t = 3) reaction from K to K ³⁺ then has a net reaction enthalpy of 81.7767 eV (equal to m = 3 in equation (36)).

K ³⁺ + 3e ⁻ → K (m) +81.7426 eV (44)
The overall reaction is as follows.

As a power source, the energy released during catalysis is much greater than the energy brought to the catalyst. The energy released is large compared to conventional chemical reactions. For example, when hydrogen gas and oxygen gas undergo the following combustion to form water, the known formation enthalpy of water is 1.48 eV per hydrogen atom, or ΔH _f = −286 KJ / mole H. is there.
H ₂ (g) + 1 / 2O ₂ (g) → H ₂ O (l) (46)
In contrast, each normal hydrogen atom undergoing catalysis (n = 1) releases a net 40.8 eV. In addition, the following catalytic transition may occur:

Once catalysis begins, hydrinos autocatalyze in a process called disproportionation. This mechanism is similar to that of inorganic ion catalysis. However, hydrino catalysis will have a higher reaction rate than that of inorganic ion catalysts due to a better matching of enthalpy to m · 27.2 eV.

The hydride ions of the present disclosure can be formed by the reaction of a hydrino, which is a hydrogen atom having a binding energy of about 13.6 / n ² eV, with an electron source. Here, n = 1 / p, and p is an integer greater than 1. The hydrino hydride ion is represented by H ⁻ (n = 1 / p) or rH ⁻ (1 / p).

  Hydrino hydride ions are distinguished from normal hydride ions consisting of a normal hydrogen nucleus and two electrons with a binding energy of about 0.8 eV. The latter is hereinafter referred to as “normal hydride ions” or “normal hydride ions”. The hydrino hydride ion consists of a hydrogen nucleus containing protium, deuterium (deuterium), tritium (tritium), and two indistinguishable electrons in a binding energy state according to equations (49-50).

  The binding energy of hydrino hydride ions can be expressed by the following equation.

Here, p is an integer greater than 1, s = 1/2, π is pi, h (Eichiba) is converted Planck's constant, mu _o is the permeability of vacuum, m _e is the electron mass, the mu _e following This is the mass of converted electrons given by the equation.

Where m _p is the proton mass, a _H is the radius of the hydrogen atom, a _o is the Bohr radius, and e is the elementary charge. The radius is given as:

The binding energy of hydrino hydride ion H ⁻ (n = 1 / p) is shown in Table 2 as a function of p, where p is an integer.

  According to the present disclosure, hydrinos having a binding energy according to formula (49-50) that is greater than the bond of normal hydride ions (approximately 0.75 eV) from p = 2 to 23 and less than that of p = 24. Hydride ions (H-) are provided. For p = 2 to p = 24 in formula (49-50), the binding energy of the hydride ion is 3,6.6, 11.2, 16.7, 22.8, 29.3, respectively. 36.1, 42.8, 49.4, 55.5, 61.0, 65.6, 69.2, 71.6, 72.4, 71.6, 68.8, 64.0, 56 .8, 47.1, 34.7, 19.3, and 0.69 eV. A typical composition comprising new hydride ions is also provided herein.

  Also exemplified are compounds consisting of one or more hydrino hydride ions and one or more other elements. Such compounds are referred to as “hydrino hydride compounds”.

Normal hydrogen species are characterized by the following binding energies.
(A) Hydride ion (“ordinary hydride ion”), 0.754 eV,
(B) a hydrogen atom (“ordinary hydrogen atom”), 13.6 eV,
(C) Diatomic hydrogen molecule, 15.3 eV (“ordinary hydrogen molecule”),
(D) a hydrogen molecular ion, 16.3 eV (“ordinary hydrogen molecular ion”), and
(E) H ₃ ⁺ , 22.6 eV (“ordinary trihydrogen molecular ion”).
Here, regarding the form of hydrogen, “ordinary” and “ordinary” are synonymous.

According to further embodiments of the present disclosure, compounds comprising at least one increased binding energy hydrogen species are provided as follows. (A) When p is an integer from 2 to 137, about 13.6 / (1 such as in the range of about 0.9 to 1.1 times 13.6 / (1 / p) ² eV. / P) a hydrogen atom having a binding energy of ² eV, (b) when p is an integer from 2 to 24,

Such as in the range of about 0.9 to 1.1 times the binding energy of

When the hydride ion (H ⁻ ), (c) H ₄ ⁺ (1 / p), (d) p is an integer from 2 to 137, the bond energy is 22.6 / (1 / p ) ² eV, such as in the range of about 0.9 1.1 times the approximately 22.6 / (1 / ^p) 2 triple hydrino molecular ion _H having the binding energy of ^{eV 3 + (1 / p)} , (E) When p is an integer from 2 to 137, about 15.3 / (1 such as in the range of about 0.9 to 1.1 times 15.3 / (1 / p) ² eV. / P) a double hydrino with a binding energy of ² eV, and (f) about 0.9 of 6.3 / (1 / p) ² eV when p is an integer, preferably 2 to 137. A double hydrino with a binding energy of about 16.3 / (1 / p) ² eV, such as in the range of 1.1 to 1.1 times.

  According to further embodiments of the present disclosure, compounds comprising at least one increased binding energy hydrogen species are provided as follows. (A) a double hydrino molecular ion having approximately the total energy as follows:

For example, it has the following energy in the range of about 0.9 to 1.1 times.

Here, p is an integer, h (Eichiba) is converted Planck constant, m _e is the electron mass, c is the speed of light in a vacuum, and, mu is converted nucleus mass. And (b) a double hydrino having the following total energy:

The following energies are in the range of about 0.9 to 1.1 times the energy.

Here, p is an integer and a _o is the Bohr radius.

According to one embodiment of the present disclosure, the compound consists of a hydrogen species with increased binding energy that is negatively charged, wherein the compound is a 1, such as a proton, normal H ₂ ⁺ or normal H ₃ ^+. Or further containing more cations.

A method is provided herein for preparing a compound comprising at least one hydrino hydride ion. Such compounds are hereinafter referred to as “hydrino hydride compounds”. The method includes reacting atomic hydrogen with a catalyst having a net reaction enthalpy of about (m / 2) · 27 eV. Here, m is an integer greater than 1, but is preferably an integer less than 400, and generates a hydrogen atom having an increased binding energy having a binding energy of about 13.6 / (1 / p) ² eV. . At this time, p is an integer, preferably an integer of 2 to 137. A further product of catalysis is energy. The increased binding energy hydrogen atoms can react with the electron source, producing a hydride with increased binding energy. A hydride ion with increased binding energy can react with at least one or more cations to produce a compound containing an increased binding energy hydride ion.

The novel hydrogen composition of the material can consist of:
(A) at least one neutral, positive or negative hydrogen species having binding energy (hereinafter referred to as “increased binding energy hydrogen species”)
This binding energy is
(I) greater than the binding energy of the corresponding normal hydrogen species, or
(Ii) Since the binding energy of normal hydrogen species is lower than the thermal energy at ambient conditions (standard temperature and pressure, STP), the corresponding normal hydrogen species is unstable, cannot be confirmed, or negative Greater than the binding energy of any hydrogen species; and
(B) at least one other element.
Hereinafter, the compound of the present disclosure is referred to as “an increased binding energy hydrogen compound”.

  “Other elements” in this context means elements other than the increased binding energy hydrogen species. Therefore, the other element can be a normal hydrogen species or any element other than hydrogen. In one group of compounds, the other elements and the increased binding energy hydrogen species are neutral. In another group of compounds, other elements and increased binding energy hydrogen species are charged such that the other elements provide a balanced charge to form a neutral compound. The former group of compounds is characterized by molecular bonds and coordination bonds, while the latter group is characterized by ionic bonds.

Further, the novel compounds and molecular ions to be provided are as follows.
(A) at least one neutral, positive or negative hydrogen species having total energy (hereinafter referred to as “binding energy increasing hydrogen species”),
This total energy is
(I) greater than the total energy of the corresponding normal hydrogen species, or
(Ii) Since the total energy of normal hydrogen species is lower than the thermal energy at ambient conditions, the corresponding normal hydrogen species is unstable, cannot be confirmed, or the total energy of any hydrogen species that is negative Greater than; and
(B) at least one other element.
The total energy of the hydrogen species is the sum of the energies that remove all electrons from the hydrogen species. The total energy of the hydrogen species according to the present disclosure is greater than the total energy of the corresponding normal hydrogen species. Even though some embodiments of hydrogen species having increased total energy have a first electron binding energy that is less than the first electron binding energy of the corresponding normal hydrogen species, the total energy described in this disclosure is increased. These hydrogen species are also referred to as “increased binding energy hydrogen species”. For example, the hydride ions of formulas (49-50) at P = 24 have a first binding energy that is less than the first binding energy of normal hydride ions, while the formula (49 The total energy of -50) hydride ions is significantly greater than the total energy of the corresponding normal hydride ions.

Also, the novel compounds and molecular ions provided herein consist of:
(A) a plurality of neutral, positive or negative hydrogen species having binding energy (hereinafter referred to as “binding energy increasing hydrogen species”),
This total energy is
(I) greater than the binding energy of the corresponding normal hydrogen species, or
(Ii) Since the binding energy of normal hydrogen species is lower than the thermal energy at ambient conditions, the corresponding normal hydrogen species is unstable, cannot be confirmed, or the binding energy of any hydrogen species that is negative Greater than; and
(B) optionally one other element.
Hereinafter, the compounds of the present disclosure are referred to as “increased binding energy hydrogen compounds”.

  The increased binding energy hydrogen species is other than one or more hydrino atoms, electrons, hydrino atoms, compounds containing at least one of the increased binding energy hydrogen species, and at least one other atom, molecule, or increased binding energy hydrogen species. It can be formed by reacting with one or more of the ions.

Further, the novel compounds and molecular ions to be provided are as follows.
(A) a plurality of neutral, positive or negative hydrogen species having total energy (hereinafter referred to as “binding energy increasing hydrogen species”),
This total energy is
(I) greater than the total energy of normal molecular hydrogen, or
(Ii) Since the total energy of normal hydrogen species is lower than the thermal energy at ambient conditions, the corresponding normal hydrogen species is unstable, cannot be confirmed, or the total energy of any hydrogen species that is negative Greater than; and
(B) optionally one other element.
Hereinafter, the compounds of the present disclosure are referred to as “increased binding energy hydrogen compounds”.

  In some embodiments, provided compounds are of the formula (49-50) where (a) P = 2 to 23 is greater than normal hydride ion binding (approximately 0.8 eV) and P = 24 is less than that A hydride ion having a binding energy according to (“increased binding energy hydride ion” or “hydrino hydride ion”); (b) hydrogen having a binding energy (about 13.6 eV) greater than the binding energy of a normal hydrogen atom Atoms (“increased binding energy hydrogen atoms” or “hydrinos”); (c) hydrogen molecules having a first binding energy greater than about 15.3 eV (“increased binding energy hydrogen molecules” or “hydrinos”); (d) about Molecular hydrogen ions having a binding energy greater than 16.3 eV (“binding energy increasing molecular hydrogen ions” or “high Comprising at least one increased binding energy hydrogen species is selected from Reno molecular ion ").

II. Power Reactor and Power System In accordance with another embodiment of the present disclosure, a hydrogen catalytic reactor is provided that generates energy and low energy hydrogen species. As shown in FIG. 1, the hydrogen catalytic reactor 70 comprises a tank 72 that includes an energy reaction mixture 74, a heat exchanger 80, and a power converter such as a steam generator 82 and a turbine 90. In an embodiment, catalysis includes reacting atomic hydrogen from source material 76 with catalyst 78 to form low energy hydrogen “hydrino” and generate power. When the reaction mixture consisting of hydrogen and catalyst reacts to form low energy hydrogen, the heat exchanger 80 absorbs the heat released by the catalytic reaction. The heat exchanger exchanges heat with the steam generator 82. The steam generator 82 absorbs heat from the exchanger 80 and generates steam. In addition, the energy reactor 70 comprises a turbine 90 that receives steam from the steam generator 82 and provides mechanical power to a generator 100 that converts the steam energy into electrical energy, which energy generates labor. Alternatively, the load receptor 110 can receive to disappear.

  In an embodiment, the energy reaction mixture 74 is comprised of an energy release material 76 such as fuel that is supplied via a supply path 62. The reaction mixture consists of a hydrogen isotope atom source, a molecular hydrogen isotope source, and a source material for catalyst 78, where about m · 27.2 eV is resonantly reduced, m is an integer, and the integer is preferably less than 400 Low energy atomic hydrogen is formed. Here, when hydrogen comes into contact with the catalyst, a reaction of hydrogen to a low energy state occurs. The catalyst may be in a dissolved state, a liquid, a gas or a solid state. The catalyst releases energy in a form such as heat to form at least one of low energy hydrogen isotope atoms, low energy hydrogen molecules, hydride ions, and low energy hydrogen compounds. Thus, the power cell also includes a low energy hydrogen chemical reactor.

The hydrogen source can be hydrogen gas, water dissociation such as thermal dissociation, water electrolysis, hydride-derived hydrogen or metal hydrogen solution-derived hydrogen. In another embodiment, the molecular hydrogen of the energy release material 76 is dissociated into atomic hydrogen by the molecular hydrogen dissociation catalyst of the mixture 74. Such dissociation catalysts or dissociates also absorb hydrogen, deuterium or tritium atoms and / or molecules, such as elements, compounds, alloys or mixtures of noble metals such as palladium and platinum, refractory metals such as molybdenum and tungsten, nickel and Transition metals such as titanium, and internal transition metals such as niobium and zirconium. Preferably, the dissociator has a high surface area such as noble metals such as Pt, Pd, Ru, Ir, Re or Rh, or Al ₂ O ₃ , Ni on SiO ₂ or combinations thereof.

  In one embodiment, the catalyst is obtained by ionizing t electrons from atoms or ions to a continuous energy level such that the total ionization energy of t electrons is about m · 27.2 eV, and t and m are each integers. Provided. The catalyst can also be provided by the transfer of t-electrons between the involved ions. The transfer of t-electrons from one ion to another provides the net enthalpy of the reaction, which allows the t-ionization energy of the electron-donating ion to be subtracted from the ionization energy of the electron-accepting ion. The sum is equal to approximately m · 27.2 eV, where t and m are each integers. In another embodiment, the catalyst comprises MH, such as NaH, having an atom M bonded to hydrogen, and the MH bond energy and the ionization energy of t electrons are summed to calculate an enthalpy of m · 27.2 eV. .

In an embodiment, the source of catalyst consists of catalyst material 78 supplied through catalyst supply passage 61 which typically provides a net enthalpy of plus or minus 1 eV to approximately (m / 2) · 27 eV. The catalyst includes hydrinos, molecules, ions, and atoms that receive energy from atomic hydrogen and hydrinos. In an embodiment, the catalyst, AlH, BiH, ClH, CoH , GeH, InH, NaH, RuH, SbH, SeH, SiH, SnH, the _{C 2, N 2, O 2} , CO 2, NO 2, and CO ₃ From molecules and from Li, Be, K, Ca, Ti, V, Cr, Mn, Fe, Co, Ni, Cu, Zn, As, Se, Kr, Rb, Sr, Nb, Mo, Pd, Sn, Te , Cs, Ce, Pr, Sm, Gd, Dy, Pb, Pt, Kr, 2K ⁺ , He ⁺ , Ti ²⁺ , Na ⁺ , Rb ⁺ , Sr ⁺ , Fe ⁺ , Mo ²⁺ , Mo ⁴⁺ , In ³⁺ , He It may include at least one species selected from ⁺ , Ar ⁺ , Xe ⁺ , Ar ²⁺ and H ⁺ , and Ne ⁺ and H ⁺ atoms or ions.

  In a power system embodiment, heat is removed by a heat exchanger having a heat exchange medium. The heat exchanger may be a water cooling wall and the medium may be water. Heat may be transferred directly for space and process heat treatment. Alternatively, a heat exchange medium such as water undergoes a phase change such as conversion to steam. This conversion may be done in a steam generator. Steam may be used to generate electricity in heating engines such as steam turbines and generators.

  An embodiment of a hydrogen catalyst energy and low energy hydrogen species generation reactor 5 for reusing or regenerating fuel according to the present disclosure is shown in FIG. 2 and includes a hydrogen source, a catalyst source, and optionally a solvent to be evaporated. A boiler 10 containing a fuel reaction mixture 11 that is a mixture, a hydrogen source 12, a steam pipe and steam generator 13, a power converter such as a turbine 14, a water condenser 16, a water formation source 17, a fuel recycler 18, and hydrogen- It consists of a dihydrino gas separator 19. In Step 1, a fuel such as a catalyst source, a multiphase gas containing a hydrogen source, a liquid, a solid or a heterogeneous mixture reacts to form hydrino and low energy hydrogen products. In step 2, the spent fuel is reprocessed and re-supplied to the boiler 10 to maintain thermal power generation. The heat generated in the boiler 10 forms steam in the pipe and the steam generator 13, and the steam is transferred to the turbine 14, and electricity is sequentially generated by supplying power to the generator. In step 3, the water is concentrated by the water condenser 16. Water may be lost by the water source 17 to complete the cycle that maintains the conversion of heat to electricity. In step 4, low energy hydrogen products such as hydrino hydride compounds and hydrino gas are removed and unreacted hydrogen is returned to the fuel reuser 18 or the hydrogen source 12 is returned to spent fuel to recycle fuel. Form. The gas product and unreacted hydrogen may be separated by a hydrogen-dihydrino gas separator 19. Product hydrino hydride compounds may be separated and removed by fuel recycler 18. The treatment may be performed in the boiler or outside the boiler using the returned fuel. Thus, the system may further include at least one of a gas and a solid transporter that moves reactants and products to remove, regenerate and resupply spent fuel. Hydrogen is added from source material 12 during fuel processing to replenish the amount used in hydrino formation. This hydrogen may include recycled hydrogen and unused hydrogen. Recycled fuel operates the power plant and maintains thermal power generation that generates electricity.

  The reactor may be operated in a continuous mode with hydrogen addition and separation and addition or replacement so that reactant decomposition is not minimized. Alternatively, the reacted fuel is continuously regenerated from the product. In one embodiment of the latter scheme, the reaction mixture consists of a species capable of generating an atomic or molecular catalyst reactant, and further an atomic hydrogen that reacts to form a hydrino, formed by the production of the catalyst and atomic hydrogen. The product species can be regenerated at least by reacting the product with hydrogen. In one embodiment, the reactor comprises a moving bed reactor that may further include a fluidized reactor portion, where the reactants are continuously fed, by-products are removed, regenerated, and returned to the reactor. . In certain embodiments, low energy hydrogen products such as hydrino hydride compounds or dihydrino molecules are recovered as the reactants are regenerated. In addition, hydrino hydride ions may be formed into other compounds or converted to dihydrino molecules during regeneration of the reactants.

  The reactor may further include a separator, if any, that separates the components of the product mixture, such as by evaporating the solvent. The separator comprises, for example, a sieve that mechanically separates due to differences in physical properties such as size. The separator may be a separator that utilizes the difference in density of the components of the mixture, such as a cyclone separator. For example, at least two of the groups selected from carbon, metals such as Eu, and inorganic products such as KBr are based on differences in density due to centrifugal force in a suitable medium such as a forced inactivated gas. It is possible to separate. Separation of components may be based on differences in dielectric constant or chargeability. For example, carbon can be removed from the mixture by an electric field and separated from the metal based on the former application of charging. If one or more components of the mixture are magnetic, separation may be performed using a magnet. Based on at least one of a series of strong magnets, or in combination with one or more sieves, stir the mixture to strongly adsorb or attract magnetic particles to the magnet, and the size difference classifies the particles into two Separation is also possible. In embodiments using a sieve and an applied magnetic field, the latter applies an additional force to gravity to obtain small magnetic particles that pass through the sieve. At this time, the other particles of the mixture remain on the sieve due to their large size.

  The reactor may further include a separator that separates one or more components based on a differential phase change or reaction. In some embodiments, the phase change comprises melting using heat and the liquid is separated from the solid by methods known in the art such as gravity filtration, pressurized gas assisted filtration, centrifugation and vacuum processing. Reactions include cracking, such as hydride cracking, or reactions that form hydrides, each of which may be performed by melting the corresponding metal and then separating and mechanically separating the hydride powder. The latter can be performed by sieving. In certain embodiments, the phase change or reaction may produce the desired reactant or intermediate. In certain embodiments, regeneration including any desired separation step may occur inside or outside the reactor.

  Other methods known to those skilled in the art can be applied to the separation of the present disclosure by applying routine experimentation. In general, mechanical separation can be divided into four groups: sedimentation, centrifugation, filtration and sieving. In one embodiment, particle separation is achieved by at least one of sieving and the use of a classifier. In order to desirably separate the products, the size and shape of the particles may be selected with the starting materials.

  The power system may further include a catalyst concentrator that maintains the catalyst vapor pressure with a temperature controller that controls the surface temperature below the temperature of the reaction cell. The surface temperature is maintained at a desired temperature that makes the vapor pressure of the catalyst desirable. In some embodiments, the catalyst concentrator is an in-cell tube grid. In embodiments where a heat exchanger is present, the flow rate of the heat transfer medium may be adjusted to a rate that maintains the concentrator at the desired temperature below the main heat exchanger. In one embodiment, the working medium is water and the flow rate at the concentrator is faster than the water-cooled wall so that the concentrator is at the desired low temperature. The separate flow paths of the working medium may recombine and move for space and process heat treatment or conversion to steam.

  A cell of the present disclosure comprises a catalyst, reaction mixture, method and system disclosed herein, where a particular cell includes a reactor and at least one member that activates, initiates, propagates and / or maintains the reaction. Acting as a regenerator. In accordance with the present disclosure, the cell comprises at least one catalyst or catalyst source, at least one atomic hydrogen source and a tank. The operating cells and systems are known to those skilled in the art. Eutectic salt electrolysis cell, plasma electrolysis reactor, barrier electrode reactor, RF plasma reactor, pressurized gas energy reactor, gas discharge energy reactor, preferably pulse discharge, more preferably pulse pinch plasma of the present disclosure Electrolytic cell energy reactors such as discharges, microwave cell energy reactors, and combinations of glow discharge cells with microwave and / or RF plasma reactors are those that produce hydrino reactions due to the reaction between hydrogen sources; One of the solid, dissolved, liquid, gaseous, and heterogeneous catalyst sources or reactants in any of the following states; including at least hydrogen and catalyst, contacting the catalyst with hydrogen or MH Tanks and reactants in which the reaction to form low energy hydrogen occurs by reacting the catalyst; sometimes low energy Comprising components for removing iodine product. In certain embodiments, the reaction to form the low energy state hydrogen is facilitated by an oxidation reaction. The oxidation reaction may increase the hydrino formation reaction rate by at least one of accepting electrons from the catalyst and neutralizing the highly charged protons formed by accepting energy from atomic hydrogen. Therefore, these cells may be operated in a manner that causes such an oxidation reaction. In some embodiments, the electrolysis or plasma cell may undergo an oxidation reaction at the anode, where hydrogen provided by a method such as sparging and the catalyst react to form hydrino via the associated oxidation reaction. .

  In the liquid fuel embodiment, the cell is operated at a temperature at which the rate of solvent decomposition is negligible relative to the power of the cell relative to the power of regenerating the fuel. In this case, the temperature is lower than the temperature at which the efficiency of power conversion becomes sufficient by a conventional method such as using a steam cycle and a low boiling point working medium can be used. In another embodiment, the temperature of the working medium may be increased using a heat pump. Therefore, the space and process heat treatment is performed using a power cell that operates at a temperature above ambient conditions, and the temperature of the working medium is increased by a member such as a heat pump. When the temperature rises sufficiently, the transition from the liquid phase to the gas phase occurs and the gas can be used for pressure volume (PV) operations. PV operation involves powering the generator and generating electricity. Thereafter, the medium may be concentrated and the concentrated working medium may be returned to the reactor cell, reheated and recycled in the power loop.

  In a reactor embodiment, a heterogeneous catalyst mixture comprising a liquid phase and a solid phase flows through the reactor. The flow can be achieved by pumping action. The mixture may be a slurry. The mixture is heated in the hot zone, so that the catalytic action of hydrogen to hydrino releases heat to maintain the hot zone. The product flows from the hot zone and the reaction mixture can be regenerated from the product. In another embodiment, at least one solid of the heterogeneous mixture may flow to the reactor by gravity feed. The solvent may flow one or more solids separately or in combination into the reactor. The reaction mixture may include at least one of the group of dissociator, high surface area (HSA) material, R—Ni, Ni, NaH, Na, NaOH and solvent.

  In some embodiments, one or more reactants, preferably a halogen source, halogen gas, oxygen source or solvent, are injected into the mixture of other reactants. Injection is controlled to optimize excess energy and power from the hydrino formation reaction. The cell temperature and rate of injection can be controlled to optimize. Other process parameters and mixing are controlled and further optimized by methods known to those skilled in the process engineering.

  For power conversion, each cell type may be connected to any known converter that converts thermal energy or plasma into mechanical or electrical power, such as heat engines, steam or gas turbine systems, Stirling engines or thermoelectronic or thermoelectric conversions. Vessel. Further, the plasma converter includes a magnetic mirror magnetohydrodynamic power converter, a plasma dynamic power converter, a gyrotron, a photon integrated microwave power converter, a charge drift power or an optoelectronic converter. In some embodiments, the cell comprises at least one cylinder of an internal combustion engine.

III. Hydrogen Gas Cell and Solid, Liquid and Heterogeneous Fuel Reactor In accordance with embodiments of the present disclosure, the hydrino and power generating reactor take the form of a reactor cell. The reactor of the present disclosure is shown in FIG. The reactant hydrino is provided by a catalytic reaction with a catalyst. Catalysis takes place in the gas phase or in the solid or liquid state.

  The reactor of FIG. 3 consists of a reaction vessel 207 having a chamber 200 that can be at a pressure higher than vacuum or air. A hydrogen source 221 communicating with the chamber 200 delivers hydrogen to the chamber via the hydrogen supply path 242. A control device 222 is installed to control the pressure and flow rate at which hydrogen flows to the tank via the hydrogen supply path 242. The pressure sensor 223 monitors the pressure in the tank. A vacuum pump 256 is used to empty the chamber via the vacuum line 257.

  In certain embodiments, the catalysis occurs in the gas phase. The catalyst can be made gaseous by maintaining the cell temperature at a high temperature. This temperature in turn determines the vapor pressure of the catalyst. Atomic and / or molecular hydrogen reactants are also maintained at the desired pressure in any pressure range. In certain embodiments, the pressure is below atmospheric, preferably in the range of about 10 millitorr to about 100 torr. In another embodiment, the pressure is determined by maintaining a mixture of a catalyst source such as a metal source and a corresponding hydride such as a metal hydride in a cell maintained at a desired operating temperature.

  A catalyst source 250 suitable for generating hydrino atoms can be placed in a catalyst vessel 295 and heated to form a gaseous catalyst. The reaction tank 207 has a catalyst supply path 241 for passing the gaseous catalyst from the catalyst container 295 to the reaction chamber 200. Alternatively, the catalyst may be placed in a chemically resistant open container such as a boat-shaped container inside the reaction vessel.

The hydrogen source can be hydrogen gas or molecular hydrogen. Hydrogen can be dissociated into atomic hydrogen by a molecular hydrogen dissociation catalyst. Such dissociation catalysts or dissociators include, for example, Raney nickel (R-Ni), gold or precious metal, and metal or precious metal on a support. The test stone or precious metal may be Pt, Pd, Ru, Ir and Rh, and the support may be at least one of Ti, Nb, Al ₂ O ₃ , SiO ₂ and combinations thereof. Further, the dissociator is Pt or Pd on carbon, which is a hydrogen excess catalyst, nickel fiber mat, Pd sheet, Ti sponge, Ti or Ni sponge or electroplated Pt or Pd, TiH, Pt black and Refractory metals such as Pd black, molybdenum and tungsten, transition metals such as nickel and titanium, internal transition metals such as niobium and zirconium, and other similar materials known to those skilled in the art. In some embodiments, the hydrogen dissociates on Pt or Pd. Support metal such as titanium or Al ₂ O ₃ may be coated with Pt or Pd. In another embodiment, the dissociator is a refractory metal such as tungsten or molybdenum, and the dissociating material can be maintained at a high temperature by a temperature regulating member 230, which member is in the form of a heating coil as shown in the cross-sectional view of FIG. May be taken. The heating coil is powered from a power supply 225. Preferably, the dissociating material is maintained at the operating temperature of the cell. In order to perform dissociation more effectively, the temperature of the dissociator may be further controlled to be higher than the cell temperature. As the temperature increases, the catalyst can be prevented from concentrating on the dissociator. A hydrogen dissociator can also be provided by a hot filament such as 280 that is powered by the supply 285.

  In some embodiments, the hydrogen dissociation occurs such that the dissociated hydrogen atoms contact the gaseous catalyst to produce hydrino atoms. The temperature of the catalyst container 295 having the catalyst container heater 298 that is powered to the power supply body 272 is controlled to maintain the catalyst vapor pressure at a desired pressure. When placing the catalyst in a boat in the reactor, the catalyst vapor pressure is maintained at a desired value by adjusting the temperature of the catalyst boat and adjusting the power supply of the boat. The cell temperature can be controlled at a desired operating temperature by superheater coil 230 powered by power supply 225. The cell (referred to as an osmosis cell) further comprises an internal reaction chamber 200 and an external hydrogen vessel 290, where hydrogen is supplied to the cell by diffusion of hydrogen through a wall 291 separating the two chambers. . The wall temperature may be adjusted with a heater that adjusts the diffusion rate. Further, the diffusion rate may be adjusted by adjusting the hydrogen pressure in the hydrogen container.

  In order to maintain the catalyst pressure at a desired value, a permeable cell may be sealed as a hydrogen source. Alternatively, the cell is further provided with a hot valve at the inlet or outlet, respectively, so that the valve in contact with the reaction gas mixture is maintained at the desired temperature. In addition, the cell may include a getter or trap 255 that selectively recovers low energy hydrogen species and / or increased binding energy hydrogen compounds, and may further include a selective valve 206 for releasing dihydrino gas products.

  In some embodiments, a reactant such as a solid fuel or heterogeneous catalytic fuel mixture 260 reacts in the vessel 200 by heating with a heater 230. Preferably, a reactant such as one or more exothermic reactants having a high reaction rate may be further added and allowed to flow into the cell 200 via the control valve 232 and the connecting portion 233. The reactant added may be a halogen source, halogen, oxygen source or solvent. Reactant 260 may include species that react with the added reactants. Halogen may be added to form a halide with reactant 260, or an oxygen source may be added to reactant 260 to form, for example, an oxide.

  The catalyst is at least one of the group of atomic lithium, potassium or cesium, NaH molecules, 2H and hydrino atoms, and the catalysis includes a disproportionation reaction. The lithium catalyst becomes gaseous by maintaining the cell temperature in the range of about 500-1000 ° C. The cell is preferably maintained in the range of about 500-750 ° C. The cell pressure is preferably maintained below the atmosphere and is in the range of about 10 millitorr to about 100 torr. Maintain catalyst metals and corresponding hydride mixtures such as lithium and lithium hydride, potassium and potassium hydride, sodium and sodium hydride, and cesium and cesium hydride in cells that maintain the desired operating temperature Most preferably, at least one of the catalyst and the hydrogen pressure is determined. The catalyst in the gas phase may contain a metal-derived lithium atom or a lithium metal source. It is preferred to maintain the lithium catalyst at a pressure determined with a mixture of lithium metal and lithium hydride in an operating temperature range of about 500-1000 ° C, most preferably in a cell in the operating temperature range of about 500-750 ° C. . In another embodiment, K, Cs and Na are replaced with Li and the catalyst is atomic K, atomic Cs and molecular NaH.

In an embodiment of a gas cell reactor consisting of a catalyst vessel or boat vessel, gaseous catalysts such as gaseous Na, NaH catalyst, or Li, K and Cs vapors are combined with the vapor in the vessel or boat vessel that is the cell vapor source. In comparison, it is maintained in the cell in an overheated state. In one embodiment, excess superheated steam inhibits catalyst concentration on the hydrogen dissociator disclosed below or at least one dissociator of metal and metal hydride molecules. In embodiments comprising Li as a catalyst from a vessel or boat, the vessel or boat is maintained at a temperature at which Li vaporizes. H ₂ can be maintained at a pressure lower than the pressure that increases the molar fraction of LiH at the vessel temperature. Pressure and temperature to permit this condition may be determined from the data plot of H ₂ pressure versus LiH mole fraction at a given isotherm known in the art. In certain embodiments, the cell reaction chamber containing the dissociator is operated at an elevated temperature so that Li does not concentrate on the wall or dissociator. H ₂ flows from the container to the cell, increasing the catalyst transport rate. Flowing from the catalyst vessel to the cell and then out of the cell is one way to remove the hydrino product and prevent hydrino product inhibition of the reaction. In another embodiment, K, Cs and Na are replaced with Li and the catalyst is atomic K, atomic Cs and molecular NaH.

  Hydrogen is supplied to the reaction from a hydrogen source. For example, hydrogen permeates from a hydrogen container and is supplied. The pressure of the hydrogen container is 10 to 10,000 torr, preferably 100 to 1000 torr, and most preferably in the range of about atmospheric pressure. The cell is operated at a temperature of about 100 ° C. to 3000 ° C., preferably about 100 ° C. to 1500 ° C., most preferably about 500 ° C. to 800 ° C.

The hydrogen source may be obtained by decomposing the added hydride. The design of the cell that provides H ₂ by permeation is a design that includes an internal metal hydride placed in a closed vessel and allows atoms H to permeate outside at high temperatures. The bath may contain Pd, Ni, Ti or Nb. In one embodiment, the hydride is placed in a sealed tube, such as a Nb tube containing hydride, and sealed at both ends with a sealant, such as Swagelock. When sealed, the hydride is an alkali or alkaline earth hydride. Alternatively, not only in the case of internal hydride reagents, but also in this case the hydride is a salt hydride, titanium hydride, vanadium, niobium and tantalum hydride, zirconium and hafnium hydride, rare earth hydride, yttrium and scandium hydrogen. And at least one of the group of hydrides, transition element hydrides, intermetallic hydrides and alloys thereof.

In some embodiments, the hydride and an operating temperature of ± 200 ° C. based on each hydride decomposition temperature is selected from at least one of the following lists:
Rare earth hydride operating temperature of about 800 ° C .; lanthanum hydride operating temperature of about 700 ° C .; gadolinium hydride operating temperature of about 750 ° C .; neodymium hydride operating temperature of about 750 ° C .; yttrium hydride about 800 ° C. An operating temperature of about 800 ° C .; an operating temperature of about 850 to 900 ° C. for ytterbium hydride; an operating temperature of about 450 ° C. for titanium hydride; an operating temperature of about 950 ° C. for cerium hydride An operating temperature of about 700 ° C. for praseodymium hydride; an operating temperature of about 600 ° C. for zirconium-titanium (50% / 50%) hydride; an alkali metal / alkali metal hydride mixture such as Rb / RbH or K / KH is An operating temperature of about 450 ° C .; and alkaline earth metal / alkaline earth hydrides such as Ba / BaH ₂ The mixture has an operating temperature of about 900-1000 ° C.

Gaseous metals can include diatomic covalent molecules. The purpose of the present disclosure is to provide atomic catalysts such as Li and K and Cs. Thus, the reactor may further comprise at least one dissociator of a metal molecule (“MM”) and a metal hydride molecule (“MH”). Preferably, the catalyst source, the H ₂ source, and the dissociators of MM, MH and HH, where M is an atomic catalyst, are suitable for operation at the desired cell conditions, eg, temperature and reactant concentration. When using a hydride source of H ₂ , in one embodiment, the decomposition temperature is the temperature range that makes the vapor pressure of the catalyst desirable. When the hydrogen source penetrates from the hydrogen vessel into the reaction chamber, suitable catalyst sources for continuous operation are Sr and Li metals. This is because their respective vapor pressures are in the desired range of 0.01 to 100 torr at the temperature at which penetration occurs. In another embodiment of the osmosis cell, the cell is operated at an elevated temperature that allows for osmosis, and then the cell temperature is lowered to a temperature that maintains the vapor pressure of the volatile catalyst at the desired pressure.

In the gas cell embodiment, the dissociator comprises a catalyst and a component that produces H from the current material. Surface catalysts such as Pt on Ti or Pd, iridium or rhodium alone or on a substrate such as Ti also serve as molecular dissociators combining the catalyst and hydrogen atoms. Preferably, the dissociator such as Pt / Al ₂ O ₃ or Pd / Al ₂ O ₃ has a high surface area.

The H ₂ source can be H ₂ gas. In this embodiment, the pressure can be monitored and adjusted. This is made possible by the catalyst and source of catalyst such as K or Cs metal and LiNH _2, respectively. Because they volatilize at low temperatures that allow the use of high temperature valves. LiNH ₂ also lowers the required operating temperature of the Li cell and is less corrosive. This allows long-term operation using feedthroughs in the case of plasma and filament cells where the filament is a hydrogen dissociator.

A further embodiment of a gas cell hydrogen reactor with NaH as catalyst comprises a reactor cell in the vessel and a filament with dissociator in Na. H ₂ may flow into the main chamber through the container. Power is controlled by controlling the gas flow rate, H ₂ pressure and Na vapor pressure. The latter can be controlled by controlling the container temperature. In another embodiment, the hydrino reaction is initiated by heating with an external heater and the atom H is provided by a dissociator.

  The reaction mixture may be stirred by methods known in the art such as mechanical stirring or mixing. The agitation system may include one or more piezoelectric transducers. Each piezoelectric transducer can provide an ultrasonic agitator. The reaction cell is vibrated and further includes a stir bar such as stainless steel or tungsten ball that is vibrated to stir the reaction mixture. In another embodiment, the mechanical agitation includes ball milling. The reactants may be mixed using these methods, preferably ball milling.

  In some embodiments, the catalyst is formed by mechanical agitation, such as at least one of agitator vibration, ultrasonic agitation, and ball milling. Sonic mechanical shock or compression, such as ultrasound, can cause a reaction or physical change in the reactants to form a catalyst, preferably NaH molecules. The reaction mixture may or may not contain a solvent. The reactant may be a solid such as solid NaH that is mechanically stirred to form NaH molecules. Alternatively, the reaction mixture may include a liquid. The mixture may have at least one Na species. The Na species may be a component of the liquid mixture or in the form of a solution. In one embodiment, a metal suspension in a solvent such as an ether, hydrocarbon, fluorinated hydrocarbon, aromatic compound or heterocyclic aromatic solvent is stirred at high speed to disperse the sodium metal. The solvent temperature may be maintained slightly above the melting point of the metal.

IV. Fuel-Type Embodiments of the present disclosure support at least one hydrogen source and catalyst source that supports a catalyst of hydrogen and forms hydrinos in at least one of the gas phase, liquid phase, and solid phase of a usable mixture of phases. A fuel containing a reaction mixture of The reactants and reactions for solid and liquid fuels provided herein are also heterogeneous fuel reactants and reactions, including phase mixtures.

  The object of the present disclosure is to provide atomic catalysts such as Li and K and Cs, and molecular catalyst NaH. The metal forms a diatomic covalent molecule. Thus, in solid fuel, liquid fuel and heterogeneous fuel embodiments, alloys, composites, composite sources that reversibly form metal catalyst M and decompose or react to provide a catalyst such as Li or NaH, Mixtures, suspensions and solutions are included in the reaction. In another embodiment, at least one of the catalyst source and the atomic hydrogen source further comprises at least one reactant that reacts to form at least one of the catalyst and atomic hydrogen. In another embodiment, the reaction mixture is formed through reaction of one or more reactants or species of the reaction mixture, or formed by physical changes, such as NaH catalyst or NaH catalyst source or Li or K, etc. Contains other catalysts.

The reaction mixture may further comprise a solid that supports the catalytic reaction on the surface. A catalyst or catalyst source such as NaH may be coated on the surface. The coating can be performed by reacting a support such as activated carbon, TiC, WC, and R—Ni with NaH by a method such as ball milling. The reaction mixture may include a heterogeneous catalyst or a heterogeneous catalyst source. In certain embodiments, a catalyst such as NaH is coated on a support such as activated carbon, TiC, WC or polymer, preferably by an incipient wetness method using an apotic solvent such as ether. Support can also be inorganic compounds such as alkali halides may preferably comprise at least one of NaF and HNaF _2. Here NaH acts as a catalyst and uses a fluorinated solvent.

  In the liquid fuel embodiment, the reaction mixture includes at least one of a catalyst source, a catalyst, a hydrogen source, and a catalyst solvent. In other embodiments, the present disclosure of solid fuel and liquid fuel further includes a composite of both and also includes a gas phase. Catalysts having reactants such as catalysts and atomic hydrogen and their source materials in multiple phases are called heterogeneous reaction mixtures and fuels are called heterogeneous fuels. Thus, the fuel is a catalyst that undergoes a transition having a reaction mixture of at least one hydrogen source transitioning to hydrino, a state shown in formula (35), and a reactant in at least one of a liquid phase, a solid phase, and a gas phase. including. Catalysis by the different phases of the catalyst arising from the reactants is well known to those skilled in the art as a heterogeneous catalyst which is an embodiment of the present disclosure. A heterogeneous catalyst provides a surface that causes a chemical reaction and includes embodiments of the present disclosure. The reactants and reactions provided herein for solid and liquid fuels are also heterogeneous fuel reactants and reactions.

For any fuel of the present disclosure, a catalyst or catalyst source such as NaH may be mixed with other components of the reaction mixture such as a support such as HSA material by methods such as mechanical mixing or ball milling. In all cases, hydrogen may be added additionally to maintain the reaction to form hydrinos. The hydrogen gas is at any desired pressure, preferably in the range of 0.1-200 atm. Alternative source materials for hydrogen are NH ₄ X (X is an anion, preferably a halide), NaBH ₄ , NaAlH ₄ , borane, and alkali metal hydrides, alkaline earth metal hydrides, preferably MgH ₂ and rare earth metals It consists of at least one of the group of metal hydrides such as hydrides, preferably LaH ₂ and GdH ₂ .

A. Support In a particular embodiment, the solid, liquid and heterogeneous fuels of the present disclosure comprise a support. The support has properties specific to its function. For example, if the support functions as an electron acceptor or conduit, it is preferred that the support is conductive. In addition, when the support disperses the reactant, the support preferably has a high surface area. In the former case, the support such as the HSA support may include a conductive polymer such as activated carbon, graphene, and heterocyclic polycyclic aromatic hydrocarbon, which are polymers. The carbon preferably includes activated carbon (AC), but also includes other forms such as mesoporous carbon, glassy carbon, coke, graphitic carbon, carbon including dissociated metals such as Pt or Pd, and wt% is 0 The transition metal powder preferably has 1 to 10 layers, more preferably 3 carbon layers, carbon coated with at least one of transition metals, preferably Ni, Co and Mn. , Having a metal or alloy coated carbon, preferably nanopowder. Metals may be inserted into the carbon. When the metal to be inserted is Na and the catalyst is NaH, the Na insertion is preferably saturated. The support preferably has a high surface area. Common classes of organic conductive polymers that act as supports are poly (acetylene), poly (pyrrole), poly (thiophene), poly (aniline), poly (fluorene), poly (3-alkylthiophene), polytetrathiafulvalene , Polynaphthalene, poly (p-phenylene sulfide), and poly (para-phenylene vinylene). These linear main chain polymers are typically known in the art as “black” or “melanin”, such as polyacetylene, polyaniline, and the like. The support may be a mixed copolymer such as one of polyacetylene, polypyrrole and polyaniline. Preferably, the conductive polymer support is at least one of typical derivatives of polyacetylene, polyaniline and polypyrrole. Other supports include elements other than carbon, such as the conductive polymer polythiazyl ((S—N) _x ).

  In another embodiment, the support is a semiconductor. It may be a Group IV element such as carbon, silicon, germanium and α-gray tin. In addition to elemental materials such as silicon and germanium, semiconductor supports include compound materials such as gallium arsenide, indium phosphide, or alloys such as silicon, germanium, or aluminum arsenide. In some embodiments, as the crystal grows, small amounts of dopants such as boron or phosphorus (eg 1 to 10 parts per million) can be added to improve the conductivity of materials such as silicon and germanium crystals. It is. The doped semiconductor can be crushed into a powder and act as a support.

In certain embodiments, the HSA support is a transition metal, noble metal, intermetallic, rare earth, actinide, lanthanide, preferably La, Pr, Nd, and Sm, Al, Ga, In, Tl, Sn, Pb, metalloid, Si, Ge, As, Sb, Te, Y, Zr, Nb, Mo, Tc, Ru, Rh, Pd, Ag, Cd, Hf, Ta, W, Re, Os, Ir, Pt, Au, Hg, alkali metal , Alkaline earth metals, and lanthanide alloys, preferably alloys containing at least two metals or elements of this group, such as LaNi ₅ and Y—Ni. The support may be a noble metal such as Pt, Pd, Au, Ir and Rh or at least one of the supported noble metals such as Pt or Pd on titanium (Pt or Pd / Ti).

In other embodiments, the HSA material is cubic boron nitride; hexagonal boron nitride; wurtzite boron nitride powder; heterodiamond; boron nitride nanotube; silicon nitride; aluminum nitride; titanium nitride (TiN); titanium aluminum nitride (TiAlN) Tungsten nitride; carbon-coated metals or alloys, preferably nanopowder, such as at least one of Co, Ni, Fe, Mn and other transition metal powders, preferably having 1 to 10, more preferably 3 carbon layers; Transition metal, preferably metal or alloy coated carbon such as at least one of Ni, Co and Mn coated carbon, preferably nanopowder; carbide, preferably powder; beryllium oxide (BeO) powder; La ₂ O ₃ , Zr ₂ O _{3, Al} 2 _{O 3,} acid such as sodium aluminate Rare earth powder; and preferably consists of at least one of carbon, such as is the fullerene, graphene or nanotube monolayer.

Carbides, for example, like a salt such as calcium carbide (CaC _2), for example, covalent compounds, such as silicon carbide (SiC) and boron carbide _{(B 4} C or BC _3), and, for example, tungsten carbide One or more binding types of interstitial compounds such as The carbide may be an acetylide such as Au ₂ C ₂ , ZnC ₂ , and CdC ₂ , or a methide such as Be ₂ C, aluminum carbide (Al ₄ C ₃ ), and an A ₃ MC type carbide. . Where A is a transition metal or rare earth metal such as Sc, Y, La—Na, Gd—Lu, and M is a metal or semimetal such as Al, Ge, In, Tl, Sn, and Pb. Is the main group element. Carbides with C ₂ ²⁻ ions are carbides M ₂ ^I C ₂ with a cation M ^I containing one of the alkali metals or coinage metals, carbides M ^II C ₂ with a cation M ^II containing an alkaline earth metal, and , Preferably at least one carbide of the carbide M ₂ ^III (C ₂ ) ₃ with a cation M ^III comprising Al, La, Pr or Tb. The carbide may include ions other than C ₂ ²⁻ , such as those in the group of YC ₂ , TbC ₂ , YbC ₂ , UC ₂ , Ce ₂ C ₃ , Pr ₂ C ₃ , and Tb ₂ C _3. . The carbide may include sesquicarbides such as Mg ₂ C ₃ , Sc ₃ C ₄ , and Li ₄ C ₃ . The carbides are Ln ₃ M (C ₂ ) ₂ , Dy ₁₂ Mn ₅ C ₁₅ , Ln _3.67 FeC ₆ , where M is Fe, Co, Ni, Ru, Rh, Os, and Ir. Ln ₃ Mn (C ₂ ) ₂ (Ln = Gd and Tb) and may include ternary carbides such as those containing transition metals and lanthanide metals that may further contain C ₂ units such as ScCrC ₂ . Carbides may also be classified as “intermediate” transition metal carbides, such as iron carbide (Fe ₃ C or FeC ₂ : Fe). Carbides include lanthanum carbides (LaC ₂ or La ₂ C ₃ ), yttrium carbides, lanthanides such as actinide carbides (MC ₂ and M ₂ C ₃ ), scandium carbides, titanium carbide (TiC), vanadium carbide, chromium carbide, It may be at least one from the group consisting of manganese carbide, cobalt carbide, niobium carbide, molybdenum carbide, tantalum carbide, zirconium carbide, and transition metal carbides such as hafnium carbide. Further, suitable carbides are Ln ₂ FeC ₄ , Sc ₃ CoC ₄ , Ln ₃ MC ₄ (M = Fe, Co, Ni, Ru, Rh, Os, Ir), Ln ₃ Mn ₂ C ₆ , Eu _{3.16. NiC 6, ScCrC 2, Th 2} NiC 2, Y 2 ReC 2, Ln 12 M 5 C 15 (M = Mn, Re), YCoC, Y 2 ReC 2, and other carbides known in the art At least one of the following.

In certain embodiments, the support is a TiC or WC and _{HfC, Mo 2 C, TaC,} YC 2, ZrC, conductive carbides, such as _Al 4 _{C 3} and _{B 4} C. The support may be a metal boride such as an MB2 boride containing material. The support or HSA material is a boride, preferably a conductive two-dimensional network boride such as MB ₂ and M is Cr, Ti, Mg, Zr and Gd (CrB ₂ , TiB ₂ , MgB ₂ , ZrB ₂ , At least one metal in GdB ₂ ).

In the embodiment of the carbon-HSA material, Na is not inserted into the carbon support and does not react with carbon to form acetylide. In some embodiments, the catalyst or catalyst source, preferably NaH, is inserted inside an HSA material such as fullerenes, carbon nanotubes and zeolites. HSA materials are further in graphite, graphene, diamond-like carbon (DLC), hydrogenated diamond-like carbon (HDLC), diamond powder, graphitic carbon, glassy carbon and Co, Ni, Mn, Fe, Y, Pd and Pt. Or carbon containing at least one other metal, or fluorinated carbon, preferably a dopant containing other elements such as fluorinated graphite, fluorinated diamond or fluorinated tetracarbon (C ₄ F). The metal is preferably a mixture such as a mixture of Co, Ni and Mn. The metal may be in any wt% ratio. Preferably, the composition to weight percent (%) ratio is about 20-25% Ni, 60-70% Co, and 5-15% Mn. The HSA material may be a fluoride-coated metal or a passivated fluoride such as carbon, or may include a metal fluoride, preferably a fluoride such as an alkali or rare earth fluoride.

  In another embodiment, the support has a pore size or layer spacing that only fits one catalyst size, such as atomic radius for Li or K and molecular scale for NaH. In the case of Li, the pore diameter or the layer interval is ideally about 1.35 to 3 mm. In the case of K, the pore diameter or layer spacing is ideally about 1.7 to 3.5 mm. In the case of NaH, the pore diameter or layer spacing is ideally about 1.5 to 5 mm. In certain embodiments, based on size identification and selection, the support provides an atomic catalyst such as Li or K and a single catalytic molecule such as NaH. A preferred support having a large surface area and an interlayer separation distance of about 3.5 mm is activated carbon. The activated carbon can be activated or reactivated by physical or chemical activation. The former activation includes carbonization or oxidation, and the latter activation includes chemical impregnation.

  The reaction mixture can further comprise a support, such as a polymer support. Polymer supports include poly (tetrafluoroethylene) such as polytetrafluoroethylene (TEFLON®), polyvinylferrocene, polystyrene, polypropylene, polyethylene, polyisoprene, poly (aminophosphazene), polyethylene glycol or oxide and polypropylene glycol Or polymers containing ether units such as oxides, preferably polyether polyols such as aryl ether, poly (tetramethylene ether) glycol (PTMEG, polytetrahydrofuran, “Terathane”, “polyTHF”), polyvinyl formal, and oxidation It may be selected from materials obtained from the reaction of epoxides such as polyethylene and polypropylene oxide. In some embodiments, the HSA includes fluorine. Examples of fluorinated HSA are polytetrafluoroethylene (TEFLON®), polytetrafluoroethylene (TEFLON®) -PFA, polyvinyl fluoride, PVF, poly (vinylidene fluoride), poly (fluorinated Vinylidene-co-hexafluoropropylene), as well as perfluoroalkoxy polymers.

B. Solid fuel Solid fuel is a catalyst or catalyst source that forms hydrinos, such as at least one catalyst selected from LiH, Li, NaH, Na, KH, K, RbH, Rb and CsH, an atomic hydrogen source, and the following functions: Consisting of one or more other solid chemical reactants: (i) by performing one reaction that occurs between one or more components of the reaction mixture, or by physical or chemical of at least one component of the reaction mixture By making the change, the reactant forms a catalyst or atomic hydrogen; and (ii) the reactant initiates, propagates and maintains the catalytic reaction, forming a hydrino. Many examples of solid fuels described in this disclosure that include a reaction mixture of a liquid fuel that includes a solvent are not meant to be inclusive of solvents. Based on the present disclosure, other reaction mixtures are taught to those skilled in the art.

In the solid fuel embodiment, the reaction mixture comprises a catalyst, a hydrogen source, and at least one of an HSA support, a getter, a dispersant, and an inert gas. The catalyst may be NaH. The inert gas can be at least one of a noble gas and nitrogen. The inert gas is preferably a mixture of Ne and N ₂ , more preferably the mixture is about 50% Ne and 50% N ₂ . The pressure is preferably in the range of about 1 Torr to 100 atmospheric pressure. The pressure of the Ne—N ₂ mixture is preferably 1 atmospheric pressure. The reaction temperature is preferably in the range of about 100 ° C to 900 ° C. The reaction mixture further comprises at least one of Na and NaOH and a reducing agent such as NaH, Sn, Zn, Fe and alkali metals. If the reaction mixture includes NaOH, it is also preferred that H ₂ is provided, and if the reaction mixture includes one or more inert gases, H ₂ includes any mixture gas. The hydrogen source may include hydrogen or hydrides and dissociators such as Pt / Ti, hydrogenated Pt / Ti, Pd, Pt or Ru / Al ₂ O ₃ , Ni, Ti or Nb powder. HSA support, the getter and at least one of Ni dispersants, Ti or Nb _{powder, R-Ni, ZrO 2,} Al 2 O 3, NaX (X = F, Cl, Br, I), Na 2 O, NaOH And at least one of a group of metal powders such as Na ₂ CO ₃ . In some embodiments, the metal catalyzes the formation of NaH molecules from source materials such as Na species and H sources. The metal may be a transition metal, a noble metal, an intermetallic compound, a rare earth metal, a lanthanide metal, an actinide metal, and other metals such as aluminum and tin.

C. Hydino Reaction Activator The hydrino reaction can be activated or initiated and propagated by one or more other chemical reactions. These reactions include (i) an exothermic reaction that provides activation energy for the hydrino reaction, (ii) a conjugation reaction that provides at least one of a catalytic source or atomic hydrogen to assist the hydrino reaction, (iii) certain embodiments A free radical reaction that acts as an electron acceptor from the catalyst during the hydrino reaction, (iv) in one embodiment, an oxidation-reduction reaction that acts as an electron acceptor from the catalyst during the hydrino reaction, (v) a halide. Anion exchange, including sulfides, hydrides, arsenides, oxides, phosphides, and in some embodiments, the action of catalysts that ionize to accept energy from atomic hydrogen to form hydrinos Providing at least one chemical environment for exchange reactions such as nitride exchange, and (vi) hydrino reactions, To promote the movement of electrons, cause a reversible phase or other physical or electronic state change, and lower energy hydrogen products to increase at least one of the range or rate of the hydrino reaction. It is possible to classify into several such as bound getters, supports or matrix-assisted hydrino reactions. In certain embodiments, the reaction mixture includes a support, preferably a conductive support that allows for an activation reaction.

In some embodiments, catalysts such as Li, K, and NaH are accelerated by removing the electrons from the catalyst so as to accelerate the rate-limiting step and accept non-radiative resonance energy transfer from atomic hydrogen to form hydrinos. It works to form hydrinos. Typical metallic forms of Li and K are converted to atomic forms, and the ionic form of NaH is molecularized using a support or HSA material such as activated carbon (AC), Pt / C, Pd / C, TiC or WC. Convert to form and disperse catalysts such as Li and K atoms and NaH molecules respectively. In consideration of surface changes in reaction with other species of the reaction mixture, the support preferably has a high surface area and high conductivity. The reaction for transferring atomic hydrogen forming hydrino requires a catalyst such as Li, K or NaH, and atomic hydrogen, and NaH acts as a catalyst and a source of atomic hydrogen during the concerted reaction. The reaction process of non-radiative energy transfer from atomic hydrogen to the catalyst, which is an integral multiple of 27.2 eV, causes the catalyst to ionize, free electrons to react, and rapidly stop due to charge accumulation. Supports such as AC also acted as conductive electron acceptors and were released from the catalytic reaction by adding a final electron acceptor reactant containing an oxidant, free radicals or their source material to the reaction mixture. The electrons are finally removed to form hydrinos. Also, a reducing agent is added to the reaction mixture to promote the oxidation reaction. The electron acceptor concert reaction is preferably exothermic and heats the reactants to accelerate the reaction rate. The activation energy of the reaction and the propagation of the reaction is realized by free radical reactions such as fast and exothermic oxidation or reaction of O ₂ or CF ₄ combined with Mg or Al, and groups such as CF _x and F and O ₂ And O serve to ultimately accept electrons from the catalyst via a support such as AC. O ₂ , O ₃ , N ₂ O, NF ₃ , M ₂ S ₂ O ₈ (M is an alkali metal), S, CS ₂ , and SO ₂ , MnI ₂ provided in the “electron acceptor reaction” section , EuBr ₂ , AgCl, etc., other oxidizing agents or group source materials may be selected alone or in combination.

Preferably, the oxidant accepts at least two electrons. Corresponding anions may be O ₂ ²⁻ , S ²⁻ , C ₂ S ₄ ²⁻ (tetrathiooxalate anion), SO ₃ ²⁻ and SO ₄ ²⁻ . Two electrons may be received from catalysts that are doubly ionized during catalysis, such as NaH and Li (formulas (25-27) and (37-39)). The addition of the electron acceptor to the reaction mixture or reactor can include solid fuel and heterogeneous catalyst embodiments, as well as electrolysis cells, glow discharge, RF, microwave and other plasma cells, barrier electrode plasma cells and continuously. It applies to all cell embodiments of the present disclosure, such as operated or pulsed mode plasma electrolysis cells. An electronically conductive, preferably non-reactive support such as AC may also be added to the reactants of each embodiment of these cells. Embodiments of microwave plasma cells include hydrogen dissociators such as a metal surface inside a plasma chamber that supports hydrogen atoms.

In an embodiment, a catalyst source, an energy reaction source such as a metal, and at least one of an oxygen source, a halogen source and a free radical source, and a reaction mixture species such as a support, a mixture of compounds or materials are used in combination. May be. The reaction elements of the reaction mixture compounds or materials may also be used in combination. For example, the fluorine or chlorine source may be a mixture of N _x F _y and N _x Cl _y , or the halogen may be mixed with a compound N _x F _y Cl _r or the like. The combination can be determined by one skilled in the art through routine experimentation.

a. Exothermic reaction In certain embodiments, the reaction mixture consists of a catalyst source or catalyst, such as at least one of NaH, K and Li, a hydrogen source or hydrogen, and at least one of performing the reaction. The reaction is preferably highly exothermic and the reaction rate is preferably fast so as to provide active energy for the hydrino catalyzed reaction. The reaction may be an oxidation reaction. A suitable oxidation reaction is the reaction of an oxygen-containing species such as a solvent, preferably an ether solvent, with a metal such as at least one of Al, Ti, Be, Si, P, rare earth metals, alkali metals and alkaline earth metals . More preferably, the exothermic reaction is an alkali or alkaline earth halides, preferably MgF _2, or Al, is formed Si, halides of P, and a rare earth metal. Suitable halide reactions include a solvent, preferably a halide-containing species such as a fluorocarbon solvent, and at least one of a metal and a metal hydride such as Al, at least one of a rare earth metal, an alkali metal and an alkaline earth metal. It is a reaction with one. The metal or metal hydride may be a catalyst or source of catalyst such as NaH, K or Li. The reaction mixture may comprise at least NaH and NaAlCl ₄ or NaAlF ₄ with the products NaCl and NaF, respectively. The reaction mixture may include a fluorosolvent having at least NaH and product NaF.

In general, the product of the exothermic reaction that provides activation energy for the hydrino reaction may be a metal oxide or metal halide, preferably a fluoride. Suitable products are Al ₂ O ₃ , M ₂ O ₃ (M = rare earth metal), TiO ₂ , Ti ₂ O ₃ , SiO ₂ , PF ₃ or PF ₅ , AlF ₃ , MgF ₂ , MF ₃ (M = rare earth _{metals), NaF, NaHF 2, KF} , is KHF 2, LiF and LiHF _2. In embodiments where Ti undergoes an exothermic reaction, the catalyst is Ti ²⁺ having a second ionization energy of 27.2 eV (m = 1 in equation (5)). The reaction mixture may include NaH, Na, NaNH2, NaOH, polytetrafluoroethylene (Teflon®), at least two of fluorocarbons, and a Ti source such as Pt / Ti or Pd / Ti. In embodiments where Al undergoes an exothermic reaction, the catalyst is AlH as shown in Table 3. The reaction mixture may consist of at least two of solvents such as NaH, Al, carbon powder, fluorocarbon, preferably hexafluorobenzene or perfluoroheptane, Na, NaOH, Li, LiH, K, KH and R-Ni. . The product of the exothermic reaction that provides the activation energy is preferably regenerated to form a hydrino and form another cycle of reactant that releases the corresponding power. The metal fluoride product is preferably regenerated to metal and fluorine gas by electrolysis. The electrolyte may also include a eutectic mixture. The metal can be hydrogenated and the carbon product and any CH ₄ and hydrocarbon products can be fluorinated to form the initial metal hydride and fluorocarbon solvent, respectively.

In an exothermic reaction embodiment for activating the hydrino transition reaction, at least one of the group of rare earth metals (M), Al, Ti and Si is M ₂ O ₃ , Al ₂ O ₃ , Ti ₂ O _{3, respectively.} And oxidized to a corresponding oxide such as SiO ₂ . The oxide is an ether solvent such as 1,4-benzodioxane (BDO) and may further contain a fluorocarbon such as hexafluorobenzene (HFB) or perfluoroheptane in order to accelerate the oxidation reaction. As an example reaction, the mixture may include NaH, activated carbon, at least one of Si and Ti, and at least one of BDO and HFB. In the case of Si as the reducing agent, the product SiO ₂ can be regenerated to Si by H ₂ reduction at high temperature or reaction with carbon to form Si and CO and CO ₂ . Particular embodiments of reaction mixtures that form hydrinos include a catalyst or catalyst source, such as at least one of Na, NaH, K, KH, Li and LiH, preferably a fast exothermic reactant source or exothermic reactant. , Activate the catalytic reaction of H, and form hydrino and support. The exothermic reactant may include an oxygen source and a species that reacts with oxygen to form an oxide. When x and y are integers, the oxygen source is H ₂ O, O ₂ , H ₂ O ₂ , MnO ₂ , oxide, carbon oxide, preferably CO or CO ₂ , nitrogen oxide, N ₂ O and NO _N x _{O y,} such as _2, sulfur _oxide, S x _{O y,} preferably _M 2 used with the oxidation catalyst, such as silver ions by case _S x _O y (M is an alkali metal) oxidizing agent, such as, _Cl 2 O Cl _x O _y such as ClO ₂ obtained from NaClO ₂ , preferably the acid is nitronium ion (NO ²⁺ ), NaOCl, I _x O _y , preferably I ₂ O ₅ , P _x O _y , S _x O Concentrated acids such as HNO ₂ , HNO ₃ , H ₂ SO ₄ , H ₂ SO ₃ , HCl, and HF that form _y and mixtures thereof, 1 of nitrites, nitrates, chlorates, sulfates, phosphates Inorganic compound Of metal oxides such as oxyanions, cobalt oxides, oxides or hydroxides of catalysts such as NaOH, organic compounds such as perchlorates and ethers whose cations are catalyst sources such as Na, K and Li An oxygen-containing functional group, preferably one of dimethoxyethane, dioxane and 1,4-benzodioxane (BDO), and the reactant species is at least one of the group of rare earth metals (M), Al, Ti and Si. And the corresponding oxides are M ₂ O ₃ , Al ₂ O ₃ , Ti ₂ O ₃ and SiO ₂ , respectively. The reactant species are Al ₂ O ₃ aluminum oxide, La ₂ O ₃ lanthanum oxide, MgO magnesium oxide, Ti ₂ O ₃ titanium oxide, Dy ₂ O ₃ dysprosium oxide, Er ₂ O ₃ erbium oxide, Eu ₂ O ₃ europium oxide, LiOH lithium hydroxide, _Ho 2 _{O 3} holmium oxide, Li ₂ O, lithium oxide, _Lu 2 _{O 3} lutetium oxide, _Nb 2 _{O 5} and niobium oxide, _Nd 2 _{O 3} neodymium oxide, SiO ₂ silicon oxide, _Pr 2 _{O 3} praseodymium oxide, Sc ₂ O ₃ scandium oxide, SrSiO ₃ strontium metasilicate, Sm ₂ O ₃ samarium oxide, Tb ₂ O ₃ terbium oxide, Tm ₂ O ₃ thulium oxide, Y ₂ O ₃ yttrium oxide and Ta ₂ O ₅ tantalum oxide, B ₂ Of the group of O ₃ boron oxide and zirconium oxide It may contain at least one oxide metal or element therein. The support may comprise carbon, preferably activated carbon. The metal or element is Al, La, Mg, Ti, Dy, Er, Eu, Li, Ho, Lu, Nb, Nd, Si, Pr, Sc, Sr, Sm, Tb, Tm, Y, Ta, B, Zr, It may be at least one of S, P, C and hydrides thereof.

In another embodiment, the oxygen source is at least one of an oxide such as M ₂ O, where M is an alkali metal, preferably a peroxidation such as Li ₂ O, Na ₂ O and K ₂ O, M ₂ O _2. M is an alkali metal, preferably a superoxide such as Li ₂ O ₂ , Na ₂ O ₂ and K ₂ O ₂ , MO ₂ , M is an alkali metal, preferably Li ₂ O ₂ , Na ₂ It can be O ₂ and K ₂ O ₂ . The ionic peroxide may further contain Ca, Sr or Ba.

In another embodiment, at least one of an exothermic reactant or a source of exothermic reactant and a source of oxygen that activates the catalytic reaction of H to form hydrino, preferably with a fast reaction rate. Are MNO ₃ , MNO, MNO ₂ , M ₃ N, M ₂ NH, MNH ₂ , MX, NH 3, MBH ₄ , MAlH ₄ , M ₃ AlH ₆ , MOH, M ₂ S, MHS, MFeSi, M ₂ CO ₃ , MHCO ₃ , M ₂ SO ₄ , MHSO ₄ , M ₃ PO ₄ , M ₂ HPO ₄ , MH ₂ PO ₄ , M ₂ MoO ₄ , MNbO ₃ , M ₂ B ₄ O ₇ (lithium tetraborate), MBO ₂ , _{M 2 WO 4, MAlCl 4,} MGaCl 4, M 2 CrO 4, M 2 Cr 2 O 7, M 2 TiO 3, MZrO 3, MAlO 2, MCoO 2, MGaO 2, M 2 _{eO 3, MMn 2 O 4,} M 4 SiO 4, M 2 SiO 3, MTaO 3, MCuCl 4, MPdCl 4, MVO 3, MIO 3, MFeO 2, MIO 4, MClO 4, MScO n, MTiO n, MVO n _{, MCrO n, MCr 2 O n} , MMn 2 O n, MFeO n, MCoO n, MNiO n, MNi 2 O n, MCuO n, and, MZnO _n, wherein, M is Li, Na, or be a K N = 1, 2, 3, or 4; oxyanion; strong acid oxyanion; oxidant; V ₂ O ₃ , I ₂ O ₅ , MnO ₂ , Re ₂ O ₇ , CrO ₃ , RuO ₂ , _{AgO, PdO, PdO 2, PtO} , PtO 2, I 2 O 4, I 2 O 5, I 2 O 9, SO 2, SO 3, CO 2, N 2 O, NO _{NO 2, N 2 O 3,} N 2 O 4, N 2 O 5, Cl 2 O, ClO 2, Cl 2 O 3, Cl 2 O 6, Cl 2 O 7, PO 2, P 2 O 3 and, Molecular oxidants such as P ₂ O ₅ ; NH ₄ X, where X is nitrate or other suitable anion known to those skilled in the art, F ⁻ , Cl ⁻ , Br ⁻ , I ⁻ , NO ₃ ⁻ , NO ₂ ⁻ , SO ₄ ²⁻ , HSO ₄ ⁻ , CoO ₂ ⁻ , IO ₃ ⁻ , IO ₄ ⁻ , TiO ₃ ⁻ , CrO ₄ ⁻ , FeO ₂ ⁻ , PO ₄ ³⁻ , HPO ₄ ²⁻ , One of the group consisting of H ₂ PO ₄ ⁻ , VO ₃ ⁻ , ClO ₄ ⁻ , and Cr ₂ O ₇ ²⁻ ; and one or more of the group consisting of other anions of the reactant Including. The reaction mixture may additionally contain a reducing agent. In an embodiment, N ₂ O ₅ is formed from the reaction of a mixture of reactants such as P ₂ O ₅ and HNO ₃ that react according to 2P ₂ O ₅ + 12HNO ₃ → 4H ₃ PO ₄ + 6N ₂ O ₅ .

In embodiments where oxygen-containing compounds or oxygen are added to the exothermic reaction, O ₂ functions as a catalyst or source of catalyst. The binding energy of the oxygen molecule is 5.165 eV, and the first, second, and third ionization energies of the oxygen atoms are 13.61806 eV, 35.11730 eV, and 54.9355 eV, respectively. Reactions: O ₂ → O + O ²⁺ , O ₂ → O + O ³⁺ , and 2O → 2O ⁺ provide a net enthalpy of about 2, 4 and 1 times E _h respectively and accept these energies A catalytic reaction to form hydrinos to form H, which causes the formation of hydrinos.

  Also, the exothermic reaction source that activates the hydrino reaction can be a metal alloy that forms a reaction between Pd and Al, preferably initiated by melting Al. The exothermic reaction preferably produces energetic particles that activate the hydrino-forming reaction. The reactant may be a pyrogen or a pyrotechnic composition. In another embodiment, the activation energy is provided by operating the reactants at a very high temperature, such as in the range of about 1000-5000 ° C, preferably about 1500-2500 ° C. The reaction vessel may contain a high temperature stainless steel alloy, a refractory metal or alloy, alumina, or carbon. Increasing the temperature of the reactants can be accomplished by heating the reactor or exothermic reaction.

The exothermic reactant may comprise a halogen element, preferably fluorine or chlorine, and a species that reacts with fluorine or chlorine to form fluoride or chloride, respectively. Suitable sources of fluorine are as follows. Fluorocarbons such as CF ₄ , hexafluorobenzene, hexadecafluoroheptane, preferably BF ₃ , B ₂ F ₄ , BCl ₃ , or BBr ₃ B _x X _y , SF _x such as fluorosilane, nitrogen fluoride , preferably from _{NF 3 N x F y, NF} 3 O, SbFx, preferably BiFx a BiF _5, preferably _N x Cl _y is NCl _3, preferably _SF 4, SF _{6, or, S} 2 F _S x _F y, such as ₁₀ (X is a halogen .x and y are integers.) or SCl is _{2 S} x _{X y,} phosphorus _{fluoride, M} 2 SiF _6, such as Na 2 SiF ₆ and _K 2 SiF ₆ in M an alkali metal, MSIF ₆ M is an alkaline earth metal such as _{MgSiF 6, GaF 3, PF 5} , MPF 6 M is an alkali metal, MaHF And M is an alkaline earth metal in MHF ₂ such as _{KHF 2, K 2 TaF 7,} KBF 4, K 2 MnF 6 _and, is a K 2 ZrF _6, wherein, Li as an alkali metal, Na, or Other similar compounds are also contemplated, such as those in which one of K is replaced with another alkali metal or alkaline earth metal. Suitable sources of chlorine are Cl ₂ gas, SbCl ₅ , and chlorocarbons such as CCl ₄ and chloroform. The reactant species may comprise at least one of the group consisting of alkali or alkaline earth metals or hydrides, rare earth metals (M), Al, Si, Ti, and P forming the corresponding fluoride or chloride. . Preferably, the reactants alkali metal corresponds to that of the catalyst, the alkaline earth hydride is MgH _2, a rare earth element is La, and, Al is nano powder. The support may comprise carbon, preferably activated carbon, mesoporous carbon, and carbon used in Li ion batteries. The reactants can be in any molar ratio. Preferably, the reactant species and fluorine or chlorine are present in approximately stoichiometric ratio as the element of fluoride or chlorine, the catalyst is present in excess, preferably in approximately the same molar ratio as the element reacting with fluorine or chlorine, and The support is present in excess.

The exothermic reactant comprises a halogen gas, preferably chlorine or bromine, or a halogen gas source such as HF, HCl, HBr, HI, preferably CF ₄ or CCl ₄ , and species that react with the halogen to form a halide. Good. Halogen source is also a source of oxygen, such as C _x O _y X _r, where X is halogen, x, y and r are known to those skilled in the art as an integer. The reactant species may include alkali or alkaline earth metals or halides, rare earth metals that form the corresponding halides, Al, Si and P. Preferably, the reactants alkali metal has a corresponding catalyst, alkaline earth hydrides MgH _2, rare earths La, Al is nano powder. The support may comprise carbon, preferably activated carbon. The reactants can be in any molar ratio. Preferably, the reactant species and the halogen are in approximately equal stoichiometric ratio (theoretical mixing ratio), the catalyst is in excess, the molar ratio is approximately the same as the element reacting with the halogen, and the support is in excess. In some embodiments, the reactant Na, NaH, K, KH, Li, catalyst source or catalyst, such as LiH and _{H 2,} halogen gas, preferably chlorine or bromine gas, Mg, MgH _2, at least one rare earth, Preferably it contains La, Gd or Pr, Al, and a support, preferably carbon such as activated carbon.

b. Free radical reaction In some embodiments, the exothermic reaction is a free radical reaction, preferably a halide or oxygen free radical reaction. The source material of the halogen group may be halogen, preferably F ₂ or Cl ₂ , or fluorocarbon, preferably CF ₄ . The F free radical source is S ₂ F ₁₀ . The reaction mixture containing halogen gas may further contain a free radical initiator. The reactor may include an ultraviolet light source to form free radicals, preferably halogen free radicals, more preferably chlorine or fluorine free radicals. Free radical initiators are known in the art, such as metal ion sources such as peroxides, azo compounds and metal salts, preferably cobalt halides such as CoCl _{2 as a} Co ²⁺ source or FeSO ₄ as a Fe ²⁺ source. It is an agent. The latter preferably reacts with an oxygen species such as H ₂ O ₂ or O ₂ . The radical may be neutral.

The oxygen species may include an atomic oxygen source. The oxygen may be singlet oxygen. In some embodiments, singlet oxygen is formed from the reaction of NaOCl and H ₂ O ₂ . In some embodiments, the oxygen source comprises O ₂ and may further comprise a free radical source or a free radical initiator to promote a free radical reaction, preferably a free radical reaction of O atoms. The free radical source or oxygen source may be at least one of ozone or ozonide. In some embodiments, the reactor includes an ozone source, such as a discharge in oxygen, to provide ozone to the reaction mixture.

The free radical source or oxygen source is further a peroxo compound, peroxide, H ₂ O ₂ , a compound containing an azo group, N ₂ O, NaOCl, Fenton reagent or similar reagent, OH radical or its source substance, perxenate ion Or alkali or alkaline earth perxenates, preferably its source material such as sodium perxenate (Na ₄ XeO ₆ ) or potassium perxenate (K ₄ XeO ₆ ), xenon tetroxide (XeO ₄ ) and perxenone An acid (H ₄ XeO ₆ ) may be included as well as at least one of a metal ion source such as a metal salt. The metal salt may be one of cobalt halides such as FeSO ₄ , AlCl ₃ , TiCl ₃ , preferably CoCl ₂ which is a Co ²⁺ source.

In some embodiments, the free radical, such as Cl are, NaH + MgH ₂ + with activated carbon (AC) support + Cl ₂ halogen gas such as a reaction mixture, such as such as to form a halogen such as Cl _2. Free radicals can be formed at temperatures as high as 200 ° C. or higher by reaction of a mixture of hydrocarbons such as Cl ₂ and CH ₄ . The halogen may have a molar concentration greater than that of the hydrocarbon. The chlorocarbon product and Cl radicals can be reacted with a reducing agent to provide an activation energy and pathway that forms hydrinos. The carbon product may be regenerated using synthesis gas (syngas) and the Fischer-Tropsch process or by direct hydrogen reduction of carbon to methane. The reaction mixture may comprise a mixture of O ₂ and Cl _{2 at} a high temperature such as 200 ° C. or higher. The mixture may be reacted to form Cl _x O _y (x and y are integers) such as ClO, Cl ₂ O and ClO ₂ . The reaction mixture can contain H ₂ and Cl ₂ at high temperatures, such as 200 ° C. and above, to react to form HCl. The reaction mixture can contain H ₂ and O ₂ with a recombination agent such as Pt / Ti, Pt / C, or Pd / C at slightly higher temperatures, such as 50 ° C. or higher, and can react to form H ₂ O. The rebinding agent may be operated at a high pressure, such as in the range above 1 atmosphere, preferably in the range of about 2-100 atmospheres. The reaction mixture may have a non-stoichiometric ratio that is advantageous for free radical and singlet oxygen formation. The system can further include an ultraviolet light or plasma source, which can form a free radical, such as RF, microwave, or glow discharge, preferably a high voltage pulsed plasma source. The reactant may further comprise a catalyst that forms at least one of atomic free radicals such as Cl, O and H, singlet oxygen and ozone. The catalyst may be a noble metal such as Pt. In embodiments that form Cl radicals, the Pt catalyst is maintained at a temperature higher than the decomposition temperature of platinum chloride such as PtCl ₂ , PtCl ₃ and PtCl _{4 with} decomposition temperatures of 581 ° C., 435 ° C. and 327 ° C., respectively. In some embodiments, Pt can be recovered from the product mixture containing the metal halide by dissolving the metal halide in a suitable solvent that does not dissolve Pt, Pd or their halides and removing the solution. The solid comprising carbon and Pt or Pd halide may be heated to form Pt or Pd on carbon by decomposition of the corresponding halide.

In some embodiments, N ₂ O, NO ₂ or NO gas is added to the reaction mixture. N ₂ O and NO ₂ can act as a NO radical source. In another embodiment, NO radicals are generated in the cell, preferably by oxidation of NH ₃ . The reaction may be a reaction of NH ₃ and O ₂ on platinum or platinum-rhodium at elevated temperatures. It is possible to produce NO, NO ₂ and N ₂ O by a known industrial method such as the Harbor method followed by the Ostwald method. In one embodiment, an example process sequence is as follows.

Specifically, the harbor method can be used to produce NH ₃ from N ₂ and H ₂ at high temperature and high pressure using a catalyst such as α-iron containing several kinds of oxides. The Ostwald process can be used to oxidize ammonia to NO, NO ₂ and N ₂ O with a catalyst such as a high temperature platinum or platinum-rhodium catalyst. Alkali nitrate can be regenerated by the method disclosed above.

  The system and reaction mixture initiate and assist the combustion reaction and provide at least one of singlet oxygen and free radicals. The combustion reactant may be a non-stoichiometric ratio that is advantageous for the formation of free radicals and singlet oxygen that react with other hydrino reactants. In some embodiments, the explosive reaction is suppressed to favor a stable reaction, or the explosive reaction is caused by a molar ratio with an appropriate reactant to obtain the desired hydrino reaction rate. In certain embodiments, the cell includes at least one cylinder of an internal combustion engine.

c. Electron acceptor reaction In certain embodiments, the reaction mixture further comprises an electron acceptor. During the catalytic reaction that forms hydrinos, when energy is transferred from atomic hydrogen to the electron acceptor, the electron acceptor may act as a sink for ions ionized from the catalyst. Electron acceptors are conductive polymers or metal supports, oxidizing agents such as Group VI elements, molecules, compounds, free radicals, species that form stable free radicals, and halogen atoms, O ₂ , C, CF _{1, 2, 3 or 4} , Si, S, P _x S _y , CS ₂ , S _x N _y and other species having high electron affinity, O and H, Au, At, Al _x O _y (x and y are integers) ), Preferably Al (OH) ₃ and R—Ni Al, ClO, Cl ₂ , F ₂ , AlO ₂ , B ₂ N, CrC ₂ , C ₂ H, CuCl ₂ , CuBr ₂ , MnX ₃ (X = halide), MoX ₃ (X = halide), NiX ₃ (X = halide), RuF _{4,5, or 6} , ScX ₄ (X = halide), WO ₃ Intermediate of reaction with AlO _2, and it may be at least one of other atoms and molecules with known high electron affinity to those skilled in the. In certain embodiments, the support acts as an electron acceptor from the catalyst because the support is ionized by accepting non-radiative resonance energy transfer from atomic hydrogen. Preferably, the support is at least one of conductive and form-stable free radicals. A suitable such support is a conductive polymer. The support may form an anion over the macrostructures such as carbon in Li-ion battery to form a C ₆ ions. In another embodiment, the support is a semiconductor that is preferably doped to promote conductivity. The reaction mixture further comprises free radicals such as O, OH, O ₂ , O ₃ , H ₂ O ₂ , F, Cl and NO, or their source materials, which are free radicals formed on the support during catalysis. Can act as a scavenger. In certain embodiments, free radicals such as NO may form a complex with a catalyst or catalyst source such as an alkali metal. In another embodiment, the support has unpaired electrons. The support is paramagnetic, such as a rare earth element or compound such as Er ₂ O ₃ . In some embodiments, a catalyst or source of catalyst such as NaH, K, Rb or Cs is impregnated into an electron acceptor such as a support and the other components of the reaction mixture are added. Preferably, the support is AC with NaH or Na inserted.

d. In the oxidation-reduction reaction embodiment, the hydrino reaction is activated by an oxidation-reduction reaction. In an empirical example, the reaction mixture includes at least two species of a catalyst, a hydrogen source, an oxidizing agent, a reducing agent, and a support group. The reaction mixture may also include a Group 13 trihalide, preferably at least one Lewis acid such as AlCl ₃ , BF ₃ , BCl ₃ , and BBr ₃ .
In one embodiment, each reaction mixture includes at least one selected from the following elements (i)-(iii).
(I) A catalyst selected from Li, LiH, K, KH, NaH, Rb, RbH, Cs, and CsH.
(Ii) _{H 2} gas, a source of _{H 2} gas, or the hydrogen source is selected from hydride.
(Iii) Halide, phosphide, boride, oxide, hydroxide, silicide, nitrogen compound, arsenide, selenide, telluride, antimonide, carbide, sulfide, hydride, carbonate, hydrogen carbonate, sulfuric acid Salt, hydrogen sulfate, phosphate, hydrogen phosphate, dihydrogen phosphate, nitrate, nitrite, permanganate, chlorate, perchlorate, chlorite, perchlorite, Hypochlorite, bromate, perbromate, bromate, perbromide, iodate, periodate, iodine salt, periodate, chromate, dichromate, tellurate An oxidant selected from one metal compound of selenate, arsenate, silicate, borate, cobalt oxide, tellurium oxide and other oxyanions. Here, these are, for example, halogen compounds, P, B, Si, N, As, S, Te, Sb, C, S, P, Mn, Cr, Co, and Te, and the metal is preferably a transition Including metal, Sn, Ga, In, alkali metal or alkaline earth metal, and the oxidant further includes the following. Lead compounds, such as halogenated _{lead, GeF 2, GeCl 2, GeBr} 2, GeI 2, GeO, GeP, GeS, halides such as GeI _4, and GeCl _4, oxide, or germanium, such as sulfides Compounds, fluorocarbons such as CF ₄ or ClCF ₃ , chlorocarbons such as CCl ₄ , O ₂ , MNO ₃ , MClO ₄ , MO ₂ , NF ₃ , N ₂ O, NO, NO ₂ , B ₃ N ₃ H boron, such as ₆ - nitrogen _{compounds, SF 6, S, sO 2} , sO 3, S 2 O 5 Cl 2, F 5 SOF, sulfur compounds such as _{M 2 S 2 O 8, S} 2 Cl 2, SCl 2 , _S x _{X y,} such as _S 2 Br _{2, or, SOCl 2, SOF 2, sO} 2 F 2, or _sO x _X y as SOBr _2, asClF _{5, X x X 'y, ClO 2} F, ClO 2 F 2, ClOF 3, ClO 3 F, and _{X x} X, such as _{ClO 2 F 3' y O z} , boron such as _B 3 _N 3 _{H 6} as - nitrogen compounds, Se, Te, Bi, as , Sb, Bi, preferably _TeF 4, _{TeF 6} a is TeX _x, TeO _x is preferably TeO ₂ or TeO _3, SeX _x is preferably from SeF _6, preferably Is SeO ₂ or SeO ₃ , SeO _x , TeO ₂ , TeO ₃ , Te (OH) ₆ , TeBr ₂ , TeCl ₂ , TeBr ₄ , TeCl ₄ , TeF ₄ , TeI ₄ , TeF ₆ , CoTe, NiT Tellurium oxide, tellurium halide or other tellurium compounds, SeO ₂ , SeO ₃ , Se ₂ Br ₂ , Se ₂ Cl ₂ , SeBr ₄ , SeCl ₄ , SeF ₄ , SeF ₆ , SeOBr ₂ , SeOCl ₂ , SeOF ₂ , SeO ₂ F ₂ , SeS ₂ , Se ₂ S ₆ , Se ₄ S ₄ , or Se ₆ S ₂ , selenium halide, Or P _x such as other selenium compounds, P, P ₂ O ₅ , P ₂ S ₅ , PF ₃ , PCl ₃ , PBr ₃ , PI ₃ , PF ₅ , PCl ₅ , PBr ₄ F, or PCl ₄ F PO _x X _y , such as X _y , POBr ₃ , POI ₃ , POCl ₃ or POF ₃ , PS _x X _y such as PSBr ₃ , PSF ₃ , PSCl ₃ (M is an alkali metal. x, y and z are integers. X and X ′ are halogen. ), P ₃ N ₅ , (Cl ₂ PN) ₃ , (Cl ₂ PN) ₄ , or phosphorus-nitrogen compounds such as (Br ₂ PN) _x , AlAs, As ₂ I ₄ , As ₂ Se, As ₄ S ₄ , AsBr ₃ , AsCl ₃ , AsF ₃ , AsI ₃ , As ₂ O ₃ , As ₂ Se ₃ , As ₂ S ₃ , As ₂ Te ₃ , AsCl ₅ , AsF ₅ , As ₂ O ₅ , As _{2 S 5} Or arsenic oxide such as As ₂ S ₅ , arsenic halide, arsenic sulfide, arsenic selenide, arsenic telluride, or other arsenic compounds, SbAs, SbBr ₃ , SbCl ₃ , SbF ₃ , SbI ₃ , Sb ₂ O ₃ , SbOCl, Sb ₂ Se ₃ , Sb ₂ (SO 4) ₃ , Sb ₂ S ₃ , Sb ₂ Te ₃ , Sb ₂ O ₄ , SbCl ₅ , SbF ₅ , SbCl ₂ F ₃ , Sb Antimony oxide such as ₂ O ₅ or Sb ₂ S ₅ , antimony halide, antimony sulfide, antimony selenide, antimony telluride or other antimony compounds, BiAsO 4, BiBr ₃ , BiCl ₃ , BiF ₃ , BiF ₅ BisOH, Bi (OH) ₃ , BiI ₃ , Bi ₂ O ₃ , BiOBr, BiOCl, BiOI, Bi ₂ Se ₃ , Bi ₂ S ₃ , Bi ₂ Te ₃ , or Bi ₂ O ₄ , bismuth oxide, halogenated bismuth , Bismuth sulfide, bismuth selenide, bismuth telluride, or other bismuth compounds, SiCl ₄ , SiBr ₄ , CrCl ₃ , ZnF ₂ , ZnBr ₂ , ZnI ₂ , MnCl ₂ , MnBr ₂ , MnI ₂ , CoBr ₂ , CoI _{2, CoCl 2, NiCl 2,} NiBr 2, _{iF 2, FeF 2, FeCl 2} , FeBr 2, FeCl 3, TiF 3, CuBr, CuBr 2, VF 3, and metal halides such as transition metal halides such as CuCl _2, metal hydroxides, or, Metal oxide, SnF ₂ , SnCl ₂ , SnBr ₂ , SnI ₂ , SnF ₄ , SnCl ₄ , SnBr ₄ , SnI ₄ , InF, InCl, InBr, InI, AgCl, AgI, AlF ₃ , AlBr ₃ , AlI _{3 3 3, CdCl 2, CdBr 2,} CdI 2, InCl 3, ZrCl 4, NbF 5, TaCl 5, MoCl 3, MoCl 5, NbCl 5, AsCl 3, TiBr 4, SeCl 2, SeCl 4, InF 3, InCl 3, PbF ₄ , TeI ₄ , WCl ₆ , OsCl ₃ , GaCl ₃ , metal halides such as PtCl ₃ , ReCl ₃ , RhCl ₃ , RuCl ₃ , Y ₂ O ₃ , FeO, Fe ₂ O ₃ , or NbO, NiO, Ni ₂ O ₃ , SnO, SnO ₂ , Ag ₂ O , AgO, Ga ₂ O, As ₂ O ₃ , SeO ₂ , TeO ₂ , In (OH) ₃ , Sn (OH) ₂ , In (OH) ₃ , Ga (OH) ₃ , and Bi (OH) ₃ Metal oxides or metal hydroxides, CO ₂ , As ₂ Se ₃ , SF ₆ , S, SbF ₃ , CF ₄ , NF ₃ , KMnO ₄ and NaMnO ₄ , permanganate, P ₂ O ₅ , nitrates such as LiNO ₃ , NaNO ₃ and KNO ₃ , boron halides such as BBr ₃ and BI ₃ , preferably halogens such as InBr ₂ , InCl ₂ and InI ₃ Group 13 element halide which is indium halide, preferably silver halide, lead halide, cadmium halide, zirconium halide which is AgCl or AgI, preferably transition metal oxide, transition metal sulfide, or transition Second or third transition which is a metal halide (a combination of Sc, Ti, V, Cr, Mn, Fe, Co, Ni, Cu or Zn and F, Cl, Br or I), preferably YF ₃ Series of halides, oxides, preferably sulfides that are Y ₂ S ₃ , or hydroxides, preferably compounds of Y, Zr, Nb, Mo, Tc, Ag, Cd, Hf, Ta, W, Os In the case of halides, compounds such as NbX ₃ , NbX ₅ , or TaX ₅ , Li ₂ S, ZnS, FeS, NiS, MnS, Cu ₂ S, CuS And metal sulfides such as _{SnS, BaBr 2, BaCl 2,} BaI 2, SrBr 2, SrI 2, CaBr 2, CaI 2, MgBr 2, or alkaline earth halide such as MgI _2, EuBr 3, LaF _{3, LaBr 3, CeBr 3,} GdF 3, rare earth halides, such as _{GdBr 3, CeI 2, EuF 2} , EuCl 2, EuBr 2, EuI 2, DyI 2, NdI 2, SmI 2, YbI 2, and TmI ₂ MB ₂ boron such as rare earth halides, metal borides such as europium boride, CrB ₂ , TiB ₂ , MgB ₂ , ZrB ₂ , and GdB ₂ , preferably in a divalent state such as product, LiCl, RbCl, or halogenated alkali, such as CsI, _Ca 3 P Metal phosphides such _{as, PtCl 2, PtBr 2, PtI} 2, PtCl 4, PdCl 2, PbBr 2, and a noble metal halides such as PbI _2, noble metal oxide, noble metal sulphide, rare earth sulfides, such as CeS , Other rare earth sulfides of La and Gd, Na ₂ TeO ₄ , Na ₂ TeO ₃ , Co (CN) ₂ , CoSb, CoAs, Co ₂ P, CoO, CoSe, CoTe, NiSb, NiAs, NiSe, Ni ₂ Metals and anions such as Si and MgSe, rare earth tellurides such as EuTe, rare earth selenides such as EuSe, rare earth nitrides such as EuN, metal nitrides such as AlN, GdN, and Mg ₃ N _{2 , F 2 O, Cl 2 O} , ClO 2, Cl 2 O 6, Cl 2 O 7, ClF, ClF 3, ClOF 3 _{ClF 5, ClO 2 F, ClO} 2 F 3, ClO 3 F, BrF 3, BrF5, I 2 O 5, IBr, ICl, and _{ICl 3, IF, IF 3,} IF 5, IF 7, an oxygen atom, such as Compounds containing at least two atoms from a group of different halogen atom combinations, second or third transition metal halides, halides, oxides, or sulfides such as OsF ₆ , PtF ₆ , or IrF ₆ Alkali metal compounds such as, alkali, alkaline earths, transition metals, rare earths, compounds that can form a group 13 metal that is preferably In, preferably a group 14 metal that is preferably Sn, rare earth hydrides Metal hydrides such as, alkaline earth hydrides, or alkaline hydrides. Here, when the oxidant is a hydride, preferably a metal hydride, the catalyst or source of catalyst may be a metal such as an alkali metal. Suitable oxidants are metal halides, metal sulfides, metal oxides, metal hydroxides, metal selenides, and metal phosphides, such as BaBr ₂ , BaCl ₂ , BaI ₂ , CaBr ₂ , MgBr _2. , or alkaline earth halide such as MgI _2, such as _{EuBr 2, EuBr 3, EuF 3} , LaF 3, GdF 3 GdBr 3, LaF 3, LaBr 3, rare earth halides, such as CeBr _3, YF ₃ Second or third transition series metal halides, metal borides such as CrB ₂ or TiB ₂ , alkali halides such as LiCl, RbCl, or CsI, Li ₂ S, ZnS, Y ₂ S ₃ , FeS, _MnS, metal sulfides such as Cu 2 S, CuS, and _Sb 2 _{S 5,} the _Ca 3 _{P 2} Metal _{phosphides, CrCl 3, ZnF 2, ZnBr} 2, ZnI 2, MnCl 2, MnBr 2, MnI 2, CoBr 2, CoI 2, CoCl 2, NiBr 2, NiF 2, FeF 2, FeCl 2, FeBr 2, Transition metal halides such as TiF ₃ , CuBr, VF ₃ , and CuCl ₂ , SnBr ₂ , SnI ₂ , InF, InCl, InBr, InI, AgCl, AgI, AlI ₃ , YF ₃ , CdCl ₂ , CdBr ₂ , CdI ₂ , metal such as InCl ₃ , ZrCl ₄ , NbF ₅ , TaCl ₅ , MoCl ₃ , MoCl ₅ , NbCl ₅ , AsCl ₃ , TiBr ₄ , SeCl ₂ , SeCl ₄ , InF ₃ , PbF ₄ , and TeI _{4 compound, Y 2 O 3, FeO,} NbO, In (OH _{3, As 2 O 3, SeO} 2, TeO 2, BI 3, CO 2, metal oxides or metal hydroxides, such as _{As 2 Se 3, Mg 3 N} 2, or a metal nitride such as AlN, Ca _{3 P 2, SF 6, S} , SbF 3, CF 4, NF 3, metal phosphides such as _{KMnO 4, NaMnO 4, P 2} O 5, LiNO 3, NaNO 3, KNO 3, and, as BBr ₃ Metal boride. _{BaBr 2, BaCl 2, EuBr 2} , EuF 3, YF 3, CrB 2, TiB 2, LiCl, RbCl, CsI, Li 2 S, ZnS, Y 2 S 3, Ca 3 P 2, MnI 2, CoI 2, NiBr ₂ , ZnBr ₂ , FeBr ₂ , SnI ₂ , InCl, AgCl, Y ₂ O ₃ , TeO ₂ , CO ₂ , SF ₆ , S, CF ₄ , NaMnO ₄ , P ₂ O ₅ , LiNO ₃ , at least 1 One suitable oxidizing agent is included. Suitable oxidizing agents _{include EuBr 2, BaBr 2, CrB 2} , MnI 2, and AgCl, at least one of lists. Suitable oxidizing agents _are, Li 2, including ZnS, and _Y 2 _{S 3,} at least one of. In some embodiments, the oxygen oxidant is Y ₂ O ₃ .

In additional examples, each reaction mixture includes at least one species selected from the following group of components (i)-(iii) described above, and (iv) an alkali metal, alkaline earth metal , Transition metals, second and third transition metals, and rare earth metals, and at least one reducing agent selected from aluminum. _{Preferably, Al, Mg, MgH 2,} Si, La, B, Zr, and Ti powders, and is one from the group of _{H 2.}

  In a further embodiment, each reaction mixture comprises at least one selected from the following genera of components (i) to (iv) described above and is AC, 1% Pt on carbon or Pd (Pt / C, Pd / C) and a support, such as a conductive support selected from carbides, preferably TiC or WC (v).

  The plurality of reactants may be in any molar ratio, but is preferably in an approximately equal molar ratio.

A suitable reaction system comprising (i) a catalyst or catalyst raw material, (ii) a hydrogen source, (iii) an oxidant, (iv) a reducing agent, and (v) a carrier is either NaH or KH as a catalyst or the catalyst source and H as a _{source, BaBr 2, BaCl 2, MgBr} 2, MgI 2, CaBr 2, EuBr 2, EuF 3, YF 3, CrB 2, TiB 2, LiCl, RbCl, CsI, Li 2 S, ZnS, Y 2 S 3, Ca ₃ P ₂ , MnI ₂ , CoI ₂ , NiBr ₂ , ZnBr ₂ , FeBr ₂ , SnI ₂ , InCl, AgCl, Y ₂ O ₃ , TeO ₂ , CO ₂ , SF ₆ , S, CF ₄ , NaMnO ₄ , P _{One of 2} O ₅ , LiNO ₃ , as an oxidizing agent, MgH ₂ may also function as a hydrogen source, but Mg or MgH ₂ as a reducing agent, and AC, TiC, or WC is included as a carrier. In the case where tin hydride is the oxidizing agent, the Sn product may function as at least one of a reducing agent and a conductor support in the catalytic mechanism.

In another suitable reaction, the system comprising (i) a catalyst or catalyst source, (ii) a hydrogen source, (iii) an oxidant and (iv) a support comprises NaH or KH as the catalyst, catalyst source and H source, It consists of one of EuBr ₂ , BaBr ₂ , CrB ₂ , MnI ₂ and AgCl as oxidant and AC, TiC or WC as support. The plurality of reactants may be in any molar ratio, but is preferably in an approximately equal molar ratio.

The catalyst, hydrogen source, oxidizing agent, reducing agent and support may be in any desired molar ratio. Reactants, catalysts comprising KH or _NaH, oxidizing agent containing at least one of CrB 2, AgCl _2, and alkaline earth, transition metal or rare earth halide, preferably or bromide such EuBr _2, BaBr ₂ and MnI ₂ reducing agent comprising a metal halide, Mg or MgH ₂ obtained from the group of iodides, and AC, in embodiments having a support comprising TiC or WC, the molar ratio is about the same. Rare earth halides can be formed by direct reaction of the corresponding halogen with a metal or hydrogen halide such as HBr. The dihalide can be formed from the trihalide by H ₂ reduction.

The additional oxidant forms an intermediate with a high dipole moment or has a high dipole moment. Preferably, species with a high dipole moment readily accept electrons from the catalyst in the catalysis reaction. The species may have a high electron affinity. In one embodiment, the electron acceptor, respectively, filled sp 3, ^3d, and Sn having a half filled shell 4f, Mn, and half filled, or approximately half, such as Gd or Eu compounds Has an electronic shell. Typical oxides of the latter _{type, LaF 3, LaBr 3, GdF} 3, GdCl 3, GdBr 3, EuBr 2, EuI 2, EuCl 2, EuF 2, EuBr 3, EuI 3, EuCl 3, and EuF ₃ . It is a metal corresponding to. In one embodiment, the oxidant has a high oxidation state and further comprises at least one of P, S, Si, and C comprising an atom with a high electronegativity such as at least one of F, Cl, or O. Including non-metallic compounds such as one. In another embodiment, the oxidant comprises a compound of a metal such as Fe and Sn having a low oxidation state, such as divalent, and further a low electrical power, such as at least one of Br or I. Consists of atoms with negative degree. A monovalent negatively charged ion such as MnO ₄ ⁻ , ClO4 ₄ ⁻ , or NO ₃ ⁻ is preferred over a divalent negatively charged ion such as CO ₃ ²⁻ or SO ₄ ^2−. . In an embodiment, the oxidant comprises a compound such as a metal halide corresponding to a metal having a low melting point so that it is melted as a reactive organism and removed from the cell. Suitable oxidants for low melting point metals are In, Ga, Ag, and Sn halides. The reactants can be in any molar ratio, but are preferably in an approximately equal molar ratio.

In certain embodiments, the reaction mixture comprises (i) a catalyst or catalyst source comprising a metal or hydride from a Group I element, (ii) a hydrogen source such as H ₂ gas or H ₂ gas source or hydride, (iii) ) Group 13, 14, 15, 16 and 17 elements; preferably elements selected from the group of F, Cl, Br, I, B, C, N, O, Al, Si, P, S, Se and Te An oxidant comprising an atom or ion or compound comprising at least one of the following: (iv) an element or hydride, preferably selected from rare earth metals such as Mg, MgH ₂ , Al, Si, B, Zr and La A reducing agent comprising the above elements or hydrides, and (v) a support that is preferably electrically conductive and preferably does not react with other species of the reaction mixture to form another compound. Suitable supports preferably include carbon impregnated with carbon such as AC, graphene, Pt or Pd / C and carbide, preferably a metal such as TiC or WC.

In some embodiments, the reaction mixture comprises (i) a catalyst or catalyst source comprising a metal or hydride from a Group I element, (ii) a hydrogen source such as H ₂ gas or H ₂ gas source or hydride, (iii) ) Halides, oxides or sulfide compounds, preferably metal halides, oxides or sulfides, more preferably IA, IIA, 3d, 4d, 5d, 6d, 7d, 8d, 9d, 10d, 11d, 12d Group elements and lanthanide halides, most preferably transition metal halides or lanthanide halide containing oxidants, (iv) elements or hydrides, preferably Mg, MgH ₂ , Al, Si, B, Zr and La, etc. A reducing agent comprising one or more elements or hydrides selected from rare earth metals, and (v) preferably conductive, preferably It consists of a support that does not react with other species of the reaction mixture to form another compound. Suitable supports preferably comprise carbon such as AC, carbide impregnated with a metal such as Pt or Pd / C, and carbide, preferably TiC or WC.

e. Exchange Reaction, Thermoreversible Reaction and Regeneration In certain embodiments, the oxidizing agent and at least one of the reducing agent, source of catalyst and catalyst may react reversibly. In certain embodiments, the oxidant is a halide, preferably a metal halide, more preferably a transition metal, tin, indium, alkali metal, alkaline earth metal and rare earth halide, most preferably a rare earth halide. The reversible reaction is preferably a halide exchange reaction. Preferably, the halide is reversibly exchanged between the oxidizing agent and at least one of the reducing agent, the catalyst source and the catalyst at a temperature between ambient temperature and 3000 ° C., preferably between ambient temperature and 1000 ° C. The reaction energy is preferably low. The reaction equilibrium may be changed to perform a hydrino reaction. The change can occur due to a temperature change, a change in reaction concentration, or a change in reaction ratio. The reaction can be maintained by hydrogenation. In a typical reaction, the exchange is

Wherein n ₁ , n ₂ , x and y are integers, X is a halide, M _ox is a metal of an oxidant, M _{red / cat} is a reducing agent, a catalyst source and at least one metal of a catalyst It is. In some embodiments, the one or more reactants are halides, and the reaction further includes reversible hydride exchange in addition to halide exchange. The reversible reaction may be controlled by adjusting the hydrogen pressure in addition to other reaction conditions such as the temperature and concentration of the reactants. The typical reaction is

である。

It is.

In certain embodiments, alkali metal halides, alkaline earth metal halides, or rare earth halides, preferably RbCl, BaBr ₂ , BaCl ₂ , EuX ₂ or GdX ₃ (where X is a halide or sulfide), most preferably oxidizing agents such as EuBr _2, the catalyst or source of catalyst, preferably NaH or KH, optionally a reducing agent, preferably reacted with Mg or MgH _2, halogen catalyst such as _{M ox} or _M ox _{H 2} and NaX or KX Forms fluoride or sulfide. The rare earth halide can be regenerated by selectively removing the catalyst, or catalyst source, and optionally the reducing agent. In one embodiment, M _ox H ₂ is pyrolyzed and hydrogen gas is removed by a method such as pumping. The halide exchange (formulas (54-55)) forms the catalyst metal. The metal may be removed as a molten liquid leaving the metal halide such as alkaline earth or rare earth halide, or as an evaporative or sublimated gas. The liquid may be removed by methods such as centrifugation or a pressurized inert gas stream. The catalyst or catalyst source is rehydrogenated. This is suitable for regenerating rare earth halides and initial reactants that recombine with the support in the original mixture. When using Mg or MgH ₂ as the reducing agent, Mg can be removed first by forming a hydride with addition of H ₂ , melting the hydride, and removing the liquid. In embodiments where X = F, MgF ₂ products by exchanging rare earths and F such EuH ₂ is can be converted to MgH _2, wherein the MgH ₂ was melt is continuously removed. The reaction may be performed under high pressure H ₂ to favor the formation and selective removal of MgH ₂ . The reducing agent can be rehydrogenated and added to other regeneration reactants to form the original reaction mixture. In another embodiment, the exchange reaction occurs between the oxidant metal sulfide or oxide and at least one of the reducing agent, the catalyst source and the catalyst. Examples of each type of system include 1.66 g KH + 1 g Mg + 2.74 g Y ₂ S ₃ +4 g AC and 1 g NaH + 1 g Mg + 2.26 g Y ₂ O ₃ +4 g AC.

  The selective removal of the catalyst, catalyst source or reducing agent is continuous and the catalyst, catalyst source or reducing agent can be at least partially recycled in the reactor. The reactor further includes a distiller or reflux member to remove the catalyst such as distiller 34, catalyst source or reducing agent of FIG. 4 and return it to the cell. Optionally it can be hydrogenated and further reacted to return the product. The reaction temperature may be circulated between a maximum value and a minimum value, and the reactants may be reused continuously by equilibrium transfer. In some embodiments, the system heat exchanger can rapidly change the cell temperature between high and low values, back and forth equilibration, and promote hydrino reactions.

The regeneration reaction may include a catalytic reaction performed with an added species such as hydrogen. In one embodiment, the source of catalyst and H is KH, and oxidant is EuBr _2. The thermally induced regeneration reaction is as follows.
2KBr + Eu → EuBr2 + ₂ + K (56)
Or _{2KBr + EuH 2 → EuBr 2 +} 2KH (57)
Instead, H ₂ functions as a source of oxidants and catalysts such as KH and EuBr ₂ or as a catalyst regeneration catalyst, respectively.
3KBr + 1 / 2H ₂ + EuH ₂ → EuBr ₃ + 3KH (58)
EuBr ₂ is then formed from EuBr ₃ by H ₂ reduction. A possible route is as follows:
EuBr ₃ + 1 / 2H ₂ → EuBr ₂ + HBr (59)
HB may be recycled as in the following equation, with a net reaction as in the following equation.
HBr + KH → KBr + H ₂ (60)
_{2KBr + EuH 2 → EuBr 2 +} 2KH (61)
The rate of the thermally promoted regeneration reaction can be increased by using different pathways known to those skilled in the art at lower energy.
2KBr + H ₂ + Eu → EuBr ₂ + 2KH (62)
_{3KBr + 3 / 2H 2 + Eu} → EuBr 3 + 3KH (63)
EuBr ₃ + 1 / 2H ₂ → EuBr ₂ + HBr (64)
Since there is an equilibrium between the metal and the corresponding hydride in the presence of H _2, the reaction given by equation (62) is possible.

The course of the reaction may include a lower energy intermediate step known to those skilled in the art as follows:
2KBr + Mg + H ₂ → MgBr ₂ + 2KH (66)
_{MgBr 2 + Eu + H 2 →} EuBr 2 + MgH 2 (67)

KH or K metal may be removed as a molten liquid or evaporating gas or sublimation gas leaving the metal halide such as alkaline earth or rare earth halide. The liquid may be removed by methods such as centrifugation or a flow of pressurized inert gas. In other embodiments, another catalyst or source of catalyst such as NaH, LiH, RbH, CsH, Na, Li, Rb, Cs is substituted with KH or K, and the oxidant is another rare earth halide or alkaline earth halogen. May comprise another metal halide, such as BaCl ₂ or BaBr ₂ .

In other embodiments, the thermoreversible reaction preferably further includes an exchange reaction between two species, each containing at least one metal atom. The exchange occurs between the catalyst metal, such as an alkali metal, and the exchange partner metal, such as an oxidant. Exchange may also occur between the oxidizing agent and the reducing agent. Species to be exchanged are halide, hydride, oxide, sulfide, nitride, boride, carbide, silicide, arsenide, selenide, tellurium compound, phosphide, nitric acid, hydrogen sulfide, carbonate, sulfate , Hydrogen sulfide, phosphate, hydrogen phosphate, dihydrogen phosphate, perchlorate, chromate, dichromate, cobalt oxide and other anions, as well as other oxyanions known to those skilled in the art And anions. At least one of the exchange partners is alkali metal, alkaline earth metal, transition metal, second row transition metal, third row transition metal, noble metal, rare earth metal, Al, Ga, In, Sn, As, Se and Te. May include. Suitable exchange anions are halides, oxides, sulfides, nitrides, phosphides and borides. Suitable metals for exchange are alkali, preferably Na or K, preferably alkaline earth metals, preferably Mg or Ba, and rare earth metals, preferably Eu or Dy, each as a metal or hydride. Examples of catalytic reactants along with examples of exchange reactions are shown below. These reactions are not exhaustive and further examples are known to those skilled in the art.
4 g AC3-3 + 1 g Mg + 1.66 g KH + 2.5 g DyI2, Ein: 135.0 kJ, dissociation energy dE: 6.1 kJ, temperature gradient change TSC: none, maximum temperature _Tmax : 403 ° C., theoretical value is 1 .89 kJ and the gain is 3.22 times.

4 g AC3-3 + 1 g Mg + 1 g NaH + 2.09 g EuF3, Ein: 185.1 kJ, dissociation energy dE: 8.0 kJ, temperature gradient change TSC: none, maximum temperature _Tmax : 463 ° C., theoretical value 1.69 kJ The gain is 4.73 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 3.7 gm CrB ₂ , Ein: 317 kJ, dissociation energy dE: 19 kJ, no temperature gradient change TSC at maximum temperature T _{max to} 340 ° C., theoretical energy is endothermic The target is 0.05 kJ and the gain is infinite.

· 0.70 g of _TiB 2, used up CA-III300 activated carbon powder of 1.66g of KH, 1 g of Mg powder and 4g (AC3-4). The energy gain was 5.1 kJ, but no rapid increase in cell temperature was observed. The maximum cell temperature is 431 ° C. and the theoretical value is zero.

-Used up 0.42 g LiCl, 1.66 g KH, 1 g Mg powder and 4 g AC3-4. The energy gain was 5.4 kJ, but no rapid increase in cell temperature was observed. The maximum cell temperature is 412 ° C., the theoretical value is 0, and the gain is infinite.

1.21 g RbCl, 1.66 g KH, 1 g Mg powder and 4 g AC3-4, energy gain was 6.0 kJ, but no rapid increase in cell temperature was observed. The maximum cell temperature is 442 ° C. and the theoretical value is zero.

4 g AC3-5 + 1 g Mg + 1.66 g KH + 0.87 g LiBr; Ein: 146.0 kJ; dissociation energy dE: 6.24 kJ; temperature gradient change TSC: not observed; maximum temperature T _max : 439 ° C., theoretical value Is endothermic.

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 7.3 gm YF ₃ ; Ein: 320 kJ; dissociation energy dE: 17 kJ; no temperature gradient change TSC at maximum temperature T _max ˜340 ° C .; 4.5X (X to 0.74 kJ ^* 5 = 3.7 kJ).

5.0 gm NaH + 5.0 gm Mg + 20.0 gm CAII-300 + 14.85 gm (dry weight) BaBr ₂ ; Ein: 328 kJ; dissociation energy dE: 16 kJ; no temperature gradient change TSC at maximum temperature T _max -320 ° C The energy gain is 160X (X to 0.02 kJ ^* 5 = 0.1 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 10.4 gm BaCl ₂ ; Ein: 331 kJ; dissociation energy dE: 18 kJ; no temperature gradient change TSC at maximum temperature T _max ˜320 ° C. The energy gain is ˜6.9X (X˜0.52 × 5 = 2.6 kJ).

5.0 gm NaH + 5.0 gm Mg + 20.0 gm CAII-300 + 13.9 gm MgI2; Ein: 315 kJ; dissociation energy dE: 16 kJ; no temperature gradient change TSC at maximum temperature T _max ˜340 ° C. The energy gain is 1.8 × (X˜1.75 × 5 = 8.75 kJ).

4 g AC3-2 + 1 g Mg + 1 g NaH + 0.97 g ZnS; Ein: 132.1 kJ: dissociation energy dE: 7.5 kJ; temperature gradient change TSC: none; maximum temperature T _max : 370 ° C., theoretical value is 1.4 kJ The gain is 5.33 times.

2.74 g Y ₂ S ₃ , 1.66 g KH, 1 g Mg powder and 4 g CA-III300 activated carbon powder (dried at 300 ° C.), energy gain was 5.2 kJ, but cell temperature was It did not rise rapidly. The maximum cell temperature is 444 ° C., the theoretical value is 0.41 kJ, and the gain is 12.64 times.

4 g AC3-5 + 1 g Mg + 1.66 g KH + 1.82 g Ca ₃ P ₂ ; Ein: 133.0 kJ: dissociation energy dE: 5.8 kJ; temperature gradient change TSC: none; maximum temperature T _max : 407 ° C., theory The value is endothermic and the gain is infinite.
20 g AC3-5 + 5 g Mg + 8.3 g KH + 9.1 g Ca3P2, Ein: 282.1 kJ: dissociation energy dE: 18.1 kJ, temperature gradient change TSC: none; maximum temperature T _max : 320 ° C., theoretical value is endothermic The gain is infinite.

In some embodiments, the thermal regeneration reaction system includes:
(I) at least one catalyst or catalyst source selected from NaH and KH;
(Ii) at least one hydrogen source selected from NaH, KH and MgH ₂ ;
_{(Iii) BaBr 2, BaCl 2} , BaI 2, CaBr 2, an alkaline earth halide such MgBr ₂ or _{MgI 2, EuBr 2, EuBr 3} , EuF 3, rare earth halides, such as DyI 2, LaF ₃ or GdF ₃ Second or third row transition metal halides such as YF ₃ , metal borides such as CrB ₂ or TiB ₂ , alkali halides such as LiCl, RbCl or CsI, Li ₂ S, ZnS or Y ₂ S _3, etc. Metal sulfides, metal oxides such as Y ₂ O ₃ , and metal phosphides such as Ca ₃ P ₂ ;
(Iv) at least one reducing agent selected from Mg and MgH ₂ ; and (v) a support selected from AC, TiC and WC.

f. In another embodiment of the getter, support, or matrix-assisted hydrino reaction , the exchange reaction is endothermic. In such embodiments, the metal compound may function as at least one of the preferred supports or matrices for the hydrino reaction or getter for the product to increase the hydrino reaction rate. Typical catalytic reactants and typical supports, matrices, or getters are given below. These reactions are not meant to be exhaustive and further examples will be known to those skilled in the art.
· _Mg of KH + 2.23g of Mg + 1.66g of AC3-5 + 1g of 4g 3 _As 2. Input energy (Ein) is 139.0 kJ. The output energy (dE) is 6.5 kJ. No rapid temperature rise (TSC). The maximum temperature (Tmax) is 393 ° C. In theory, endothermic reaction. Gain is infinite.
20 g AC3-5 + 5 g Mg + 8.3 g KH + 11.2 g Mg3As2. Input energy (Ein) is 298.6 kJ. The output energy (dE) is 21.8 kJ. No rapid temperature rise (TSC). The maximum temperature (Tmax) is 315 ° C. In theory, endothermic reaction. Gain is infinite.
1.01 g Mg ₃ N ₂ , 1.66 g KH, 1 g Mg powder, and 4 g AC3-4 in a 1 inch very rugged cell. The energy gain is 5.2 kJ. However, there was no rapid rise in temperature. Maximum cell temperature is 401 ° C. 0 in theory. Gain is infinite.
• 0.41 g AlN, 1.66 g KH, 1 g Mg powder, and 4 g AC3-5 in a 1 inch very rugged cell. The energy gain is 4.9kJ. However, there was no rapid rise in temperature. Maximum cell temperature is 407 ° C. In theory, endothermic reaction.
In an embodiment, the thermally regenerating reaction system is composed of at least two elements selected from the following (i) to (v).
(I) at least one catalyst or catalyst source selected from NaH, KH, and MgH ₂ ;
(Ii) At least one hydrogen source selected from NaH and KH.
(Iii) at least one oxidant, matrix, second support or getter selected from metal nitrides such as Mg ₃ N ₂ or AlN and metal arsenides such as Mg ₃ As ₂ .
(Iv) At least one reducing agent selected from Mg and MgH ₂ .
(V) At least one support selected from AC, TiC, or WC.

D. Liquid fuel: organic molten solvent system Further embodiments include a molten solid or liquid solvent such as a molten salt contained in chamber 200. The liquid solvent may be evaporated by operating the cell at a temperature above the boiling point of the solvent. A reactant such as a catalyst is dissolved and suspended in a solvent or reactant that forms the catalyst, and H is suspended and dissolved in the solvent. The evaporated solvent acts as a gas containing a catalyst, increases the rate of the hydrogen catalyst reaction, and forms hydrino. The molten solid or evaporating solvent can be maintained by being heated by the heater 230. The reaction mixture further includes a solid support such as an HSA material. The reaction takes place at the surface because there exists an interrelationship between the molten solid, liquid or gaseous solvent and a catalyst such as K or Li and H or NaH and hydrogen. In embodiments using heterogeneous catalysts, the solvent of the mixture may increase the catalytic reaction rate.

In embodiments that include hydrogen gas, H ₂ may be bubbled through the solution. In another embodiment, the concentration of dissolved H ₂ is enhanced cells pressurized. In a further embodiment, it is preferred that the reactants be stirred at a high speed at temperatures as high as the boiling point of the organic solvent and as high as the melting point of the inorganic solvent.

  The organic solvent reaction mixture is preferably heated at a temperature in the range of about 26 ° C to 400 ° C, more preferably in the range of about 100 ° C to 300 ° C. The inorganic solvent mixture superheats to a temperature above that at which the solvent is liquid and below that at which all NaH molecules are decomposed.

a. Organic Solvent The organic solvent may contain one or more moieties that can be modified to another solvent by adding a functional group. The moieties are alkanes, cyclic alkanes, alkenes, cyclic alkenes, alkynes, aromatics, heterocycles and combinations thereof, ethers, halogenated hydrocarbons (fluorinated, chlorinated, brominated, iodinated hydrocarbons), preferably fluorinated And at least one hydrocarbon such as amines, sulfides, nitriles, phosphoramides (eg, OP (N (CH ₃ ) ₂ ) ₃ ), and aminophosphazenes. Groups are alkyl, cycloalkyl, alkoxycarbonyl, cyano, carbamoyl, heterocycles containing C, O, N, S, sulfo, sulfamoyl, alkoxysulfamoyl, phosphono, hydroxyl, halogen, alkoxy, alkylthiol, acyloxy, aryl Alkenyl, aliphatic, acyl, carboxyl, amino, cyanoalkoxy, diazonium, carboxyalkylcarboxamide, alkenylthio, cyanoalkoxycarbonyl, carbamoylalkoxycarbonyl, alkoxycarbonylamino, cyanoalkylamino, alkoxycarbonylalkylamino, sulfoalkylamino, alkyl Sulfamoylalkylamino, oxide, hydroxyalkyl, carboxyalkylcarbonyloxy, cyanoalkyl, Ruboxyalkylthio, arylamino, heteroarylamino, alkoxycarbonyl, alkylcarbonyloxy, cyanoalkoxy, alkoxycarbonylalkoxy, carbamoylalkoxy, carbamoylalkylcarbonyloxy, sulfoalkoxy, nitro, alkoxyaryl, halogenaryl, aminoaryl, alkylaminoaryl , Tolyl, alkenylaryl, allylaryl, alkenyloxyaryl, allyloxyaryl, cyanoaryl, carbamoylaryl, carboxyaryl, alkoxycarbonylaryl, alkylcarbonyloxyaryl, sulfoaryl, alkoxysulfoaryl, sulfamoylaryl and nitroaryl One may be included. Preferably, the group is alkyl, cycloalkyl, alkoxy, cyano, C, O, N, S containing heterocycle, sulfo, phosphono, halogen, alkoxy, alkylthiol, aryl, alkenyl, aliphatic, acyl, alkylamino, It includes at least one of alkenylthio, arylamino, heteroarylamino, halogenaryl, aminoaryl, alkylaminoaryl, alkenylaryl, allylaryl, alkenyloxyaryl, allyloxyaryl and cyanoaryl groups.

  The catalyst may be at least one of NaH molecules, Li and K. In the latter case, LiH and KH can act as catalyst sources. The solvent may be an organic solvent. The solvent may be substantially evaporated at the cell operating temperature, preferably above the boiling point of the solvent. The solvent is preferably polar. The solvent may be an aprotic solvent. Polar and aprotic solvents are solvents that share ionic solubility with protic solvents such as methanol, ethanol, formic acid, hydrogen fluoride and ammonia, but do not have acidic hydrogen. These solvents generally have a high dielectric constant and high polarity. Examples include dimethyl sulfoxide, dimethylformamide, 1,4-dioxane, and hexamethylphosphoramide.

  In one embodiment of the present disclosure, the solvent is 1,4-dioxane, 1,3-dioxane, trioxane, acetylacetaldehyde dimethyl acetal, 1,4-benzodioxane, 3-dimethylaminoanisole, 2,2-dimethyl-1 , 3-dioxolane, 1,2-dimethoxyethane, NN-dimethylformamide dimethyl acetal, NN-dimethylformamide ethylene acetal, diethyl ether, diisopropyl ether, methylal (dimethoxymethane), tetrahydropyran dibenzodioxane, n-butyl Ethyl ether, di-n-butyl ether, allyl ethyl ether, diethylene glycol dibutyl ether, bis (2-ethylhexyl) ether, sec-butyl ethyl ether, dicyclohexyl ether, die Lenglycol diethyl ether, 3,4-dihydro-1H-2-benzopyran, 2,2'-dimethoxybiphenyl, 1,6-dimethoxyhexane, substituted aromatic ethers such as methoxybenzene, methoxytoluene, 2,5-dimethoxytoluene Diphenoxybenzene such as 1,4-diphenoxybenzene, allylphenyl ether, dibenzyl ether, benzylphenyl ether, n-butylphenyl ether, trimethoxytoluene such as 3,4,5-trimethoxytoluene, 2,2 '-Dinaphthyl ether, 2- [2- (benzyloxy) ethyl] -5,5-dimethyl-1,3-dioxane, 1,3-benzodioxole, veratrol (1,2-dimethoxybenzene), anisole , Bis (phenyl) ether, 1,4-die Crown ethers such as xin, dibenzodioxin or dibenzo [1,4] dioxin, divinyl ether, dicyclohexano-18-crown-6, dibenzo-18-crown-6, 15-crown-5, and 18-crown-6 , Bis (4-methylphenyl) ether, bis (2-cyanoethyl) ether, bis (2-dimethylaminoethyl) ether, and at least one of the group of bis [2- (vinyloxy) ethyl] ether. In embodiments that include Na and a hydrogen source, ether is a typical solvent because Na is somewhat soluble in ether and stabilizes sodium ions. These features are convenient for hydrino reactions. In addition to NaH, K or Li can also act as a catalyst for the reaction mixture additionally containing an ether solvent.

In an embodiment, the solvent or HSA material includes functional groups with high bonding moments such as C—O, C═O, C≡N, and C—F. The molecules of the solvent or HSA material may have a high dipole moment. Preferably, the solvent or HSA is an ether, nitrile or halogenated hydrocarbon such as a fluorinated hydrocarbon, preferably consisting of at least one having a very stable bond and preferably polar. Preferably, the fluorocarbon solvent has the formula C _n F _{2n + 2} and some H may be F or aromatic. In another embodiment, the solvent or HSA comprises at least one of the group consisting of a fluorinated organic molecule, a fluorinated hydrocarbon, a fluorinated alkoxy compound, and a fluorinated ether. Typical fluorinated solvents are 1,2-dimethoxy-4-fluorobenzene, flower reverse enzene which is hexa, perfluoroheptane, octafluoronaphthalene, octafluorotoluene, 2H-perfluoro-5,8,11,14. Oxaoctadecane which is tetramethyl-3,6,9,12,15-penta, oxaoctadecane which is perfluoro-5,8,11,14-tetramethyl-3,6,9,12,15-penta, perfluoro (Hydrophenanthrene which is deca that is tetra) and perfluoro-1,3,5-trimethylcyclohexane. Typical fluorinated HSAs are polytetrafluoroethylene (TEFLON®), polytetrafluoroethylene (TEFLON®) -PFA, vinyl fluoride resin, PVF, poly (vinylidene fluoride), poly ( Vinylidene fluoride-co-hexafluoropropylene) and perfluoroalkoxy polymers. Suitable reaction mixtures include octafluoronaphthalene, NaH, and supports such as Ac, TiC, WC, or R-Ni. The reactants can be in any desired ratio, such as octafluoronaphthalene (45 wt%), NaH (10 wt%), and R-Ni (45 wt%).

Examples of other solvents, include fluorocarbon such as fluorocarbon having the formula C _{n F} 2n _{+ 2,} which has several H in place of F, in some cases aromatic. In some embodiments, the fluorinated solvent is perfluoro-methane, perfluoro-ethane, perfluoro-propane, perfluoro-heptane, perfluoro-pentane, perfluoro-hexane, and perfluoro-cyclohexane and other linear and Branched perfluoro-alkanes and partially F-substituted alkanes, bis (difluoromethyl) ether, 1,3-bis (trifluoromethyl) benzene, 1,4-bis (trifluoromethyl) benzene, 2,2 ′, 3,3 ′, 4,4 ′, 5,5 ′, 6,6′-decafluoro-1,1′-biphenyl, o-difluorobenzene, m-difluorobenzene, p-difluorobenzene, 4,4′- Difluoro-1,1′-biphenyl, 1,1-difluorocyclohexane, 1,1-difluoroethane, 1,2-diph Oroethane, 1,1-difluoroethene, cis-1,2-difluoroethene, trans-1,2-difluoroethene, difluoromethane, 2- (difluoromethoxy) -1,1,1-trifluoroethane, 2,2 -Difluoropropane, fluorobenzene, 2-fluoro-1,1'-biphenyl, 4-fluoro-1,1'-biphenyl, 1-fluorobutane, 2-fluorobutane, fluorocyclohexane, 1-fluorocyclohexane, 1-fluoro Decane, fluoroethane, fluoroethene, 1-fluoroheptane, 1-fluorohexane, fluoromethane, 1-fluoro-2-methoxybenzene, 1-fluoro-3-methoxybenzene, 1-fluoro-4-methoxybenzene, (fluoro Methyl) benzene, 2-fluoro-2-methylpropyl Bread, 1-fluoronaphthalene, 2-fluoronaphthalene, 1-fluorooctane, 1-fluoropentane, 1-fluoropropane, 2-fluoropropane, cis-1-fluoropropane, trans-1-fluoropropene, 2-fluoropropane , 3-fluoropropene, 2-fluoropyridine, 3-fluoropyridine, 2-fluorotoluene, 3-fluorotoluene, 4-fluorotoluene, 1-fluoro-2- (trifluoromethyl) benzene, 1-fluoro-3- (Trifluoromethyl) benzene, 1-fluoro-4- (trifluoromethyl) benzene, 1,1,1,2,3,3,3-heptafluoropropane, hexafluorobenzene, 1,1,2,3 4,4-hexafluoro-1,3-butadiene, 1,1,1,4,4 -Hexafluoro-2-butyne, hexafluorocyclobutene, hexafluoroethane, 1,1,1,2,3,3-hexafluoropropane, methyl pentafluoroethyl ether, pentafluorobenzene, pentafluoroethane , Pentafluoromethoxybenzene, 1,1,1,2,2-pentafluoropropane, 2,3,4,5,6-pentafluorotoluene, 1,1,2,4,4-pentafluoro-3- ( Trifluoromethyl) -1,3-butadiene, perfluorobutane, perfluoro-2-butene, perfluoro-2-butyltetrahydrofuran, perfluorocyclobutane, perfluorocyclohexane, perfluorocyclohexene, perfluorodecalin, perfluorodecane, Perfluorodimethoxymethane, per Fluoro-2,3-dimethylbutane, perfluoroethyl ethyl ether, perfluoroethyl 2,2,2-trifluoroethyl ether, perfluoroheptane, perfluoro-1-heptane, perfluorohexane, perfluorohexane Fluoro-1-hexene, perfluoroisobutane, perfluoroisobutene, perfluoroisopropyl methyl ether, perfluoromethylcyclohexane, perfluoro-2-methylpentane, perfluoro-3-methylpentane, perfluoronaphthalene, perfluorononane , Perfluorooctane, perfluorooctylsulfonyl fluoride, perfluorooxetane, perfluoropentane, perfluoropan, perfluoropropene, perfluoropropyl methyl ether, perfluoro Pyridine, perfluorotoluene, perfluorotripropylamine, 1,1,1,2-tetrafluoroethane, 1,1,2,2-tetrafluoroethane, 1,2,2,2-tetrafluoroethyl difluoroethyl Ether, tetrafluoromethane, triflumizole, trifluoroperazine, 1,2,4-trifluorobenzene, 1,3,5-trifluorobenzene, 1,1,1-trifluoroethane, 1,1,2 -Trifluoroethane, trifluoroethene, 2,2,2-trifluoroethyl methyl ether, trifluoromethane, trifluoromethyl difluoromethyl ether, trifluoromethyl 1,1,2,2-tetrafluoroethyl Ether, 1,1,1-trifluoropropane, 3,3,3-trifluoropro , 3,3,3-trifluoro-1-propyne, triflupromazine, undecaandefluorocyclohexane, pentafluorobenzonitrile, trifluoroacetonitrile, (trifluoromethyl) benzene, 3- (trifluoromethyl) benzo It contains at least one of the groups and derivatives of nitrile, 4- (trifluoromethyl) benzonitrile, trifluoro (trifluoromethyl) loxylan and tris (perfluorobutyl) amine.

In another embodiment, the solvent comprises hydrocarbons such as straight chain and branched alkanes, alkenes, alkynes and hydrocarbons having functional groups on the aromatic list. The hydrocarbon solvents are acenaphthene, acenaphthylene, allylbenzene, 1-allylcyclohexene, allylcyclopentane, anthracene, benz [a] anthracene, benzene, benzo [c] chrysene, benzo [g] chrysene, benzo [b] fluoranthene, benzo [J] fluoranthene, benzo [k] fluoranthene, 11H-benzo [a] fluorine, 11H-benzo [b] fluorine, benzo [ghi] perylene, benzo [c] phenanthrene, benzo [a] pyrene, benzo [e] pyrene Benzo [b] triphenylene, 9,9′-bianthracene, bicyclo [2.2.1] heptane, bicyclo [4.1.0] heptane, bicyclo [2,2,1] hept-2-ene, , 1'-bicyclopentyl, 1,1'-binaphthalene, 2,2'-binaphthalene , Biphenyl, 1,3-bis (1-methylethenyl) benzene, (trans) -1,3-butadienylbenzene, 1,3-butadiyne, butane, 1-butene, cis-2-butene, trans-2 -Butene, (trans-1-butenyl) benzene, 2-butenylbenzene, 3-butenylbenzene, 1-butene-3-ene, butylbenzene, secondary butylbenzene, (±), tertiary butylbenzene 2-butyl-1,1′-biphenyl, butylcyclohexane, secondary butylcyclohexane, tertiary butylcyclohexane, butylcyclopentane, 1-tertiary butyl l-3,5-dimethylbenzene, 5-butyldocosane, 11-butyldocosane, 1-tertiary butyl-4-ethylbenzene, 1-tertiary butyl-2-methylbenzene, 1-tertiary butyl 3-methylbenzene, 1-tertiary-butyl-4-methylbenzene, 1-butylnaphthalene, 2-butylnaphthalene, 5-butylnonane, camphene, (+), camphene, (−), 3-carene, (+ ), Α-carotene, β-carotene, β, ψ-carotene, ψ, ψ-carotene, ψ, ψ-carotene-16-ol, cholestane, (5α), cholestane, (5β), cyclobutane, cyclobutene, cyclodecane, Cyclododecane, 1,5,9-cyclodecatriene, cis-cyclododecene, trans-cyclododecene, 1,3-cycloheptadiene, cycloheptane, 1,3,5-cycloheptatriene, cycloheptene, 1,3-cyclohexadiene 1,4-cyclohexadiene, cyclohexane, cyclohexene, 1-cyclohexen-1-ylben Zen, cyclohexylbenzene, cyclohexylcyclohexane, cyclononane, 1,4-cyclooctadiene, cis, cis-1,5-cyclooctadiene, cyclooctane, 1,3,5,7-cyclooctatetraene, 1,3, 5-cyclooctatetriene, cis-cyclooctene, trans-cyclooctene, cyclooctyne, cyclopentadecane, 1,3-cyclopentadiene, cyclopentane, cyclopentene, cyclopentylbenzene, 1,3-decadiene, 1,9-decadiene, Cis-decahydronaphthalene, trans-decahydronaphthalene, decane, 1-decene, cis-2-decene, trans-2-decene, cis-5-decene, trans-5-decene, decylbenzene, decylcyclohexane, decylcyclo Pentane, 11 Decylheneicosan, 1-decylnaphthalene, 1-decyne, 5-decyne, dibenz [a, h] anthracene, dibenz [a, j] anthracene, dibenzo [b, k] chrysene, dibenzo [a, e] pyrene, Dibenzo [a, h] pyrene, dibenzo [a, i] pyrene, dibenzo [a, l] pyrene, o-diethylbenzene, m-diethylbenzene, p-diethylbenzene, 1,1-diethylcyclohexane, 1,2-dihydrobenz [ j] aceanthrylene, 9,10-dihydro-9,10 [1 ′, 2 ′]-benzenoanthracene, 16,17-dihydro-15H-cyclopenta [a] phenanthrene, 2,3-dihydro-1-methyl -1H-indene, 1,2-dihydronaphthalene, 1,4-dihydronaphthalene, 9,10-dihydrophenant Len, 2,3-dihydro-1,1,3-trimethyl-3-phenyl-1H-indene, 1,2-diisopropylbenzene, 1,3-diisopropylbenzene, 1,4-diisopropylbenzene, 2,6-diisopropyl Naphthalene, 7,12-dimethylbenz [a] anthracene, 2,2′-dimethylbiphenyl, 2,3-dimethyl-1,3-butadiene, 2,2-dimethylbutane, 2,3-dimethylbutane, 2,3 -Dimethyl-1-butene, 3,3-dimethyl-1-butene, 2,3-dimethyl-2-butene, 3,3-dimethyl-1-butyne, 1,1-dimethylcyclohexane, cis-1,3- Dimethylcyclohexane, trans-1,3-dimethylcyclohexane, cis-1,4-dimethylcyclohexane, trans-1,4-dimethylcyclo Rhohexane, 1,2-dimethylcyclohexane, 1,3-dimethylcyclohexene, 1,1-dimethylcyclopentane, cis-1,2-dimethylcyclopentane, trans-1,2-dimethylcyclopentane, cis-1,3- Dimethylcyclopentane, trans-1,3-dimethylcyclopentane, 1,2-dimethylcyclopentene, 1,5-dimethylcyclopentene, 1,2-dimethylenecyclohexane, 2,6-dimethyl-1,5-heptadiene, 2, 2-dimethylheptane, 2,3-dimethylheptane, 2,4-dimethylheptane, 2,5-dimethylheptane, 2,6-dimethylheptane, 3,3-dimethylheptane, 3,4-dimethylheptane, 3,5 -Dimethylheptane, 4,4-dimethylheptane, 2,5-dimethyl-1,5- Xadiene, 2,5-dimethyl-2,4-hexadiene, 2,2-dimethylhexane, 2,3-dimethylhexane, 2,4-dimethylhexane, 2,5-dimethylhexane, 3,3-dimethylhexane, 3 , 4-dimethylhexane, 2,3-dimethyl-1-hexene, 5,5-dimethyl-1-hexene, 2,3-dimethyl-2-hexene, 2,5-dimethyl-2-hexene, cis-2, 2-dimethyl-3-hexene, trans-2,2-dimethyl-3-hexene, 1- (1,5-dimethyl-4-hexenyl) -4-methylbenzene, 1,1-dimethylindane, 1,4- Dimethyl-7-isopropylazulene, 1,6-dimethyl-4-isopropylnaphthalene, 2,4-dimethyl-3-isopropylpentane, 1,2-dimethylnaphthalene 1,3-dimethylnaphthalene, 1,4-dimethylnaphthalene, 1,5-dimethylnaphthalene, 1,6-dimethylnaphthalene, 1,7-dimethylnaphthalene, 1,8-dimethylnaphthalene, 2,3-dimethylnaphthalene, 2, , 6-dimethylnaphthalene, 2,7-dimethylnaphthalene, 3,7-dimethyl-1,6-octadiene, 2,2-dimethyloctane, 2,3-dimethyloctane, 2,4-dimethyloctane, 2,5- Dimethyloctane, 2,6-dimethyloctane, 2,7-dimethyloctane, 3,4-dimethyloctane, 3,6-dimethyloctane, cis-3,7-dimethyl-1,3,6-octatriene, trans- 3,7-dimethyl-1,3,6-octatriene, 3,7-dimethyl-1,3,7-octatriene, cis, cis 2,6-dimethyl-2,4,6-octatriene, trans, trans-2,6-dimethyl, 2,4,6-octatriene, 3,7-dimethyl-1-octene, dimethyl-1,3- Pentadiene, 2,2-dimethylpentane, 2,3-dimethylpentane, 2,4-dimethylpentane, 3,3-dimethylpentane, 2,3-dimethyl-1-pentene, 2,4-dimethyl-1-pentene, 3,3-dimethyl-1-pentene, 3,4-dimethyl-1-pentene, 2,3-dimethyl-2-pentene, 2,4-dimethyl-2-pentene, cis-3,4-dimethyl-2- Pentene, cis-3,4-dimethyl-2-pentene, trans-3,4-dimethyl-2-pentene, cis-4,4-dimethyl-2-pentene, trans-4,4-dimethyl-2-pente 4,4-dimethyl-1-pentyne, 4,4-dimethyl-2-pentyne, (1,1-dimethylpropyl) benzene, (2,2-dimethylpropyl) benzene, 2,7-dimethylpyrene, 9, 10-diphenylanthracene, trans, trans-1,4-diphenyl-1,3-butadiene, 1,4-diphenyl-1,3-butadiyne, 1,1-diphenylbutane, 1,2-diphenylbutane, 1,4 -Diphenylbutane, 1,3-diphenyl-1-butene, 1,1-diphenylethane, 1,2-diphenylethane, 1,1-diphenylethane, 1,6-diphenyl-1,3,5-hexatriene, Diphenylmethane, 1,3-diphenylpropane, 2,2-diphenylpropane, 1,1-diphenyl-1-propene, 1,2-di (p-tri ) Ethane, o-divinylbenzene, m-divinylbenzene, p-divinylbenzene, docosan, 1-docosene, 5,7-dodecadiine, dodecane, dodecylcyclohexane, 1-dodecine, 6-dodecyne, dotriacontane, eicosan, ergo Stan, (5α), ergostan, (5β), ethane, ethylbenzene, ethylcyclohexane, 1-ethylcyclohexene, ethylcyclopentane, 1-ethylcyclopentene, 1-ethyl-2,4-dimethylbenzene, 1-ethyl-3 , 5-dimethylbenzene, 2-ethyl-1,3-dimethylbenzene, 3-ethyl-1,2-dimethylbenzene, 4-ethyl-1,2-dimethylbenzene, 3-ethyl-2,2-dimethylpentane, 3-ethyl-2,3-dimethylpentane, 3-ethylheptane 4-ethylheptane, 3-ethylhexane, ethylidenecyclohexane, 1-ethyl-2-isopropylbenzene, 2-ethyl-3-methyl-1-butene, trans-1-ethyl-4-methylcyclohexane, 1-ethyl-1 -Methylcyclopentane, cis-1-ethyl-2-methylcyclopentane, trans-1-ethyl-2-methylcyclopentane, cis-1-ethyl-3-methylcyclopentane, trans-1-ethyl-3-ethyl Cyclopentane, 3-ethyl-4-methylhexane, 4-ethyl-2methylhexane, 3-ethyl-2-methylpentane, 3-ethyl-3-methylpentane, 3-ethyl-2-methyl-1-pentene, 1-ethylnaphthalene, 2-ethylnaphthalene, 3-ethyloctane, 4-ethyloctane, 3-ethyl Rupentane, 2-ethyl-1-pentene, 3-ethyl-1-pentene, 3-ethyl-1-pentene, 3-ethyl-2-pentene, 2-ethylstyrene, 3-ethylstyrene, 4-ethylstyrene, 2 -Ethyltoluene, 3-ethyltoluene, 4-ethyltoluene, 1-ethyl-2,4,5-trimethylbenzene, 2-ethyl-1,3,5-trimethylbenzene, fluoranthene, fulvene, heneicosane, hentria contane, Heptacosane, heptadecane, 1-heptadecene, heptadecylbenzene, 1,6-heptadiene, 1,6-heptadiyne, 2,2,4,4,6,8,8-heptamethylnonane, heptane, 1-heptene, cis- 2-heptene, trans-2-heptene, cis-3-heptene, trans-3-heptene, heptyl Chlohexane, heptylcyclopentane, 1-heptin, 2-heptin, 3-heptin, hexacene, hexacosane, hexadecane, 1-hexadecene, hexadecylbenzene, 1-hexadecine, cis-1,3-hexadiene, trans-1,3 Hexadiene, cis-1,4-hexadiene, trans-1,4-hexadiene, 1,5-hexadiene, cis, cis-2,4-hexadiene, trans, cis-2,4-hexadiene, trans, trans-2 , 4-hexadiene, 1,5-hexadiene-3-yne, 1,5-hexadiyne, 2,4-hexadiyne, hexaethylbenzene, cis-1,2,3,5,6,8a-hexahydro-4,7- Dimethyl-1-isopropylnaphthalene, (1S), hexamethylbenzene, 2,6, 0,15,19,23- hexamethyltetracosane co Sun, hexane, hexatriacontane, cis -
1,3,5-hexatriene, trans-1,3,5-hexatriene, 1-hexene, cis-2-hexene, trans-2-hexene, cis-3-hexene, trans-3-hexene, hexylbenzene , Hexylcyclohexane, hexylcyclopentane, 1-hexylnaphthalene, 1-hexyl-1,2,3,4-tetrahydronaphthalene, 1-hexyne, 2-hexyne, 3-hexyne, indane, indeno [1,2,3- cd] pyrene, isobutane, isobutene, isobutylbenzene, isobutylcyclohexane, isobutylcyclopentane, isopentane, isopentylbenzene, isopropenylbenzene, p-isopropenylisopropylbenzene, p-isopropenylstyrene, isopropylcyclohexane, 4-isopropiyl Heptane, 1-isopropyl-2-methylbenzene, 1-isopropyl-3-methylbenzene, 1-isopropyl-4-methylbenzene, 5-isopropyl-2-methyl-1,3-cyclohexadiene, (R), 1- Isopropyl naphthalene, 2-isopropyl naphthalene, d-limonene, l-limonene, [2,2] metacyclophane, 1-methylanthracene, 2-methylanthracene, 9-methylanthracene, 7-methylbenz [a] anthracene, 8- Methylbenz [a] anthracene, 9-methylbenz [a] anthracene, 10-methylbenz [a] anthracene, 12-methylbenz [a] anthracene, 1-methyl-2-benzylbenzene, 1-methyl-4-benzylbenzene, 2- Methyl biphenyl, 3-methyl biphe 4-methylbiphenyl, 3-methyl-1,2-butadiene, 2-methyl-1,3-butadiene, 2-methyl-1-butene, 3-methyl-1-butene, 2-methyl-2-butene 2-methyl-1-butene-3-yne, 3-methyl-1-butyne, 3-methylchrysene, 5-methylchrysene, 6-methylchrysene, 2-methyl-1,3-cyclohexadiene, 1-methyl Cyclohexene, 3-methylcyclohexene, (±), 4-methylcyclohexene, 1-methyl-1,3-cyclopentadiene, methylcyclopentane, 1-methylcyclopentene, 3-methylcyclopentene, 4-methylcyclopentene, 2-methyldecane, 3-methyldecane, 4-methyldecane, 4-methyl-2,4-diphenyl-1-pentene, methylenecyclohexa , 3-methyleneheptane, 4-methylene-1-isopropylcyclohexene, 5- (1-methylethylidene) -1,3-cyclopentadiene, 1-methyl-9H-fluorene, 9-methyl-9H-fluorene, 2-methyl Heptane, 3-methylheptane, 4-methylheptane, 2-methyl-1-heptene, 6-methyl-1-heptene, 2-methyl-2-heptene, cis-3-methyl-2-heptene, 2-methylhexane 3-methylhexane, 2-methyl-1-hexene, 3-methyl-1-hexene, 4-methyl-1-hexene, 5-methyl-1-hexene, 2-methyl-2-hexene, cis-3- Methyl-2-hexene, cis-4-methyl-2-hexene, trans-4-methyl-2-hexene, cis-5-methyl-2-hexene, tiger Su-5-methyl-2-hexene, cis-2-methyl-3-hexene, trans-2-methyl-3-hexene, cis-3-methyl-3-hexene, trans-3-methyl-3-hexene, 5-methyl-1-hexyne, 5-methyl-2-hexyne, 2-methyl-3-hexyne, cis-1-methyl-4-isopropylcyclohexane, trans-1-methyl-4-isopropylcyclohexane, 1-methyl- 4-isopropylcyclohexene, 1-methyl-7-isopropylphenanthrene, 3-methyl-4-methylenehexane, 1-methyl-4- (5-methyl-1-methylene-4-hexenyl) cyclohexene, (S), 1- Methyl-4- (1-methylvinyl) benzene, 1-methylnaphthalene, 2-methylnaphthalene, 2-methylnonane, 3- Methylnonane, 4-methylnonane, 5-methylnonane, 2-methyl-1-nonene, 2-methyl-2-norbornene, 2-methyloctane, 3-methyloctane, 4-methyloctane, 2-methyl-1-octene, 7 -Methyl-1-octene, cis-2-methyl-1,3-pentadiene, 3-methyl-1,3-pentadiene, 4-methyl-1,3-pentadiene, 2-methylpentane, 3-methylpentane, 2 -Methyl-1-pentene, 3-methyl-1-pentene, 4-methyl-1-pentene, 2-methyl-2-pentene, 3-methyl-cis-2-pentene, 3-methyl-trans-2-pentene 4-methyl-cis-2-pentene, 4-methyl-trans-2-pentene, 3-methyl-3-penten-1-yne, 4-methyl-1-pentyne, -Methyl-2-pentyne, 1-methylphenanthrene, 3-methylphenanthrene, 4-methylphenanthrene, 2-methyl-1-propene, trimer, cis- (1-methyl-1-propenyl) benzene, trans- ( 1-methyl-1-propenyl) benzene, 1-methyl-2-propylbenzene, 1-methyl-3-propylbenzene, 1-methylpyrene, 2-methylpyrene, 2-methylstyrene, 3-methylstyrene, 4-methylstyrene 2-methylandecane, 3-methylandecane, 1-methyl-4-vinylcyclohexane, β-myrcene, naphthacene, naphthalene, nonadecane, 1,8-nonadiene, 1,8-nonadiene, nonane, 1-nonene, Nonylbenzene, nonylcyclohexane, nonylcyclopentane, 1-nonylnaphthalene , 1-nonine, octacosane, octadecahydrochrysene, octadecane, 1-octadecene, octadecylbenzene, octadecylcyclohexane, 1,7-octadiene, 1,7-octadiyne, 1,2,3,4,5,6,7 , 8-octahydroanthracene, octahydroindene, 1,2,3,4,5,6,7,8-octahydrophenanthrene, octane, 1,3,5,7-octatetraene, 1-octene, cis 2-octene, cis-3-octene, trans-3-octene, cis-4-octene, trans-4-octene, 1-octene-3-yne, octylbenzene, octylcyclohexane, octylcyclopentane, 1-octyne 2-octyne, 3-octyne, 4-octyne, 1,3-pentadiyne, pentaeth Benzene, pentamethylbenzene, 2,2,4,6,6-pentamethylheptane, 2,2,4,6,6-pentamethyl-3-heptene, 2,2,3,3,4-pentamethylpentane, 2,2,3,4,4-pentamethylpentane, pentane, pentaphen, pentatriacontane, 1-pentene, cis-2-pentene, trans-2-pentene, 1-pentene-3-yne, 1-pentene- 4-in, cis-3-penten-1-in, trans-3-penten-1-in, pentylbenzene, pentylcyclohexane, pentylcyclopentane, 1-pentylnaphthalene, 1-pentyne, 2-pentyne, perylene, α -Ferlandolene, β-Ferandolene, phenanthrene, phenylacetylene, 9-phenylanthracene, 2-phenyl- , 3-butadiene, 2-phenyl-1-butene, 1-phenyl-1H-indene, 1-phenylnaphthalene, 2-phenylnaphthalene, 5′-phenyl-1,1 ′: 3 ′, 1 ″ -terphenyl, Picene, propane, propene, cis-1-propenylbenzene, trans-1-propenylbenzene, propylbenzene, propylcyclohexane, propylcyclopentane, 4-propylheptane, 1-propylnaphthalene, pyrene, 1,1 ′: 4 ′, 1 ″: 4 ″, 1 ″ ′-quaterphenyl, spiro [5.5] andecane, squalene, cis-stilbene, trans-stilbene, styrene, o-terphenyl, m-terphenyl, p-terphenyl, α -Terpinene, γ-terpinene, tetracosane, tetradecahydrophenanthrene, tetradecane Tetradecylbenzene, tetradecylcyclohexane, 1,2,3,5-tetraethylbenzene, 1,2,3,4-tetrahydro-1,5-dimethylnaphthalene, 1,2,3,4-tetrahydro-1-methylnaphthalene 1,2,3,4-tetrahydro-5-methylnaphthalene, 1,2,3,4-tetrahydro-6-methylnaphthalene, 1,2,3,4-tetrahydronaphthalene, 1,2,3,4-tetrahydro Phenanthrene, 1,2,3,4-tetrahydro-1,1,6-trimethylnaphthalene, 1,2,3,4-tetramethylbenzene, 1,2,3,5-tetramethylbenzene, 1,2,4 , 5-tetramethylbenzene, 2,2,3,3-tetramethylbutane, 1,2,3,4-tetramethylcyclohexane, 1,1,3,3-tetra Tylcyclopentane, 1,1,2,2-tetramethylcyclopropane, 2,2,3,3-tetramethylhexane, 2,2,5,5-tetramethylhexane, 3,3,4,4-tetra Methylhexane, 2,2,3,3-tetramethylpentane, 2,2,3,4-tetramethylpentane, 2,2,4,4-tetramethylpentane, 2,3,3,4-tetramethylpentane 1,1,4,4-tetraphenyl-1,3-butadiene, 1,1,2,2-tetraphenylethane, 1,1,2,2-tetraphenylethene, tetraphenylmethane, 5,6, 11,12-tetraphenyl naphthacene, triacontane, tricosane, tricyclo ^{[3.3.1 3,7]} decane, tridecane, 1-tridecene, tridecyl benzene, tridecyl cyclohexane 1-tridecine, 1,2,3-triethylbenzene, 1,2,4-triethylbenzene, 1,3,5-triethylbenzene, 1,2,4-triisopropylbenzene, 1,3,5-triisopropylbenzene 1,2,3-trimethylbenzene, 1,2,4-trimethylbenzene, 1,3,5-trimethylbenzene, 1,7,7-trimethylbicyclo [2.2.1] heptane, 1,7,7 -Trimethylbicyclo [2.2.1] hept-2-ene, 2,2,3-trimethylbutane, 2,3,3-trimethyl-1-butene, 1,1,2-trimethylcyclohexane, 1,1, 3-trimethylcyclopentane, 1α, 2α, 4β-1,2,4-trimethylcyclopentane, 2,2,6-trimethylheptane, 2,5,5-trimethylheptane, 3, , 5-trimethylheptane, 3,4,5-trimethylheptane, 2,2,3-trimethylhexane, 2,2,4-trimethylhexane, 2,3,3-trimethylpentane, 2,3,4-trimethylpentane 2,3,3-trimethyl-1-pentene, 2,4,4-trimethyl-1-pentene, 2,3,4-trimethyl-2-pentene, 1,1,2-triphenylethane, 1,1 , 2-triphenylethene, triphenylmethane, tritriacontane, 1,10-andadiene, andecane, 1-andedecane, cis-2-andedecane, trans-2-andedecane, cis-4-andedecane, trans-4-andedecane Cis-5-decane, trans-5-andedecane, anddecylbenzene, 1-undecine, 2-undecine, vinylcyclo Hexane, 1-vinylcyclohexane, 4-vinylcyclohexane, vinylcyclopentane, 6-vinyl-6-methyl-1-isopropyl-3- (1-methylethylidene) cyclohexene, (S), 1-vinylnaphthalene, It may be at least one of the derivatives of the group consisting of 2-vinylnaphthalene, 2-vinyl-5-norbornene, o-xylene, m-xylene, and p-xylene.

  In another embodiment, the solvent is tributylamine, triethylamine, triisopropylamine, N, N-dimethylaniline, tris (N, N-dimethylaniline), allyldiethylamine, amines such as allyldimethylamine, benzo [f] quinoline, Bis [4- (dimethylamino) phenyl] methane, 4,4′bis- (dimethylamino) triphenylmethane, butyldimethylamine, pentane, hexane, heptane, octane, cyclopentane, cyclohexane, dipentene, methylcyclohexane, 2- Hydrocarbon solvents such as methylpentane, octane, tetrahydrofuran (THF), alkanes such as pinene, styrene, terpinene and mineral oil, alkenes and alkynes, toluene, o-xylene, m-xylene, p-xylene, ethylben , Cumene (isopropylbenzene), p-cymene (1-methyl-4-isopropylbenzene), mesitylene (1,3,5-trimethylbenzene), propylbenzene, pseudocumene (1,2,4-trimethylbenzene), naphthalene , Decalin (cis and trans decahydronaphthalene), tetralin (1,2,3,4-tetrahydronaphthalene), pyrrole, furan, 2,5-diphenylfuran, thiophene, imidazole, pyridine, pyrimidine, pyrazine, quinoline, isoquinoline , Indole, acridine, 1,2-dimethylindole, 9,9′-dioxane ethylidene, 2,6-lutidine (2,6-dimethylpyridine), 2-picoline (2-methylpyridine) Aromatic and acetonitrile Nitrile groups, such as finely propanenitrile comprises at least one. In certain embodiments, the amino group is attached to aryl. Suitable amino solvents are preferably N, N-, such as N-benzyl-N-ethylaniline having a plurality of alkylated amino groups 0 on 1,3,5-tris- (N, N-dimethylamino) benzene. Dimethylaniline analogue.

In another embodiment, the solvent is dimethylformamide (DMF), dimethylacetamide (DMA), dimethyl sulfoxide (DMSO), 1,3-dimethyl-2-imidazolidinone (DMI), hexamethylphosphoric acid amide (HMPA), N-methyl-2-pyrrolidone (NMP), 4-dimethylaminobenzaldehyde, acetone, dimethylacetone-1,3-dicarboxylate, 3 ′, 4′-dimethylacetophenone, dimethyl methylphosphonate, hexamethylcyclotrisiloxane, hexamethyl Phosphorous acid triamide, tributyl phosphite, tributyl borate, triethyl borate, tri-n-butyl borate, triphenyl boron, triethyl phosphite, triethyl phosphine, tri-n-butyl phosphine, boric acid Trimethyl borate Methylene, trimethyl phosphite, triphenyl phosphite, tris (phenyl) phosphine, ferrocene, nickelocene, organometallic compounds, dimethyl selenium, dimethyl telluride, tetraethyl lead, ethyl trimethyl lead, tetra-n-butyl lead, phenyl Organometallic compounds such as thiobenzene and diphenyl selenide, trimethylstibine, tetra-n-butylgermanium, tetrapropyltitanate, tetrabutyltitanate, tributylaluminate, tributylaluminum, triethylstibine, trimethylarsine, Alkyl sulfides such as trimethylindium and triphenylstibine, diethyl sulfide and bis (phenyl) sulfide, alkyl selenides such as diethyl selenide, alkyl esters such as diethyl telluride Luluide, diethyl sulfoxide, allyl ethyl ether, aluminum ethanol adduct, aluminum ethoxide, aluminum sec-butoxide, trimethyl borate, triethyl borate, tripropyl borate, tributyl borate, trihexyl borate, triphenyl stibine, 1,3-benzodioxole, benzofuran, 2H-1-benzopyran, benzothiazole, benzo [b] thiophene, benzoxazole, N-benzyl-N-ethylaniline, benzyl ethyl ether, benzyl methyl ether, benzyl phenyl ether 2,2′-bipyridine, 1,3-bis (1-methyl-4-piperidyl) propane, bis (4-methylphenyl) ether, bis (phenyl) ether, bis (4-methylphenyl) sulfide, bis (Mechi Ruthio) methane, 1,2-bis (N-morpholino) ethane, 2,2′-bithiophene, 1- (2-butoxyethoxy) -2-propanol, 1-butoxy-4-methylbenzene, 4- [3- (4-Butoxyphenoxy) propyl] morpholine, butyl ethyl ether, sec-butyl ether, t-butyl ethyl ether, butyl ethyl sulfide, t-butyl ethyl sulfide, butyl isobutyl ether, t-butyl isobutyl ether, t-butyl isopropyl Ether, 1-t-butyl-4-methoxybenzene, butyl methyl ether, sec-butyl methyl ether, butyl phenyl ether, N-butyl piperidine, butyl propyl ether, butyl vinyl ether, t-butyl vinyl ether, dibenzyl ether, 1 , 4-Dibutoxybe , 1,2-dibutoxyethane, dibutoxymethane, dibutyl ether, di-secondary butyl ether, di-tert-butyl ether, dicyclomine hydrochloride, diethyl ether, dicyclopentyl ether, 1,2-diethoxybenzene, 1 , 4-diethoxybenzene, 1,1-diethoxy-N, N-dimethylmethanamine, 1,1-dimethoxyethane, 1,2-dimethoxyethane, dimethoxymethane, 2- (diethoxymethyl) furan, 1,1 -Diethoxypentane, 1,1-diethoxypropane, 2,2-diethoxypropane, 3,3-diethoxy-1-propene, 3,3-diethoxy-1-propyne, N, N-diethylaniline, diethyleneglyco- Rudibutyl ether, diethylene glycol diethyl ether, diethylene glycol Methyl ether, diethyl telluride, difurfuryl ether, diheptyl ether, dihexyl ether, 2,3-dihydro-1,4-benzodioxine, 2,3-dihydrobenzofuran, 3,4-dihydro-1H-2-benzopyran, 3,4-dihydro-2H-1-benzopyran, 2,5-dihydro-2,5-dimethoxyfuran, 2,3-dihydro-1,4-dioxin, 3,6-dihydro-4-methyl-2H-pyran 4,5-dihydro-2-methylthiazole, 3,4-dihydro-2H-pyran, 3,6-dihydro-2H-pyran, diisopentyl, ether, diisopropyl ether, 1,2-dimethoxybenzene, 1, 3-dimethoxybenzene, 1,4-dimethoxybenzene, 1,2-dimethoxyethane, 4,8-dimethoxyph [2,3-b] quinoline, dimethoxymethane, 1,2-dimethoxy-4-methylbenzene, 1,3-dimethoxy-5-methylbenzene, 1,4-dimethoxy-2-methylbenzene, 1,2-dimethyl -1H-imidazole, 1,3-dimethyl-1H-indole, dimethyl selenide, 1,3-dioxane, 1,3-dioxepane, 1,3-dioxolane, 1,2-diphenoxyethane, diphenyl selenide, 1 , 2-dipropoxyethane, dipropoxymethane, dipropyl ether, divinyl ether, divinyl sulfide, 3-ethoxy-N, N-diethylaniline, 2-ethoxy-3,4-dihydro-2H-pyran, 1-ethoxy- 2-methoxyethane, ethyltrimethyllead, indolizine, 4-methoxypyridine, 6-methoxyquinoline, 1 -Methyl-3-phenoxybenzene, 1-methyl-4- (phenylthio) benzene, methyltriethyllead, 1,4-oxathiane, oxazole, oxepane, pteridine, tetraethoxygermane, titanium (IV) n-butoxide, tetratitanate Propyl, tributyl aluminate, tributylaluminum, tributyl borate, tributyl phosphite, 1,3,5-triethoxybenzene, triethyl borate, triethylphosphine, triethyl phosphite, triethylstibine, trimethylindium, phosphorous acid Trimethyl, trimethylstibine, triphenylstibine, N- (1-cyclopenten-1-yl) pyrrolidine, cyclopentyl methyl sulfide, decamethylcyclopentasiloxane, decamethyltetrasiloxane, N, N-di Ril-2-propen-1-amine, diallyl sulfide, dibenzofuran, benzo [b] thiophene, dibenzothiophene, dibenzyl sulfide, N, N-dibutylaniline, 2,6-di-tert-butylpyridine, dibutyl sulfide, di Secondary-butyl sulfide, di-tertiary-butyl sulfide, didecyl ether, diethylmethylamine, N, N-diethyl-2-methylaniline, N, N-diethyl-4-methylaniline, N, N-diethyl -1-naphthaleneamine, N, N-diethyl-10H-phenothiazine-10-ethanamine, N, N-diethyl-α-phenylbenzenemethanamine, diethyl sulfide, diheptyl sulfide, dihexyl sulfide, 2,3-dihydrofuran, 2 , 5-dihydrofuran, 2,3-dihydro-2-methylbenzofuran, 2,3-dihydrothio Phen, 2,5-dihydrothiophene, diisobutyl sulfide, diisopentyl sulfide, diisopropyl sulfide, 1,2-dimethoxy-4-allylbenzene, 4,7-dimethoxy-5-allyl-1,3-benzodioxole, 4, 4'-dimethoxy-1,1'-biphenyl, 1,1-dimethoxydodecane, (2,2-dimethoxyethyl) benzene, 1,1-dimethoxyhexadecane, 1,2-dimethoxy-4- (1-propenyl) benzene 4,5-dimethoxy-6- (2-propenyl) -1,3 benzodioxole, 1,2-dimethoxy-4-vinylbenzene, 2- (p-dimethylaminostyryl) benzothiazole, 2,6-dimethyl Anisole, 3,5-dimethylanisole, 2,5-dimethylbenzoxazole, N, N-dimethylbenzylamino N, N-dimethyl-N′-benzyl-N′-2-pyridinyl-1,2-ethanediamine, 4′-dimethyl-2,2′-bipyridine, dimethyldecylamine, dimethyl ether, (1,1-dimethyl) Ethoxy) benzene, 2,5-dimethylfuran, N, N-dimethyl-1-naphthylamine, N, N-dimethyl-2-naphthylamine, 2,9-dimethyl-1,10-phenanthroline, 1,4-dimethylpiperazine, 1,2-dimethylpiperidine, N, N-dimethyl-1-propanamine, 2,3-dimethylpyrazine, 2,5-dimethylpyrazine, 2,6-dimethylpyrazine, 1,3-dimethyl-1H-pyrazole N, N-dimethyl-2-pyridinamine, N, N-dimethyl-4-pyridinamine, 2,3-dimethylpyridine, 2,4-dimethyl Lysine, 2,5-dimethylpyridine, 2,6-dimethylpyridine, 3,4-dimethylpyridine, 3,5-dimethylpyridine, 4,6-dimethylpyrimidine, 1,2-dimethylpyrrolidine, 2,4-dimethylquinoline 2,6-dimethylquinoline, 2,7-dimethylquinoline, 2,3-dimethylquinoxaline, dimethyl sulfide, dimethyl telluride, 2,5-dimethyl-1,3,4-thiadiazole, 2,7-dimethylthianthrene 2,4-dimethylthiazole, 4,5-dimethylthiazole, 2,3-dimethylthiophene, 2,4-dimethylthiophene, 2,5-dimethylthiophene, 3,4-dimethylthiophene, 2,6-dimethyl-4 -Tridecyl morpholine, dinonyl ether, dioctyl ether, dioctyl sulfide, dipentyl ether Ter, dipentyl sulfide, 2,5-diphenyloxazole, 1- (3,3-diphenylpropyl) piperidine, 1,4-bis (4-methyl-5-phenyloxazol-2-yl) benzene, diphenyl sulfide, N, N-dipropylaniline, dipropyl sulfide, 1,3-dithiane, 1,4-dithiane, 1,3-dithiolane, 1-dodecylpiperidine, dothiepine, doxepin, doxylamine, 1-ethoxy-3-methylbenzene, 1-ethoxy -4-methylbenzene, 2-ethoxy-2-methylbutane, 1-ethoxynaphthalene, 2-ethoxynaphthalene, 2-ethyl-1H-benzimidazole, 9-ethyl-9H-carbazole, ethyldimethylamine, 3-ethyl-2 , 5-dimethylpyrazine, 2-ethylfuran, ethylhexyl ether 1-ethyl-1H-imidazole, ethyl isopentyl ether, ethyl isopropyl ether, N-ethyl-N-isopropyl-2-propanamine, ethyl isopropyl sulfide, 1-ethyl-4-methoxybenzene, N-ethyl-N- Methylaniline, 1-ethyl-2-methyl-1H-benzimidazole, 2-ethyl-2-methyl-1,3-dioxalane, ethyl methyl ether, 2-ethyl-5-methylpyrazine, 3-ethyl-4-methyl Pyridine, 4-ethyl-2-methylpyridine, ethylmethyl sulfide, N-ethylmorpholine, 1-ethylpiperidine, ethylpropyl ether, 2- (1-ethylpropyl) pyridine, 4- (1-ethylpropyl) pyridine, Ethylpropyl sulfide, 2-ethylpyrazine, 2-ethylpyridine, -Ethylpyridine, 4-ethylpyridine, 1-ethyl-1H-pyrrole, 2-ethyltetrahydrofuran, (ethylthio) benzene, ethyl thiocyanate, 1- (ethylthio) -4-methylbenzene, 2-ethylthiophene, ethyl vinyl ether, hexa Butyl distanoxane, hexadecyl dimethylamine, hexadecyl vinyl ether, 2,3,4,6,7,8-hexahydropyrrolo [1,2-a] pyrimidine, hexahydro-1,3,5-triphenyl-1 , 3,5-triazine, hydrocotalnin, hydrohydrastine, imipramine, isobutyldimethylamine, isopropyl methyl ether, isopropyl methyl sulfide, isopropyl propyl sulfide, (isopropyl thio) benzene, isopropyl vinyl ether, mebuhydride Rollin, 2-methoxy-1,1′-biphenyl, 4-methoxy-1,1′-biphenyl, 1-methoxy-1,3-butadiene, 2-methoxy-1,3-butadiene, 1-methoxy-1- Buten-3-yne, methoxycyclohexane, (2-methoxyethoxy) ethene, 2- (2-methoxyethyl) pyridine, 2-methoxyfuran, 4-methoxyfuro [2,3-b] quinoline, 2-methoxy-2- Methylbutane, 2- (methoxymethyl) furan, 1-methoxynaphthalene, 2-methoxynaphthalene, trans-1-methoxy-4- (2-phenylvinyl) benzene, 2-methoxy-1-propene, 3-methoxy-1- Propene, trans-1-methoxy-4- (1-propenyl) benzene, 1-methoxy-4- (2-propenyl) benzene, 1- Toxi-4-propylbenzene, 2-methoxypyridine, 3-methoxypyridine, 3-methoxypyridine, (2-methoxyvinyl) benzene, 2-methylanisole, 3-methylanisole, 4-methylanisole, 1-methyl-1H -Benzimazole, 2-methylbenzofuran, 2-methylbenzothiazole, 2-methylbenzoxazole, 4-methyl-N, N-bis (4-methylphenyl) aniline, [(3-methylbutoxy) methyl] benzene, 1- [2- (3-methylbutoxy) -2-phenylethyl] pyrrolidine, methyl tert-butyl ether, 3-methyl-9H-carbazole, 9-methyl-9H-carbazole, 2-methyl-N, N-dimethylaniline, 3-methyl-N, N-dimethylaniline, 4-methyl-N, N-di Methylaniline, methyldioctylamine, 4-methyl-1,3-dioxane, 2-methyl-1,3-dioxolane, methyldiphenylamine, 1- (1-methylethoxy) butane, 2- [2- (1-methylethoxy) ) Ethyl] pyridine, 1- (1-methylethoxy) propane, 2-methylfuran, 3-methylfuran, 1-methylimidazole, 1-methyl-1H-indole, 1-methylisoquinoline, 3-methylisoquinoline, 4- Methylisoxazole, 5-methylisoxazole, 4-methylmorpholine, methyl-1-naphthylamine, 2-methyloxazole, 4-methyloxazole, 5-methyloxazole, 2-methyl-2-oxazoline, 3- ( 4-methyl-3-pentenyl) furan, methylpentyl ether, sulfurized methyl Rupentyl, methyl tert-pentyl sulfide, 10-methyl-10H-phenothiazine, N-methyl-N-phenylbenzenemethanamine, 1-methyl-N-phenyl-N-benzyl-4-piperidineamine, 2-methyl-5 -Phenylpyridine, 1-ethylpiperidine, 4- (2-methylpropenyl) morpholine, methylpropyl ether, 1-methyl-2-propylpiperidine, (S), methylpropyl sulfide, N-methyl-N-2-propyl Benzenemethanamine, 2-methylpyrazine, 1-methyl-1H-pyrazole, 3-methylpyridine, 4-methylpyridine, 2-methylpyrimidine, 4-methylpyrimidine, 5-methylpyrimidine, 1-methylpyrrole, N-methyl Pyrrolidine, 3- (1-methyl-2-pyrrolidinyl) pyridine, ±), 2-methylquinoline, 3-methylquinoline, 4-methylquinoline, 5-methylquinoline, 6-methylquinoline, 7-methylquinoline, 8-methylquinoline, 2-methylquinoxaline, 2-methyltetrahydrofuran, 2- Methylthiazole, 4-methylthiazole, (methylthio) benzene, (methylthio) ethene, [(methylthio) methyl] benzene, 2-methylthiophene, 3-methylthiophene, 3- (methylthio) -1-propene, methysticin, 2- (4-morpholinothio) benzothiazole, myristicin, 1,5-naphthyridine, 1,6-naphthyridine, nicothelin, octylphenyl ether, orphenadrine, papaverine, 2- (3-pentenyl) pyridine, perazine, phenanthridine 1,7-phenant Phosphorus, 1,10-phenanthroline, 4,7-phenanthroline, phenazine, phendimetrazine, phenindamine, 9-phenylacridine, N-phenyl-N-benzylbenzenemethanamine, 2- (2-phenylethyl) pyridine, 2 -Phenylfuran, 1-phenyl-1H-imidazole, 4-phenylmorpholine, 1-phenylpiperidine, phenylpropyl ether, 4- (3-phenylpropyl) pyridine, 2-phenylpyridine, 3-phenylpyridine, 4-phenylpyridine 1-phenyl-1H-pyrrole, 1-phenylpyrrolidine, 2-phenylquinoline, phenyl vinyl ether, piperotal, promazine, promethazine, trans-5- (1-propenyl) -1,3-benzodioxole, 5-propyl 1,3-benzodioxole, 2-propylpyridine, 4-propylpyridine, (propylthio) benzene, propyl vinyl ether, 4H-pyran, pyrantel, pyrilamine, quinazoline, safrole, 2,2 ': 6', 2 "- Terpyridine, 2,2 ′: 5,2 ″ -terthiophene, tetrabutyl titanate, tetraethoxymethane, tetraethylene glycol dimethyl ether, N, N, N ′, N′-tetraethyl-1,2-ethanediamine, 1,2 , 3,4-tetrahydro-6,7-dimethoxy-1,2-dimethylisoquinoline, (±), 4,5,6,7-tetrahydro-3,6-dimethylbenzofuran, cis-tetrahydro-2,5-dimethyl Thiophene, 3,4,5,6-tetrahydro-7-methoxy-2H-azepine, 1,2,3,6- Trahydro-1-methyl-4-phenylpyridine, tetrahydro-3-methyl-2H-tipyran, 2,3,4,5-tetrahydro-6-propylpyridine, tetrahydropyran, 5,6,7,8-tetrahydroquinoline, Tetrahydrothiophene, N, N, 2,6-tetramethylaniline, N, N, N ′, N′-tetramethyl-1,4-benzenediamine, N, N, N ′, N′-tetramethyl- [1 , 1′-biphenyl] -4,4′-diamine, N, N, N ′, N′-tetramethyl-1,4-butanediamine, N, N, N ′, N′-tetramethyl-1,2, -Ethanediamine, N, N, N ', N'-tetramethyl-1,6-hexanediamine, tenaldine, tenenyldiamine, thiacycloxan, 1,2,5-thiadiazole, thianthrene, thiazole, thiepa , Thiethylperazine, thioridazine, 9H-thioxanthene, tipepidine, tributylamine, 1,1,1-triethoxyethane, triethoxymethane, 1,1,1-triethoxypropane, triethylaluminum, triethylamine, triethylarsine, triethylene Glycol dimethyl ether, triphen morph, trihexyl amine, trihexyl borate, triisobutyl aluminate, triisobutyl aluminum, triisobutylamine, triisopentylamine, triisopropoxymethane, triisopropyl borate, triisopropyl phosphate, 1, 3,5-trimethoxybenzene, trimethoxyboroxine, 1,1,1-trimethoxyethane, trimethoxymethane, trimethylaluminum, trimethylamine, trimethyl Luarsine, trimethylborane, trimethylborate, 1,2,4-trimethylpiperazine, trimethylpyrazine, 2,3,6-trimethylpyridine, 2,4,6-trimethylpyridine, 1,2,5-trimethyl-1H-pyrolol N, N, 2-trimethyl-6-quinolinamine, triphenylarsine, triphenyl phosphate, 2,4,6-triphenyl-1,3,5-triazine, triprolidine, tripropylamine, tripropylborane , Tripropyl borate, tripropyl phosphate, tris (4-dimethylaminophenyl) methane, tris (ethylthio) methane, tris (2-methylphenyl) phosphine, tris (3-methylphenyl) phosphine, tris (4-methyl Phenyl) phosphine, 2,46-tris (2-pyridinyl) -1,3,5-thiazine, tris (o-tolyl) phosphite, 9-vinyl-9H-carbazole, 2-vinylfuran, 1-vinyl-2-methoxybenzene, 1-vinyl-3-methoxybenzene 1-vinyl-4-methoxybenzene, 2-vinylpyridine, 3-vinylpyridine, 4-vinylpyridine, 9H-xanthene, dibenzofuran, 3,4-dihydro-2H-benzopyran, alberine, aluminum 2-butoxide, aluminum iso Propoxide, antazoline, 1-benzylpiperidine, 2-benzylpyridine, 4-benzylpyridine, 1-benzyl-1H-pyrrole, (benzylthio) benzene, 2,2′-bipyridine, 2,3′-bipyridine, 2,4 '-Bipyridine, 3,3'-bipyridine, 4,4'-bipyridine, 2,2'-biki Norin, 1,3-bis (1-methyl-4-piperidyl) propane, butyl methyl sulfide, t-butyl methyl sulfide, 4-butyl morpholine, 4-t-butyl pyridine, 2-butyl thiophene, cosperin, cyclidine, 4- Silicon solvents such as (3-cyclohexen-1-yl) pyridine, cyclohexyldiethylamine, cyclohexyldimethylamine, silane, disilane, siloxane and disiloxane, preferably hexamethyldisiloxane, (CH ₃ ) ₃ SiOCH ₂ CH ₂ CH ₃ and (CH ₃ ) ₂ Si (OCHCH ₂ CH ₃ ) ₂ , halogenated silanes, siloxanes, and disiloxanes, preferably fluorinated and ionic liquids such as imidazolium and alkylimidazolium salts, preferably Is methyl chloride Of potassium and groups and derivatives of other similar compounds containing at least as a one.

  The solvent may include a polymer. Preferably, the polymer solvent lowers the vapor pressure at the cell operating temperature and the polymer is liquid at the cell operating temperature. One such polymerization solvent includes polypropylene glycol or oxidized polypropylene.

  Other solvents are solvents known in the art that have the property of solvating NaH molecules. The solvent mixture can be in any molar ratio. Suitable solvents are toluene, naphthalene, hexafluorobenzene, 1,4-dioxane, 1,3-dioxane, trioxane, 1,4-benzodioxane, 1,2-dimethoxyethane and N, N-dimethylaniline, bis (phenyl ) Comprising at least one of the group of ether, 1,4-dioxin, dibenzodioxin or dibenzo [1,4] dioxin and divinyl ether.

In embodiments that include a liquid solvent, the catalyst NaH is at least one of the components of the reaction mixture and is formed from the reaction mixture. The reaction mixture is _{NaH, Na, NH 3, NaNH} 2, Na 2 NH, Na 3 N, H 2 O, NaOH, NaX (X is an anion, preferably a _{halide), R-Ni, NaBH 4} , NaAlH 4, Ni, Pt black, Pd black, Na, at least one R-Ni doped with Na species such as, HSA support NaOH and NaH, adsorbent, dispersing agents, hydrogen source such as _{H 2,} as well as the hydrogen dissociation material It may further comprise at least one of the group. It is preferred that the support does not form an oxide with a reaction mixture such as NaOH and a solvent such as ether, preferably a component of BDO. In this case, the support may be a noble metal such as at least one of Pt, Pd, Au, Ir and Rh, or a supported noble metal such as Pt or Pd on titanium (Pt or Pd / Ti).

  A typical reaction mixture comprises at least one of NaH or a source of NaH, a high surface area nickel powder, a high surface area cobalt powder, and a rare earth metal powder, preferably La, and preferably 1,4-benzodioxane. It consists of an ether solvent which is (BDO).

  In one embodiment, the reaction mixture comprises NaH + solvent + support, wherein (1) the support is carbon, such as reduced high surface area Ni powder, La powder, and nanotubes, preferably single layer graphite, graphene, diamond Dopant containing carbon-like carbon (DLC), hydrogenated diamond-like carbon (HDLC), diamond powder, graphitic carbon, glassy carbon, carbon containing other metals such as Pd or Pt / carbon or other elements such as fluorinated carbon Preferably comprising at least one support selected from fluorinated graphite or fluorinated diamond; (2) the solvent is 1,4-dibenzodioxane (BDO), dimethoxyethane (DME), 1,4-dioxane and biphenyl ether Ethers such as N, N-dimethylaniline (DMAn), Fluorine-substituted alkanes or hexafluorobenzene, hexamethylphosphoramide (HMPA), including aryl such as protonic acid and toluene. In other embodiments, at least one of Na, K, KH, Li and LiH replaces NaH. In certain embodiments, the reaction mixture comprises a species from the group Na, NaH, NaF, a solvent, preferably a fluorinated carbon-based solvent, and an HSA material such as carbon, preferably a single-walled nanotube.

  Suitable reaction mixtures are: (1) NaH, hexafluorobenzene, and at least one of single-walled nanotubes, Pt powder, activated carbon and Al, La, Y doped mesoporous carbon, or Ni powder or corresponding carbide, 2) NaH or KH, 1,4-dibenzodioxan (BDO), La powder, at least one of Nd powder, and carbides of Al, La, Y and Ni, (3) NaH, dioxane, and Co or Nd powder , (4) at least one of the group of NaH, NaOH, BDO and polytetrafluoroethylene (Teflon®) powder. The weight percent may be any ratio, and is preferably about the same amount. In another embodiment, the reaction mixture comprises a species selected from Na, NaH, a solvent, preferably an ether solvent, and a metal, preferably an HSA material such as a rare earth. A suitable reaction mixture comprises NaH, 1,4-dibenzodioxane (BDO), and La. The weight percent may be any ratio, preferably about 10/45/45 wt% for each. In another exemplary power cell embodiment, the reaction mixture comprises NaH, R-Ni or high surface area Ni powder and an ether solvent. In certain chemical cell embodiments, the reaction mixture further comprises an adsorbent of hydrino hydride ions and a molecular hydrino such as an alkali halide, preferably a sodium halide such as at least one of NaF, NaCl, NaBr, and NaI. Including.

In some embodiments, the solvent has a halogen functionality, preferably fluorine. Suitable reaction mixtures comprise at least one of hexafluorobenzene and octafluoronaphthalene added to a catalyst such as NaH and mixed with a support such as activated carbon, fluoropolymer or R-Ni. In some embodiments, the reaction mixture comprises Na, NaH, a solvent, preferably a fluorinated solvent, and one or more species selected from the group of HSA materials. The HSA material is a metal or alloy coated with carbon, such as at least one of Co, Ni, Fe, Mn, and preferably 1-10 carbon layers and more preferably according to methods known to those skilled in the art Transition metal powder having three layers, preferably nanopowder; transition metal, preferably Ni, Co and Mn coated carbon and fluoride, preferably metal or alloy coated carbon such as metal fluoride, preferably at least one of nanopowder May be included. The metal is preferably a metal that can be coated with a non-reactive layer of fluoride such as steel, nickel, copper or monel metal. The coated metal may be a high surface area powder. Other suitable metals are rare earths such as La coated with fluoride, and may include LaF _x such as LaF ₃ . In certain embodiments, the metal fluoride is more stable than MF, where M is a catalyst or catalyst source such as Li, Na, and K. In a further embodiment, the reaction mixture further comprises a fluoride, such as a metal fluoride. Fluorides include catalytic metals such as NaF, KF and LiF, and also transition metals, noble metals, intermetallic compounds, rare earths, lanthanides, preferably La or Gd, and actinide metals, Al, Ga, In, Tl, Sn. , Pb, metalloid, B, Si, Ge, As, Sb, Te, Y, Zr, Nb, Mo, Tc, Ru, Rh, Pd, Ag, Cd, Hf, Ta, W, Re, Os, Ir, Pt , Au, Hg, alkali metals and alkaline earth metals. The fluoride may include an adsorbent as well as an HSA material. In some embodiments, the metal may include an alloy such as LaNi ₅ and a Ni-Y alloy or carbide, preferably resistant to inorganic fluoride formation.

Suitable fluorinated solvents for regeneration is CF _4. A suitable support or HSA material for the fluorinated solvent for the NaH catalyst is NaF. In an embodiment, the reaction mixture consists of at least NaH, CF ₄ and NaF. Other fluorine-based supports or getters include M ₂ SiF ₆ (M is an alkali metal, eg, Na ₂ SiF ₆ and K ₂ SiF ₆ ), MSiF ₆ (M is an alkaline earth metal, eg, MgSiF ₆ , GaF ₃ , PF ₅ ), MPF ₆ (M is an alkali metal), MHF ₂ (M is an alkali metal. For example, NaHF ₂ and KHF ₂ , K ₂ TaF ₇ , KBF ₄ , K ₂ MnF ₆ , and K ₂ ZrF ₆ ), Other similar compounds are also contemplated, for example, one of Li, Na, or K as the alkali metal, and another alkali or alkaline earth metal substituted.

In one embodiment, the solvent consists of fluorine and at least one other element, wherein the fluoride based on at least one other element is thermodynamically or kinetically stable to the NaH reaction. Moreover, it is preferable that it is a liquid of the cell operation temperature which can be 200 degreeC-700 degreeC. Other elements can be Si, Te, Se or Sb. The solvent is Si _x F _y , and x and y are integers. In another embodiment, the chemical characteristics of the solvent with NaH or any other reactant of the reaction mixture, NaF and H ₂ is preferably such that reversibly react to fluorinated solvents containing carbon and NaH reversible Chemical properties. In embodiments comprising NaH and fluorinated solvents, NaH is less reactive than the Na for any C-F bonds, H ₂ is supplied to the fluorinated solvent reaction of H ₂ to reduce the amount of Na.

In some embodiments, at least one of the fluorinated solvent and the HSA material is protected from attack to form NaF. Fluorocarbons are stable to strong bases, and in certain embodiments, the NaH catalyst source is a strong base. Current material _{Na, NaH, NaNH 2, NH} 3, NaOH, at least one of Na ₂ O, a hydrogen source, such as at least one of hydride and _{H 2,} and the dissociation thereof. Reactions that form catalyst NaH, some of which can be regenerated, are exemplified by formulas (158-161), (168) and (177-183) shown below. The NaOH cycle to form the NaH catalyst is shown in equations (158-161). The reaction shown in Formula (158) limits the amount of Na that reacts with the fluorocarbon solvent. A reducing agent can be added to the NaOH-containing reaction mixture to form an oxide of NaH and the reducing agent. Further, the hydrogen-containing oxides that can generate NaOH can be reduced and the reactants can be reused. Hydrogen may be dissociated by a dissociator. The reducing agent may be a metal having a corresponding oxide that can be reduced by hydrogen, such as Cr, Fe, Sn, and Zn. Alternatively, an oxide such as ZnO can be reduced to a metal by heating to a high temperature such as about 1750 ° C. In another embodiment, the fluorinated solvent is an ether, preferably one of dibenzodioxin, dibenzo-1,4-dioxane, dioxane and dimethoxyethane, toluene, xylene, benzene, naphthalene, naphthacene, phenanthrene, chrysene, fluoranthene and pyrene. May be substituted with another type, such as at least one of at least one of the hydrocarbons. The support may preferably be at least one metal of La, Pr, Co and Nd.

Suitable reaction mixtures consist of a NaH or NaH source, a solvent, preferably a hydrocarbon such as CF ₄ , hexafluorobenzene (HFB) or perfluoroheptane, preferably a support comprising carbon and metal, optionally hydrogen. The carbon preferably includes activated carbon (AC), but other forms such as glassy carbon, coke, graphitic carbon, and carbon with dissociator metals such as Pt or Pd with wt% 0.1-5 wt%. May be included. The metal is at least one of metal powder, hydride or carbide, for example at least one of the group of alkali metals, alkaline earth metals, preferably Mg as MgH ₂ , carbides such as Al or Al ₄ C ₃ as metal, Nanopowder coated with rare earth metal or carbide, preferably La, metal or alloy, preferably carbon such as at least one of Co, Ni, Fe, Mn, and preferably 1-10 layers, more preferably 3 layers of carbon Other transition metal powders with layers and metal or alloy coated carbon, preferably nanopowder such as transition metals, preferably at least one form of Ni, Co and Mn coated carbon. The metal may also interact with carbon. When the metal to be inserted is Na and the catalyst is NaH, the Na insertion is preferably saturated. The reactants (1) NaH (14wt%) , HFB (14wt%), AC (58wt%) and _{MgH 2 (14wt%); (} 2) NaH (14wt%), HFB (14wt%), AC (58wt% ) And Al (14 wt%); (3) NaH (14 wt%), HFB (14 wt%), AC (58 wt%) and Al ₄ C ₃ (14 wt%); (4) NaH (14 wt%), HFB (14 wt) %), AC (58 wt%) and Co coated nano powder (14 wt%); (5) Optional, such as NaH (14 wt%), HFB (14 wt%), AC (58 wt%) and La (14 wt%) It is possible to achieve a desirable ratio. In other embodiments, AC, activated carbon is replaced with mesoporous carbon, and in other embodiments the solvent is preferably 2-3 times more than the other reactants. In other embodiments, another catalyst such as K or Li replaces the NaH catalyst.

In one general embodiment, the reaction mixture includes a component called a protective or blocking agent that at least partially inhibits an unwanted reaction between one component of the mixture and another. is there. It is preferred that the protective or blocking agent does not react with the solvent or support. Strong bases are non-reactive with fluorocarbons; whereas Na is reactive. Thus, in one embodiment, at least one of H ₂ , NaOH, NaNH ₂ and NH ₃ is added to the reaction mixture as a blocking agent and reacted with any Na formed during the hydrino-forming reaction to provide a fluorocarbon support. Suppresses reaction with support such as body. By way of example, the reaction mixture is NaH; a blocking agent such as at least one of NaOH, NaNH ₂ , NH ₃ , H ₂ ; a solvent such as BDO, crown ether, polypropylene oxide, CF ₄ and at least one of HFB; and polytetra It consists of a support comprising at least one fluorocarbon such as fluoroethylene (Teflon®) powder. By way of example, protective agents are hydrides and carbides. The protective reactant may be a metal support. The reaction may include an ether solvent such as NaH, BDO, a metal hydride such as a rare earth metal hydride, or a carbide such as at least one of Al, rare earth and transition metal carbide.

In a second general embodiment, the reaction mixture is substantially stable over time for inter-component reactions other than hydrino formation. Preferably, a solvent such as a polar solvent does not react with the catalyst or support. For example, at suitably low reaction temperatures, such as below 350 ° C., the ether solvent is non-reactive with NaH as the catalyst source, fluorocarbon support, rare earth powder, hydride or carbide. Thus, by way of example, the reaction mixture consists of an ether solvent such as NaH, BDO, dioxane or crown ether, and a rare metal powder support such as La powder. Another support is formed of an alloy which is resistant to reaction with the solvent, such as LaNi _5.

In a third general embodiment, the reaction mixture consists of reactants that form hydrinos in high yield, although side reactions between components also occur. The reactants may be regenerated by running another cycle to form hydrinos. Typical reaction mixtures include fluorocarbon solvents such as NaH, CF ₄ , and polytetrafluoroethylene (Teflon®), fluorinated graphite, activated carbon, graphene, and mesoporous carbon, as well as Al , La, Co, Ni, Mn, Y, and Fe powder, and a support such as at least one of their carbides. Preferably, the metal and carbide comprise a mixture such as one of Ni, Co, Mn. The metal and carbide may be in any weight percent ratio. Preferably, the composition to weight percent (%) ratio is about 20 to 25% Ni, 60 to 70% Co, and 5 to 15% Mn. In another, the metal and carbide consist of a mixture of Ni, Co, Mn, Fe, S, and other elements such as one of Ca. The metal, carbide, and other elements may be in any weight ratio. Preferably, the composition and weight percent (%) ratio is about 20 ± 5% Ni, 65 ± 5% Co, 10 ± 5% Mn, 1 ± 5% Fe, 1% ± 2S, and 0.5 ±. 2% Ca. In other embodiments, the carbon support is a higher surface area carbon such as activated carbon or mesoporous carbon, and a thermodynamic than NaF, such as nickel, iron, iridium, vanadium, lead, molybdenum, and tungsten. Consisting of at least one metal that forms a non-stable fluoride.

  Other embodiments include reaction mixtures comprising any combination of these three general embodiments based on them, any combination thereof, or alternative reaction strategies or pathways.

In some embodiments, one or more sources material to provide a catalyst and atomic hydrogen such as LiNH ₂ amides, imides such as _Li 2 NH, in the catalytic metals including nitrides and NH _3, such as Li ₃ N Consists of at least one. These types of reactions provide both Li atoms and atomic hydrogen. Also, K, Cs and Na replace Li, and the catalyst is atom K, atom Cs and molecule NaH. In another embodiment of the reaction mixture comprising a liquid solvent, the catalyst is Li. The reaction mixture is _{Li, LiNH 2, Li 2 NH} , Li 3 N, LiNO 3, LiX, NH 4 X (X is an anion, preferably a _halide), NH 3, of the group of R-Ni type, HSA support , adsorbent, dispersions may further comprise a source of hydrogen and hydrogen dissociation material such as H _2.

b. Inorganic solvent In another embodiment, the reaction mixture comprises at least one inorganic solvent. The solvent additionally contains a molten inorganic compound such as a molten salt. The inorganic solvent may be molten NaOH. In some embodiments, the reaction mixture comprises a catalyst, a hydrogen source, and an inorganic catalyst solvent. The catalyst may be at least one of NaH molecules, Li and K. The solvent may be at least one of a molten or fused salt or eutectic mixture, such as at least one of the molten salts of the group of alkali halides and alkaline earth halides. The inorganic solvent of the NaH catalytic reaction mixture may comprise a low melting eutectic mixture of a mixture of alkali halides such as NaCl and KCl. The solvent has a low melting point salt, preferably a Na salt such as NaI (660 ° C.), NaAlCl ₄ (160 ° C.), at least one of NaAlF ₄ , and a metal halide in which M is a metal and X is more stable than NaX. It may be a compound of the same class as NaMX ₄ which is a halide. The reaction mixture may further comprise a support such as R-Ni.

The inorganic solvent of the Li catalyst reaction mixture may comprise a low melting eutectic mixture of a mixture of alkali halides such as LiCl and KCl. The molten salt solvent may include a fluorine-based solvent that is stable to NaH. LaF _{3 has} a melting point of 1493 ° C. and NaF has a melting point of 996 ° C. A ball mill mixture containing appropriate fluoride, optionally other fluorides, includes a fluoride-salt solvent that is stable to NaH and preferably melts in the range of 600 ° C to 700 ° C. In molten salt embodiments, the reaction mixture is NaF + KF-LiF (11.5-42.0-46.5) MP = 454 ° C NaH + salt mixture, such as LiF-KF (52% -48%). It consists of a NaH + salt mixture such as MP = 492 ° C.

V. Regeneration System and Reaction A schematic diagram of a fuel recycling or regeneration system according to the present disclosure is shown in FIG. In some embodiments, the by-product of the hydrino reaction includes a metal halide MX, preferably NaX or KX. In that case, the fuel recycler 18 (FIG. 4) includes a separator 21 for separating inorganic compounds such as NaX from the support. In one embodiment, the separator or member thereof comprises a moving device or cyclone separator 22 that performs separation based on density differences of species. The further separator or member thereof consists of a magnetic separator 23, which is a magnetic particle such as nickel or iron that is drawn by a magnet while a non-magnetic material such as MX flows through the separator. In another embodiment, the separator or member thereof is a fractionated product solubilization or suspension system that includes a component solvent wash 25 that dissolves, suspends and separates at least one component more widely than another. And a compound recovery system 26 such as a solvent evaporator 27 and a compound collector 28. Alternatively, the recovery system consists of a precipitator 29 and a compound dryer and collector 30. In one embodiment, waste heat from the turbine 14 and water concentrator 16 shown in FIG. 4 is utilized to heat at least one of the evaporator 27 and the dryer 30 (FIG. 4). The heat for heating any other member in the stage of the recycler 18 (FIG. 4) may include waste heat.

  The fuel recycler 18 (FIG. 4) further comprises an electrolyzer 31 that electrolyzes the recovered MX into metal and halogen gas or other halogenated product or halide product. In certain embodiments, electrolysis occurs in the power reactor 36, preferably from a melt, such as a eutectic melt. The electrolysis gas and the metal product are collected separately in the highly volatile gas collector 32 and the metal collector 33, which may further comprise a metal distiller or separator 34, respectively, in the case of a metal mixture. If the initial reactant is a hydride, the metal is hydrogenated by a hydrogenation reactor 35, which can have a cell 36 that can be at or below atmospheric pressure and an inlet for the metal and hydride. It comprises an outlet 37, a hydrogen gas inlet 38 and its valve 39, a hydrogen supply device 40, a gas outlet 41 and its valve 42, a pump 43, a heater 44, and a pressure temperature meter 45. In one embodiment, the hydrogen supply 40 includes an aqueous electrolyzer with hydrogen and an oxygen gas separator. The isolated metal product is at least partially halogenated in a halogenation reactor 46, which can be a cell 47, a carbon inlet and a halogenation product that can be at a pressure lower or higher than atmospheric pressure. It consists of a material outlet 48, a fluorine gas inlet 49 and its valve 50, a halogen gas supplier 51, a gas outlet 52 and its valve 53, a pump 54, a heater 55, and a pressure temperature measuring device 56. Preferably, the reactor also contains a catalyst and other reactants to bring the metal 57 as a product into a halide of the desired oxidation state and stoichiometry. At least two of the metal or metal hydride, metal halide, support and other initial reactants are mixed in the mixer 58 for another power generation cycle and then reused in the boiler 10.

As an example, for hydrino and regeneration reactions, the reaction mixture consists of NaH catalyst, Mg, MnI ₂ and a support, activated carbon, WC or TiC. In some embodiments, the exothermic reaction source is
2KH + MnI ₂ → 2KI + Mn + H ₂ (86)
_{Mg + MnI 2 → MgI 2 +} Mn (87)
It is an oxidation reaction of a metal hydride with MnI ₂ . KI and MgI ₂ can be electrolyzed from the molten salt to I ₂ , K and Mg. Melt electrolysis may be performed using Downs cells or modified Downs cells. Mn may be separated using a mechanical separator, optionally a sieve. Unreacted Mg or MgH ₂ can be melted and separated by separating the solid and liquid phases. Iodides for electrolysis are obtained from a rinse of the reaction product in a suitable solvent such as deoxygenated water. The solution is filtered to remove a support such as AC, and possibly transition metals. The solid is centrifuged and dried using waste heat from the power system. Alternatively, they may be melted and then the liquid and solid phases separated to separate the halides. In another embodiment, lighter AC may be first separated from other reaction products by methods such as cyclone separation. K and Mg are incompatible, and separated metals such as K may be hydrogenated with H ₂ gas, preferably from electrolysis of H ₂ O. Metal iodides may be formed by known reactions with separated metals or metals not separated from AC. In some embodiments, Mn reacts with HI, to form a MnI _{2, H 2} is recycled to react with _{I 2,} to form a HI. In other embodiments, other metals, preferably transition metals, replace Mn. Another reducing agent such as Al can replace Mg. Another halide, preferably chloride, can replace the iodide. LiH, KH, RbH or CsH can replace NaH.

As an example, for hydrino and regeneration reactions, the reaction mixture consists of NaH catalyst, Mg, AgCl and support, activated carbon. In some embodiments, the exothermic reaction source is
KH + AgCl → KCl + Ag + 1 / 2H ₂ (88)
Mg + 2AgCl → MgCl ₂ + 2Ag (89)
This is an oxidation reaction of a metal hydride with AgCl. KCl and MgCl ₂ can be electrolyzed from the molten salt to Cl ₂ , K and Mg. Melt electrolysis may be performed using Downs cells or modified Downs cells. Ag may be separated using a mechanical separator, optionally a sieve. Unreacted Mg or MgH ₂ melts and can be separated by separating the solid and liquid phases. Chloride for electrolysis is obtained from a rinse of the reaction product in a suitable solvent such as deoxygenated water. The solution is filtered to remove a support such as AC and optionally Ag metal. The solid is centrifuged and dried using waste heat from the power system. Alternatively, they may be melted and then the liquid and solid phases are separated to separate the halides. In another embodiment, lighter AC may be first separated from other reaction products by methods such as cyclone separation. K and Mg are incompatible, and separated metals such as K may be hydrogenated with H ₂ gas, preferably from electrolysis of H ₂ O. Metal chlorides may be formed by known reactions with separated metals or metals not separated from AC. In some embodiments, Ag reacts with Cl ₂ to form AgCl, and H ₂ is recycled and reacts with I ₂ to form HI. In other embodiments, another metal, preferably a transition metal or In, replaces Ag. Another reducing agent such as Al can replace Mg. Another halide, preferably chloride, can replace the iodide. LiH, KH, RbH or CsH replaces NaH.

In certain embodiments, the reaction mixture is regenerated from the hydrino reaction product. As an example, for hydrino and regeneration reactions, the solid fuel reaction mixture consists of KH or NaH catalyst, Mg or MgH ₂ , and alkaline earth halides such as BaBr ₂ and support, activated carbon, WC or preferably TiC. . In some embodiments, the exothermic reaction source is
2KH + Mg + BaBr ₂ → 2KBr + Ba + MgH ₂ (90)
2NaH + Mg + BaBr ₂ → 2NaBr + Ba + MgH ₂ (91)
An oxidation reaction of the metal hydride or metal by BaBr ₂ like. Ba, _magnesium, MgH 2, NaBr and each melting point of KBr, 727 ℃, 650 ℃, 327 ℃, is 747 ° C. and 734 ° C.. Therefore, when the maintaining MgH ₂ by adding _{H 2,} preferentially melt the MgH _2, by separating the liquid from the reaction product mixture, MgH ₂ from barium and any Ba-Mg intermetallic compound Can be separated. In some cases, it can be pyrolyzed to Mg. The remaining reaction product may then be added to the electrolysis melt. The solid support and Ba are preferably precipitated to form a separable layer. Alternatively, Ba can be melted and separated as a liquid. Thereafter electrolysis of NaBr or KBr, may form an alkali metal and Br _2. The latter reacts with Ba, forming a BaBr _2. Alternatively, Ba is the cathode and BaBr ₂ is formed directly in the anode compartment. The alkali metal is hydrogenated after electrolysis or formed in the cathode compartment during electrolysis by bubbling H ₂ in the cathode compartment. The MgH ₂ or Mg, NaH or KH, BaBr ₂ and support are then returned to the reaction mixture. In another embodiment, in another embodiment, another alkaline earth halide replaces BaBr _2, preferably BaCl ₂ . In another embodiment, the regenerative reaction occurs without electrolysis due to the small energy difference between the reactants and the product. The reaction shown in equations (90-91) can be reversed by changing reaction conditions such as temperature or hydrogen pressure. Alternatively, the molten or volatile species, such as K or Na, can be selectively removed and manipulated to reverse the reaction to regenerate a reactant or species that can be further reacted, returned to the cell, A reaction mixture is formed. In another embodiment, volatile species are used to maintain a reversible reaction between a catalyst or catalyst source such as NaH, KH, Na or K and an initial oxide such as an alkaline earth halide or rare earth halide. May be continuously refluxed. In some embodiments, a distiller such as distiller 34 shown in FIG. 4 is used to allow reflux. In another embodiment, reaction conditions such as temperature or hydrogen pressure can be changed to reverse the reaction. In this case, the reaction is initially carried out in the forward direction to form hydrino and reaction mixture products. Thereafter, products other than low energy hydrogen are converted to initial reactants. This can be achieved by varying the reaction conditions, optionally by at least partially adding or removing the same or different product or reactant as originally used or formed. Thus, the forward reaction and the regeneration reaction are performed in alternating cycles. Hydrogen may be added to supplement the hydrogen consumed by hydrino formation. In another embodiment, reaction conditions such as elevated temperatures are maintained. At this temperature, the reversible reaction is optimized so that forward and retrograde reactions occur in a manner that allows hydrino formation to be maximized, preferably maximized.

As an example, in the hydrino and regeneration reactions, the solid fuel reaction mixture NaH catalyst, Mg, FeBr _2, and the support consists of activated carbon. In one embodiment, the exothermic reaction source is 2NaH + FeBr ₂ → 2NaBr + Fe + H ₂ (92)
Mg + FeBr ₂ → MgBr ₂ + Fe (93)
This is an oxidation reaction of metal hydride with FeBr ₂ . NaBr and MgBr ₂ may electrolysis to _Br 2, Na and Mg from molten salt. Melt electrolysis may be performed using a Downs cell or a modified Downs cell. Fe is ferromagnetic and may be magnetically separated using a mechanical separator, optionally a sieve. In another embodiment, the ferromagnetic Ni may be replaced with Fe. Unreacted Mg or MgH ₂ can be melted and separated by separating the solid and liquid phases. The bromide for electrolysis is obtained from a rinse of the reaction product in a suitable solvent such as deoxygenated water. The solution is filtered to remove a support such as AC, and possibly transition metals. The solid is centrifuged and dried using waste heat from the power system. Alternatively, they may be melted and then the liquid and solid phase separated to separate the halide. In another embodiment, lighter AC may be first separated from other reaction products by methods such as cyclone separation. Na and Mg are incompatible, and separated metals such as Na may be hydrogenated with H ₂ gas, preferably from electrolysis of H ₂ O. Metal bromides may be formed by known reactions with separated metals or metals not separated from AC. In some embodiments, Fe reacts with HBr to form FeBr ₂ , and H ₂ is recycled and reacts with Br ₂ to form HBr. In other embodiments, other metals, preferably transition metals, replace Fe. Another reducing agent such as Al can replace Mg. Another halide, preferably chloride, can be substituted for bromide. LiH, KH, RbH or CsH replaces NaH.

As an example, in the hydrino reaction and regeneration reaction, the solid fuel reaction mixture KH or NaH catalyst, Mg or MgH2, SnBr _2, and a support, activated carbon, consisting of WC or TiC. In some embodiments, the exothermic reaction source is
2KH + SnBr ₂ → 2KBr + Sn + H ₂ (94)
2NaH + SnBr ₂ → 2NaBr + Sn + H ₂ (95)
Mg + SnBr ₂ → MgBr ₂ + Sn (96)
An oxidation reaction of the metal hydride or metal by SnBr ₂ like. The melting points of tin, magnesium, MgH ₂ , NaBr and KBr are 119 ° C., 650 ° C., 327 ° C., 747 ° C. and 734 ° C., respectively. As shown in the diagram of the alloy phase, it has been found that a tin-magnesium alloy melts at, for example, 400 ° C. or more when Mg is about 5 wt%. In some embodiments, tin and magnesium metals and alloys are separated from the support and halide by melting the metals and alloys and separating the liquid and solid phases. The alloy can react with H _{2 at} temperatures that form MgH ₂ solids and tin metal. Separate the solid and liquid phases to obtain MgH ₂ and tin. MgH ₂ can be pyrolyzed to Mg and H ₂ . Alternatively, H ₂ may be added to the in situ reaction product at a temperature selected to convert any unreacted Mg and any Sn—Mg alloy to solid MgH ₂ and liquid tin. Tin can be selectively removed. Thereafter, MgH ₂ is heated and removed as a liquid. Next, the halide is separated from the support by a method such as (1) melting and phase separation, (2) cyclone separation due to a concentration difference in which a high density support such as WC is preferred, or (3) sieving according to a size difference. Can be removed. Alternatively, the halide may be dissolved in a suitable solvent, and the liquid and solid phases may be separated by a method such as filtration. The liquid is evaporated and then the halide is electrolyzed from the melt to Na or K, optionally Mg metal, which are incompatible with each other. In another embodiment, sodium halide, preferably Na metal regenerated by electrolysis of the same halide formed in the hydrino reactor, is used to form K by reduction of the halide. Furthermore, to recover a halogen gas such as Br ₂ from the electrolysis melt, reacted with Sn was isolated and reused for another cycle hydrino reaction with NaH or KH, and Mg or MgH ₂ SnBr ₂ Form. Here, the hydride is formed by hydrogenation with H ₂ gas. In some embodiments, HBr is formed and reacts with Sn, forming a SnBr _2. HBr may be formed by the reaction of Br ₂ and H ₂ or during electrolysis by bubbling H ₂ over the anode which has the advantage of reducing electrolysis energy. In other embodiments, another metal may replace Sn, preferably a transition metal, and another halide may replace Br such as I.

In another embodiment, at the initial stage, all reaction products react with aqueous HBr, concentrate the solution and precipitate SnBr ₂ from the MgBr ₂ and KBr solutions. Other suitable solvents and separation methods may be used to separate the salts. Thereafter, MgBr ₂ and KBr are electrolyzed into Mg and K. Alternatively, Mg or MgH ₂ is first removed by working parts or selective solvent methods so that only KBr requires electrolysis. In some embodiments, Sn is removed as a melt from solid MgH ₂ that can be formed during or after the hydrino reaction by adding H ₂ . MgH ₂ or Mg, KBr and the support are then added to the electrolysis melt. Since the support has a large particle size, it settles in the deposition region. MgH ₂ and KBr form part of the melt and separate based on density. Mg and K are incompatible, and K also forms a separate phase so that Mg and K are recovered separately. In some cases, the anode may be Sn so that K, Mg and SnBr ₂ become electrolysis products. Or the anode is a liquid tin, or liquid tin, separated at the anode to react with bromine, and in some cases forming SnBr _2. In this case, the energy gap for regeneration is the compound gap corresponding to the element product at both electrodes versus the high element gap. In a further embodiment, the reactant consists of KH, a support and SnI ₂ or SnBr ₂ . Sn is removed as a liquid, KX and residual products such as the support are added to the electrolysis melt, and the support is separated based on density. In this case, a high density support such as WC is preferred.

The reactant consists of an oxygen compound, an oxide product such as an oxide of a catalyst or catalyst source such as NaH, Li or K and an oxide of a reducing agent such as Mg, MgH ₂ , Al, Ti, B, Zr or La. Can be formed. In certain embodiments, the reactants are regenerated by reacting an oxide with a hydrogen halide acid, preferably an acid such as HCl, to form a corresponding halide such as a chloride. In certain embodiments, carbon oxide species such as carbonates, bicarbonates, and carboxylic acid species such as oxalic acid or oxalate can be reduced to metals or metal hydrides. Preferably, at least one of Li, K, Na, LiH, KH, NaH, Al, Mg and MgH ₂ reacts with a species containing carbon and oxygen to form the corresponding metal oxide or hydroxide and carbon To do. Each corresponding metal can be regenerated by electrolysis. Electrolysis may be performed using a molten salt such as a eutectic mixture. A halogen gas electrolysis product such as chlorine gas may be used to form the corresponding acid such as HCL as part of the regeneration cycle. HX, which is a hydrogen halide acid, may be formed by reacting a halogen gas and a hydrogen gas, and optionally dissolving the hydrogen halide gas in water. Hydrogen gas is preferably formed by electrolysis of water. The oxygen may be a reactant of the hydrino reaction mixture or may be reacted to form an oxygen source for the hydrino reaction mixture. The step of reacting the oxide hydrino-reactive organism with the acid may include rinsing the product with the acid to form a solution containing the metal salt. In one embodiment, the hydrino reaction mixture and the corresponding product mixture comprise a support such as carbon, preferably activated carbon. The metal oxide can be separated from the support by dissolving it in an aqueous acid. Thus, the product is rinsed with acid and further filtered to separate the components of the reaction mixture. Water can be removed by evaporation using heat from the power system, preferably waste heat, and salts such as metal chlorides can be added to the electrolysis mixture to form metal and halogen gases. In certain embodiments, any methane or hydrocarbon product is rearranged to hydrogen, optionally carbon or carbon dioxide. Alternatively, methane was separated from the gas product mixture and was commercially available. In another embodiment, methane can be formed into other hydrocarbon products by methods known in the art such as the Fischer-Tropsch reaction. Methane formation can be inhibited by adding interfering gases such as inert gases and maintaining unsuitable conditions such as hydrogen pressure or temperature reduction.

In another embodiment, the metal oxide is electrolyzed directly from the eutectic mixture. An oxide such as MgO can be reacted with water to form a hydroxide such as Mg (OH) ₂ . In some embodiments, the hydroxide is reduced. The reducing agent may be an alkali metal or hydride such as Na or NaH. The product hydroxide can be directly electrolyzed as a molten salt. Hydrino reaction products such as alkali metal hydroxides can also be used as commercial products and the corresponding acquired halides. The halide can then be electrolyzed into halogen gas and metal. Halogen gas may be used as a commercial industrial gas. The metal can be hydrogenated with hydrogen gas, preferably for water electrolysis, and provided to the reactor as part of a hydrino reaction mixture.

Reducing agents such as alkali metals can be regenerated from products containing the corresponding compounds, preferably NaOH or Na ₂ O, using methods and systems known to those skilled in the art. One method involves electrolysis in a mixture such as a eutectic mixture. In further embodiments, the reducing agent product may include at least some oxides, such as a reducing agent metal oxide (eg, MgO). The hydroxide or oxide can be dissolved in a weak acid such as hydrochloric acid to form the corresponding salt such as NaCl or MgCl ₂ . The treatment using an acid includes an anhydrous reaction. The gas may be flowing at low pressure. The salt may be treated with a product reducing agent such as an alkali or alkaline earth metal to form the original reducing agent. In some embodiments, the second reducing agent is an alkaline earth metal, preferably Ca, which reduces NaCl or MgCl ₂ to Na or Mg metal. The additional product of CaCl ₃ is recovered and reused. In an alternative embodiment, the oxide is reduced with H ₂ at an elevated temperature.

As an example, for hydrino and regeneration reactions, the reaction mixture consists of NaH catalyst, MgH ₂ , O ₂ and a support, activated carbon. In one embodiment, the exothermic reaction source is MgH ₂ + O ₂ → Mg (OH) ₂ (97)
_{MgH 2 + 1.5O 2 + C →} MgO 3 + H 2 (98)
NaH + 3 / 2O ₂ + C → NaHCO ₃ (99)
2NaH + O ₂ → 2NaOH (100)
It is an oxidation reaction of metal hydride by O ₂ such as. Any MgO product can be converted to a hydroxide by reaction with water MgO + H ₂ O → Mg (OH) ₂ (101)
Sodium or magnesium carbonate, bicarbonate, and other species containing carbon and oxygen are Na or NaH:
NaH + Na ₂ CO ₃ → 3NaOH + C + 1 / H ₂ (102)
NaH + 1 / 3MgCO ₃ → NaOH + 1 / 3C + 1 / 3Mg (103)
Can be reduced.
2Na + Mg (OH) ₂ → 2NaOH + Mg (104)
Can be reduced to Mg. Thereafter, NaOH directly from the melt, it is possible to electrolysis to Na metal and NaH and _{O 2.} A Kastner method may be used. The preferred cathode and anode for the basic solution is nickel. The anode may be a noble metal such as carbon, Pt, a support such as Ti coated with a noble metal such as Pt, or a positionally stable anode. In another embodiment, NaOH can be converted to NaCl by reaction with HCl, and the NaCl electrolysis gas Cl ₂ can react with H ₂ by electrolysis of water to form HCl. Molten NaCl electrolysis may be performed using Downs cells or modified Downs cells. Alternatively, HCl may be generated by chlor-alkali electrolysis. This electrolyzed aqueous NaCl is obtained from a rinse of the reaction product with aqueous HCl. Preferably, waste heat from the power system may be used to filter the solution to remove a support such as AC that can be centrifuged or dried.

In one embodiment, the reaction step comprises (1) rinsing the product with aqueous HCl to form a metal chloride from species such as hydroxide, oxide and carbonate, (2) water gas change reaction and Fisher. Using a Tropsch reaction to convert any CO ₂ released to water and C by H ₂ reduction, reusing C as a support in step 10, and in steps 1, 4 or 5 A step of using water, (3) a step of filtering and drying a support such as AC, wherein the drying may include a step of centrifuging, and (4) electricity of water to H ₂ and O ₂ Decomposing and providing steps 8-10, (5) optionally forming H ₂ and HCl from electrolysis of aqueous NaCl to provide steps 1 and 9, (6) isolating the metal chloride, (7) metal chloride melt as metal Electrolysis of step into fine chlorine, to form a HCl by the reaction of (8) Cl ₂ and H _2, providing a step 1, was hydrogenated (9) any metal, corresponding by reaction with hydrogen starting Forming a reactant, and (10) adding O ₂ from step 4 or forming an initial reaction mixture using O ₂ isolated from the atmosphere.

In another embodiment, the at least one electrical decomposed into Mg and O ₂ from the melt of magnesium oxide and magnesium hydroxide. The melt is a NaOH melt, and Na can also be electrolyzed. In certain embodiments, carbon oxides such as carbonates and bicarbonates can decompose into at least one of CO and CO ₂ that is added to the reaction mixture as an oxygen source. Alternatively, carbon oxide species such as CO ₂ and CO can be reduced to carbon and water by hydrogen. CO ₂ and CO may be reduced by a water gas shift reaction and a Fischer-Tropsch reaction.

In a typical hydrino and regeneration reaction, the reaction mixture, NaH catalyst, _MgH 2, CF ₄ and the support consists of activated carbon. In the examples, the source of the exothermic reaction is an oxidation reaction of metal hydride with CF ₄ as shown below.
2MgH ₂ + CF ₄ → C + 2MgF ₂ + 2H ₂ (105)
2MgH ₂ + CF ₄ → CH ₄ + 2MgF ₂ (106)
4NaH + CF ₄ → C + 4NaF + 2H ₂ (107)
4NaH + CF ₄ → CH ₄ + 4NaF (108)
NaF and MgF ₂ may be electrolyzed to F ₂ , Na, and Mg from a molten salt that may additionally contain HF. Na and Mg are immiscible and the separated metal may be hydrogenated, preferably with H ₂ gas from electrolysis of H ₂ O. F ₂ gas may react with carbon and any CH ₄ reaction product to regenerate CF ₄ . Instead, and preferably, the anode of the electrolysis cell is made of carbon and the current and electrolysis conditions are maintained so that CF ₄ is the anodic electrolysis product.

In a typical hydrino the regeneration reaction, the reaction mixture NaH _{catalyst, MgH 2, P 2 O 5} (P 4 O 10), and the support and consists of activated carbon. In the examples, for example, the source of the exothermic reaction is an oxidation reaction of a metal hydride with P ₂ O ₅ as follows.
5MgH ₂ + P ₂ O ₅ → 5MgO + 2P + 5H ₂ (109)
5NaH + P ₂ O ₅ → 5NaOH + 2P (110)
Phosphorus can be converted to P ₂ O ₅ by combustion in O ₂ .
2P + 2.5O ₂ → P ₂ O ₅ (111)
The MgO product may be converted to hydroxide by reaction with water.
MgO + H ₂ O → Mg (OH) ₂ (112)
Mg (OH) ₂ can be reduced to Mg using Na or NaH.
2Na + Mg (OH) ₂ → 2NaOH + Mg (113)
And NaOH can be electrolyzed directly from the melt to Na metal and NaH and O ₂ , or NaCl electrolysis gas Cl ₂ may react with H ₂ from electrolysis of water to produce HCl. However, NaOH may change to NaCl by reaction with HCl. In an embodiment, metals such as Na and Mg may be converted to the corresponding hydrides, preferably by reaction with H ₂ from the electrolysis of water.

In a typical hydrino and regeneration reactions, the solid fuel reaction mixture, NaH _catalyst, MgH 2, NaNO _3, and a support, consisting of activated carbon. In the examples, the source of the exothermic reaction is an oxidation reaction of metal hydride with NaNO ₃ as follows.
NaNO ₃ + NaH + C → Na ₂ NO ₃ + 1 / 2N ₂ + 1 / 2H ₂ (114)
NaNO ₃ + 1 / 2H ₂ + 2NaH → 3NaOH + 1 / 2N ₂ (115)
NaNO ₃ + 3MgH ₂ → 3MgO + NaH + 1 / 2N ₂ + 5 / 2H ₂ (116)
Sodium or magnesium carbonate, hydrogen carbonate, and other species consisting of carbon and oxygen may be reduced with Na or NaH.
NaH + Na ₂ CO ₃ → 3NaOH + C + 1 / H ₂ (117)
NaH + 1 / 3MgCO ₃ → NaOH + 1 / 3C + 1 / 3Mg (118)
Carbonate can also be resolved from the aqueous medium to hydroxides and CO _2.
Na ₂ CO ₃ + H ₂ O → 2NaOH + CO ₂ (119)
The released CO ₂ may be reacted to water and C by reduction with H ₂ using a water gas shift reaction and a Fischer-Tropsch reaction.
CO ₂ + H ₂ → CO + H ₂ O (120)
CO + H ₂ → C + H ₂ O (121)
The MgO product may be converted to hydroxide by reaction with water.
MgO + H ₂ O → Mg (OH) ₂ (122)
Mg (OH) ₂ can be reduced to Mg using Na or NaH.
2Na + Mg (OH) ₂ → 2NaOH + Mg (123)
The alkali nitrate can be regenerated using methods known to those skilled in the art. In an embodiment, NO ₂ can be generated by known industrial methods, such as by the Ostwald method following the Harbor method. In one embodiment, a typical sequence of steps is as follows.

Specifically, the Harbor process may be used to generate NH ₃ from N ₂ and H ₂ at high temperatures and pressures using a catalyst such as α-iron that contains some oxide. . Hot with a catalyst such as platinum or platinum-rhodium catalysts, the oxidation of ammonia to the NO _2, may Ostwald method is used. The heat may be waste heat from the power system. NO ₂ may be dissolved in water to form nitric acid that reacts with NaOH, Na ₂ CO ₃ or NaHCO ₃ to form sodium nitrate. And the remaining NaOH can be electrolyzed directly from the melt to Na metal and NaH and O ₂ , or it may react with H ₂ from the electrolysis of water so that the NaCl electrolysis gas Cl ₂ forms HCl. Where not, it may be converted to NaCl by reaction with HCl. In an embodiment, metals such as Na and Mg may be converted to the corresponding hydrides, preferably by reaction with H ₂ from the electrolysis of water. In other embodiments, Li and K replace Na.

In a typical hydrino and regeneration reaction, the reaction mixture, NaH catalyst, _MgH 2, SF _6, the support consists of activated carbon. In the examples, the source of the exothermic reaction is an oxidation reaction of metal hydride with SF ₆ as follows.
4MgH ₂ + SF ₆ → 3MgF ₂ + 4H ₂ + MgS (125)
7NaH + SF ₆ → 6NaF + 3H ₂ + NaHS (126)
NaF and MgF ₂ and sulfide may be electrolyzed to Na and Mg from a molten salt that may additionally contain HF. Fluorine electrolysis gas, in order to form a good SF ₆ gas is dynamically removed, it may react with sulfide. Separation of SF ₆ from F ₂ may be by a medium known as molecular sieve, membrane separation, or methods known to those skilled in the art such as cryogenic distillation. NaHS melts at 350 ° C. and may become part of the molten electrolysis mixture. Any MgS product may react with Na to form NaHS, where the reaction occurs in situ during electrolysis. S and metals may be products made during electrolysis. Alternatively, the metal, as a more stable fluoride is formed, or, as can be added to F ₂ to form a fluoride, may be a minority.
3MgH ₂ + SF ₆ → 3MgF ₂ + 3H ₂ + S (127)
6NaH + SF ₆ → 6NaF + 3H ₂ + S (128)
NaF and MgF ₂ may be electrolyzed to F ₂ , Na, and Mg from a molten salt that may additionally contain HF. Na and Mg are immiscible and the separated metal may be hydrogenated with H ₂ gas, preferably consisting of electrolysis of H ₂ O. F ₂ gas may be reacted with sulfur to regenerate SF ₆ .

In a typical hydrino and regeneration reaction, the reaction mixture, NaH catalyst, _MgH 2, NF _3, and a support, consisting of activated carbon. In the examples, the source of the exothermic reaction is an oxidation reaction of metal hydride with NF ₃ as follows.
3MgH ₂ + 2NF ₃ → 3MgF ₂ + 3H ₂ + N ₂ (129)
6MgH ₂ + 2NF ₃ → 3MgF ₂ + Mg ₃ N ₂ + 6H ₂ (130)
3NaH + NF ₃ → 3NaF + 1 / 2N ₂ + 1.5H ₂ (131)
NaF and MgF ₂ may be electrolyzed from a molten salt, which may additionally contain HF, to F ₂ , Na, and Mg. The conversion from Mg ₃ N ₂ to MgF ₂ may occur in the melt. Na and Mg are immiscible and the separated metal may be hydrogenated with H ₂ gas, preferably from electrolysis of H ₂ O. F ₂ gas may react with NH ₃ , preferably in a copper packed reactor, to form NF ₃ . Ammonia may be made from the Harbor Act. Alternatively, NF ₃ may be formed by electrolysis of NH ₄ F in anhydrous HF.

In a typical hydrino and regeneration reactions, the solid fuel reaction mixture, NaH _{catalyst, MgH 2, Na 2 S 2} O 8 and the support consists of activated carbon. In the examples, the source of the exothermic reaction is the oxidation reaction of metal hydride with Na ₂ S ₂ O ₈ as follows.
8MgH ₂ + Na ₂ S ₂ O ₈
→ 2MgS + 2NaOH + 6MgO + 6H ₂ (132)
7MgH ₂ + Na ₂ S ₂ O ₈ + C
→ 2MgS + Na ₂ CO ₃ + 5MgO + 7H ₂ (133)
10NaH + Na ₂ S ₂ O ₈ → 2Na ₂ S + 8NaOH + H ₂ (134)
9NaH + Na ₂ S ₂ O ₈ + C
→ 2Na ₂ S + Na ₂ CO ₃ + 5NaOH + 2H ₂ (135)
Any MgO product may be converted to hydroxide by reaction with water.
MgO + H ₂ O → Mg (OH) ₂ (136)
Sodium or magnesium carbonate, hydrogen carbonate, and other species consisting of carbon and oxygen may be reduced with Na or NaH.
NaH + Na ₂ CO ₃ → 3NaOH + C + 1 / H ₂ (137)
NaH + 1 / 3MgCO ₃
→ NaOH + 1 / 3C + 1 / 3Mg (138)
MgS can be burned in oxygen, hydrolyzed, exchanged with Na to form sodium sulfate, and electrolyzed to Na ₂ S ₂ O ₈ .
2MgS + 10H ₂ O + 2NaOH
→ Na ₂ S ₂ O ₈ + 2Mg (OH) ₂ + 9H ₂ (139)
Na ₂ S can be burned in oxygen, hydrolyzed to sodium sulfate, and electrolyzed to form Na ₂ S ₂ O ₈ .
2Na ₂ S + 10H ₂ O → Na ₂ S ₂ O ₈ + 2NaOH + 9H ₂ (140)
Mg (OH) ₂ can be reduced to Mg using Na or NaH.
2Na + Mg (OH) ₂ → 2NaOH + Mg (141)
NaOH can then be electrolyzed directly from the melt to Na metal and NaH and O ₂ , or from electrolysis of water so that the NaCl electrolysis gas Cl ₂ forms HCl and H ₂ . Where it may react, it may be converted to NaCl by reaction with HCl.

In a typical hydrino and regeneration reactions, the solid fuel reaction mixture, NaH catalyst, _MgH 2, S, and support, consisting of activated carbon. In the examples, the source of the exothermic reaction is an oxidation reaction of metal hydride with S as follows.
MgH ₂ + S → MgS + H ₂ (142)
2NaH + S → Na ₂ S + H ₂ (143)
Magnesium sulfide may be converted to hydroxide by reaction with water.
MgS + 2H ₂ O → 2Mg (OH) ₂ + H ₂ S (144)
H ₂ S may be decomposed at high temperatures or may be used to convert SO ₂ to S. Sodium sulfide can be converted to hydroxide by combustion and hydrolysis.
Na ₂ S + 1.5O ₂ → Na ₂ O + SO ₂
Na ₂ O + H ₂ O → 2 NaOH (145)
Mg (OH) ₂ can be reduced to Mg using Na or NaH.
2Na + Mg (OH) ₂ → 2NaOH + Mg (146)
NaOH can then be electrolyzed directly from the melt to Na metal and NaH and O ₂ , or the NaCl electrolysis gas Cl ₂ can be reacted with H ₂ from the electrolysis of water to form HCl. Whereas, NaOH may be converted to NaCl by reaction with HCl.
SO ₂ + 2H ₂ S → 3S + 2H ₂ O (147)
In an embodiment, metals such as Na and Mg may be converted to the corresponding hydrides, preferably by reaction with H ₂ from the electrolysis of water. In other embodiments, S and metal may be regenerated from the melt by electrolysis.

In a typical hydrino and regeneration reaction, the reaction mixture NaH _catalyst, MgH _{2, N} 2 O, and support, consisting of activated carbon. In the examples, the source of the exothermic reaction is an oxidation reaction of metal hydride with N ₂ O as follows.
4MgH ₂ + N ₂ O → MgO + Mg ₃ N ₂ + 4H ₂ (148)
NaH + 3N ₂ O + C → NaHCO ₃ + 3N ₂ + 1 / 2H ₂ (149)
The MgO product may be converted to hydroxide by reaction with water.
MgO + H ₂ O → Mg (OH) ₂ (150)
Magnesium nitride may also be hydrolyzed to magnesium hydroxide.
Mg ₃ H ₂ + 6H ₂ O → 3Mg (OH) ₂ + 3H ₂ + N ₂ (151)
Sodium carbonate, hydrogen carbonate, and other species consisting of carbon and oxygen may be reduced with Na or NaH.
NaH + Na ₂ CO ₃ → 3NaOH + C + 1 / H ₂ (152)
Mg (OH) ₂ can be reduced to Mg using Na or NaH.
2Na + Mg (OH) ₂ → 2NaOH + Mg (153)
And NaOH can be electrolyzed directly from the melt into Na metal and NaH and O ₂ , or NaCl electrolysis gas Cl ₂ can be combined with H ₂ from electrolysis of water to form HCl. Where reaction may occur, NaOH may be converted to NaCl by reaction with HCl. The ammonia produced from the Harbor process is oxidized (equation (124)) and the temperature is controlled to support the production of N ₂ O that is separated from other gases of the steady state reaction product.

In a typical hydrino and regeneration reactions, comprising the reaction mixture NaH catalyst, _MgH 2, Cl _2, the support (active carbon, WC, or like TiC). The reactor may further comprise a source of high energy light (preferably extreme ultraviolet light), preferably separating Cl ₂ to initiate the hydrino reaction. In the examples, the source of the exothermic reaction is a metal hydride oxidation reaction with Cl ₂ as follows.
2NaH + Cl ₂ → 2NaCl + H ₂ (154)
MgH ₂ + Cl ₂ → MgCl ₂ + H ₂ (155)
NaCl and MgCl ₂ may be electrolyzed from the molten salt to Cl ₂ , Na, and Mg. Molten NaCl electrolysis may be performed using a Downs cell or a modified Downs cell. The NaCl for this electrolysis may come from washing the reaction product with an aqueous solution. The solution may be centrifuged and filtered to remove a support such as AC (activated carbon) that may be dried, preferably using waste heat from the power system. Na and Mg are immiscible and the separated metal may be hydrogenated, preferably with H ₂ gas from the electrolysis of H ₂ O. A typical result is as follows.
Start with 4 g WC + 1 g MgH 2 + 1 g NaH + 0.01 mol Cl ₂ UV lamp, dissociate Cl ₂ to produce Cl. Input energy (Ein) is 162.9 kJ. The output energy (dE) is 16.0 kJ. The rapid rise in temperature (TSC) is 23-42 ° C. Maximum temperature (Tmax): 85 ° C. Theoretically 7.10 kJ. Gain is 2.25 times.

NaH reproduction, K or Li or reactant containing the catalyst or source of catalyst such as their hydrides, alkali metal or hydride reducing agents such as preferably Mg, MgH2 or Al, oxidizing agents such as NF ₃ by electrolysis Is possible. Preferably, the metal fluoride product is regenerated to metal and fluorine gas by electrolysis. The electrolyte may include a eutectic mixture. Further, the mixed solution may contain HF. NF ₃ may be regenerated by electrolysis of NH ₄ F in anhydrous HF. In another embodiment, NH ₃ is reacted with F ₂ in a reactor, such as a copper filled reactor. F ₂ may be produced by electrolysis using a positionally stable anode or carbon anode utilizing conditions that favor the F ₂ product. SF ₆ may be regenerated by reaction of S with F ₂ . Any metal nitride that can be formed by the hydrino reaction is thermally decomposed, H ₂ reduced, oxidized to an oxide or hydroxide and reacted to a halide, followed by electrolysis, and the metal halide melted and electrolyzed. It can be regenerated by at least one of the reactions with the halogen gas during the period. NCl ₃ can be formed by the reaction of ammonia and chlorine gas, or the reaction of an ammonium salt such as NH ₄ Cl and chlorine gas. Chlorine gas may be obtained from electrolysis of chloride salts, such as from the product reaction mixture. NH ₃ is formed by the Harbor method, and hydrogen is preferably obtained from electrolysis of water. In one embodiment, NCl ₃ is formed in situ in the reactor by reaction of at least one of ammonium salts such as NH ₃ and NH ₄ Cl with Cl ₂ gas. In some embodiments, BiF ₅ can be regenerated by reaction of BiF ₃ with F ₂ formed from electrolysis of metal fluorides.

In embodiments where the oxygen or halogen source material optionally acts as a reactant for an exothermic activation reaction, the oxide or halide product is preferably regenerated by electrolysis. The electrolyte comprises a eutectic mixture such as Al ₂ O ₃ and Na ₃ AlF ₆ ; MgF ₂ , NaF and HF; Na ₃ AlF ₆ ; NaF, SiF ₄ and HF; and a mixture of AlF ₃ , NaF and HF. Good. Electrolysis of SiF ₄ to Si and F ₂ may form an alkali fluoride eutectic mixture. Due to the low miscibility of Mg and Na, they can be separated in the melt phase. Since the miscibility of Al and Na is low, it can be separated in the melt phase. In another embodiment, the electrolysis product can be separated by distillation. In a further embodiment, Ti ₂ O ₃ is regenerated by reaction with C and Cl ₂ to form CO and TiCl ₄ . This forms a Ti and MgCl ₂ further react with Mg. Mg and Cl ₂ may be regenerated by electrolysis. When MgO is a product, Mg can be regenerated by the pigeon method. In some embodiments, MgO reacts with Si to form SiO ₂ and concentrated Mg gas. The product SiO ₂ can be regenerated to Si by H ₂ reduction at high temperature or by reaction with carbon forming Si and CO and CO ₂ . In another embodiment, Si is regenerated by electrolysis using methods such as electrolysis of solid oxides in molten calcium chloride. In some embodiments, chlorates or perchlorates such as alkali chlorates or perchlorates are regenerated by electrolytic oxidation. The brine can be oxidized electrolytically to chlorate and perchlorate.

  In order to regenerate the reactant, the oxide covering the metal support that may be formed may be removed with dilute acid after separation from the reactant or product mixture. In another embodiment, carbide is produced from the oxide by reaction with carbon releasing carbon monoxide or carbon dioxide.

  If the reaction mixture contains a solvent, the solvent may be separated from other reactants or products and regenerated by removal of the solvent by evaporation, or by filtration or centrifugation that retains the solid. If other volatile components such as alkali metals are present, they may be selectively removed by heating to a suitable high temperature so that they evaporate. For example, a metal such that Na metal is recovered by distillation or a support such as carbon remains. Na is rehydrogenated to NaH and returned to carbon with the added solvent to regenerate the reaction mixture. Isolated solids such as R-Ni can also be regenerated separately. The separated R-Ni can be hydrogenated by exposure to hydrogen gas at a pressure in the range of 0.1 to 300 atm.

  If the solvent decomposes during the catalytic reaction to form hydrino, the solvent can be regenerated. For example, the degradation product of DMF may be dimethylamine, carbon monoxide, formic acid, sodium formate and formaldehyde. In some embodiments, dimethylformamide is formed by catalytic reaction of dimethylamine and carbon monoxide in methanol or by reaction of methyl formate with dimethylamine. It can also be prepared by reacting dimethylamine with formic acid.

  In some embodiments, by way of example, the ether solvent may be regenerated from the product of the reaction mixture. Preferably, the reaction mixture and conditions are selected such that the ether reaction rate is minimal compared to the rate at which hydrinos form, where there is less ether degradation compared to the energy generated from the hydrino reaction. Therefore, the ether may be returned to the original together with the ether decomposition product removed if necessary. Alternatively, the ether and reaction conditions may be selected such that the ether reaction product is isolated and regenerates the ether.

Some embodiments include at least one of the following: HSA is fluoride, HSA is metal, and the solvent is fluorinated. The metal fluoride may be a reaction product. Metal and fluorine gas can be regenerated by metal decomposition. The electrolyte includes fluorides such as NaF, MgF ₂ , AlF _3, or LaF ₃ , and also includes other species and other salts such as at least one HF that lowers the melting point of the fluoride, eg, US Pat. No. 5,427. , 657. Excess HF may dissolve the LaF _3. The electrode is carbon, such as graphite, and can also form fluorocarbon as a desirable decomposition product. In certain embodiments, at least one metal or alloy coated with carbon, such as carbon coated Co, Ni, Fe, etc., preferably nanopowder, other transition metal powders or alloys, and metal coated carbon, preferably nanopowder, such as The carbon coated with the transition metal or alloy, preferably at least one Ni, Co, Fe and Mn coated carbon comprises magnetic particles. A magnet can be used to separate the magnetic particles from a mixture, such as a mixture of fluoride and carbon, such as NaF. The collected particles can be reused as part of the reaction mixture to form hydrinos.

In an embodiment, a catalyst or source of catalyst, such as NaF, and a fluorinated solvent is regenerated from a product consisting of NaF by separation of the product followed by electrolysis. The method of NaF sequestration may be washing of the mixture with a low boiling polar solvent followed by one or more filtrations and distillations to give NaF solids. The electrolysis may be a molten salt electrolysis. The molten salt may be a mixture such as a eutectic mixture. Preferably, the mixture consists of NaF and HF, as is known in the art. Sodium metal and fluorine gas may be collected from the electrolysis. Na may be reacted with H to form NaH. The fluorine gas may react with the hydrocarbon to form a fluorinated hydrocarbon that may function as a solvent. The HF fluorinated product can be returned to the electrolysis mixture. Alternatively, hydrocarbons and carbon products such as benzene and graphitic carbon can be fluorinated and returned to the reaction mixture, respectively. The carbon can be broken down into smaller fluoride fragments with lower melting points to function as solvents by methods known in the art. The solvent may consist of a mixture. The degree of fluorination can be used as a method to control the hydrogen catalyzed reaction rate. In an embodiment, CF ₄ is produced using a carbon electrode by electrolysis of a molten fluoride, preferably an alkali fluoride, or by reaction of carbon dioxide with fluorine gas. Any CH ₄ and hydrocarbon product may be fluorinated to CF ₄ and fluorocarbon.

Suitable fluorinated HSA materials and methods for fluorinated carbon to form the HSA material include U.S. Pat. No. 3,929,920, U.S. Pat. No. 3,925,492, U.S. Pat. No. 3,925,263, and U.S. Pat. It may be known in the art as disclosed in US Pat. No. 4,886,921. Further methods include the preparation of poly-difluoride disclosed in US Pat. No. 4,139,474, the continuous fluorination of carbon disclosed in US Pat. No. 4,447,663, US A process for producing fluorinated graphite mainly comprising poly-difluoride represented by the formula (C ₂ F) _n disclosed in US Pat. No. 4,423,261, US Pat. No. 3,925,263 For preparing poly-difluoride disclosed in US Pat. No. 4,872,032, for preparing fluorinated graphite disclosed in US Pat. No. 3,872,032, disclosed in US Pat. No. 4,243,615. A process for preparing poly-difluorocarbons, a process for preparing fluorinated graphite by catalytic reaction between carbon and fluorine gas as disclosed in US Pat. No. 4,438,086, US Pat. No. 3,929 , 918 Synthesis of Tsu graphite, U.S. disclosed in Patent No. 3,925,492 poly - preparing a fluorocarbon, and Lagow et, J. C. S. Including a mechanism that provides a new synthetic approach to graphite-fluorine chemistry disclosed in Dalton, 1268 (1974), the materials disclosed herein include HSA materials. Monel metal, nickel, steel or copper is used as one kind of reactor material in consideration of corrosion by fluorine gas. Carbon materials include amorphous carbon such as carbon black, petroleum coke, petroleum pitch coke and charcoal, crystalline graphite such as natural graphite, graphene and artificial graphite, fullerene and preferably single-walled nanotubes. Na is preferably not inserted into the carbon support to form an acetylide. Such a carbon material can be used in various forms. In general, it is preferred that the powdered carbon material has an average particle size of 50 microns or less, although larger particles are preferred. In addition to the powdered carbon material, other forms are also suitable. The carbon material may be in the form of blocks, spheres, rods and fibers. The reaction may be carried out in a reactor selected from a fluid bed reactor, a rotary kiln reactor, and a tray tower reactor.

In another embodiment, the fluorinated carbon is regenerated using additives. Carbon may also be fluorinated with inorganic reactants such as CoF ₃ outside the cell or in situ. Co to play added to the reactor, CoF, CoF ₂ and one inorganic fluorinated reactant source such as a CoF ₃ is further contained in the reaction mixture, otherwise it from the reaction mixture to form a hydrino Alternatively, from another reagent such as F ₂ gas, a fluorinated catalytic metal such as Pt or Pd may optionally be added to form during cell operation. The additive may be NH ₃ which may form NH ₄ F. At least one of carbon and hydrocarbon may react with NH ₄ F to fluorinate. In certain embodiments, the reaction mixture further comprises HNaF ₂ and may be reacted with carbon to be fluorinated. The fluorocarbon may be formed in situ or outside the hydrino reactor. Fluorocarbons can also act as solvents or HSA materials.

In embodiments where at least one of the solvent, support or adsorbent comprises fluorine, if the solvent or support is a fluorinated organic and a fluoride of a catalytic metal such as NaHF ₂ and NaF, the product will likely contain carbon. . This is also true for low energy hydrogen products such as molecular hydrino gas that can be released or recovered. F ₂ may be used to etch carbon as CF ₄ gas that can be used as a reactant in another cycle of the reaction that generates power. Residual products of NaF and NaHF ₂ can be electrolyzed to Na and F ₂ . Na reacts with hydrogen to form NaH, to etch the carbon product using F _2. Combine NaH, residual NaF and CF ₄ and perform another cycle of the power generation reaction to form hydrinos. In other embodiments, Li, K, Rb or Cs may be replaced with Na.

VI. Other Liquid and Proportional-Fuel Examples In the present disclosure, “Liquid-Solvent Examples” includes corresponding fuels and any reaction mixtures consisting of liquid solvents such as liquid fuels and promiscuous fuels.

In another embodiment comprising a liquid solvent, one of atomic sodium and molecular NaH is a reaction between at least one other compound or element and the molecular, ionic, or metallic form of Na Supplied by Sources of Na or NaH include metallic Na, inorganic compounds containing Na, such as NaOH, and NaNH ₂ , NaNH ₂ , and Na ₂ O, NaX (X is a halide), and NaH (s And at least one other suitable Na compound such as The other element may be H, a displacing agent, or a reducing agent. The reaction mixture (1) a _{solvent, (2) Na (m)} , NaH, NaNH 2, Na 2 CO 3, Na 2 O, NaOH, NaOH -doped -R-Ni, NaX (X is halogen), and, NaX A source of sodium such as at least one of the doped R—Ni, (3) a source of hydrogen such as H ₂ gas and dissociator and hydride, (4) an alkali or alkaline earth metal, preferably Li And (5) metals such as alkali metals, alkaline earth metals, lanthanides, transition metals such as Ti, metal alloys such as aluminum, B, AlHg, NaPb, NaAl, LiAl In combination with at least one and further a reducing agent such as alkaline earth halide, transition metal halide, lanthanide halide, and aluminum halide or A reducing agent such as a source of metal in Germany, it may comprise at least one of. Other suitable reducing agents consist of metal hydrides such as LiBH ₄ , NaBH ₄ , LiAlH ₄ , or NaAlH ₄ . Preferably, the reducing agent reacts with NaOH to form NaH molecules and Na products such as Na, NaH (s), and Na ₂ O. The source of NaH may be R-Ni consisting of a reactant such as a reducing agent to form a NaH catalyst such as an alkali or alkaline earth metal or R-Ni Al intermetallic alloy and NaOH. Furthermore, typical reagents are alkali or alkaline earth metals, and preferably Br or I, but AlX ₃ , MgX ₂ , LaX ₃ , CeX ₃ , and TiX _n when X is halogen. It is an oxidizing agent. In addition, the reaction mixture may contain a dispersant such as getter or at least one of Na ₂ CO ₃ , Na ₃ SO ₄ , and Na ₃ PO ₄ , which may be doped with a dissociator such as R—Ni. It may consist of another compound containing. The reaction mixture may further comprise a support, where the support is a support that may be doped with at least one reactant of the mixture. The support may preferably have a large surface area that favors the productivity of the NaH catalyst from the reaction mixture. The support is Al ₂ O ₃ , such as R-Ni, Al, Sn, γ-, β-, or α-alumina, sodium aluminate (β-alumina has other ions such as Na ⁺ specific with _{Na 2} O · 11Al 2 O ₃ is a _{composition.),} lanthanide oxides such as M 2 _{O 3} (preferably, M = La, Sm, Dy , Pr, Tb, Gd, and Er), Si, silica, silicates, zeolites, lanthanides, transition metals, metal alloys such as alkaline earth alloys with alkali and Na, rare earth metals, Ni-supported SiO ₂ —Al ₂ O ₃ or SiO ₂ , and It may comprise at least one of the group consisting of platinum, palladium or other supporting metals such as at least one of alumina supported on ruthenium. The support may have a high surface area, and, R-Ni, zeolites, silicates, aluminates, alumina, alumina nanoparticles, porous _{Al 2 O 3, Pt, Ru} , or Pd / Al ₂ Including high surface area (HSA) materials such as O ₃ , carbon, Pt or Pd / C, inorganic compounds such as Na ₂ CO ₃ , silica and zeolitic materials, preferably Y zeolite powder, carbon such as fullerenes or nanotubes It's okay. In an embodiment, a support such as Al ₂ O ₃ (and a dissociator Al ₂ O ₃ support, if present) is used with a reducing agent such as a lanthanide to form a surface modified support. react. In the examples, surface Al is exchanged with lanthanides to form lanthanide substituted supports. This support may be doped with a source of NaH molecules such as NaOH and may be reacted with a reducing agent such as a lanthanide. Subsequent reaction of the lanthanide substituted support with lanthanide will not change that much, and surface doped NaOH can be reduced to NaH catalyst by reaction with the reducing agent lanthanide.

Where the reaction mixture includes a source of NaH catalyst, in embodiments including a liquid solvent, the source of NaH may be an alloy of Na and a source of hydrogen. Alloys include sodium metal and one or more alkali or alkaline earth metals, transition metals, Al, Sn, Bi, Ag, In, Pb, Hg, Si, Zr, B, Pt, Pd, or other It may include at least one of those known in the art, such as a metal alloy, and the H source may be H ₂ or a hydride.

  Reagents such as a source of NaH molecules, a source of sodium, a source of NaH, a source of hydrogen, a displacing agent, and a reducing agent are present in any desired molar ratio. Each is a molar ratio greater than 0 and less than 100%. Preferably, the molar ratio is similar.

In the liquid-solvent embodiment, the reaction mixture may be a solvent, a source of Na or Na, a source of NaH or NaH, a metal hydride or source of metal hydride, a reactant or reactant to form a metal hydride. Including at least one series of the group consisting of a source, a hydrogen dissociator, and a source of hydrogen. The reaction mixture may further comprise a support. The reactant to form the metal hydride may comprise a lanthanide, preferably La or Gd. In an example, La may react reversibly with NaH to form LaH _n (n = 1, 2, 3). In the examples, the hydride exchange reaction forms a NaH catalyst. The reversible-general reaction is given by:

The reaction given by equation (156) applies to the other MH-type catalysts given in Table 3. The reaction may initiate the formation of hydrogen that may be dissociated to form atomic hydrogen that reacts with Na to form NaH catalyst. The dissociator is preferably at least one of Pt, Pd, or Ru / Al2O3 powder, Pt / Ti, and R-Ni. Preferentially, the dissociator support, such as Al ₂ O ₃ , contains at least surface La substitution instead of Al, or Pt, Pd, or Ru / M ₂ O ₃ where M is a lanthanide Including things. The dissociator may be separated from the rest of the reaction mixture as the separator passes atomic hydrogen.

The solvent was removed and the addition of H _2, are separated NaH and lanthanum hydride by sieving, by heating the lanthanum hydride to form a La, by mixing La and NaH, the reaction mixture is carried out In the examples, examples of suitable liquid-solvents that may be regenerated include a reaction mixture consisting of solvent, NaH, La, and Pd on Al ₂ O ₃ powder. Alternatively, regeneration involves separating Na and lanthanum hydride by dissolving Na and removing the liquid, heating lanthanum hydride to form La, and hydrogenating Na to NaH. A step, mixing La and NaH, and adding a solvent. La and NaH may be mixed by a ball mill.

In the liquid-solvent embodiment, a high surface area material such as R-Ni is doped with NaX (X = F, Cl, Br, I). The doped R-Ni reacts with a reagent that will replace the halide to form at least one of Na and NaH. In an embodiment, the reactant is at least an alkali or alkaline earth metal, preferably at least one of K, Rb, Cs. In another embodiment, the reactant is preferably KH, RbH, CsH, MgH _2, and at least one of CaH _2, alkali or alkaline earth hydrides. The reactants can be both alkali metal and alkaline earth hydrides. The reversible-general reaction is given by:

A. NaOH catalyzed reaction to form NaH catalyst The reaction in which NaOH and Na become Na ₂ O and NaH is as follows.
NaOH + 2Na → Na ₂ O + NaH (158)
The exothermic reaction can promote the formation of NaH (g). Thus, Na metal can function as a reducing agent to form catalyst NaH (g). Other examples of suitable reducing agents with a highly exothermic reduction reaction similar to the source of NaH include alkali metals, alkaline earth metals such as at least one of Mg and Ca, LiBH ₄ , NaBH ₄ , LiAlH ₄ , or Metal hydrides such as NaAlH ₄ , transition metals such as B, Al, Ti, La, Sm, Dy, Pr, Tb, Gd, and at least one of Er, preferably La, Tb, And Sm, but lanthanides. Preferably, the reaction mixture comprises a high surface area material (HSA material) with a solvent, a dopant such as NaOH containing a source of NaH catalyst. Preferably, conversion of the dopant on the material with high surface area to the catalyst is accomplished. The conversion may be caused by a reduction reaction. In addition to Na, other preferred reducing agents are other alkali metals, Ti, lanthanides, or Al. Preferably, the reaction mixture comprises NaOH doped in an HSA material, preferably R-Ni where the reducing agent is Na or intermetallic Al. The reaction mixture may further comprise a source of H such as hydride or H ₂ gas and a dissociator. In some embodiments, the H source is hydrogenated R—Ni.

In the liquid-solvent example, Na ₂ O formed as the product of a reaction that produces a NaH catalyst as given by formula (158) forms NaOH that can further function as a source of NaH catalyst. Reacts with a source of hydrogen. In the examples, where there is atomic hydrogen, the regeneration reaction of NaOH from formula (158) is as follows.
Na ₂ O + H → NaOH + Na
ΔH = −11.6 kJ / mole NaOH (159)
NaH → Na + H (1/3)
ΔH = −10,500 kJ / mole H (160)
NaH → Na + H (1/4)
ΔH = −19,700 kJ / mole H (161)
Thus, a small amount of NaOH and Na with atomic hydrogen or a source of atomic hydrogen, in turn, forms hydrino mass production through multiple cycles of the regeneration reaction as given by equations (158-161). , Function as a catalyst source of NaH catalyst. In the examples, the reaction given by formula (158-161) proceeds with NaH and H to form hydrinos, and from the reaction given by formula (162), Al (OH) ₃ is derived from NaOH and NaH. Can act as a source.
3Na + Al (OH) ₃
→ NaOH + NaAlO ₂ + NaH + 1 / 2H ₂ (162)
In the liquid-solvent embodiment, the intermetallic compound of Al functions as a reducing agent that forms a NaH catalyst. The reversible reaction is given as follows.
3NaOH + 2Al → Al ₂ O ₃ + 3NaH (163)
This exothermic reaction promotes the formation of NaH (g) so that regeneration of NaH occurs from Na in the presence of atomic hydrogen so as to promote the very exothermic reaction given by formula (25-30). Can do.

  Two examples of suitable liquid-solvents are: Na serves as a reducing agent, a first reaction mixture of Na and R—Ni containing about 0.5 wt% NaOH, and an intermetallic compound Al as the reducing agent. And a second reaction mixture of R—Ni containing about 0.5 wt% NaOH. The reaction mixture may be regenerated by adding NaOH and NaH that may function as H source and reducing agent.

  In the liquid-solvent embodiment, for the energy reactor, a source of NaH, such as NaOH, is regenerated by the addition of a source of hydrogen and a dissociator, such as at least one of hydride and hydrogen gas. The hydride and dissociator may be hydrogenated R—Ni. In another embodiment, a source of NaH, such as R-Ni doped with NaOH, is regenerated by at least one of rehydrogenation, addition of NaH, and addition of NaOH. Here, the addition is by physical mixing. Initially, the solvent may be removed and mixing may be performed mechanically, such as by a ball mill.

In the liquid-solvent embodiment, the reaction mixture further includes an oxide-shaped reactant that reacts with NaOH or Na ₂ O to form a very stable oxide and NaH. Such reactant composition is cerium, magnesium, lanthanide, titanium, or aluminum, or a compound thereof, AlX ₃ , MgX ₂ , LaX ₃ , CeX ₃ , and TiX _n (where X is a halide). Preferably, it consists of compounds such as Br or I) and reducing compounds such as alkali or alkaline earth metals. In an embodiment, the source of NaH catalyst comprises R-Ni consisting of a sodium compound such as NaOH at the surface. The reaction of NaOH with an oxide-forming reactant such as AlX ₃ , MgX ₂ , LaX ₃ , CeX ₃ , TiX _n , and alkali metal M is NaH, MX, and Al ₂ O. ₃ , MgO, La ₂ O ₃ , Ce ₂ O ₃ , and Ti ₂ O ₃ are formed.

In the liquid-solvent embodiment, the reaction mixture consists of NaOH-doped R-Ni and an alkali or alkaline earth metal added to form at least one of Na and NaH molecules. Na is further reacted with H from sources such as hydride or H ₂ gas, such as R-Ni to form a NaH catalyst. The catalysis reaction following the NaH reaction forms the H state given by equation (35). The addition of alkali or alkaline earth metal M may reduce Na ⁺ to Na by reaction.
NaOH + M to MOH + Na (164)
2NaOH + M → M (OH) ₂ + 2Na (165)
M may also react with NaOH to form H as well as Na.
2NaOH + M → Na ₂ O + H ₂ + MO (166)
Na ₂ O + M → M ₂ O + 2Na (167)
And catalyst NaH may be formed by reaction.
Na + H → NaH (168)
Similar to the reaction from R-Ni and any added source of H, it may be formed by reacting with H from the reaction as given by formula (166). Na is a suitable reducing agent. Because it is a further source of NaH.

Hydrogen may be added to reduce NaOH and form a NaH catalyst.
NaOH + H ₂ → NaH + H ₂ O (169)
The R-Ni H may reduce NaOH to Na metal and water removed by the pump. The organic solvent may be removed first before the reduction, or a molten inorganic solvent may be used.

In the liquid-solvent embodiment, the reaction mixture includes one or more compounds that react with a source of NaH to form a NaH catalyst. The source may be NaOH. _Compounds, LiNH _{2, Li} 2 _NH, and may comprise at least one of Li ₃ N. The reaction mixture may further comprise a source of hydrogen such as H _2. In the examples, to form NaH and lithium hydroxide, the reaction of sodium hydroxide and lithium amide is as follows.
NaOH + LiNH ₂
→ LiOH + NaH + 1 / 2N ₂ + LiH (170)

In order to form NaH and lithium hydroxide, the reaction of sodium hydroxide with lithium imide is as follows.
NaOH + Li ₂ NH
→ Li ₂ O + NaH + 1 / 2N ₂ + 1 / 2H ₂ (171)
And in order to form NaH and lithium hydroxide, reaction of sodium hydroxide and lithium nitride is as follows.
NaOH + Li ₃ N
→ Li ₂ O + NaH + 1 / 2N ₂ + Li (172)

B. In the alkaline earth hydroxide catalyzed liquid-solvent embodiment for forming NaH catalyst, a source of H is provided to the source of Na to form catalyst NaH. The Na source may be a metal. The source of H may be a hydroxide. The hydroxide may be at least one of alkali, alkaline earth hydroxide, transition metal hydroxide, Al (OH) ₃ . In an embodiment, Na reacts with hydroxide to form the corresponding oxide and NaH catalyst. In the example where the hydroxide is Mg (OH) ₂ , the product is MgO. In the example where the hydroxide is Ca (OH) ₂ , the product is CaO. Alkaline earth oxides may react with water to regenerate the hydroxides. The hydroxide can be collected as a precipitate by methods such as filtration and centrifugation.

For example, in the examples, the reaction for forming the NaH catalyst and the regeneration cycle for Mg (OH) ₂ are performed according to the following reaction formula.
3Na + Mg (OH) ₂ → 2NaH + MgO + Na ₂ O (173)
MgO + H ₂ O → Mg (OH) ₂ (174)
In the liquid-solvent example, the reaction to form the NaH catalyst and the regeneration cycle for Ca (OH) ₂ is performed according to the following reaction equation.
4Na + Ca (OH) ₂ → 2NaH + CaO + Na ₂ O (175)
CaO + H ₂ O → Ca (OH) ₂ (176)

C. Na / N alloy reaction solids to form NaH catalyst and alkali metals in liquid state are metals. To produce an M or MH catalyst, M is an alkali metal and the liquid or heterogeneous fuel reaction mixture is an M / N alloy reactant. In an embodiment, the reaction mixture, liquid fuel reaction, heterogeneous fuel reaction, and regeneration reaction include those of the M / N system where the fuel produces at least one of a catalyst and atomic hydrogen.

In an embodiment, the reaction mixture consists of one or more compounds that react with a source of NaH to form a NaH catalyst. The reaction _{mixture, Na, NaH, NaNH 2,} Na 2 NH, Na 3 N, NH 3, dissociation agents, a hydrogen source such as _{H 2} gas or a hydride, support and, NaX (X is a halide At least one of the group consisting of getters such as The dissociator is preferably Pt, Ru, or Pd / Al ₂ O ₃ powder. The dissociator may comprise Pt or Pd on a high surface area support that is suitably inert to Na. The dissociator may be Pt or Pd on carbon or Pd / Al ₂ O ₃ . The latter support may comprise a protective surface coating of a material such as NaAlO _2. The reactants may be present in any wt%.

When the reaction mixture may be regenerated by addition of _{H 2,} a suitable liquid - Examples of the solvent include solvents, Na or NaH, NaNH ₂ and consists of the reaction mixture of _Al 2 _{O 3} powder on Pd.

In the examples, NaNH ₂ is added to the reaction mixture. NaNH ₂ generates NaH by a reversible reaction.
Na ₂ + NaNH ₂ → NaH + Na ₂ NH (177)
2NaH + NaNH ₂ → NaH (g) + Na ₂ NH + H ₂ (178)

In the hydrino reaction cycle, Na—Na and NaNH ₂ react to form NaH molecules and Na ₂ NH. NaH forms hydrino and Na. Thus, the reaction is reversible, as by the following reaction.
Na ₂ NH + H ₂ → NaNH ₂ + NaH (179)
Na ₂ NH + Na + H → NaNH ₂ + Na ₂ (180)

  In an example, the NaH of formula (179) is a molecule such that this reaction is another that produces a catalyst.

The reaction of sodium amide and hydrogen to form ammonia and sodium hydride is as follows.
H ₂ + NaNH ₂ → NH ₃ + NaH (181)
In the liquid-solvent example, the reaction is reversible. The reaction can be facilitated to form NaH by increasing the H ₂ concentration. Alternatively, the positive reaction can be facilitated by the formation of atomic hydrogen using a dissociator. The reaction is given as follows.
2H + NaNH ₂ → NH ₃ + NaH (182)
The exothermic reaction can promote the formation of NaH (g).

In the liquid-solvent embodiment, the NaH catalyst is formed from the reaction of NaNH ₂ and hydrogen, but the hydrogen is preferably atomic hydrogen as given by reaction equation (181-182). The ratio of reactants can be any desired amount. Preferably, the ratio is approximately stoichiometric to those of formula (181-182). Where the catalytic reaction is given by formula (25-30) and sodium amide is formed with additional NaH catalyst by reaction of Na with ammonia, the reaction forming the catalyst was reacted to form hydrino. To replace it, it is reversible with the addition of a source of H such as H ₂ gas or hydride.
NH ₃ + Na ₂ → NaNH ₂ + NaH (183)

Liquid - In the examples of the solvent, HSA material, NaNH ₂ is doped. The doped HSA material reacts with the reagent that will replace the amide group to form at least one of Na and NaH. In the examples, the reactant is preferably Li, but is an alkali or alkaline earth metal. In another embodiment, the reactant is preferably LiH, but is an alkali or alkaline earth hydride. The reactants can be both alkali metal and alkaline earth hydrides. In addition to that provided by any other reagent in the reaction mixture, such as hydride, HSA material, and displacement reagent, a source of H, such as H ₂ gas, may be further provided.

In liquid-solvent examples, sodium amide undergoes a reaction with lithium to form lithium amide, imide, or nitrogen compounds and Na or NaH catalyst. The reaction of lithium imide and sodium amide to form NaH with lithium is as follows.
2Li + NaNH ₂ → Li ₂ NH + NaH (184)
The reaction of sodium amide and lithium hydride to form lithium amide and NaH is as follows.
LiH + NaNH ₂ → LiNH ₂ + NaH (185)
The reaction of sodium amide, lithium and hydrogen to form lithium amide and NaH is as follows.
Li + 1 / 2H ₂ + NaNH ₂ → LiNH ₂ + NaH (186)
In the liquid-solvent example, the reaction of the mixture forms Na, and the reactant further includes a source of H that reacts with Na to form catalytic NaH by a reaction such as the following.
Li + NaNH ₂ to LiNH ₂ + Na (187)
Na + H to NaH (188)
LiH + NaNH ₂ to LiNH ₂ + Na (189)

Liquid - In the examples of the solvent, the reaction product preferably comprises NaNH ₂ which is a reaction product replacing NaNH2 amide groups such as an alkali or alkaline earth metal is Li, and additionally, MH (M = Li, Na, K, Rb, Cs, Mg, Ca, Sr, and Ba), H ₂ , a hydrogen dissociator, and a source of H such as at least one of the hydrides.

The reaction mixture reagents such as solvent, M, MH, NaH, NaNH ₂ , HSA material, hydride, and dissociator are present in any desired molar ratio. Each of M, MH, NaNH ₂ and the dissociator is in molar ratio greater than 0 and less than 100%, preferably these molar ratios are similar.

Other examples of liquid-solvent systems that generate molecular catalyst NaH include Na and NaBH ₄ or NH ₄ X, where X is an anion such as a halogen. Molecular NaH catalyst can be produced by the reaction of Na ₂ and NaBH ₄ .
Na ₂ + NaBH ₄ → NaBH ₃ + Na + NaH (190)
NH ₄ X can produce NaNH ₂ and H ₂ .
Na ₂ + NH ₄ X → NaX + NaNH ₂ + H ₂ (191)

And NaH catalyst is Eqs. (177-189). In another liquid-solvent embodiment, the reaction mechanism by which the Na / N system forms the hydrino catalyst NaH is as follows.
_{NH 4 X + Na-Na →} NaH + NH 3 + NaX (192)

D. An additional MH type catalyst and another catalyst system of reaction type MH comprises aluminum. The binding energy of AlH is 2.98 eV. The first and second ionization energies of Al are 5.985768 eV and 18.82855 eV, respectively. Based on these energies, AlH binding energy plus Al double ionization to Al ²⁺ (t = 2) is 27.79 eV (27.2 eV) equal to m = 1 in equation (36), so AlH Molecules can function as catalysts and H sources. The catalytic reaction is given as follows.

Al ²⁺ + 2e ⁻ + H → AlH + 27.79 eV (194)
Here, the total reaction is as follows.

In the liquid-solvent embodiment, the reaction mixture includes at least one of AlH molecules and a source of AlH molecules. The source of AlH molecules may include a source of hydrogen, which is Al metal and preferably atomic hydrogen. The source of hydrogen may be a hydride, preferably R-Ni. In another embodiment, the catalyst AlH is produced by the reaction of a reducing agent with an oxide or Al hydroxide. The reducing agent includes at least one of the previously given NaOH reducing agents. In an embodiment, a source of H is fed to the source of Al to form the catalyst AlH. The Al source may be a metal. The source of H may be a hydroxide. The hydroxide may be at least one of alkali, alkaline earth hydroxide, transition metal hydroxide, and Al (OH) ₃ .

Raney nickel can be prepared by the following two reaction steps.
Ni + 3Al → NiAl ₃ (or Ni ₂ Al ₃ ) (196)

Na [Al (OH) ₄ ] is immediately dissolved in high concentration NaOH. It can be washed with deoxygenated water. The prepared Ni contains Al (about 10 wt%, can vary), is porous, and has a large surface area. It contains a large amount of H, both in the Ni lattice and in the form of Ni—AlH _x (x = 1, 2, 3).

  R-Ni may react with another element to cause chemical release of AlH molecules. The AlH molecules are then catalyzed by the reaction given by equations (193-195). In an embodiment, AlH release is caused by a reduction reaction, etching, or alloy formation. Such other element M is an alkali or alkaline earth metal that reacts with the Ni portion of R-Ni, causing the AlHx component to release subsequently catalyzed AlH molecules. In an embodiment, M may react with Al hydroxide or oxide to form Al metal that may further react with H to form AlH. The reaction can be initiated by heating, and the reaction rate can be controlled by controlling the temperature. Solvent, M (alkali or alkaline earth metal), and R-Ni are present in any desired molar ratio. Each of the solvent, M, and R-Ni is greater than 0 and less than 100% in molar ratio. Preferably, the molar ratios of M and R-Ni are similar.

  In liquid-solvent embodiments, in the art, such as alloys or R-Ni containing at least one of Ni, Cu, Si, Fe, Ru, Co, Pd, Pt, and other elements and compounds. AlH sources include known Al alloys or other Raney metals and R-Ni. The R—Ni or alloy may further comprise a promoter such as at least one of Zn, Mo, Fe, and Cr. R-Ni is a W.S. R. Grace Rainey 2400, Rainey 2800, Rainey 2813, Rainey 3201, Rainey 4200, or at least one of etched or Na-doped embodiments of these materials. In another liquid-solvent embodiment of the AlH catalyst system, the ratio of Al to Ni is in the range of about 10-90%, preferably in the range of about 10-50%, and more preferably about 10-30%. In this range, the source of the catalyst comprises a Ni / Al alloy. The source of the catalyst may include palladium or platinum, and may further include Al as the Raney metal.

Another catalyst system of type MH contains chlorine. The binding energy of HCl is 4.4703 eV. The first, second, and third ionization energies of Cl are 12.96764 eV, 23.814 eV, and 39.61 eV, respectively. Based on these energies, the binding energy of HCl plus the triple ionization of Cl to Cl ³⁺ (t = 3) is 80.86 eV (3.227.2 eV) equal to m = 3 in Equation (36). As such, HCl can function as a catalyst and H source. The catalytic reaction is given as follows.

Cl ³⁺ + 3e ⁻ + H → HCl + 80.86 eV (199)
The total reaction is as follows.

In the liquid-solvent example, the reaction mixture includes HCl or a source of HCl. The source may be NH ₄ Cl or a solid acid and a chloride such as an alkali or alkaline earth chloride. The solid acid may be at least one of MHSO ₄ , MHCO ₃ , MH ₂ PO ₄ , and MHPO ₄ . Here, M is a cation such as an alkali or alkaline earth cation. Other such solid acids are known to those skilled in the art. In an example, the reaction mixture includes a strong acid such as H ₂ SO ₄ and an ionic compound such as NaCl. Reaction of an ionic compound such as NaCl with an acid produces HCl to function as a hydrino catalyst and H source.

In general, t-electrons from each M-hydrogen bond plus atom M at successive energy levels, such that the sum of t-electron binding energy and ionization energy is approximately 3.27.2 eV, where m is an integer. MH type hydrogen catalysts that produce hydrinos provided by ionization of are given in Table 3. Each MH catalyst is given in the first column and the corresponding MH bond energy is given in column 2. The atom M of the MH species provided in the first column is ionized, but in column 2 provides a net reaction enthalpy of 3.27.2 eV for the addition of binding energy. The enthalpy of the catalyst is given in the eighth column, while the value of m is given in the ninth column. The electrons that contribute to ionization are given with respect to the ionization potential (also called ionization energy or binding energy). For example, the binding energy of NaH (1.9245 eV) is given in column 2. The ionization potential of the n-th electronic atom or ion is designated by IP _n, given by CRC. That is, for ^{example, Na + 5.13908eV → Na + +} e - and ^{Na + + 47.2864eV → Na 2+ +} e -. A first ionization potential, IP ₁ = 5.13908 eV, and a second ionization potential, IP ₂ = 47.2864 eV, are given in the second and third columns, respectively. The net reaction enthalpy for NaH bond scission and Na double ionization is 54.35 eV, given in the eighth column, and m = 2 in equation (36), the ninth column Given in. Additionally, H can react with each of the MH molecules given in Table 3, so that, as given by the typical equation (23), relative to the catalytically reactive organism of MH alone, Only one quantum number p is increased (equation (35)) to form a hydrino.

In other liquid-solvent examples of MH type catalysts, the reactants include sources of SbH, SiH, SnH, and InH. In an example providing catalyst MH, the sources are M and H ₂ sources, and MH _x consisting of one of Sb, Si, Sn, and In and a source of H ₂ , and SbH ₃ , SiH _4. , SnH ₄ , and InH ₃ .

The liquid-solvent reaction mixture further comprises a source of H and a source of catalyst, wherein at least one source of H and catalyst may be a solid acid or NH ₄ X, further wherein an HCl catalyst is added. To form X is a halogen, but preferably Cl. Preferably, the reaction mixture is a halogen where X is preferably Cl, but the solvent, NH ₄ X, solid acid, NaX, LiX, KX, NaH, LiH, KH, Na, Li, K, support, hydrogen A dissociator and at least one of H ₂ may be included. Solid acids include NaHSO ₄ , KHSO ₄ , LiHSO ₄ , NaHCO ₃ , KHCO ₃ , LiHCO ₃ , Na ₂ HPO ₄ , K ₂ HPO ₄ , Li ₂ HPO ₄ , NaH ₂ PO ₄ , KH ₂ PO ₄ , and LiH it may be a ₂ PO _4. The catalyst may be at least one of NaH, Li, K, and HCl. The reaction mixture may further comprise at least one of a dissociator and a support.

In each case the MH sources of M alloys such as AlH and Al, respectively, the alloy may be hydrogenated with a source of H _2, such as H ₂ gas. H ₂ can be supplied to the alloy during the reaction. Alternatively, H ₂ can be supplied to form the desired amount of H alloy with changes in H pressure during the reaction. In this case, the initial H ₂ pressure may be about zero. The alloy may be activated by the addition of a metal such as an alkali or alkaline earth metal. For the MH catalyst and source of MH, the hydrogen gas may be maintained in the range of about 1 Torr to 100 atm, preferably about 100 Torr to 10 atm, more preferably about 500 Torr to 2 atm. In other embodiments, the source of hydrogen is from a hydride such as an alkali or alkaline earth metal hydride or a transition metal hydride.

  When two H atoms ionize, one H atom undergoes a transition so as to form the state given by equation (35), while the dense atomic hydrogen is a three-body collision reaction to form a hydrino. Can go through. The reaction is given as follows.

2H ⁺ + 2e ⁻ → 2H [a _H ] +27.21 eV (202)
The total reaction is as follows:

In another example, the reaction is given as follows.

2H _fast ⁺ 2e ⁻ → 2H [a _H ] +54.4 eV (205)
Furthermore, the overall reaction is as follows:

In the liquid-solvent embodiment, the material supplying the H atoms at high density is R-Ni. Atomic hydrogen may be from at least one of dissociation of H ₂ from a H ₂ source, such as H ₂ gas supplied to the cell, and decomposition of H in R-Ni. The alkali or alkaline earth metal M and R-Ni may react to enhance the production of atomic hydrogen layers to cause catalysis. R-Ni separated R-Ni from a solvent that could be regenerated by evaporating metal M followed by addition of hydrogen to rehydride.

VII. Additional H autocatalytic reaction In another catalytic reaction involving only H atoms, two hot H ₂ molecules collide and 3 H atoms are 3.2 · 27.2 eV for the fourth H atom. Dissociate to function as a catalyst. The three atoms resonate and non-radiatively receive 81.6 eV from the fourth hydrogen atom, and 3H functions as a catalyst. The reaction between the four hydrogen atoms is as follows.

3H _fast ⁺ + 3e ⁻ → 3H + 81.6 eV (208)
The total reaction is as follows:

The extreme ultraviolet continuous emission band according to H * [a _H / (3 + 1)] of the intermediate of formula (207) is predicted to block at a short wavelength at 122.4 eV (10.1 nm) and extend to a longer wavelength. Is done.

In general, the transition from H to H [a _H / (p = 3 + 1)] upon receipt of 3 · 27.2 eV gives a continuous band with a short wavelength cut at the next energy.

The energy is given by:

This corresponds to 91.2 / m ² nm and extends to a longer wavelength than the corresponding cutoff.

When another catalytic reaction involving collisions of H ₂ with hot H occurs, each of the two H atoms receives 13.6 eV to form a third atom, and against the third atom , Ionized to function as a 27.2 eV catalyst. And from the third hydrogen atom so that 2H functions as a catalyst, the two atoms can receive 27.2 eV resonantly and non-radioactively, the reaction between hydrogen is given by It is done.

2H ⁺ + 2e ⁻ → 2H + 27.2 eV (212)
The total reaction is as follows:

The extreme ultraviolet continuous emission band due to the H * [a _H / (1 + 1)] intermediate of formula (211) is predicted to have a short wavelength cutoff at 13.6 eV (91.2 nm) and extend to a longer wavelength. Where the H atom functions as a catalyst by accepting at 27.2 eV from the second hydrogen atom, the high density allows another reaction to give a continuous band of 91.2.

  In the presence of a high magnetic field, the short-wavelength block at the final state hydrino atom binding energy causes the ionized electrons to move directly to the fractional state along with the released binding energy as a continuum band.

The extreme ultraviolet continuous radiation bands are expected to extend to longer wavelengths with short wavelength cutoffs at 54.4 eV (22.8 nm) and 122.4 eV (10.1 nm), respectively. H (1/4) is the preferred state due to multipolarization and corresponding selection rules. Extreme ultraviolet continuous radiation has a short wavelength cutoff at 217.6 eV (5.7 nm) and is expected to extend to longer wavelengths.

The ionization potential of the molecular hydrino H ₂ (1 / p) is as follows:
IP ₁ = E _T [H ₂ ⁺ (1 / p)] − E _T (H ₂ (1 / p))
= -P ² 16.13392 eV-p ³ 0.118755 eV
− (− P ² 31.351 eV-p ³ 0.326469 eV)
= P ² 15.2171 eV + p ³ 0.207714 eV (216)
The molecular hydrino H ₂ (1 / p) binding energy E _D is given as follows:
E _D = −p ² 27.20 eV-E _T
= -P ² 27.20 eV
− (− P ² 31.351 eV-p ³ 0.326469 eV)
= P ² 4.151 eV-p ³ 0.326469 eV (217)
Another aspect of the present disclosure consists of a source of EUV radiation. The light source includes an element that excites the molecular hydrino gas to the ionization threshold and the molecular hydrino gas. The deexcitation energy is given by equation (216). The excitation may be with a particle beam, preferably an electron beam. Molecular hydrino gas may be trapped in a matrix, preferably in an alkali or alkaline earth halide crystal. The crystal may be bombarded with an electron beam at a high energy such as 2 kV, which results in excitation followed by deexcitation emission. In another embodiment, deexcitation further results in the breaking of molecular hydrino bonds. The difference in energy given by equations (216) and (217) gives the emission energy as follows:
E _emission = p ² 11.0661 eV-p ³ 0.118755 eV
(218)
For p = 4, the radiation is 7.3 nm (169.5 eV), which is extreme ultraviolet (EUV). This light could be used for EUV lithography to make microelectronic devices.

In examples, as revealed herein, a source of Rb ⁺ such as Rb or hydride, or a source of Cs such as Cs metal or hydride, respectively, is used as the source of Rb ⁺ or Cs catalyst. , Each may function.

Hydrino hydride ions may react with an oxidizing agent such as oxygen or sulfur to form molecular hydrinos. A typical reaction is as follows.
^{2H - (1 / p) +} S → H 2 (1 / p) + S 2- (219)
^{2H - (1 / p) +} O 2 → H 2 (1 / p) + O 2 2- (220)
Thus, in embodiments of hydrino chemistry, hydrino hydride may be converted to molecular hydrino when it is the desired product.

VIII. Hydrogen Gas Emission Power and Plasma Cell and Reactor The hydrogen gas emission power, plasma cell and reactor of the present disclosure are shown in FIG. The hydrogen gas discharge power, plasma cell, and reactor of FIG. The hydrogen source 322 supplies hydrogen to the chamber 300 by the control valve 325 through the hydrogen supply passage 342. The catalyst is contained in the cell chamber 300. A voltage and current source 330 allows current to pass between the cathode 305 and the anode 320. The current may be reversible.

  In an embodiment, the cathode 305 material may be a source of catalyst such as Fe, Dy, Be, and Pd. In another embodiment of hydrogen gas discharge power, plasma cell and reactor, the wall of vessel 313 is electrically conductive and functions as a cathode to replace electrode 305, and anode 320 is a cavity such as a stainless steel cavity anode. May be. The release may evaporate the catalyst source to become a catalyst. Molecular hydrogen may be dissociated by release, thereby forming hydrogen atoms and generating hydrinos and energy. Additional dissociation may be provided by the hydrogen dissociator in the chamber.

  Another embodiment of a hydrogen gas discharge power and a plasma cell and a reactor catalyzed in the gas phase utilizes a controllable gaseous catalyst. Gaseous hydrogen atoms for conversion to hydrino are supplied by the release of molecular hydrogen gas. The gas release cell 307 has a catalyst supply passage 341 for passing the gaseous catalyst 350 from the catalyst reservoir 395 to the reaction chamber 300. The catalyst reservoir 395 is heated by a catalyst reservoir heater 392 having a power source 372 in order to supply a gaseous catalyst to the reaction chamber 300. By controlling the temperature of the catalyst reservoir 395 by adjusting the heater 392 with the power source 372, the catalyst vapor pressure is controlled. The reactor further includes an optional vent valve 301. A chemically resistant open mouth container, such as stainless steel, tungsten, or a ceramic boat, may be placed in the gas release cell and contain a catalyst. With a boat heater that uses an associated power source to supply the gaseous catalyst to the reaction chamber, the catalyst in the catalyst boat may be heated. Alternatively, the incandescent gas release cell is operated at a high temperature so that the catalyst in the boat is sublimated, boiled, volatilized into the gas phase. By controlling the temperature of the boat or discharge cell by adjusting the heater with its power source, the catalyst vapor pressure is controlled. In order to prevent the catalyst from agglomerating in the cell, the temperature is maintained above the temperature of the catalyst source, catalyst reservoir 395, or catalyst boat.

In an example, catalysis occurs in the gas phase, lithium is the catalyst, and the source of atomic lithium such as lithium metal or lithium compound such as LiNH ₂ is within the range of about 300-1000 ° C. It is made gaseous by maintaining the temperature. Most preferably, the cell is maintained in the range of about 500-750 ° C. The atomic and / or molecular hydrogen reactant is preferably in the range of about 100 millitorr to about 100 torr, but is maintained at a pressure below atmospheric pressure. Most preferably, the pressure is determined by maintaining a mixture of lithium metal and lithium hydride in the cell maintained at the desired operating temperature. The operating temperature range is preferably in the range of about 300-1000 ° C, and most preferably the pressure can be achieved for cells in the operating temperature range of 300-750 ° C. The cell can be controlled to the desired operating temperature by a heating coil such as 380 in FIG. The cell may further include an inner reaction chamber 300 and an outer hydrogen reservoir 390, and hydrogen may be supplied to the cell by diffusion of hydrogen through a wall 313 separating the two chambers. The wall temperature may be controlled using a heater to control the diffusion rate. The diffusion rate may be further controlled by controlling the hydrogen pressure with a hydrogen reservoir.

With _{Li, LiNH 2, Li 2 NH} , Li 3 N, LiNO 3, LiX, NH 4 X (X is _{halogen), NH 3, LiBH 4,} LiAlH 4, and the reaction mixture consisting of seeds of the group of _{H 2} In another embodiment of the system, at least one of the reactants is regenerated by adding one or more reagents and by plasma regeneration. The plasma may be one gas such as NH ₃ and H ₂ . The plasma may be maintained as is (in the reaction cell) or in an external cell that communicates with the reaction cell. In another embodiment, K, Cs, and Na replace Na with Li where the catalyst is atom K, atom Cs, and molecule NaH.

  To maintain the catalyst pressure at the desired level, the cell with permeation as a hydrogen source may be sealed. Alternatively, the cell may further include a heat-resistant valve at each inlet or outlet so that the valve in contact with the reaction gas mixture is maintained at the desired temperature.

  By isolating the cell and applying auxiliary heater power with the heater 380, the plasma cell temperature can be independently controlled over a wide range. In this way, the catalyst vapor pressure can be controlled independently of the plasma power.

  The discharge voltage may be in the range of about 100 to 10,000 volts. The current may be in any desired range at the desired voltage. Furthermore, the plasma may be pulsed with any desired frequency range, offset voltage, peak voltage, peak power, and waveform.

  In another embodiment, the plasma may be generated in a liquid medium, such as the solvent of the catalyst or the species of reactant that is the source of the catalyst.

IX. Fuel Cell and Battery In the embodiment of the fuel cell and battery 400 shown in FIG. 6, the hydrino reactant comprising the solid fuel or the heterogeneous catalyst comprises a reactant for the corresponding half-cell reaction. During operation, the catalyst reacts with atomic hydrogen and energy transfer results in ionization of the catalyst. The reaction may occur in the anode compartment 402 because the anode 410 ultimately accepts ionized electron current. At least one of Li, K, and NaH may function as a catalyst to form hydrinos. The reaction step of energy transfer from atomic hydrogen to the catalyst in a nonradiative state of integer multiples of 27.2 eV results in an ionized catalyst and free electrons. A support such as AC may function as a conductive electron acceptor in electrical contact with the anode. The final electron-acceptor reactant is a source of positively charged counter ions, free radicals that are components of the cathode cell reaction mixture that ultimately handles the electrons released from the catalytic reaction to form hydrinos. Or a source thereof. The oxidant or cathode-cell reaction mixture is present in the cathode compartment 401 with the cathode 405. Preferably, the oxidizing agent is at least one of oxygen or a source of oxygen, preferably a halogen or halogen source that is F ₂ or Cl ₂ , CF ₄ , SF ₆ , and NF ₃ . During operation, counter ions such as catalyst ions may move to the anode compartment, preferably through the salt bridge 420 to the cathode compartment. Each cell reaction may be supplied by additional reactants, and the product may be removed through passages 460 and 461 to a reservoir or product source for product storage 430 and 431. Absent.

  In certain embodiments, a power, chemical, battery and fuel cell system disclosed herein that regenerates reactants and maintains the reaction to form lower energy hydrogen is disclosed in hydrinos. Except that only the hydrogen consumed in forming the water needs to be replaced, it can be a closed system and the consumed hydrogen fuel can be obtained from the electrolysis of water.

X. Chemical Reactors The present disclosure also relates to other reactors for producing the increased binding energy hydrogen compounds of the present disclosure, such as dihydrino molecules and hydrino hydride compounds. Further products of catalysis depend on the cell type but are power and optionally plasma and light. Such a reactor is hereinafter referred to as a “hydrogen reactor” or “hydrogen cell”. The hydrogen reactor includes a cell for making hydrinos. The cells for making hydrinos may be in the form of chemical reactors or gaseous fuel cells such as gas discharge cells, plasma torch cells, or microwave power cells. Typical examples of cells for making hydrinos may be in the form of liquid fuel cells (cells), solid fuel cells (cells), and non-uniform fuel cells (cells). Each of these cells comprises (i) a source of atomic hydrogen; and (ii) at least one catalyst selected from a solid catalyst, a molten catalyst, a liquid catalyst, a gaseous catalyst, or a mixture thereof for making hydrinos And (iii) a vessel for reacting hydrogen and a catalyst for making hydrinos. The term “hydrogen”, as used herein and considered by this disclosure, includes not only protium ( ¹ H) but also deuterium ( ² H) and tritium ( ³ H) unless otherwise specified. Including. When deuterium is used as the reactant for the hydrino reaction, the relative traces of the helium or tritium products of the heterogeneous and solid fuels are expected.

In the embodiment of the chemical reactor to synthesize compounds consisting of lower-energy hydrogen, such as hydrino hydride compounds, an iron counterion, preferably iron carbide, iron oxide, or FeI ₂ or FeI _An iron hydrino hydride film is synthesized using an iron salt containing iron in a positive oxidation state that reacts with H ⁻ (1 / P) by substitution of a volatile iron salt such as ₃ . The catalyst can be K, NaH, or Li. H can be present from dissociating agents such as _{H 2} and R-Ni or Pt / _Al 2 _{O 3.} In another embodiment, the iron hydrino hydride comprises a dissociator such as R—Ni and a source of hydrogen such as H ₂ gas, and a catalyst such as NaH, Li, or K, the operating temperature of the reactor. Formed from a source of iron such as iron hydride that decomposes at Manganese hydrino hydride is a dissociator such as R—Ni and a source of hydrogen such as H ₂ gas, a catalyst such as NaH, Li, or K, Mn which decomposes at the operating temperature of the reactor ( II) It may be formed from a manganese source such as an organometallic such as 2,4-pentanedionate. In the examples, the reactor is maintained in a temperature range of about 25 ° C to 800 ° C, preferably in the range of about 400 ° C to 500 ° C.

Since the alkali metal is a covalent diatomic molecule in the gas phase, in embodiments, the catalyst that forms the increased binding energy hydrogen compound is formed from the source by reaction with at least one other element. A catalyst such as K or Li may be produced by dispersion of K or Li metal in an alkali halide such as KX or LiX to form KHX LiHX where X is a halogen. Catalyst K or Li may be produced by reaction of atomic H with evaporated K ₂ or Li ₂ to form LiH and Li or KH and K, respectively. The increased binding energy hydrogen compound may be MHX. Here, M is an alkali metal, H is a hydrino hydride, and X is a monovalent negatively charged ion, preferably one of halogen and HCO ₃ ⁻ . In an example, the reaction mixture to form KHCl or KHI where H is a hydrino hydride is a K metal (X = Cl, I) covered with K metal and a dissociator, preferably a nickel screen and R -Each containing nickel metal such as Ni. With the addition of hydrogen, the reaction is carried out by maintaining the reaction mixture at an elevated temperature, preferably in the range of 400-700 ° C. Preferably, the hydrogen pressure is maintained at a gauge pressure of about 5 PSI. Thus, MX is placed on K, K atoms move through the halogen lattice, the halogen functions to disperse K, acts as a dissociator for K ₂ and forms KHX. Therefore, it reacts with the interface with H from a dissociator such as R-Ni or nickel screen.

Suitable reaction mixtures for the synthesis of hydrino hydride compounds include at least two series from the group consisting of a catalyst, a source of hydrogen, an oxidizing agent, a reducing agent, and a support, wherein the oxidizing agent is _{S 2 Cl 2, SCl 2,} S 2 Br 2, S 2 F 2, CS 2, Sb 2 S 5, S x X y, SOCl 2, SOF 2, sO 2 F 2, SOBr 2, P such as, _{P 2 O 5, P 2 S} 5, sO x X y , such _{as, PF 3, PCl 3, PBr} 3, PI 3, PF 5, PCl 5, PBr 4 F, or, _PCl 4 F, P, such as _{x X y, POBr 3, POI} 3, POCl 3, _{or, POF 3, PO x X y} , pSBr 3 such _{as, PSF 3, PSCl 3, PS} x X y, P 3 N 5 , such as, (Cl _{2 PN) 3,} or ( _{l2PN) 4, (Br 2 PN} ) x, phosphorus, such as _-. nitrogen compound (M is an alkali metal .x and y are integers .X _{halogen), O 2, N 2 O} , and _TeO 2. _{Then, SF 6, S, SO 2} , SO 3, S 2 O 5 Cl 2, F 5 SOF, M 2 S 2 O 8, sulfur, such as, phosphorus, and at least one source of oxygen. The oxidizing agent is a source of halogen, preferably fluorine, and may include, for example, CF ₄ , NF ₃ , or CrF ₂ . The mixture may also include getters as sources of phosphorus or sulfur such as MgS and MHS (Mi is an alkali metal). Suitable getters are compounds or atoms that produce a hydrino hydride peak, which is the high magnetic field of the normal H peak, and an NMR peak shifted to a high magnetic field with normal H. Suitable getters include the elements S, P, O, Se, and Te, or include compounds that include S, P, O, Se, and Te. General properties of suitable getters for hydrino hydride ions are in basic form, in doped basic form, or other elements that trap and stabilize hydrino hydride ions. Together, it forms a chain, fold or ring. Preferably, H ⁻ (1 / p) can be observed by solid or solution NMR. In another example, NaH or HCl functions as a catalyst. Suitable reaction mixtures include MX and M′HSO 4. Here, Na and K are preferable, but M and M ′ are alkali metals, preferably Cl, but X is a halogen element.

(1) NaH catalyst, MgH ₂ , SF ₆ , and activated carbon (AC), (2) NaH catalyst, MgH ₂ , S, and activated carbon (AC), (3) NaH catalyst, MgH ₂ , K ₂ S ₂ O ₈ , Ag and AC, (4) KH catalyst, MgH ₂ , K ₂ S ₂ O ₈ , and AC, (5) MH catalyst (M = Li, Na, K), Al, or MgH ₂ , O ₂ , K ₂ S ₂ O ₈ and AC, (6) KH catalyst, Al, CF ₄ and AC, (7) NaH catalyst t, Al, NF ₃ and AC, (8) KH catalyst, MgH ₂ , N ₂ O, and AC, (9) NaH catalyst, MgH ₂ , O ₂ , and activated carbon (AC), (10) NaH catalyst, MgH ₂ , CF ₄ , and AC, (11) MH _{catalyst, MgH 2, (M = Li} , Na, _{or, K) P 2 O 5 (} P 4 O 10 ) And AC, (12) MH catalyst, MgH ₂ , MNO ₃ , (M = Li, Na, or K) and AC, (13) NaH or KH catalyst, Mg, Ca, or Sr, preferably the _{FeCl 2, FeBr 2, NiBr 2} , a transition metal halide MnI _2, a, or, EuBr2, rare earth halides, such as and,, AC, and, (14) NaH catalyst, Al, CS ₂ and, A reaction mixture containing at least one of AC is a suitable system for producing powders and for producing lower energy hydrogen compounds. In another example of the exemplary reaction mixture given above, the catalytic cation comprises one of Li, Na, K, Rb, or Cs, and the other species of the reaction mixture is selected from reaction 1-14. Chosen from them. The reactants can be in any desired ratio.

  The hydrino reaction product is at least one of normal molecular hydrogen or hydride ions and hydrogen molecules having proton NMR peaks shifted to the high magnetic field side of hydrogen hydride, respectively. In an embodiment, the hydrogen product is associated with elements other than hydrogen. Here, the proton NMR peak shifts from that of a compound, species or normal molecule having the same molecular formula as its product to a higher magnetic field, or the compound, species or normal molecule is stable at room temperature. is not.

In an embodiment, the power and increased binding energy hydrogen compounds are LiNO ₃ , NaNO ₃ , KNO ₃ , LiH, NaH, KH, Li, Na, K, H ₂ , a support such as carbon, for example activated carbon, preferably it is MgH _2, produced by a reaction mixture comprising two or more metals or metal hydride reducing agent. The reactants can be in any molar ratio. Preferably, the reaction mixture comprises 9.3 mole% MH, 8.6 mole% MgH ₂ , 74 mole% AC, 7.86 mole% MNO ₃ (M is Li, Na, or K). Here, the various mol% can be changed within the range of a factor of 10 (10 times) with plus or minus of those given for various types. The product molecule hydrino and hydrino hydride ions with the preferred quarter state can be observed using liquid NMR at about 1.22 ppm and -3.85 ppm, respectively. This is done by extracting the product mixture with an NMR solvent (preferably deuterated DFM). The product M ₂ CO ₃ may function as a getter for hydrino hydride ions to form compounds such as MHMHCO ₃ .

In another embodiment, the power and increased binding energy hydrogen compounds are LiH, NaH, KH, Li, Na, K, H ₂ , a metal or metal hydride reducing agent, preferably MgH ₂ or Al powder, preferably Produced by a reaction mixture comprising nanopowder, a support such as carbon, preferably a source of fluorine such as activated carbon, fluorine gas or fluorocarbon, preferably two or more of the species consisting of CF4 or hexafluorobenzene (HFB) Is done. The reactants can be in any molar ratio. Preferably, the reaction mixture is 9.8 mole% MH, 9.1 mole% MgH ₂ or 9 mole% Al nanopowder, 79 mole% AC, 2.4 mole% CF ₄ or HFB (M is Li, Na, Or K). Here, the various mol% can be changed within the range of a factor of 10 (10 times) with plus or minus of those given for various types. The product molecule hydrino and hydrino hydride ions having the preferred quarter state can be observed using liquid NMR at about 1.22 ppm and -3.86 ppm, respectively. This is done by extracting the product mixture with an NMR solvent (preferably deuterated DFM or CDCl ₃ ).

In another embodiment, the power and increased binding energy hydrogen compounds are LiH, NaH, KH, Li, Na, K, H ₂ , preferably MgH ₂ or Al powder or metal or metal hydride reducing agent, carbon support, such as, preferably activated carbon, and are preferably produced by a reaction mixture containing 2 or more from seed of fluorine source is SF _6. The reactants can be in any molar ratio. Preferably, the reaction mixture consists of 10 mole% MH, 9.1 mole% MgH ₂ or 9 mole% Al powder, 78.8 mole% AC, 24 mole% SF ₆ (M is Li, Na or K). . Here, the various mol% can be changed within the range of a factor of 10 (10 times) with plus or minus of those given for various types. Suitable reaction mixture, NaH, MgH2, or include Mg, AC, and the SF ₆ in these molar ratios. The product molecule hydrino and hydrino hydride ions having the preferred quarter state can be observed using liquid NMR at about 1.22 ppm and -3.86 ppm, respectively. This is done by extracting the product mixture with an NMR solvent (preferably deuterated DFM or CDCl ₃ ).

In another embodiment, the binding energy hydrogen compound and increased power, LiH, NaH, KH, Li , Na, K, H 2, a metal or a metal hydride reducing agent is preferably MgH ₂ or Al powder, carbon A support such as activated carbon and preferably at least one source of sulfur, phosphorus and oxygen, preferably S or P powder, SF ₆ , CS ₂ , P ₂ O ₅ , and MNO ₃ (M is an alkali Formed by a reaction mixture of two or more of the species consisting of (metal). The reactants can be in any molar ratio. Preferably, the reaction mixture is from 8.1 mole% MH, 7.5 mole% MgH ₂ or Al powder, 65 mole% AC, and 19.5 mole% S (M is Li, Na or K). Become. Here, the various mol% can be changed within the range of a factor of 10 (10 times) with plus or minus of those given for various types. Suitable reaction mixtures contain NaH, MgH2, or Mg, AC, and S in these molar ratios. The product molecule hydrino and hydrino hydride ions having the preferred quarter state can be observed using liquid NMR at about 1.22 ppm and -3.86 ppm, respectively. This is done by extracting the product mixture with an NMR solvent (preferably deuterated DFM or CDCl ₃ ).

In another embodiment, power and increased binding energy hydrogen compounds are produced by a reaction mixture comprising NaHS. Hydrino hydride ions may be separated from NaHS. In an embodiment, to form H ₂ (1/4) to form H ⁻ (1/4), which may further react with a source of protons such as a solvent (preferably H ₂ O). First, a solid phase reaction takes place in NaHS.

  In an embodiment, the hydrino hydride compound may be purified. The purification method includes at least one of the steps of performing extraction and recrystallization using a suitable solvent. This method may further include other techniques for chromatography and separation of inorganic compounds known to those skilled in the art.

  In the liquid-fuel embodiment, the solvent has a halogen functionality, preferably fluorine. A suitable reaction mixture consists of at least one of hexafluorobenzene and octafluoronaphthalene added to a catalyst such as NaH and mixed with activated carbon, a fluorinated polymer, or a support such as R-Ni. The reaction mixture may consist of energetic materials that may be used in applications known to those skilled in the art. Suitable applications with high energy balance are propellants and piston-engine fuel. In an embodiment, the desired product is at least one of the collected fullerenes and nanotubes.

In an embodiment, the molecular hydrino H ₂ (1 / p), and preferably H ₂ (1/4), provides the corresponding hydride ions that may be used in applications such as hydride batteries and surface coatings. A product that is further reduced to form. Molecular hydrino bonds may be broken by collision methods. H ₂ (1 / p) may be dissociated via energy collisions with ions or electrons in plasma or beam state. The dissociated hydrino atoms may then react to form the desired hydride ion.

In a further embodiment, the molecular hydrino H ₂ (1 / p), preferably H ₂ (1/4), is a product used as a contrast agent for nuclear magnetic resonance imaging (MRI). This contrast agent is inhaled and images the lungs. Here, compared to normal H, its high field chemical shift allows it to be discernable and selective. In another embodiment, at least one of the lower energy hydrogen compound and the lower energy hydrogen species, eg, H ⁻ (1 / p) is an antilipidemic agent, an anticholesterol agent, a contraceptive agent, an anticoagulant Anti-inflammatory drugs, immunosuppressive drugs, antiarrhythmic drugs, antineoplastic drugs, antihypertensive drugs, epinephrine blockers, cardiac inotropic drugs, antidepressants, diuretics, antifungal drugs, antibacterial drugs, anti-anxiety drugs, sedatives , Muscle relaxants, anticonvulsants, drugs for the treatment of ulcer disease, drugs for the treatment of asthma and hypersensitivity reactions, antithromboembolic drugs, drugs for the treatment of muscular dystrophy, drugs that cause therapeutic miscarriage Drugs for the treatment of anemia, drugs for improving allograft survival, drugs for the treatment of purine metabolism disorders, drugs for the treatment of ischemic heart disease, drugs for the treatment of anesthetic withdrawal, Secondary transmitter inosit Agents that activate the effect of Le triphosphate ester, agents that interfere with spinal reflexes, and antiviral drugs, including drugs for the treatment of AIDS, is a medicament comprising at least one from the group consisting of. In naturally occurring formulations, at least one of the low-energy hydrogen compound and the low-energy hydrogen species is made to have a desired concentration, such as a naturally occurring higher concentration.

XI. Experiment
A. The energy and power balance of the catalytic reaction mixture listed on the right hand side of each water-flow, batch calorimeter input infra is approximately 130.3 cm ³ in volume (inner diameter (ID) is 1.5 inches, length). Is 4.5 inches, wall thickness is 0.2 inches) or 1988 cm ³ volume (inner diameter (ID) 3.75 inches, length 11 inches, wall thickness 0.75 inches) A water flow calorimeter comprising a stainless steel reactor, an external water cooling medium coil that recovered over 99% of the energy released into the cell so that the error is less than ± 1%, and a vacuum chamber containing each cell It was obtained by using. Energy recovery was determined by integrating the total output power _PT over time. The power was given by:

here,

Is the mass flow rate, Cp is the specific heat of water, and ΔT is the absolute value of the temperature difference between the inlet and outlet. The reaction was initiated by applying the correct power to the external heater. In particular, 100-200 W power (130.3 cm ³ cells) or 800-1000 W power (1988 cm ³ cells) was supplied to the heater. During this heating period, the reagent reached the threshold temperature of the hydrino reaction, and the onset of the reaction was typically confirmed by a sudden rise in cell temperature. When the cell temperature reached about 400-500 ° C, the input power was set to zero. After 50 minutes, the program led the power to zero. The chamber was re-pressurized with 1000 Torr helium to increase the rate of heat transfer to the cooling medium. The maximum change in water temperature (outlet temperature minus inlet temperature) was about 1.2 ° C. The assembly was allowed to reach full equilibrium for 24 hours, as confirmed by observation of full equilibrium in the flow thermistor.

In each test, the energy input and energy output were calculated by integration of the corresponding power. At each time increment, the thermal energy in the coolant flow is: water density at 19 ° C. (0.998 kg / liter), water specific heat (4.181 kJ / kg ° C.), corrected temperature difference, and time. Was calculated using equation (221). Values were summed over all experiments to obtain total energy output. The total energy E _T from the cell must be equal to the sum of the energy input E _in and the net energy E _net . Therefore, the net energy was obtained by the following formula.
E _net = E _T -E _in (222)
From the energy balance condition, E _ex was determined for the maximum theoretical energy E _{mt as} follows.
E _ex = E _net -E _mt (223)

  The calibration test results showed better heat coupling than 98% of the resistance input to the output coolant. The control without excess heat was so accurate that the calorimeter had an error of less than 1%, with correction with calibration. Tmax is the maximum cell temperature, Ein is the input energy, and dE is the measured output energy that is excessive from the input energy. All energy is exothermic. A given positive value indicates the magnitude of energy.

[Metal halides, oxides, and sulfides]
20 g AC3-5 + 5 g Mg + 8.3 g KH + 11.2 g Mg3As2 298.6 kJ, output energy (dE) 21.8 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 315 ° C. Theoretically endothermic. Gain is infinite.

20 g AC3-5 + 5 g Mg + 8.3 g KH + 9.1 g Ca3P2. The input energy (Ein) is 282.1 kJ. The output energy (dE) is 18.1 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 320 ° C. Endothermic reaction. Gain is infinite.

Rowan verification: 7.47 gm KH + 4.5 gm Mg + 18.0 gm TiC + 14.04 gm EuBr2. The input energy (Ein) is 321.1 kJ. The output energy (dE) is 40.5 kJ. Maximum temperature (Tmax) to 340 ° C. Energy gain ~ 6.5X (1.37 kJ x 4.5 = 6.16 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 3.5 gm TiB2. The input energy (Ein) is 299 kJ. The output energy (dE) is 10 kJ. Maximum temperature (Tmax) to 320 ° C. No rapid temperature rise (TSC). Energy gain to X (X to 0 kJ, 1 inch cell: excess energy: 5.1 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 6.05 gm RbCl. Input energy (Ein) is 311 kJ. The output energy (dE) is 18 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 340 ° C. The energy gain is ~ X (X ~ 0 kJ; 1 inch cell: excess energy is ~ 6.0 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 2.3 gm Li2S. Input energy (Ein) is 323kJ. The output energy (dE) is 12 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 340 ° C. Energy gain is ˜X (X˜0 kJ; 1 inch cell: excess energy is ˜5.0 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 5.05 gm Mg3N2. Input energy (Ein) is 323kJ. The output energy (dE) is 11 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 330 ° C. Energy gain is ~ (X ~ 0 kJ; 1 inch cell: excess energy ~ ~ 5.2 kJ).

4 g AC3-5 + 1 g Mg + 1.66 g KH + 3.55 g PtBr2. The input energy (Ein) is 95.0 kJ. The output energy (dE) is 15.7 kJ. Rapid increase in temperature (TSC) is 108-327 ° C. Maximum temperature (Tmax): 346 ° C. Theoretically, 6.66 kJ. Gain is 2.36 times.

4 g AC3-5 + 1 g Mg + 1 g NaH + 3.55 g PtBr2. Input energy (Ein) is 94.0 kJ. The output energy (dE) is 14.3 kJ. Rapid increase in temperature (TSC) at 100-256 ° C. Maximum temperature (Tmax): 326 ° C. Theoretically, the gain is 6.03 kJ and the gain is 2.37 times.

4 g WC + 1 g MgH2 + 1 g NaH + 0.01 mol Cl2. Start of dissociation of Cl ₂ to Cl with a UV lamp. Input energy (Ein) is 162.9 kJ. The output energy (dE) is 16.0 kJ. Rapid increase in temperature (TSC) at 23-42 ° C. Maximum temperature (Tmax): 85 ° C. Theoretically, 7.10 kJ. Gain is 2.25 times.

-4gAC3-5 + 1gMg + 1.66gKH + 2.66gPdBr2, input energy (Ein) is 113.0kJ. The output energy (dE) is 11.7 kJ. There is a rapid temperature rise (TSC) at 133-276 ° C. Maximum temperature (Tmax): 370 ° C. Theoretically, it is 6.43kJ and the gain is 1.82.

-4gAC3-5 + 1gMg + 1gNaH + 2.66gPdBr2, input energy (Ein) is 116.0kJ. The output energy (dE) is 9.4 kJ. There is a rapid temperature rise (TSC) at 110-217 ° C. Maximum temperature (Tmax): 361 ° C. Theoretically, it is 5.81 kJ and the gain is 1.63 times.

-4gAC3-5 + 1gMg + 1.66gKH + 3.60gPdI2, input energy (Ein) is 142.0kJ. The output energy (dE) is 7.8 kJ. Rapid increase in temperature (TSC) at 177-342 ° C. Maximum temperature (Tmax): 403 ° C. In theory, the gain is 5.51 kJ and the gain is 1.41 times.

-0.41 g AlN + 1.66 g KH + 1 g Mg powder + 4 g AC3-5 in a 1 inch very rugged cell. The energy gain is 4.9kJ. However, there was no rapid rise in temperature. Maximum cell temperature is 407 ° C. In theory, endothermic reactivity.

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 3.7 gm CrB2. The input energy (Ein) is 317 kJ. The output energy (dE) is 19 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 340 ° C. The theoretical energy is 0.05 kJ of endothermic reactivity. Gain is infinite.

8.3 gm KH + 5.0 gm NEWMg + 20.0 gm CAII-300 + 9.36 gm AgCl. The input energy (Ein) is 99 kJ. The output energy (dE) is 43 kJ. A small rapid temperature rise (TSC) at ~ 250 ° C. Maximum temperature (Tmax) to 340 ° C. The energy gain is -2.3X (X = 18.88 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm NEWTiC (G06U055) +7.2 gm AgCl. Input energy (Ein) is 315 kJ. The output energy (dE) is 25 kJ. A small rapid temperature rise (TSC) at ~ 250 ° C. Maximum temperature (Tmax) to 340 ° C. The energy gain is ~ 1.72X (X = 14.52kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 11.3 gm Y2O3 (with a gain of ~ 4XTiC). Input energy (Ein) is 353 kJ. The output energy (dE) is 23 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 350 ° C. The energy gain is ˜4X (X˜1.18 kJ * 5 = 5.9 kJ).

4.15 gm KH + 2.5 gm Mg + 10.0 gm CAII-300 + 39.8 gm EuBr. Input energy (Ein) is 323kJ. The output energy (dE) is 27 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 350 ° C. The energy gain is 2.26X (X = 11.93 kJ).

4 g AC3-5 + 1 g Mg + 1 g NaH + 2.23 g Mg3As2, 133.0 kJ. The output energy (dE) is 5.8 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 371 ° C. Theoretically reactive. Gain is infinite.

4 g AC3-5 + 1 g Mg + 1.66 g KH + 2.23 g Mg3As2. Input energy (Ein) is 139.0 kJ. The output energy (dE) is 6.5 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 393 ° C. Theoretically reactive. Gain is infinite.

4 g AC3-5 + 1 g Mg + 1.66 g KH + 1.82 g Ca3P2. The input energy (Ein) is 133.0 kJ. The output energy (dE) is 5.8 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 407 ° C. Theoretically reactive. Gain is infinite.

4 g AC3-5 + 1 g Mg + 1 g NaH + 3.97 g WCl6. Input energy (Ein) is 99.0 kJ. The output energy (dE) is 21.84 kJ. Rapid increase in temperature (TSC) at 100-342 ° C. Maximum temperature (Tmax): 375 ° C. 16.7 in theory. Gain is 1.3 times.

Finished 2.60 g CsI, 1.66 g KH, 1 g Mg powder, and 4 g AC3-4 in a 1 inch very rugged cell. The energy gain was 4.9 kJ. However, no rapid increase in cell temperature was observed. Maximum cell temperature is 406 ° C. 0 in theory. Gain is infinite.

0.42 g LiCl, 1.66 g KH, 1 g Mg powder, and 4 g AC3-4 were finished. The energy gain is 5.4kJ. However, no rapid increase in cell temperature was observed. Maximum cell temperature is 412 ° C. 0 in theory. Gain is infinite.

-4gAC3-4 + 1gMg + 1gNaH + 1.21gRbCl, input energy (Ein) is 136.0kJ. The output energy (dE) is 5.2 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 372 ° C. 0 in theory. Gain is infinite.

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 10.0 gm CaBr2. Input energy (Ein) is 323kJ. The output energy (dE) is 27 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 340 ° C. The energy gain is ˜3.0X (X˜1.71 kJ * 5 = 8.55 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 7.3 gm YF3. The input energy (Ein) is 320 kJ. The output energy (dE) is 17 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 340 ° C. The energy gain is ˜4.5X (X˜0.74 kJ * 5 = 3.7 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 14.0 gm dry SnBr2. The input energy (Ein) is 299 kJ. The output energy (dE) is 36 kJ. There is a small rapid temperature rise (TSC) at ~ 130 ° C. Maximum temperature (Tmax) to 350 ° C. The energy gain is ˜1.23X (X˜5.85 kJ × 5 = 29.25 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 15.6 gm EuBr2. The input energy (Ein) is 291 kJ. The output energy (dE) is 45 kJ. A small temperature spike (TSC) at ~ 50 ° C. Maximum temperature (Tmax) to 320 ° C. The energy gain is ˜32X (X˜0.28 kJ × 5 = 1.4 kJ), and the gain is ˜6.5 X (1.37 kJ × 5 = 6.85 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 11.25 gm dry ZnBr2. Input energy (Ein) is 288 kJ. The output energy (dE) is 45 kJ. A small rapid temperature rise (TSC) at ~ 200 ° C. Maximum temperature (Tmax) to 350 ° C. The energy gain is ˜2.1X (X˜4.19 kJ × 5 = 20.9 kJ).

5.0 gm NaH + 5.0 gm Mg + 20.0 gm CAII-300 + SF6. Input energy (Ein) is 77.7 kJ. The output energy (dE) is 105 kJ. Maximum temperature (Tmax) to 400 ° C. The energy gain is ˜1.43X (where X is 0.03 mole SF6 to 73 kJ).

5.0 gm NaH + 5.0 gm Mg + 20.0 gm CAII-300 + SF6. Input energy (Ein) is 217 kJ. The output energy (dE) is 84 kJ. Maximum temperature (Tmax) to 400 ° C. The energy gain is ˜1.15X (where X is 0.03 mole SF6 to 73 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 7.2 gm AgCl. Input energy (Ein) is 357 kJ. The output energy (dE) is 25 kJ. A small rapid temperature rise (TSC) at ~ 250 ° C. Maximum temperature (Tmax) to 340 ° C. The energy gain is ~ 1.72X (X ~ 14.52kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 7.2 gm AgCl. Input energy (Ein) is 487 kJ. The output energy (dE) is 34 kJ. A small rapid temperature rise (TSC) at ~ 250 ° C. Maximum temperature (Tmax) to 340 ° C. The energy gain is ~ 2.34X (X ~ 14.52kJ).

20 g AC3-4 + 8.3 g Ca + 5 g NaH + 15.5 g MnI2. The input energy (Ein) is 181.5 kJ. The output energy (dE) is 61.3 kJ. Rapid increase in temperature (TSC) at 159-233 ° C. Maximum temperature (Tmax): 283 ° C. Theoretically 29.5 kJ. Gain is 2.08 times.

・ 4gAC3-4 + 1.66gCa + 1.66gKH + 3.09gMnI2, input energy (Ein) is 113.0kJ. The output energy (dE) is 15.8 kJ. Rapid increase in temperature (TSC) at 228-384 ° C. Maximum temperature (Tmax): 395 ° C. Theoretically, 6.68kJ. Gain is 2.37 times.

4 g AC3-4 + 1 g Mg + 1.66 g KH + 0.46 g Li2S. Input energy (Ein) is 144.0 kJ. The output energy (dE) is 5.0 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 419 ° C. Theoretically reactive.

• 1.01 g Mg3N2, 1.66 g KH, 1 g Mg powder, and 4 g AC3-4 in a 1 inch very rugged cell. The energy gain is 5.2 kJ. However, there was no rapid rise in temperature. Maximum cell temperature is 401 ° C. 0 in theory.

1.21 g RbCl, 1.66 g KH, 1 g Mg powder, and 4 g AC3-4. The energy gain is 6.0 kJ. However, there was no rapid rise in temperature. Maximum cell temperature is 442 ° C. 0 in theory.

2.24 g Zn3N2, 1.66 g KH, 1 g Mg powder, and 4 g AC3-4 were finished. The energy gain is 5.5 kJ. However, there was no rapid rise in temperature. Maximum cell temperature is 410 ° C. Theoretically 4.41 kJ. Gain is 1.25 times.

4 g AC3-4 + 1 g Mg + 1 g NaH + 1.77 g PdCl2. Input energy (Ein) is 89.0 kJ. The output energy (dE) is 10.5 kJ. Rapid increase in temperature (TSC) is 83-204 ° C. Maximum temperature (Tmax): 306 ° C. Theoretically 6.14 kJ. Gain is 1.7 times.

0.74 g CrB2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3-4) in a 1 inch extremely rugged cell. The energy gain is 4.3 kJ. However, there was no rapid rise in temperature. Maximum cell temperature is 404 ° C. 0 in theory.

• 0.70 g TiB2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3-4) were finished. The energy gain is 5.1 kJ. However, there was no rapid rise in temperature. Maximum cell temperature is 431 ° C. 0 in theory.

5.0 gm NaH + 5.0 gm Mg + 20.0 gm CAII-300 + 14.85 gm BaBr2 (dry). Input energy (Ein) is 328 kJ. The output energy (dE) is 16 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 320 ° C. The energy gain is 160X (X to 0.02 kJ * 5 = 0.1 kJ).

1.0 gm NaH + 1.0 gm Mg + 4.0 gm CAII-300 + 2.97 gm BaBr2 (dry). The input energy (Ein) is 140 kJ. The output energy (dE) is 3 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 360 ° C. Energy gain is ~ 150X (X ~ 0.02kJ).

5.0 gm NaH + 5.0 gm Mg + 20.0 gm CAII-300 + 13.9 gm MgI2. Input energy (Ein) is 315 kJ. The output energy (dE) is 16 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 340 ° C. The energy gain is ˜1.8X (X˜1.75 × 5 = 8.75 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 9.2 gm MgBr2. Input energy (Ein) is 334kJ. The output energy (dE) is 24 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 340 ° C. The energy gain is -2.1X (X-2.23x5 = 11.5 kJ).

20 g AC3-3 + 8.3 g KH + 7.2 g AgCl. Input energy (Ein) is 286.6 kJ. The output energy (dE) is 29.5 kJ. Rapid increase in temperature (TSC) at 327-391 ° C. Maximum temperature (Tmax): 394 ° C. Theoretically, 13.57 kJ. Gain is 2.17 times.

4 g AC3-3 + 1 g MgH2 + 1.66 g KH + 1.44 g AgCl. Input energy (Ein) is 151.0 kJ. The output energy (dE) is 4.8 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 397 ° C. Theoretically 2.53 kJ. Gain is 1.89 times.

4 g AC3-3 + 1 g Mg + 1 g NaH + 1.48 g Ca3N2. Input energy (Ein) is 140.0 kJ. The output energy (dE) is 4.9 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 392 ° C. Theoretically 2.01 kJ. Gain is 2.21 times.

4 g AC3-3 + 1 g Mg + 1 g NaH + 1.86 g InCl2. Input energy (Ein) is 125.0 kJ. The output energy (dE) is 7.9 kJ. There is a rapid temperature rise (TSC) at 163-259 ° C. Maximum temperature (Tmax): 374 ° C. Theoretically 4.22 kJ. Gain is 1.87 times.

4 g AC3-3 + 1 g Mg + 1.66 g KH + 1.86 g InCl2. The input energy (Ein) is 105.0 kJ. The output energy (dE) is 7.5 kJ. Rapid increase in temperature (TSC) at 186-302 ° C. Maximum temperature (Tmax): 370 ° C. Theoretically 4.7 kJ. Gain is 1.59 times.

4 g AC3-3 + 1 g Mg + 1.66 g KH + 2.5 g DyI2. The input energy (Ein) is 135.0 kJ. The output energy (dE) is 6.1 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 403 ° C. Theoretically, 1.89 kJ. The gain is 3.22.

• 3.92 g EuBr3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3-3) in a 1 inch extremely rugged cell. The energy gain is 10.5kJ. However, there was no rapid increase in cell temperature. Maximum cell temperature is 429 ° C. Theoretically 3.4 kJ. Gain is 3 times.

-4.56 g AsI3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon end powder (AC3-3). The energy gain is 13.5kJ. However, the rapid rise in cell temperature is 166 ° C (237-403 ° C). Maximum cell temperature is 425 ° C. Theoretically, 8.65 kJ. The gain is 1.56 times.

4 g AC3-3 + 1 g Mg + 1 g NaH + 2.09 g EuF3. Input energy (Ein) is 185.1 kJ. The output energy (dE) is 8.0 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 463 ° C. Theoretically 1.69kJ. Gain is 4.73 times.

4 g AC3-3 + 1 g Mg + 1.66 g KH + 1.27 g AgF. Input energy (Ein) is 127.0 kJ. The output energy (dE) is 6.04 kJ. Rapid increase in temperature (TSC) at 84-190 ° C. Maximum temperature (Tmax): 369 ° C. Theoretically 3.58kJ. Gain is 1.69 times.

4 g AC3-3 + 1 g Mg + 1 g NaH + 3.92 g EuBr3. The input energy (Ein) is 162.5 kJ. The output energy (dE) is 7.54 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 471 ° C. Theoretically 3.41 kJ. Gain is 2.21 times.

• 2.09 g EuF3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3-3) in a 1 inch extremely rugged cell. The energy gain is 5.5 kJ. However, there was no rapid increase in cell temperature. Maximum cell temperature is 417 ° C. Theoretically 1.71 kJ. Gain is 3.25 times.

3.29 g YBr3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3-3). The energy gain is 7.0 kJ. However, there was no rapid increase in cell temperature. Maximum cell temperature is 44 ° C. Theoretically 4.16 kJ. Gain is 1.68 times.

5.0 gm NaH + 5.0 gm Mg + 20.0 gm CAII-300 + 19.5 gm BaI2. Input energy (Ein) is 334kJ. The output energy (dE) is 13 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 350 ° C. The energy gain is ˜2.95X (X˜0.88 kJ × 5 = 4.4 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 10.4 gm BaCl2. The input energy (Ein) is 331 kJ. The output energy (dE) is 18 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 320 ° C. The energy gain is ~ 6.9X (X ~ 0.52x5 = 2.6kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 39.8 gm LaF. Input energy (Ein) is 338 kJ. Output energy (dE) is 7 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 320 ° C. The energy gain is 1.9X (X-3.65kJ).

5.0 gm NaH + 5.0 gm Mg + 20.0 gm CAII-300 + 14.85 gm BaBr2 (dry). The input energy (Ein) is 280 kJ. The output energy (dE) is 10 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 320 ° C. The energy gain is ˜100X (X˜0.01 = 0.02 × 5 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 14.85 gm BaBr2 (dry). Input energy (Ein) is 267 kJ. Output energy (dE) is 8 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 360 ° C. The energy gain is ~ 2.5X (X ~ 3.2kJ).

5.0 gm NaH + 5.0 gm Mg + 20.0 gm TiC + 4.85 gm ZnS. The input energy (Ein) is 319 kJ. The output energy (dE) is 12 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 340 ° C. Energy gain is ~ 1.5X (X ~ 8.0kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 7.2 gm AgCl (dried 070109). The input energy (Ein) is 219 kJ. The output energy (dE) is 26 kJ. A small rapid temperature rise (TSC) at ~ 250 ° C. Maximum temperature (Tmax) to 340 ° C. Energy gain is ~ 1.8X (X ~ 14.52kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 11.3 gm Y2O3. The input energy (Ein) is 339 kJ. The output energy (dE) is 24 kJ. There is a small rapid temperature rise (TSC) from at to 300 ° C. Maximum temperature (Tmax) to 350 ° C. The energy gain is -4.0X (X-5.9kJwithNaH).

4 g AC3-3 + 1 g Mg + 1 g NaH + 1.95 g YCl3. Input energy (Ein) is 137.0 kJ. The output energy (dE) is 7.1 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 384 ° C. Theoretically 3.3 kJ. Gain is 2.15 times.

• 4.70 g YI3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3-1) in a 1 inch extremely rugged cell. The energy gain is 6.9kJ. However, there was no rapid increase in cell temperature. Maximum cell temperature is 426 ° C. Theoretically, 3.37 kJ. Gain is 2.04 times.

1.51 g SnO2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3-1). Energy gain is 9.4kJ. However, there was no rapid increase in cell temperature. Maximum cell temperature is 460 ° C. Theoretically 7.06 kJ. The gain is 1.33 times.

• 4.56 g AsI3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3-1). The energy gain is 11.5kJ. There is a rapid rise in cell temperature at 144 ° C (221-365 ° C). Maximum cell temperature is 463 ° C. Theoretically, 8.65 kJ. The gain is 1.33 times.

3.09 g MnI2, 1.66 g KH, 1 g Mg powder, and 4 g STiC-1 (TiC from Sigma-Aldrich). The energy gain is 9.6 kJ. There is a rapid rise in cell temperature at 137 ° C (38-175 ° C). Maximum cell temperature is 396 ° C. Theoretically 3.73 kJ. Gain is 2.57 times.

3.99 g SeBr4, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3-1). The energy gain is 20.9kJ. There is a rapid rise in cell temperature at 224 ° C (47-271 ° C). Maximum cell temperature is 383 ° C. Theoretically, 16.93 kJ. The gain is 1.23 times.

20 g AC3-3 + 5 g Mg + 8.3 g KH + 11.65 g AgI. Input energy (Ein) is 238.6 kJ. The output energy (dE) is 31.7 kJ. Rapid temperature rise (TSC) is 230-316 ° C. Maximum temperature (Tmax): 317 ° C. Theoretically 12.3 kJ. Gain is 2.57 times.

4 g AC3-3 + 1 g Mg + 1.66 g KH + 0.91 g CoS. Input energy (Ein) is 145.1 kJ. The output energy (dE) is 8.7 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 420 ° C. Theoretically 2.63 kJ. The gain is 3.3 times.

4 g AC3-3 + 1 g Mg + 1.66 g KH + 1.84 g MgBr2. Input energy (Ein) is 134.1 kJ. The output energy (dE) is 5.75 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 400 ° C. Theoretically 2.23 kJ. The gain is 2.58 times.

5.02 g SbI3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3-1). The energy gain is 12.2 kJ. There is a rapid rise in cell temperature at 154 ° C (141-295 ° C). Maximum cell temperature is 379 ° C. Theoretically, 9.71 kJ. Gain is 1.26 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 7.2 gm AgCl. Input energy (Ein) is 304 kJ. The output energy (dE) is 30 kJ. There is a small rapid temperature rise (TSC) at ~ 275 ° C. Maximum temperature (Tmax) to 340 ° C. Energy gain is ~ 2.1X (X ~ 14.52kJ).

-KH1.66gm + Mg1.0gm + TiC5.0gm + BaBr22.97gmLaddedBaBr2-KH-Mg-TiC, input energy (Ein) is 130kJ. The output energy (dE) is 2 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 360 ° C. Theoretically 0.64 kJ. Gain is 3 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 4.8 gm CuS. Input energy (Ein) is 318 kJ. The output energy (dE) is 30 kJ. A small rapid temperature rise (TSC) at ~ 250 ° C. Maximum temperature (Tmax) to 360 ° C. The energy gain is ~ 2.1X (X ~ 14.4kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 4.35 gm MnS. Input energy (Ein) is 326kJ. The output energy (dE) is 14 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 350 ° C. The energy gain is ~ 2.2X (X ~ 6.3kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 10.7 gm GdF3. The input energy (Ein) is 339 kJ. Output energy (dE) is 7 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 360 ° C. The energy gain is ~ 2.54X (X ~ 2.75kJ).

20 g AC3-2 + 5 g Mg + 8.3 g KH + 7.2 g AgCl. Input energy (Ein) is 327.1 kJ. The output energy (dE) is 40.4 kJ. Rapid increase in temperature (TSC) at 288-318 ° C. Maximum temperature (Tmax): 326 ° C. Theoretically, 14.52 kJ. Gain is 2.78 times.

20 g AC3-2 + 5 g Mg + 8.3 g KH + 7.2 g CuBr. The input energy (Ein) is 205.1 kJ. The output energy (dE) is 22.5 kJ. Rapid increase in temperature (TSC) at 216-268 ° C. Maximum temperature (Tmax): 280 ° C. Theoretically, 13.46 kJ. Gain is 1.67 times.

4 g AC3-2 + 1 g Mg + 1 g NaH + 1.46 g YF3. Input energy (Ein) is 157.0 kJ. The output energy (dE) is 4.3 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 405 ° C. Theoretically 0.77. Gain is 5.65 times.

4 g AC3-2 + 1 g Mg + 1.66 g KH + 1.46 g YF3. Input energy (Ein) is 137.0 kJ. The output energy (dE) is 5.6 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 398 ° C. Theoretically 0.74. Gain is 7.54 times.

• 11.3 g Y 2 O 3, 5 g NaH, 5 g Mg powder, and 20 g CA-III300 activated carbon powder (AC3-2) in a 2 inch extremely rugged cell. The energy gain is 24.5kJ. However, there was no rapid increase in cell temperature. Maximum cell temperature is 386 ° C. 5.9 in theory. Gain is 4.2 times.

4 g AC3-2 + 1 g Mg + 1 g NaH + 3.91 g BaI2. The input energy (Ein) is 135.0 kJ. The output energy (dE) is 5.3 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 378 ° C. Theoretically 0.1 kJ. Gain is 51 times.

4 g AC3-2 + 1 g Mg + 1.66 g KH + 3.91 g BaI2. Input energy (Ein) is 123.1 kJ. The output energy (dE) is 3.3 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 390 ° C. Theoretically 0.88 kJ. Gain is 3.8 times.

4 g AC3-2 + 1 g Mg + 1.66 g KH + 2.08 g BaCl2. The input energy (Ein) is 141.0 kJ. The output energy (dE) is 5.5 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 403 ° C. Theoretically 0.52 kJ. Gain is 10.5 times.

4 g AC3-2 + 1 g Mg + 1.66 g KH + 3.42 g SrI2. Input energy (Ein) is 128.2kJ. The output energy (dE) is 4.35 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 383 ° C. Theoretically 1.62 kJ. The gain is 3.3 times.

4.04 g Sb2S5, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3-2) were finished. The energy gain is 18.0kJ. Rapid increase in temperature is observed at 251 ° C (224-475 ° C). The maximum temperature (Tmax) is 481 ° C. In theory, it is 12.7 kJ. Gain is 1.4 times.

4 g AC3-2 + 1 g Mg + 1 g NaH + 0.97 g ZnS. The input energy (Ein) is 132.1 kJ. The output energy (dE) is 7.5 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 370 ° C. Theoretically 1.4 kJ. Gain is 5.33 times.

4 g AC3-2 + 1 g Mg + 1 g NaH + 3.12 g EuBr2. The input energy (Ein) is 135.0 kJ. The output energy (dE) is 5.0 kJ. Rapid increase in temperature (TSC) at 114-182 ° C. Maximum temperature (Tmax): 371 ° C. Theoretically, the endothermic reactivity is +0.35 kJ. Gain is infinite.

4 g AC3-2 + 1 g Mg + 1.66 g KH + 3.12 g EuBr2. The input energy (Ein) is 122.0 kJ. The output energy (dE) is 9.4 kJ. Rapid increase in temperature (TSC) at 73-135 ° C. Maximum temperature (Tmax): 385 ° C. Theoretically 0.28 kJ. Gain is 34 times.

4 g CA3-2 + 1 g Mg + 1.66 g KH + 3.67 g PbBr2. Input energy (Ein) is 126.0 kJ. The output energy (dE) is 6.98 kJ. Rapid increase in temperature (TSC) is observed at 270-408 ° C. Maximum temperature (Tmax): 421 ° C. Theoretically 5.17 kJ. Gain is 1.35 times.

4 g CA3-2 + 1 g Mg + 1 g NaH + 1.27 g AgF. Input energy (Ein) is 125.0 kJ. The output energy (dE) is 7.21 kJ. Rapid increase in temperature (TSC) at 74-175 ° C. Maximum temperature (Tmax): 372 ° C. Theoretically 3.58kJ. Gain is doubled.

1.80 g GdBr3 (0.01 mol GdBr3 was 3.97 g, but not enough GdBr3), 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder AC3-1) . The energy gain is 2.8 kJ. However, no rapid increase in cell temperature was observed. Maximum cell temperature is 431 ° C. Theoretically 1.84kJ. The gain is 1.52.

0.97 g ZnS, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3-1). The energy gain is 4.0 kJ. However, no rapid increase in cell temperature was observed. Maximum cell temperature is 444 ° C. Theoretically 1.61 kJ. Gain is 2.49 times.

3.92 g BI3 (in PP vial), 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3-1). The energy gain is 13.2 kJ. Change in cell temperature gradient is 87 ° C (152-239 ° C). Maximum cell temperature is 465 ° C. In theory, it is 9.7 kJ. Gain is 1.36 times.

4 g AC3-2 + 1 g Mg + 1 g NaH + 3.2 g HfCl4. The input energy (Ein) is 131.0 kJ. The output energy (dE) is 10.5 kJ. There is a rapid temperature rise (TSC) at 277-439 ° C. Maximum temperature (Tmax): 440 ° C. Theoretically 8.1 kJ. Gain is 1.29 times.

4 g AC3-2 + 1 g Mg + 1.66 g KH + 3.2 g HfCl4. Input energy (Ein) is 125.0 kJ. The output energy (dE) is 11.5 kJ. Rapid increase in temperature (TSC) at 254 to 357 ° C. Maximum temperature (Tmax): 405 ° C. Theoretically 9.06 kJ. Gain is 1.27 times.

4 g CA3-2 + 1 g Mg + 1.66 g KH + 2.97 g BaBr2. The input energy (Ein) is 132.1 kJ. The output energy (dE) is 4.65 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 361 ° C. Theoretically 0.64 kJ. Gain is 7.24 times.

4 g CA3-2 + 1 g Mg + 1.66 g KH + 2.35 g AgI. Input energy (Ein) is 142.9 kJ. The output energy (dE) is 7.32 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 420 ° C. Theoretically 2.46 kJ. Gain is 2.98 times.

• 4.12 g PI3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3-1) were finished. The energy gain is 13.8kJ. The rapid rise in cell temperature is 189 ° C (184-373 ° C). Maximum cell temperature is 438 ° C. Theoretically, 11.1 kJ. Gain is 1.24 times.

1.57 g SnF2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3-1). The energy gain is 7.9 kJ. Change in cell temperature gradient is 72 ° C (149-221 ° C). Maximum cell temperature is 407 ° C. Theoretically, 5.28 kJ. Gain is 1.5 times.

1.96 g LaF3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3-1). The energy gain is 4.2 kJ. No sudden rise in cell temperature. Maximum cell temperature is 442 ° C. Theoretically 0.68 kJ. Gain is 6.16 times.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 2.78 g MgI2. Input energy (Ein) is 129.0 kJ. The output energy (dE) is 6.6 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 371 ° C. 1.75 kJ in theory. Gain is 3.8 times.

4 g CAIII-300 + 1 g Mg + 1.66 g KH + 2.48 g SrBr2. Input energy (Ein) is 137.0 kJ. The output energy (dE) is 6.1 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 402 ° C. Theoretically 1.35 kJ. Gain is 4.54 times.

4 g CA3-2 + 1 g Mg + 1.66 g KH + 2.0 g CaBr2. Input energy (Ein) is 147.0 kJ. The output energy (dE) is 6.33 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 445 ° C. Theoretically 1.71 kJ. The gain is 3.7 times.

4 g CA3-2 + 1 g Mg + 1 g NaH + 2.97 g BaBr2. The input energy (Ein) is 140.1 kJ. The output energy (dE) is 8.01 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 405 ° C. Theoretically 0.02kJ. The gain is 483 times.

0.90 g CrF2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3-1) were finished. The energy gain is 4.7 kJ. There was no sudden rise in cell temperature. Maximum cell temperature is 415 ° C. Theoretically 3.46kJ. Gain is 1.36 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 7.5 gm InCl. The input energy (Ein) is 275 kJ. The output energy (dE) is 26 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 340 ° C. The energy gain is ~ 2.2X (X ~ 11.45kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 12.1 gm InI. The input energy (Ein) is 320 kJ. The output energy (dE) is 12 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 340 ° C. The energy gain is ~ 1.25X (X ~ 9.6kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 9.75 gm InBr. Input energy (Ein) is 323kJ. The output energy (dE) is 17 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 340 ° C. The energy gain is -1.7X (X-10kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 15.45 gm MnI2. Demonstration experiment for Dr. Peter Jansson. Input energy (Ein) is 292kJ. The output energy (dE) is 45 kJ. There is a small rapid temperature rise (TSC) at ~ 30 ° C. Maximum temperature (Tmax) to 340 ° C. The energy gain is ~ 2.43X (X ~ 18.5kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 10.8 gm FeBr2 (FeBr2 manufactured by STREMC Chemicals). Demonstration experiment for Dr. Peter Jansson. Input energy (Ein) is 308 kJ. The output energy (dE) is 46 kJ. Rapid increase in temperature (TSC) at ~ 220 ° C. Maximum temperature (Tmax) to 330 ° C. The energy gain is ˜1.84X (X˜25 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 15.65 gm CoI2. Input energy (Ein) is 243 kJ. The output energy (dE) is 55 kJ. A small rapid temperature rise (TSC) at ~ 170 ° C. Maximum temperature (Tmax) to 330 ° C. Theoretically 26.35 kJ. Gain is 2.08 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 11.0 gm NiBr2. Input energy (Ein) is 270 kJ. The output energy (dE) is 45 kJ. Rapid increase in temperature (TSC) at ~ 220 ° C. Maximum temperature (Tmax) to 340 ° C. Theoretically 23 kJ. Gain is 1.95 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 10.8 gm FeBr2 (FeBr2 manufactured by STREMC Chemicals). The input energy (Ein) is 291 kJ. The output energy (dE) is 38 kJ. Rapid increase in temperature (TSC) at ~ 200 ° C. Maximum temperature (Tmax) to 330 ° C. Theoretically 25 kJ. The gain is 1.52.

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 11.25 gm ZnBr2. Input energy (Ein) is 302kJ. The output energy (dE) is 42 kJ. A small rapid temperature rise (TSC) at ~ 200 ° C. Maximum temperature (Tmax) to 375 ° C. The energy gain is ˜2X (X˜20.9 kJ).

8.30 gm KH + 5.0 gm Mg + 20.0 gm TiC + 19.85 gm GdBr3. Input energy (Ein) is 308 kJ. The output energy (dE) is 26 kJ. Rapid increase in temperature (TSC) at ~ 250 ° C. Maximum temperature (Tmax) to 340 ° C. The energy gain is ˜1.3X (X˜20.3 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 4.35 gm MnS. Input energy (Ein) is 349 kJ. The output energy (dE) is 24 kJ. Rapid increase in temperature (TSC) at ~ 260 ° C. Maximum temperature (Tmax) to 350 ° C. The energy gain is ~ 3.6X (X ~ 6.6kJ).

4 g CAIII-300 + 1 g Mg + 1 g NaH + 3.79 g LaBr3. Input energy (Ein) is 143.0 kJ. The output energy (dE) is 4.8 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 392 ° C. Theoretically 2.46 kJ. Gain is 1.96 times.

4 g CAIII-300 + 1 g Mg + 1.66 g KH + 3.80 g CeBr3. Input energy (Ein) is 145.0 kJ. The output energy (dE) is 7.6 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 413 ° C. Theoretically 3.84kJ. Gain is 1.97 times.

4 g CAIII-300 + 1 g Mg + 1.66 g KH + 1.44 g AgCl. Input energy (Ein) is 136.2 kJ. The output energy (dE) is 7.14 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 420 ° C. Theoretically 2.90kJ. Gain is 2.46 times.

4 g CAIII-300 + 1 g Mg + 1.66 g KH + 1.60 g Cu2S. Input energy (Ein) is 137.0 kJ. The output energy (dE) is 5.5 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 405 ° C. Theoretically 2.67 kJ. Gain is 2.06 times.

2.54 g TeI4 (0.01 mol TeI4 is 6.35 g but not enough TeI4), 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3 -1). The energy gain is 8.3 kJ. There is a rapid rise in cell temperature at 113 ° C (202-315 ° C). Maximum cell temperature is 395 ° C. Theoretically, 5.61 kJ. Gain is 1.48 times.

2.51 g BBr3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (AC3-1). The energy gain is 12.4 kJ. The cell temperature gradient change is 52 ° C (77-129 ° C). There is a sudden rise in cell temperature at 88 ° C (245-333 ° C). Maximum cell temperature is 438 ° C. Theoretically, 9.28 kJ. Gain is 1.34 times.

4 g CAIII-300 + 1 g Mg + 1.0 g NaH + 3.59 g TaCl5. The input energy (Ein) is 102.0 kJ. The output energy (dE) is 16.9 kJ. There is a rapid temperature rise (TSC) at 80-293 ° C. Maximum temperature (Tmax): 366 ° C. Theoretically, 11.89 kJ. Gain is 1.42 times.

• 2.72 g CdBr2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 6.6 kJ. There is a sudden rise in cell temperature at 56 ° C (253-309 ° C). Maximum cell temperature is 414 ° C. Theoretically 4.31 kJ. Gain is 1.53 times.

2.73 g MoCl5, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 20.1kJ. There is a rapid rise in cell temperature at 240 ° C (67-307 ° C). Maximum cell temperature is 511 ° C. Theoretically, 15.04 kJ. Gain is 1.34 times.

2.75 g InBr2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 7.3 kJ. There was no sudden rise in cell temperature. Maximum cell temperature is 481 ° C. Theoretically 4.46 kJ. Gain is 1.64 times.

1.88 g NbF5, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 15.5kJ. There was no sudden rise in cell temperature. Maximum cell temperature is 448 ° C. Theoretically, 11.36 kJ. Gain is 1.36 times.

2.33 g ZrCl4, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 12.9 kJ. The rapid rise in cell temperature is 156 ° C (311-467 ° C). Maximum cell temperature is 472 ° C. Theoretically, 8.82 kJ. Gain is 1.46 times.

3.66 g CdI2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 6.7 kJ. The cell temperature gradient change is 74 ° C (125-199 ° C). Maximum cell temperature is 417 ° C. Theoretically 4.12 kJ. Gain is 1.62 times.

4 g CAIII-300 + 1 g Mg + 1.66 g KH + 2.64 g GdCl3. Input energy (Ein) is 127.0 kJ. The output energy (dE) is 4.82 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 395 ° C. Theoretically 3.54 kJ. Gain is 1.36 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 7.5 gm InCl. Input energy (Ein) is 305 kJ. The output energy (dE) is 32 kJ. A small rapid temperature rise (TSC) at ~ 150 ° C. Maximum temperature (Tmax) to 350 ° C. The energy gain is ˜2.8X (X˜11.5 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm WC + 15.65 gm CoI2. Input energy (Ein) is 306 kJ. The output energy (dE) is 41 kJ. A small rapid temperature rise (TSC) is observed at ~ 200C. Maximum temperature (Tmax) to 350 ° C. The energy gain is ~ 1.55X (X ~ 26.4kJ).

5.0 gm NaH + 5.0 gm Mg + 20.0 gm WC + 19.85 gm GdBr3. The input energy (Ein) is 309 kJ. The output energy (dE) is 28 kJ. A small rapid temperature rise (TSC) at ~ 250 ° C. Maximum temperature (Tmax) to 340 ° C. The energy gain is ˜1.8X (X˜15.6 kJ).

4.98 gm KH + 3.0 gm Mg + 12.0 gm CAII-300 + 5.85 gm InBr3X system. The input energy (Ein) is 297 kJ. The output energy (dE) is 13 kJ. A small rapid temperature rise (TSC) at ~ 200 ° C. Maximum temperature (Tmax) to 330 ° C. The energy gain is -1.3X (X-10kJ).

4 g CAIII-300 + 1 g Mg + 1 g NaH + 2.26 g Y2O3. Input energy (Ein) is 133.1 kJ. The output energy (dE) is 5.2 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 384 ° C. Theoretically 1.18 kJ. Gain is 4.44 times.

4.11 g ZrBr4, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 11.2 kJ. The rapid increase in cell temperature is 154 ° C (280-434 ° C). Maximum cell temperature is 444 ° C. Theoretically, 9.31 kJ. Gain is 1.2 times.

5.99 g ZrI4, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 11.3 kJ. The rapid rise in cell temperature is 200 ° C (214-414 ° C). Maximum cell temperature is 454 ° C. 9.4kJ in theory. Gain is 1.2 times.

2.70 g NbCl5, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 16.4kJ. The rapid rise in cell temperature is 213 ° C (137-350 ° C). Maximum cell temperature is 395 ° C. Theoretically, 13.40 kJ. Gain is 1.22 times.

2.02 g MoCl 3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 12.1 kJ. There was no rapid increase in cell temperature. Maximum cell temperature is 536 ° C. Theoretically, 8.48kJ. Gain is 1.43 times.

3.13 g NiI2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 8.0 kJ. The rapid rise in cell temperature is 33 ° C (335-368 ° C). Maximum cell temperature is 438 ° C. Theoretically 5.89kJ. Gain is 1.36 times.

3.87 g As2Se3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 12.3 kJ. The rapid rise in cell temperature is 241 ° C (195-436 ° C). Maximum cell temperature is 446 ° C. 8.4kJ in theory. Gain is 1.46 times.

2.74 g Y2S3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 5.2 kJ. There was no rapid increase in cell temperature. Maximum cell temperature is 444 ° C. Theoretically 0.41 kJ. The gain is 12.64 times.

4 g CAIII-300 + 1 g Mg + 1.66 g KH + 3.79 g LaBr3. Input energy (Ein) is 147.1 kJ. The output energy (dE) is 7.1 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 443 ° C. Theoretically, 3.39 kJ. Gain is doubled.

4 g CAIII-300 + 1 g Mg + 1.66 g KH + 2.15 g MnBr2. Input energy (Ein) is 124.0 kJ. The output energy (dE) is 5.55 kJ. Rapid increase in temperature (TSC) at 360-405 ° C. Maximum temperature (Tmax): 411 ° C. Theoretically 3.63 kJ. Gain is 1.53 times.

2.60 g Bi (OH) 3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 14.8kJ. The rapid increase in cell temperature is 173 ° C (202-375 ° C). Maximum cell temperature is 452 ° C. Theoretically, 12.23 kJ. Gain is 1.2 times.

-8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 18.5 gm SnI2 (Strem). The input energy (Ein) is 244 kJ. The output energy (dE) is 53 kJ. Rapid increase in temperature (TSC) at ~ 150 ° C. Maximum temperature (Tmax) to 330 ° C. Theoretically 28.1 kJ. Gain is 1.9 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 10.8 gm FeBr2. Input energy (Ein) is 335 kJ. The output energy (dE) is 43 kJ. Rapid increase in temperature (TSC) at ~ 250 ° C. Maximum temperature (Tmax) to 375 ° C. Theoretically 22 kJ. Gain is 1.95 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm WC + 10.8 gm FeBr2. Input energy (Ein) is 335 kJ. The output energy (dE) is 32 kJ. Rapid increase in temperature (TSC) at ~ 230 ° C. Maximum temperature (Tmax) to 360 ° C. Theoretically 22 kJ. Gain is 1.45 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 15.45 gm MnI2 (made by Strem). The input energy (Ein) is 269 kJ. The output energy (dE) is 49 kJ. A small temperature spike (TSC) at ~ 50 ° C. Maximum temperature (Tmax) to 350 ° C. The energy gain is ~ 3.4X (X ~ 14.8kJ).

4 g CAIII-300 + 1.66 g Ca + 1 g NaH + 3.09 g MnI2. The input energy (Ein) is 112.0 kJ. The output energy (dE) is 9.98 kJ. Rapid increase in temperature (TSC) at 178-374 ° C. Maximum temperature (Tmax): 383 ° C. Theoretically 5.90kJ. Gain is 1.69 times.

0.96 g CuS, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 5.5 kJ. There was no rapid increase in cell temperature. Maximum cell temperature is 409 ° C. Theoretically 2.93 kJ. Gain is 1.88 times.

0.87 g MnS, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 4.7 kJ. There was no rapid increase in cell temperature. Maximum cell temperature is 412 ° C. Theoretically 1.32 kJ. Gain is 3.57 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm TiC + 15.45 gm MnI2. The input energy (Ein) is 269 kJ. The output energy (dE) is 49 kJ. A small temperature spike (TSC) at ~ 50 ° C. Maximum temperature (Tmax) to 350 ° C. Theoretically, 18.65 kJ. Gain is 2.6 times.

5.0 gm NaH + 5.0 gm Mg + 20.0 gm TiC + 11.0 gm NiBr2. Input energy (Ein) is 245 kJ. The output energy (dE) is 43 kJ. Rapid increase in temperature (TSC) at ~ 200 ° C. With maximum temperature (Tmax) to 310 ° C. Theoretically 26 kJ. Gain is 1.6 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 6.3 gm MnCl2. The input energy (Ein) is 333 kJ. The output energy (dE) is 34 kJ. Rapid increase in temperature (TSC) at ~ 250 ° C. Maximum temperature (Tmax) to 340 ° C. Theoretically 17.6 kJ. Gain is doubled.

2.42 g InI, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 4.4 kJ. There was no rapid increase in cell temperature. Maximum cell temperature is 438 ° C. 1.92kJ in theory. Gain is 2.3 times.

1.72 g InF3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 9.2kJ. There was no rapid increase in cell temperature. Maximum cell temperature is 446 ° C. Theoretically 5 kJ. Gain is 1.85 times.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 1.98 g As2O3. The input energy (Ein) is 110.5 kJ. The output energy (dE) is 17.1 kJ. Rapid increase in temperature (TSC): 325-452 ° C. Maximum temperature (Tmax): 471 ° C. Theoretically, 11.48 kJ. Gain is 1.49 times.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 4.66 g Bi2O3. Input energy (Ein) is 152.0 kJ. The output energy (dE) is 17.7 kJ. Rapid increase in temperature (TSC) at 185-403 ° C. Maximum temperature (Tmax): 481 ° C. Theoretically 13.8 kJ. Gain is 1.28 times.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 2.02 g MoCl3. Input energy (Ein) is 118.0 kJ. The output energy (dE) is 11.10 kJ. Rapid increase in temperature (TSC) at 342-496 ° C. Maximum temperature (Tmax): 496C. Theoretically, 7.76 kJ. Gain is 1.43 times.

2.83 g PbF4, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 13.9kJ. The rapid rise in cell temperature is 245C (217-462 ° C). Maximum cell temperature is 464 ° C. Theoretically, 13.38 kJ. Gain is 1.32 times.

2.78 g PbCl2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 C). The energy gain is 6.8 kJ. There was no rapid increase in cell temperature. Maximum cell temperature is 488 ° C. Theoretically 5.22 kJ. Gain is 1.3 times.

・ 4gCAIII-300 + 1.66gKH + 2.19gNiBr2, input energy (Ein) is 136.0kJ. The output energy (dE) is 7.5 kJ. Rapid increase in temperature (TSC) at 275-350C. Maximum temperature (Tmax): 385C. Theoretically 4.6 kJ. Gain is 1.6 times.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 2.74 g MoCl5. Input energy (Ein) is 96.0 kJ. The output energy (dE) is 19.0 kJ. Rapid rise in temperature (TSC) at 86-334C. Maximum temperature (Tmax): 373C. Theoretically, 14.06 kJ. Gain is 1.35 times.

4 g CAIII-300 + 1.66 g Ca + 1 g NaH + 2.19 g NiBr2. Input energy (Ein) is 127.1 kJ. The output energy (dE) is 10.69 kJ. Rapid temperature rise (TSC) is 300-420C. Maximum temperature (Tmax): 10.69C. Theoretically, 7.67 kJ. Gain is 1.39 times.

5.90 g BiI3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 C). The energy gain is 10.9kJ. The cell temperature gradient change is 70C (217-287C). Maximum cell temperature is 458 ° C. Theoretically, 8.87 kJ. The gain is 1.23 times.

1.79 g SbF3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 C). The energy gain is 11.7 kJ. The rapid increase in cell temperature is 169C (138-307C). Maximum cell temperature is 454 ° C. Theoretically, it is 9.21 kJ. Gain is 1.27 times.

4 g CAIII-300 + 1.66 g Ca + 1 g NaH + 3.09 g MnI2. The input energy (Ein) is 111.0 kJ. The output energy (dE) is 12.6 kJ. Rapid increase in temperature (TSC) is observed at 178-340C. Maximum temperature (Tmax): 373C. 5.9kJ in theory. Gain is 2.13 times.

4 g CAIII-300 + 1.66 g Ca + 1 g NaH + 1.34 g CuCl2. Input energy (Ein) is 135.2kJ. The output energy (dE) is 12.26 kJ. Rapid rise in temperature (TSC) is present at 250-390C. Maximum temperature (Tmax): 437C. Theoretically 8.55 kJ. Gain is 1.43 times.

1.50 g InCl, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 C). The energy gain is 5.1 kJ. There was no rapid increase in cell temperature. Maximum cell temperature is 410 ° C. Theoretically 2.29 kJ. The gain is 2.22.

2.21 g InCl3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 C). The energy gain is 10.9kJ. The rapid rise in cell temperature is 191C (235-426C). Maximum cell temperature is 431 ° C. Theoretically 7.11 kJ. Gain is 1.5 times.

1.95 g InBr, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 C). The energy gain is 6.0 kJ. There was no rapid increase in cell temperature. Maximum cell temperature is 435 ° C. 2kJ in theory. Gain is 3 times.

3.55 g InBr3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300C). The energy gain is 9.1 kJ. The rapid rise in cell temperature is at 152C (156-308C). Maximum cell temperature is 386 ° C. Theoretically 6.92kJ. Gain is 1.3 times.

4 g CAIII-300 + 1.66 g KH + 3.79 g SnI2. Input energy (Ein) is 169.1 kJ. The output energy (dE) is 6.0 kJ. Rapid temperature increase (TSC): 200-289C. Maximum temperature (Tmax): 431C. Theoretically, 4.03 kJ. Gain is 1.49 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm WC + 10.75 gm MnBr2. The input energy (Ein) is 309 kJ. The output energy (dE) is 35 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 335C. The energy gain is ˜1.9X (X˜18.1 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 10.75 gm MnBr2. The input energy (Ein) is 280 kJ. The output energy (dE) is 41 kJ. Rapid rise in temperature (TSC) is present at ~ 280C. Maximum temperature (Tmax) to 350C. The energy gain is ~ 2.2X (X ~ 18.1kJ).

• With 1.66 gm KH + 1.0 gm Mg + 4.0 gm TiC + 1.05 gm TiF35X cell # 1086CAII-300. Input energy (Ein) is 143 kJ. The output energy (dE) is 6 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 280C. Theoretically 2.5 kJ. Gain is 2.4 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 4.7 gm FeF2. The input energy (Ein) is 280 kJ. The output energy (dE) is 40 kJ. Rapid increase in temperature (TSC) at ~ 260C. Maximum temperature (Tmax) to 340C. Theoretically 20.65 kJ. Gain is 1.93 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 5.1 gm CuF2. The input energy (Ein) is 203 kJ. The output energy (dE) is 57 kJ. Rapid increase in temperature (TSC) is ~ 125C. Maximum temperature (Tmax) to 280C. It is 29kJ in theory. Gain is 1.96 times.

83.0 gm KH + 50.0 gm Mg + 200.0 gm WC + 185 gm SnI2URS. The input energy (Ein) is 1310 kJ. The output energy (dE) is 428 kJ. Rapid increase in temperature (TSC) at 140C. Maximum temperature (Tmax) to 350C. It is 200kJ in theory. The gain is 2.14 times.

061009KAWFC1 # 11021.0 gm NaH + 1.0 gm Mg + 4.0 gm WC + 3.97 gm GdBr3. Input energy (Ein) is 148kJ. Output energy (dE) is 7 kJ. There is a small rapid temperature rise (TSC) at ~ 300 ° C. Maximum temperature (Tmax) to 420 ° C. The energy gain is ~ 3.5X (X ~ 2kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 3.6 gm FeO. Input energy (Ein) is 355 kJ. The output energy (dE) is 24 kJ. A small rapid temperature rise (TSC) at ~ 260 ° C. Maximum temperature (Tmax) to 360 ° C. The energy gain is ˜1.45X (X˜16.6 kJ).

83.0 gm KH + 50.0 gm Mg + 200.0 gm WC + 185 gm SnI2ROWAN. The input energy (Ein) is 1379 kJ. The output energy (dE) is 416 kJ. Rapid increase in temperature (TSC) at ~ 140 ° C. Maximum temperature (Tmax) to 350 ° C. It is 200kJ in theory. Gain is doubled.

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 15.65 gm CoI2. Input energy (Ein) is 361 kJ. The output energy (dE) is 69 kJ. Rapid increase in temperature (TSC) at ~ 200 ° C. Maximum temperature (Tmax) to 410 ° C. Theoretically 26.35 kJ. Gain is 2.6 times.

8.3 gm KH + 5.0 gm + 20.0 gm CAII300 + 4.4 gm FeS. Input energy (Ein) is 312kJ. The output energy (dE) is 22 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 350 ° C. The energy gain is ~ 1.7X (X ~ 12.3kJ).

8.3 gm KH + 40.0 gm WC + 18.5 gm SnI2. Input energy (Ein) is 315 kJ. The output energy (dE) is 27 kJ. There is a small rapid temperature rise (TSC) at ~ 140 ° C. Maximum temperature (Tmax) to 340 ° C. The energy gain is ˜1.35X (X˜20 kJ).

5.0 gm NaH + 5.0 gm Mg + 20.0 gm WC + 15.45 gm MnI2. The input energy (Ein) is 108 kJ. The output energy (dE) is 30 kJ. Rapid increase in temperature (TSC) at ~ 70 ° C. Maximum temperature (Tmax) to 170 ° C. Theoretically 14.8 kJ. Gain is doubled.

5.0 gm NaH + 5.0 gm Mg + 20.0 gm WC + 11.0 gm NiBr2. Input energy (Ein) is 248 kJ. The output energy (dE) is 34 kJ. Rapid increase in temperature (TSC) is observed at ~ 170 ° C. Maximum temperature (Tmax) to 300 ° C. The energy gain is ~ 1.7X (X ~ 20kJ). Theoretically 26.25 kJ. Gain is 1.3 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm WC + 11.0 gm NiBr2. The input energy (Ein) is 291 kJ. The output energy (dE) is 30 kJ. A small rapid temperature rise (TSC) at ~ 250 ° C. Maximum temperature (Tmax) to 340 ° C. Energy gain is ~ 1.5X (X ~ 20kJ). Theoretically 26.25 kJ. Gain is 1.14 times.

Repeat 5.0 gm NaH + 5.0 gm Mg + 20.0 gm WC + 11.0 gm NiBr2 cell # 1105. Input energy (Ein) is 242 kJ. The output energy (dE) is 33 kJ. Rapid increase in temperature (TSC) at ~ 70 ° C. Maximum temperature (Tmax) to 280 ° C. The energy gain is ˜1.65X (X˜20 kJ).

5.0 gm NaH + 5.0 gm Mg + 20.0 gm CAII-300 + 11.1 gm InCl3. Input energy (Ein) is 189kJ. The output energy (dE) is 48 kJ. A small temperature spike (TSC) is present at ~ 80 ° C. Maximum temperature (Tmax) to 260 ° C. The energy gain is ~ 1.5X (X ~ 31kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 15.45 gm MnI2. Input energy (Ein) is 248 kJ. The output energy (dE) is 46 kJ. A small rapid temperature rise (TSC) at ~ 200 ° C. Maximum temperature (Tmax) to 325 ° C. The energy gain is ˜3X (X˜14.8 kJ).

2.96 g FeBr3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 12.5 kJ. The rapid increase in cell temperature is 77 ° C (72-149 ° C). Maximum cell temperature is 418 ° C. Theoretically, 8.35 kJ. Gain is 1.5 times.

0.72 g FeO, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 6.7 kJ. There was no rapid increase in cell temperature. Maximum cell temperature is 448 ° C. Theoretically 3.3 kJ. Gain is doubled.

1.26 g MnCl 2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 8.6 kJ. There was no rapid increase in cell temperature. Maximum cell temperature is 437 ° C. Theoretically 3.52 kJ. Gain is 2.45 times.

1.13 g FeF 3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 12.6 kJ. There was no rapid increase in cell temperature. Maximum cell temperature is 618 ° C. Theoretically, 6.44kJ. Gain is 1.96 times.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 3.97 g GdBr3. Input energy (Ein) is 143.1 kJ. The output energy (dE) is 5.4 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 403 ° C. Theoretically 1.99 kJ. Gain is 2.73 times.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 1.57 g SnF2. Input energy (Ein) is 139.0 kJ. The output energy (dE) is 7.24 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 413 ° C. Theoretically, 5.28 kJ. Gain is 1.37 times.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 4.04 g Sb2S5. Input energy (Ein) is 125.0 kJ. The output energy (dE) is 19.3 kJ. Rapid increase in temperature (TSC) at 421-651 ° C. Maximum temperature (Tmax): 651 ° C. Theoretically 12.37 kJ. The gain is 1.56 times.

1.36 g ZnCl2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 <0> C). The energy gain is 6.6 kJ. There was no rapid increase in cell temperature. Maximum cell temperature is 402 ° C. Theoretically 4.34 kJ. The gain is 1.52.

1.03 g ZnF2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 6.5 kJ. There was no rapid increase in cell temperature. Maximum cell temperature is 427 ° C. Theoretically 3.76 kJ. Gain is 1.73 times.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 2.22 g InCl3. The experimental output energy (dE) is −12.6 kJ. The following reaction is considered: InCl3 (c) + 3NaH (c) + 1.5Mg (c) = 3NaCl (c) + In (c) + 1.5MgH2 (c) Q = −640.45 kJ / reaction. The theoretical chemical reaction energy is -6.4 kJ. Excess heat is -6.2 kJ. 2.0X excess heat.

1.08 g VF3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 9.5kJ. There was no rapid increase in cell temperature. Maximum cell temperature is 447 ° C. Theoretically 4.9 kJ. Gain is 1.94 times.

8.3 g KH + 5.0 g Mg + 20.0 g AC (II-300) +5.4 g VF3. Input energy (Ein) is 286 kJ. The output energy (dE) is 58 kJ. Theoretically 24.5kJ. Gain is 2.3 times.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 1.72 g InF3. Input energy (Ein) is 134.0 kJ. The output energy (dE) is 8.1 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 391 ° C. Theoretically 5 kJ. Gain is 1.62 times.

4 g CAIII-300 + 1 g Mg + 1.66 g KH + 1.02 g CuF2. The experimental output energy (dE) is -9.4 kJ. The following reaction is considered: CuF2 (c) + Mg (c) = MgF2 (c) + Cu (c) Q = −581.5 kJ / reaction. The theoretical chemical reaction energy is -5.82 kJ. Excess heat is -3.59 kJ. 1.6X excess heat.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 2.83 g PbF4. The experimental output energy (dE) is -17.6 kJ. The following reaction is considered: PbF4 (c) + 2Mg (c) + 4NaH (c) = 2MgH2 (c) + 4NaF (c) + Pb (c) Q = −1290.0 kJ / reaction. The theoretical chemical reaction energy is −12.9 kJ. Excess heat is: -4.7 kJ. 1.4X excess heat.

1.66 gm KH + 1.0 gm Mg + 4.0 gm TiC + 6.26 gm SnI4. Input energy (Ein) is 97kJ. The output energy (dE) is 17 kJ. Rapid increase in temperature (TSC) at ~ 150 ° C. Maximum temperature (Tmax) to 370 ° C. Theoretically 10.1 kJ. Gain is 1.7 times.

4 g CAIII-300 + 1 g Mg + 1.66 g KH + 3.7 g TiBr4. The experimental output energy (dE) is −16.1 kJ. The following reaction is considered: TiBr4 (c) + 4KH (c) + 2Mg (c) + C (s) = 4 KBr (c) + TiC (c) + 2MgH2 (c) Q = −1062.3 kJ / reaction. The theoretical chemical reaction energy is -10.7 kJ. Excess heat is: -5.4 kJ. 1.5X excess heat.

BI3
4 g CAIII-300 + 1 g Mg + 1 g NaH + 2.4 g BI3. Input energy (Ein) is 128.1 kJ. The output energy (dE) is 7.9 kJ. There is a rapid temperature rise (TSC) at 180-263 ° C. Maximum temperature (Tmax): 365 ° C. Theoretically 5.55 kJ. Gain is 1.4 times.

MnBr2
4 g CAIII-300 + 1 g Mg + 1.66 g KH + 2.15 g MnBr2. The experimental output energy (dE) is -7.0 kJ. The following reaction is considered: MnBr2 (c) + 2KH (c) + Mg (c) = 2KBr (c) + Mn (c) + MgH2 (c) Q = -362.6 kJ / reaction. The theoretical chemical reaction energy is -3.63 kJ. Excess heat is -3.4 kJ. 1.9X excess heat.

8.3 gm KH + 5.0 gm Mg + 20.0 gm WC + 10.75 gm MnBr2. The input energy (Ein) is 309 kJ. The output energy (dE) is 35 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 335 ° C. The energy gain is ˜1.9X (X˜18.1 kJ).

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 10.75 gm MnBr2. The input energy (Ein) is 280 kJ. The output energy (dE) is 41 kJ. Rapid increase in temperature (TSC) at ~ 280 ° C. Maximum temperature (Tmax) to 350 ° C. The energy gain is ~ 2.2X (X ~ 18.1kJ).

FeF2
4 g CAIII-300 + 1 g Mg + 1.66 g KH + 0.94 g FeF2. The experimental output energy (dE) is -9.8 kJ. The following reaction is considered: FeF2 (c) + Mg (c) = MgF2 (c) + Fe (c) Q = −412.9 kJ / reaction. The theoretical chemical reaction energy is -4.13 kJ. Excess heat is -5.67 kJ. 2.4X excess heat.

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 4.7 gm FeF2. The input energy (Ein) is 280 kJ. The output energy (dE) is 40 kJ. Rapid increase in temperature (TSC) at ~ 260 ° C. Maximum temperature (Tmax) to 340 ° C. Theoretically 20.65 kJ. Gain is 1.94 times.

TiF3
1.66 gm KH + 1.0 gm Mg + 4.0 gm TiC + 1.05 gm TiF3 (with 5X cell # 1086CAII-300). Input energy (Ein) is 143 kJ. The output energy (dE) is 6 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 280 ° C. 2.5 in theory. Gain is 2.4 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 5.25 gm TiF3. The input energy (Ein) is 268 kJ. Output energy (dE) is 7 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 280 ° C. There is no energy gain (X to 21.7 kJ).

CuF2
8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 5.1 gm CuF2. The input energy (Ein) is 203 kJ. The output energy (dE) is 57 kJ. Rapid increase in temperature (TSC) at ~ 125 ° C. Maximum temperature (Tmax) to 280 ° C. Theoretically 29.1 kJ. Gain is doubled.

MnI2
-4.0 gm NaH + 4.0 gm Mg + 16.0 gm CAII-300 + 12.36 gm MnI2 (4X scale up). Input energy (Ein) is 253 kJ. The output energy (dE) is 30 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 300 ° C. Theoretically, it is 11.8kJ. Gain is 2.5 times.

• Calorimetric measurements on 3.09 g MnI2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 8.8 kJ. The rapid rise in cell temperature is 92 ° C (172-264 ° C). Maximum cell temperature is 410 ° C. Theoretically 2.96 kJ. Gain is 3 times.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 3.09 g MnI2. Input energy (Ein) is 126.1 kJ. The output energy (dE) is 8.0 kJ. Rapid increase in temperature (TSC) at 157-241 ° C. Maximum temperature (Tmax): 385 ° C. Theoretically 2.96 kJ. Gain is 2.69 times.

ZnBr2
2.25 g ZnBr2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 10.3 kJ. The rapid rise in cell temperature is 82 ° C (253-335 ° C). Maximum cell temperature is 456 ° C. Theoretically 3.56 kJ. Gain is 2.9 times.

5.0 gm NaH + 5.0 gm Mg + 20.0 gm CAII-300 + 11.25 gm ZnBr2. The input energy (Ein) is 291 kJ. The output energy (dE) is 26 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 330 ° C. In theory, it is 17.8 kJ. Gain is 1.46 times.

CoCl2
1.3 g CoCl2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 10.4 kJ. The cell temperature gradient change is 105 ° C (316-421 ° C). Maximum cell temperature is 450 ° C. Theoretically 5.2 kJ. Gain is doubled.

1.3 g CoCl2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 9.6 kJ. The rapid increase in cell temperature is 181 ° C (295-476 ° C). Maximum cell temperature is 478 ° C. Theoretically 5.2 kJ. Gain is 1.89 times.

SnBr2
2.8 g of SnBr2, 1.66 g of KH, 1 g of Mg powder, and 4 g of CA-III300 activated carbon powder (dried at 300 ° C.) were used. The energy amplification was 14.2 kJ. The rapid rise in temperature is 148 ° C (148-296 ° C). Maximum cell temperature is 376 ° C. Theoretically, 3.75kJ. Gain is 3.78 times.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 2.79 g SnBr2. Input energy (Ein) is 116.0 kJ. The output energy (dE) is 7.7 kJ. Rapid increase in temperature (TSC) at 135-236 ° C. Maximum temperature (Tmax): 370 ° C. Theoretically, 3.75kJ. Gain is doubled.

8.3 gm KH + 5.0 gm Mg powder + 20.0 gm CAII300 + 11.4 gm SnBr2. The input energy (Ein) is 211 kJ. The output energy (dE) is 41 kJ. Rapid increase in temperature (TSC) is observed at ~ 170 ° C. Maximum temperature (Tmax) to 300 ° C. Theoretically 15.5 kJ. Gain is 2.6 times.

8.3 gm KH 8.3 gm + 5.0 gm Mg5.0 gm + 20.0 gm TiC 20.0 gm + 14.0 gm SnBr2. Input energy (Ein) is 229 kJ. The output energy (dE) is 46 kJ. Rapid increase in temperature (TSC) at ~ 150 ° C. Maximum temperature (Tmax) to 310 ° C. Gain is ~ 2.4X (X ~ 19kJ). In theory, it is 18.8 kJ. Gain is 2.4 times.

1.66 gm KH + 1.0 gm Mg + 4.0 gm WC + 2.8 gm SnBr2. The input energy (Ein) is 101 kJ. The output energy (dE) is 10 kJ. Rapid increase in temperature (TSC) at ~ 150 ° C. Maximum temperature (Tmax) to 350 ° C. Theoretically, 3.75kJ. Gain is 2.66 times.

4 g CAIII-300 + 1.66 g KH + 2.79 g SnBr2. The input energy (Ein) is 132.0 kJ. The output energy (dE) is 9.6 kJ. Rapid increase in temperature (TSC) is present at 168-263. Maximum temperature (Tmax): 381 ° C. Theoretically 4.29 kJ. Gain is 2.25 times.

1 g Mg + 1.66 g KH + 2.79 g SnBr2. The input energy (Ein) is 123.0 kJ. The output energy (dE) is 7.82 kJ. There is a rapid temperature rise (TSC) at 125-220 ° C. Maximum temperature (Tmax): 386 ° C. Theoretically, 5.85 kJ. The gain is 1.33 times.

SnI2
-6.64 gm KH + 4.0 gm Mg powder + 18.0 gm TiC + 14.8 gm SnI2. Input energy (Ein) is 232 kJ. The output energy (dE) is 47 kJ. Rapid increase in temperature (TSC) at ~ 150 ° C. Maximum temperature (Tmax) to 280 ° C. The energy gain is ~ 3.6X (X ~ 12.8kJ). Theoretically 12.6 kJ. The gain is 3.7 times.

3.7 g SnI2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 11.9kJ. There was no rapid increase in cell temperature. Maximum cell temperature is 455 ° C. Theoretically 3.2 kJ. The gain is 3.7 times.

1.6 gm KH + 1.0 gm Mg powder + 4.0 gm TiC + 3.7 gm SnI2. Input energy (Ein) is 162 kJ. The output energy (dE) is 13 kJ. Rapid increase in temperature (TSC) at 100 ° C. Maximum temperature (Tmax) to 490 ° C. Theoretically 3.2 kJ. Gain is 4 times.

8.3 gm KH + 5.0 gm Mg powder + 20.0 gm CAII300 + 18.5 gm SnI2. The input energy (Ein) is 221 kJ. The output energy (dE) is 47 kJ. Rapid increase in temperature (TSC) is observed at ~ 170 ° C. Maximum temperature (Tmax) to 300 ° C. In theory, it is 15.9 kJ. Gain is 3 times.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 3.73 g SnI2. The input energy (Ein) is 121.9 kJ. The output energy (dE) is 7.56 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 391 ° C. Theoretically 3.2 kJ. Gain is 2.36 times.

-1.66g KH + 3.79g SnI2, input energy (Ein) is 114.0kJ. The output energy (dE) is 8.8 kJ. Rapid increase in temperature (TSC) at 161-259 ° C. Maximum temperature (Tmax): 359 ° C. 4kJ in theory. Gain is 2.17 times.

SnCl2
5.0 gm NaH + 5.0 gm Mg + 20.0 gm CAII-300 + 9.6 gm SnCl2. Input energy (Ein) is 181 kJ. The output energy (dE) is 30 kJ. Rapid increase in temperature (TSC) at ~ 140 ° C. Maximum temperature (Tmax) to 280 ° C. In theory, it is 19 kJ. Gain is 1.57 times.

NiBr2
4 g CAIII-300 + 1 g Mg + 1 g NaH + 2.19 g NiBr2. Input energy (Ein) is 126.0 kJ. The output energy (dE) is 12.01 kJ. Rapid increase in temperature (TSC) at 290-370 ° C. Maximum temperature (Tmax): 417 ° C. 4kJ in theory. Gain is 3 times.

-1.0 gm NaH + 1.0 gm MgH2 powder + 4.0 gm TiC) mixture + 2.2 gm NiBr2. The input energy (Ein) is 121 kJ. The output energy (dE) is 11 kJ. Temperature gradient jump is 260 ° C. Maximum temperature (Tmax) to 390 ° C. 4kJ in theory. Gain is 2.75 times.

4 g CAIII-300 + 1 g Al + 1 g NaH + 2.19 g NiBr2. The input energy (Ein) is 122.0 kJ. The output energy (dE) is 7.78 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 392 ° C. 4kJ in theory. Gain is 1.95 times.

4 g CAIII-300 + 1 g Mg + 0.33 g LiH + 2.19 g NiBr2. Input energy (Ein) is 128.0 kJ. The output energy (dE) is 10.72 kJ. Rapid increase in temperature (TSC) at 270-436 ° C. Maximum temperature (Tmax): 440 ° C. 4kJ in theory. Gain is 2.68 times.

4 g CAIII-300 + 1 g Mg + 1.66 g KH + 2.19 g NiBr2. Input energy (Ein) is 126.0 kJ. The output energy (dE) is 10.45 kJ. Rapid increase in temperature (TSC) at 285-423 ° C. Maximum temperature (Tmax): 423 ° C. 4kJ in theory. Gain is 2.6 times.

4g CAIII-300 + 1g MgH2 + 1g NaH + 2.19g NiBr2. Input energy (Ein) is 138.1 kJ. The output energy (dE) is 8.12 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 425 ° C. 4kJ in theory. Gain is doubled.

-5.0 gm NaH + 5.0 gm Mg powder + 20.0 gm of activated carbon CAII300) mixture + 11.0 gm NiBr2 (theoretical 23.6 kJ), input energy (Ein) is 224 kJ. The output energy (dE) is 53 kJ. Temperature gradient jump is 160 ° C. Maximum temperature (Tmax) to 280 ° C. Theoretically 20 kJ. Gain is 2.65 times.

1.0 gm NaH + 1.0 gm Mg + 4.0 gm WC + 2.2 gm NiBr2. The input energy (Ein) is 197 kJ. The output energy (dE) is 11 kJ. A small rapid temperature rise (TSC) at ~ 200 ° C. Maximum temperature (Tmax) to 500 ° C. 4kJ in theory. Gain is 2.75 times.

50.0 gm NaH + 50.0 gm Mg + 200.0 gm CAII-300 + 109.5 gm NiBr2. The input energy (Ein) is 1990 kJ. The output energy (dE) is 577 kJ. Rapid increase in temperature (TSC) at ~ 140 ° C. Maximum temperature (Tmax) to 980 ° C. 199kJ in theory. Gain is 2.9 times.

Control without Mg: 4 g CAIII-300 + 1 g NaH + 2.19 g NiBr2. Input energy (Ein) is 134.0 kJ. The output energy (dE) is 5.37 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 375 ° C. Theoretically 3.98 kJ. Gain is 1.35 times.

Control: 1 g Mg + 1 g NaH + 2.19 g NiBr2. Input energy (Ein) is 129.0 kJ. The output energy (dE) is 5.13 kJ. Rapid increase in temperature (TSC) at 195-310 ° C. Maximum temperature (Tmax): 416 ° C. Theoretically, 5.25 kJ.

Control: 1 g NaH + 2.19 g NiBr2. Input energy (Ein) is 138.2kJ. The output energy (dE) is -0.18 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 377 ° C. Theoretically 3.98 kJ.

CuCl2
4 g CAIII-300 + 1 g Mg + 1 g NaH + 1.34 g CuCl2. Input energy (Ein) is 119.0 kJ. The output energy (dE) is 10.5 kJ. Rapid increase in temperature (TSC) at 250-381 ° C. Maximum temperature (Tmax): 393 ° C. Theoretically 4.9 kJ. Gain is 2.15 times.

4 g CAIII-300 + 1 g Al + 1 g NaH + 1.34 g CuCl2. Input energy (Ein) is 126.0 kJ. The output energy (dE) is 7.4 kJ. Rapid increase in temperature (TSC) at 229-354 ° C. Maximum temperature (Tmax): 418 ° C. Theoretically 4.9 kJ. Gain is 1.5 times.

4g CAIII-300 + 1g MgH2 + 1g NaH + 1.34g CuCl2. Input energy (Ein) is 144.0 kJ. The output energy (dE) is 8.3 kJ. Rapid increase in temperature (TSC) at 229-314 ° C. Maximum temperature (Tmax): 409 ° C. Theoretically 4.9 kJ. Gain is 1.69 times.

-5.0 gm NaH + 5.0 gm MgPowder + 20.0 gm activated carbon CAII300) mixture + 10.75 gm CuCl2 (theoretical 45 kJ). The input energy (Ein) is 268 kJ. The output energy (dE) is 80 kJ. Temp. slopeJumpat210Cwith maximum temperature (Tmax) to 360 ° C. It is 39kJ in theory. Gain is doubled.

1.4 g CuCl2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 <0> C) in a 1 inch extremely rugged cell. The energy gain is 14.6 kJ. The rapid increase in cell temperature is 190 ° C (188-378 ° C). Maximum cell temperature is 437 ° C. Theoretically 4.9 kJ. Gain is 3 times.

8.3 gm KH + 5.0 gm Mg powder + 20.0 gm CAII-300 + 6.7 gm CuCl2. Input energy (Ein) is 255 kJ. The output energy (dE) is 55 kJ. Rapid increase in temperature (TSC) at ~ 200 ° C. Maximum temperature (Tmax) to 320 ° C. Theoretically 24.5kJ. The gain is 2.24 times.

CuCl
4 g CAIII-300 + 1 g Mg + 1 g NaH + 1 g CuCl. Input energy (Ein) is 128.1 kJ. The output energy (dE) is 4.94 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 395 ° C. Theoretically 2.18 kJ. Gain is 2.26 times.

CoI2
4 g CAIII-300 + 1 g Mg + 1 g NaH + 3.13 g CoI2. The input energy (Ein) is 141.1 kJ. The output energy (dE) is 9.7 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 411 ° C. The following reaction is considered: 2NaH (c) + CoI2 (c) + Mg (c) = 2NaI (c) + Co (c) + MgH2 (c) Q = −449.8 kJ / reaction. The theoretical chemical reaction energy is -4.50 kJ. Excess heat is -5.18 kJ. Gain is 1.9 times.

3.13 g CoI2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 10.7 kJ. The rapid increase in cell temperature is 117 ° C (248-365 ° C). Maximum cell temperature is 438 ° C. Theoretically, 5.27 kJ. Gain is 2.03 times.

ZnI2
4 g CAIII-300 + 1 g Mg + 1 g NaH + 3.19 g ZnI2. Input energy (Ein) is 157.1 kJ. The output energy (dE) is 5.8 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 330 ° C. The following reaction is considered: 2NaH (c) + ZnI2 (c) + Mg (c) = 2NaI (c) + Zn (c) + MgH2 (c) Q = −330.47 kJ / reaction. The theoretical chemical reaction energy is −3.30 kJ. Excess heat is -2.50 kJ. Gain is 1.75 times.

3.19 g ZnI2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 5.9kJ. The cell temperature gradient change is 79 ° C (180-259 ° C). Maximum cell temperature is 423 ° C. Theoretically 4.29 kJ. The gain is 1.38 times.

NiF2
4 g CAIII-300 + 1 g Mg + 1 g NaH + 0.97 g NiF2. The input energy (Ein) is 135.0 kJ. The output energy (dE) is 7.9 kJ. There is a rapid temperature rise (TSC): 253-335 ° C. Maximum temperature (Tmax): 385 ° C. The following reaction is considered: 2NaH (c) + NiF2 (c) + Mg (c) = 2NaF (c) + Ni (c) + MgH2 (c) Q = −464.4 kJ / reaction. The theoretical chemical reaction energy is -4.64 kJ. Excess heat is -3.24 kJ. Gain is 1.7 times.

0.97 g NiF2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 8.7 kJ. The cell temperature gradient change is 63 ° C (256-319 ° C). Maximum cell temperature is 410 ° C. Theoretically, 5.25 kJ. Gain is 1.66 times.

CoBr2
4 g CAIII-300 + 1 g Mg + 1 g NaH + 2.19 g CoBr2. Input energy (Ein) is 140.0 kJ. The output energy (dE) is 7.6 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 461 ° C. The following reaction is considered: 2NaH (c) + CoBr2 (c) + Mg (c) = 2NaBr (c) + Co (c) + MgH2 (c) Q = −464 kJ / reaction. The theoretical chemical reaction energy is -4.64 kJ. Excess heat is -2.9 kJ. Gain is 1.64 times.

2.19 g CoBr2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 10.4 kJ. The rapid increase in cell temperature is 110 ° C (306-416 ° C). Maximum cell temperature is 450 ° C. Theoretically, 5.27 kJ. Gain is 1.97 times.

2.19 g CoBr2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 10.2 kJ. There was no rapid increase in cell temperature. Maximum cell temperature is 446 ° C. Theoretically, 5.27 kJ. Gain is 1.94 times.

FeCl2
4 g CAIII-300 + 1 g Mg + 1 g NaH + 1.27 g FeCl2. Input energy (Ein) is 155.0 kJ. The output energy (dE) is 10.5 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 450 ° C. Theoretically 3.68kJ. Gain is 2.85 times.

4 g CAIII-300 + 1 g Al + 1 g NaH + 1.27 g FeCl2. Input energy (Ein) is 141.7 kJ. The output energy (dE) is 7.0 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax): 440 ° C. Theoretically 3.68kJ. Gain is 1.9 times.

• 1.3 g FeCl 2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.) in a 1 inch very sturdy cell. The energy gain is 11.5 kJ. The rapid rise in cell temperature is 142 ° C (287-429 ° C). Maximum cell temperature is 448 ° C. Theoretically 4.1 kJ. Gain is 2.8 times.

-5.0 gm NaH + 5.0 gm Mg powder + 20.0 gm activated carbon CAII300) mixture + 6.35 gm FeCl2. Input energy (Ein) is 296kJ. The output energy (dE) is 37 kJ. Temperature gradient jump is 220 ° C. Maximum temperature (Tmax) to 330 ° C. Theoretically, it is 18.4kJ. Gain is doubled.

FeCl3
2.7 g FeCl 3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 21.3 kJ. The rapid increase in cell temperature is 205 ° C (147-352 ° C). Maximum cell temperature is 445 ° C. Theoretically 10.8 kJ. Gain is 1.97 times.

1.0 gm NaH + 1.0 gm Mg powder + 4.0 gm TiC + 1.6 gm FeCl3. Input energy (Ein) is 88 kJ. The output energy (dE) is 14 kJ. Rapid temperature increase (TSC) at 80 ° C. Maximum temperature (Tmax) to 350 ° C. Theoretically, 6.65 kJ. Gain is 2.1 times.

8.3 gm KH + 5.0 gm MgH2 powder + 20.0 gm CAII300 + 8.1 gm FeCl3. Input energy (Ein) is 253 kJ. The output energy (dE) is 52 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 300 ° C. Theoretically 33 kJ. The gain is 1.56 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 6.5 gm FeCl2. The input energy (Ein) is 299 kJ. The output energy (dE) is 44 kJ. No rapid temperature rise (TSC). Maximum temperature (Tmax) to 350 ° C. In theory, it is 18.9 kJ. Gain is 2.3 times.

FeBr2
4 g CAIII-300 + 1 g Mg + 1.66 g KH + 2.16 g FeBr2. Input energy (Ein) is 144.0 kJ. The output energy (dE) is 9.90 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 455 ° C. Theoretically 3.6 kJ. Gain is 2.75 times.

4 g CAIII-300 + 1 g MgH 2 + 1 g NaH + 2.16 g FeBr 2. The input energy (Ein) is 142.0 kJ. The output energy (dE) is 8.81 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 428 ° C. Theoretically 3.6 kJ. Gain is 2.44 times.

4 g CAIII-300 + 1 g MgH2 + 0.33 g LiH + 2.16 g FeBr2. Input energy (Ein) is 164.0 kJ. The output energy (dE) is 8.68 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 450 ° C. Theoretically 3.6 kJ. Gain is 2.4 times.

4 g CAIII-300 + 1 g MgH2 + 1.66 g KH + 2.16 g FeBr2. Input energy (Ein) is 159.8 kJ. The output energy (dE) is 9.07 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 459 ° C. Theoretically 3.6 kJ. Gain is 2.5 times.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 2.96 g FeBr2. The experimental output energy (dE) is -6.7 kJ. The following reaction is considered: 2NaH (c) + FeBr2 (c) + Mg (c) = 2NaBr (c) + Fe (c) + MgH2 (c) Q = −435.1 kJ / reaction. The theoretical chemical reaction energy is -4.35 kJ. Excess heat is -2.35 kJ. 1.54X excess heat.

NiCl2
4 g CAIII-300 + 1 g Mg + 1 g NaH + 1.30 g NiCl2. The input energy (Ein) is 112.0 kJ. The output energy (dE) is 9.7 kJ. Rapid increase in temperature (TSC) at 230-368 ° C. Maximum temperature (Tmax): 376 ° C. 4kJ in theory. Gain is 2.4 times.

-1.3 g NiCl2, 0.33 g LiH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 <0> C) in a very sturdy cell of 1 inch. The energy gain is 9.2kJ. Temperature gradient change is 100 ° C (205-305 ° C). Maximum cell temperature is 432 ° C. 4kJ in theory. Gain is 2.3 times.

• 1.3 g NiCl2, 0.33 g LiH, 1 g Al powder, and 4 g CA-III300 activated carbon powder (dried at 300 <0> C) in a very sturdy cell of 1 inch. The energy gain is 8.0 kJ. Temperature gradient change is 85 ° C (206-291 ° C). Maximum cell temperature is 447 ° C. 4kJ in theory. Gain is doubled.

CuBr
4 g CAIII-300 + 1 g Mg + 1 g NaH + 1.44 g CuBr. Input energy (Ein) is 125.0 kJ. The output energy (dE) is 4.67 kJ. There is no rapid increase in temperature (TSC). Maximum temperature (Tmax): 382 ° C. 2kJ in theory. Gain is 2.33 times.

4 g CAIII-300 + 1 g Mg + 1.66 g KH + 1.44 g CuBr. The experimental output energy (dE) is -7.6 kJ. The following reaction is considered: CuBr (c) + KH (c) + 0.5Mg (c) = KBr (c) + Cu (c) + 0.5MgH2 (c) Q = −269.2 kJ / reaction. The theoretical chemical reaction energy is -2.70 kJ. Excess heat is -4.90 kJ. 2.8X excess heat.

CuBr2
4 g CAIII-300 + 1 g Mg + 1 g NaH + 2.23 g CuBr2. Input energy (Ein) is 118.1 kJ. The output energy (dE) is 8.04 kJ. Rapid increase in temperature (TSC) at 108-180 ° C. Maximum temperature (Tmax): 369 ° C. Theoretically, 4.68 kJ. Gain is 1.7 times.

SnF4
2.0 g SnF4, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 18.4kJ. There is no rapid rise in temperature. Maximum cell temperature is 576 ° C. 9.3 kJ in theory. Gain is 1.98 times.

AlI3
4.1 g AlI3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 10.1 kJ. There is no rapid rise in temperature. Maximum cell temperature is 412 ° C. Theoretically, 6.68kJ. Gain is 1.51 times.

8.3 gm KH + 5.0 gm Mg + 20.0 gm CAII-300 + 0.5 gm AlI32. Input energy (Ein) is 318 kJ. The output energy (dE) is 48 kJ. Theoretically 33.4 kJ. Gain is 1.4 times.

SiCl4
1.7 g SiCl 4, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 12.6 kJ. The rapid rise in temperature is 68 ° C (36-434 ° C. Maximum cell temperature is 473 ° C. Theoretically 7.32 kJ. Gain is 1.72.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 0.01 mol SiCl4 (1.15 cc). Input energy (Ein) is 114.0 kJ. The output energy (dE) is 14.19 kJ. There is a rapid temperature rise (TSC) at 260-410 ° C. Maximum temperature (Tmax): 423 ° C. Theoretically 7.32 kJ. Gain is 1.94 times.

AlBr3
2.7 g AlBr3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 7.5 kJ. There is no rapid rise in temperature. Maximum cell temperature is 412 ° C. Theoretically 4.46 kJ. Gain is 1.68 times.

FeCl3
2.7 g FeCl 3, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 21.3 kJ. The rapid rise in temperature is 205 ° C (147-352 ° C). Maximum cell temperature is 445 ° C. Theoretically 10.8 kJ. Gain is 1.97 times.

SeBr4
4 g CAIII-300 + 1 g Mg + 1 g NaH + 3.99 g SeBr4. The input energy (Ein) is 112.0 kJ. The output energy (dE) is 23.40 kJ. Rapid increase in temperature (TSC) at 132-448 ° C. Maximum temperature (Tmax): 448 ° C. Theoretically, 15.7 kJ. Gain is 1.5 times.

SnBr4
4 g CAIII-300 + 1 g Mg + 1 g NaH + 4.38 g SnBr4. Input energy (Ein) is 98.0 kJ. The output energy (dE) is 12.44 kJ. Rapid increase in temperature (TSC) at 120-270 ° C. Maximum temperature (Tmax): 359 ° C. 8.4kJ in theory. Gain is 1.48 times.

8.3 gm KH + 5.0 gm Mg powder + 20.0 gm CAII300 + 22.0 gm SnBr4. Input energy (Ein) is 163 kJ. The output energy (dE) is 78 kJ. Rapid temperature increase (TSC) at 60 ° C. Maximum temperature (Tmax) to 290 ° C. It is 42kJ in theory. Gain is 1.86 times.

SiBr4
3.5 g SiBr4, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.). The energy gain is 11.9kJ. The rapid rise in temperature is 99 ° C (304-403 ° C). Maximum cell temperature is 449 ° C. Theoretically, 7.62 kJ. The gain is 1.56 times.

TeBr4
4 g CAIII-300 + 1 g Mg + 1 g NaH + 4.47 g TeBr4. Input energy (Ein) is 99.0 kJ. The output energy (dE) is 18.4 kJ. Rapid increase in temperature (TSC) at 186-411 ° C. Maximum temperature (Tmax): 418 ° C. Theoretically, 11.3 kJ. Gain is 1.63 times.

4 g CAIII-300 + 1 g Al + 1 g NaH + 4.47 g TeBr4. The input energy (Ein) is 101.0 kJ. The output energy (dE) is 14.7 kJ. There is a rapid temperature rise (TSC) at 144-305 ° C. Maximum temperature (Tmax): 374 ° C. In theory, it is 11.4kJ. Gain is 1.29 times.

-4.5 g TeBr4, 1.66 g KH, 1 g MgH2 powder, and 4 g CA-III300 activated carbon powder (dried at 300 <0> C) in a 1-inch very rugged cell. The energy gain is 19.1 kJ. The rapid rise in temperature is 218 ° C (172-390 ° C). Maximum cell temperature is 410 ° C. Theoretically, 12.65 kJ. Gain is 1.5 times.

• 4.5 g TeBr4, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.) in a very sturdy cell of 1 inch. The energy gain is 23.5kJ. The rapid rise in temperature is 247 ° C (184-431 ° C). Maximum cell temperature is 436 ° C. Theoretically 12.4 kJ. Gain is 1.89 times.

6.64 gm KH + 4.0 gm Mg powder + 16 gm activated carbon CAII300) +18 gm TeBr4 (in kJ theory) (80% of 5X scale up). The input energy (Ein) is 213 kJ. The output energy (dE) is 77 kJ. Temperature gradient jump is 140 ° C. Maximum temperature (Tmax) to 320 ° C. Theoretically 48.4 kJ. Gain is 1.59 times.

TeCl4
4 g CAIII-300 + 1 g Mg + 1 g NaH + 2.7 g TeCl4. Input energy (Ein) is 99.0 kJ. The output energy (dE) is 16.76 kJ. Rapid increase in temperature (TSC) is 114-300 ° C. Maximum temperature (Tmax): 385 ° C. It is 13kJ in theory. Gain is 1.29 times.

-2.7 g TeCl4, 0.33 g LiH, 1 g MgH2 powder, and 4 g CA-III300 activated carbon powder (dried at 300 <0> C) in a 1-inch very rugged cell. The energy gain is 20.4kJ. The rapid rise in temperature is 140 ° C (138-278 ° C). Maximum cell temperature is 399 ° C. Theoretically 12.1 kJ. Gain is 1.69 times.

-2.7 g TeCl4, 0.33 g LiH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 <0> C) in a 1-inch very rugged cell. The energy gain is 17.2 kJ. The rapid rise in temperature is 240 ° C (137-377 ° C). Maximum cell temperature is 398 ° C. Theoretically 12.8 kJ. Gain is 1.34 times.

-2.7 g TeCl4, 1.66 g KH, 1 g MgH2 powder, and 4 g CA-III300 activated carbon powder (dried at 300 <0> C) in a 1 inch very rugged cell. The energy gain is 15.6 kJ. The rapid rise in temperature is 216 ° C (139-355 ° C). Maximum cell temperature is 358 ° C. Theoretically 12.1 kJ. Gain is 1.29 times.

• 2.7 g TeCl4, 1.66 g KH, 1 g Al powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.) in a 1 inch very rugged cell. The energy gain is 19.4kJ. The rapid rise in temperature is 202 ° C (89-291 ° C). Maximum cell temperature is 543 ° C. Theoretically, it is 10.9kJ. Gain is 1.78 times.

• 2.7 g TeCl4, 0.33 g LiH, 1 g Al powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.) in a 1 inch very rugged cell. The energy gain is 19.0 kJ. The rapid rise in temperature is 288 ° C (155-443 ° C). Maximum cell temperature is 443 ° C. Theoretically, it is 10.9kJ. Gain is 1.74 times.

2.7 g TeCl4, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 <0> C) in a 1 inch very rugged cell. The energy gain is 17.7 kJ. The rapid increase in temperature is 208 ° C (84-292 ° C). Maximum cell temperature is 396 ° C. It is 13kJ in theory. Gain is 1.36 times.

• 2.7 g TeCl4, 1.66 g KH, 1 g Al powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.) in a 1 inch very rugged cell. The energy gain is 18.7 kJ. The rapid rise in temperature is 224 ° C (112-336 ° C). Maximum cell temperature is 398 ° C. It is 12kJ in theory. The gain is 1.56 times.

SeCl4
4 g CAIII-300 + 1 g Mg + 1 g NaH + 2.21 g SeCl4. Input energy (Ein) is 93.0 kJ. The output energy (dE) is 22.14 kJ. There is a rapid temperature rise (TSC) at 141-435 ° C. Maximum temperature (Tmax): 435 ° C. In theory, it is 15 kJ. Gain is 1.48 times.

4 g CAIII-300 + 1 g Mg + 1.66 g KH + 2.20 g SeCl4. The experimental output energy (dE) is −25.2 kJ. The following reaction is considered: SeCl4 (c) + 4KH (c) + 3Mg (c) = 4KCl (c) + MgSe (c) + 2MgH2 (c) Q = -1750.4 kJ / reaction. The theoretical chemical reaction energy is -17.5 kJ. Excess heat is -7.7 kJ. 1.44X excess heat.

CF4
50 gm NaH + 50 gm Al + 200 gm activated carbon CAII300 + 0.3 mole CF4 45PSIG reservoir cell volume is 2221.8 CC. Input energy (Ein) is 2190kJ. The output energy (dE) is 482 kJ. Temperature jump is 200 ° C. Maximum temperature (Tmax) to 760 ° C. 345kJ in theory. Gain is 1.4 times.

CF4 of 50.0 gm NaH + 50 gm Mg powder + 200 gm activated carbon CAII-300 + 75-9.9 PSIG (after emptying). Reservoir volume is 1800 CC, n = 0.356 mole for this pressure drop. The theoretical energy is ~ 392kJ. The input energy (Ein) is 1810 kJ. The output energy (dE) is 765 kJ. Temperature gradient jump is 170 ° C. Maximum temperature (Tmax) is ~ 1000 ° C. The gain is 765/392 = 1.95X.

1.0 gm NaH + (1.0 gm Mg powder + 4 gm activated carbon CAII300) ball mill + 0.0123 mole CF4. The theoretical energy is ˜13.6 kJ). Input energy (Ein) is 143 kJ. The output energy (dE) is 25 kJ. Temperature gradient jump is at 250 ° C. Maximum temperature (Tmax) to 500 ° C. Energy gain is ~ 1.8X.

1.0 gm NaH + (1.0 gm Mg powder + 4 gm activated carbon CAII-3004 gm) ball mill + ~ 0.01 mole CF4. The theoretical energy is ~ 10.2 kJ. The input energy (Ein) is 121 kJ. The output energy (dE) is 18 kJ. Temperature gradient jump is 260 ° C. Maximum temperature (Tmax) to 500 ° C. The energy gain is ~ 1.7X.

-1.0 gm NaH + (1.0 gm Mg powder + 4 gm activated carbon CAII-3004 gm) ball mill + 0.006 mole CF4. The theoretical energy is -7.2 kJ). Input energy (Ein) is 133 kJ. The output energy (dE) is 15 kJ. Temperature gradient jump is 300 ° C. Maximum temperature (Tmax) to 440 ° C. Energy gain is ~ 2.0X.

4 g CAIII-300 + 1 g MgH2 + 3.55 g Rb + 0.0082 mol CF4 + 0.0063 mol H2. Input energy (Ein) is 76.0 kJ. The output energy (dE) is 20.72 kJ. Rapid increase in temperature (TSC) at 30-200 ° C. Maximum temperature (Tmax): 348 ° C. 10kJ in theory. Gain is doubled.

SF6
50 gm NaH + 50 gm MgH2 + 200 gm activated carbon CAII300 + 0.29 mole SF6 43PSIG reservoir cell volume is 2221.8 CC. Input energy (Ein) is 1760kJ. The output energy (dE) is 920 kJ. Temperature gradient jump is ~ 140 ° C. Maximum temperature (Tmax) to 1100 ° C. Theoretically 638 kJ. Gain is 1.44 times.

-4 g CAIII-300 + 1 g MgH2 + 1 g NaH + 0.0094 mol SF6. Input energy (Ein) is 96.7 kJ. The output energy (dE) is 33.14 kJ. Rapid increase in temperature (TSC) at 110-455 ° C. Maximum temperature (Tmax): 455 ° C. Theoretically 20.65 kJ. The excess is 12.5 kJ. Gain is 1.6 times.

1.0 gm NaH + 1.0 gm Al powder + 4 gm activated carbon CAII300) ball mill + 0.01 mole SF6. The theoretical energy is ~ 20 kJ). Input energy (Ein) is 95 kJ. The output energy (dE) is 30 kJ. Temperature gradient change is ~ 100 ° C. Maximum temperature (Tmax) to 400 ° C. Theoretically 20.4 kJ. The excess is 9.6 kJ. Gain is 1.47 times.

1.0 gm NaH + 1.0 gm MgH2 powder + 4 gm activated carbon CAII300) ball mill + 0.01 mole SF6. The theoretical energy is ~ 22kJ). Input energy (Ein) is 85 kJ. The output energy (dE) is 28 kJ. Temperature gradient change is ~ 110 ° C. Maximum temperature (Tmax) to 410 ° C. Theoretically 22 kJ. The excess is 6 kJ. Gain is 1.27 times.

1.0 gm NaH + 1.0 gm Al nanopowder + 4 gm activated carbon CAII300) ball mill + 0.005 mole SF6. The input energy (Ein) is 107 kJ. The output energy (dE) is 21 kJ. Temperature gradient change is ~ 160 ° C. Maximum temperature (Tmax) to 380 ° C. Theoretically 10.2 kJ. Gain is doubled.

1.0 gm NaH + 1.0 gm Mg powder + 4 gm activated carbon CAII300) ball mill + 0.005 mole SF6. Input energy (Ein) is 104kJ. The output energy (dE) is 18 kJ. Temperature gradient change is ~ 150 ° C. Maximum temperature (Tmax) to 370 ° C. Theoretically 12.5 kJ. The excess is 5.5 kJ. Gain is 1.44 times.

1.0 gm NaH + 1.0 gm MgH2 powder + 4 gm activated carbon CAII300) ball mill + 0.0025 mole SF6. The theoretical energy is ~ 5.5 kJ). Input energy (Ein) is 100 kJ. The output energy (dE) is 10 kJ. Temperature gradient change is ~ 160 ° C. Maximum temperature (Tmax) to 335 ° C. Theoretically 5.5 kJ. Gain is 1.8 times.

4 g CAIII-300 + 0.5 g B + 1 g NaH + 0.0047 mol SF6. The input energy (Ein) is 112.0 kJ. The output energy (dE) is 15.14 kJ. Rapid increase in temperature (TSC) is 210-350 ° C. Maximum temperature (Tmax): 409 ° C. Theoretically 10.12 kJ. The excess is 5 kJ. Gain is 1.49 times.

4 g CAIII-300 + 1 g MgH2 + 1.66 g KH + 0.00929 mol SF6 (cell temperature rose to 29 ° C. when SF6 was met). Input energy (Ein) is 66.0 kJ. The output energy (dE) is 26.11 kJ. Rapid increase in temperature (TSC) at 37-375 ° C. Maximum temperature (Tmax): 375 ° C. Theoretically 20.4 kJ. Gain is 1.28 times.

4 g CAIII-300 + 1 g Mg + 0.33 g LiH + 0.00929 mol SF6 (cell temperature rose to 26 ° C. when SF6 was met). Input energy (Ein) is 128.0 kJ. The output energy (dE) is 32.45 kJ. Rapid increase in temperature (TSC) at 275-540 ° C. Maximum temperature (Tmax): 550 ° C. Theoretically 23.2 kJ. Gain is 1.4 times.

4 g CAIII-300 + 1 g S + 1 g NaH + 0.0106 mol SF6 (online). Input energy (Ein) is 86.0 kJ. The output energy (dE) is 18.1 kJ. There is a rapid temperature rise (TSC) at 51-313 ° C. Maximum temperature (Tmax): 354 ° C. Theoretically 11.2kJ. Gain is 1.6 times.

• 5.0 gm NaH + 5.0 gm MgH2 + 20.0 gm activated carbon CAII300) ball mill + SF640PSIG. 0.026 mole online (theoretical energy is ~ 57 kJ) 2 inch cell. Input energy (Ein) is 224kJ. The output energy (dE) is 86 kJ. Temperature jump is 150 ° C. Maximum temperature (Tmax) to 350 ° C. The theory is 57 kJ. Gain is 1.5 times.

TeO2
4g CAIII-300 + 1g MgH2 + 1g NaH + 1.6g TeO2. Input energy (Ein) is 325.1 kJ. The output energy (dE) is 18.46 kJ. There is a rapid temperature rise (TSC) at 210-440 ° C. Maximum temperature (Tmax): 440 ° C. Theoretically, 9.67 kJ. The excess is 8.8 kJ. Gain is 1.9 times.

4 g CAIII-300 + 2 g MgH2 + 2 g NaH + 3.2 g TeO2. The input energy (Ein) is 103.0 kJ. The output energy (dE) is 31.6 kJ. Rapid increase in temperature (TSC) at 185-491 ° C. Maximum temperature (Tmax): 498 ° C. Theoretically, 17.28 kJ. Gain is 1.83 times.

-1.6 g TeO2, 0.33 g LiH, 1 g Al powder, and 4 g CA-III300 activated carbon powder (dried at 300 <0> C) in a 1 inch very rugged cell. The energy gain is 18.1 kJ. There is no rapid rise in temperature. Maximum cell temperature is 637 ° C. Theoretically, 8.66 kJ. Gain is 2.1 times.

1.6 g TeO2, 1.66 g KH, 1 g MgH2 powder, and 4 g CA-III300 activated carbon powder (dried at 300 <0> C) in a 1-inch very rugged cell. The energy gain is 22.0 kJ. The rapid rise in temperature is 233 ° C (316-549 ° C). Maximum cell temperature is 554 ° C. Theoretically, 8.64 kJ. Gain is 2.55 times.

1.6 g TeO2, 1.66 g KH, 1 g Mg powder, and 4 g CA-III300 activated carbon powder (dried at 300 <0> C) in a 1-inch very rugged cell. The energy gain is 20.3 kJ. The rapid rise in temperature is 274 ° C (268-542 ° C). Maximum cell temperature is 549 ° C. Theoretically, it is 10.9kJ. Gain is 1.86 times.

-5.0 gm NaH + 5.0 gm MgH2 powder + 20 gm activated carbon CAII300) ball mill + 8.0 gm TeO2. Input energy (Ein) is 253 kJ. The output energy (dE) is 77 kJ. Temperature gradient jump is 200 ° C. Maximum temperature (Tmax) to 400 ° C. Theoretically 48.35 kJ. Gain is 1.6 times.

1.0 gm NaH + 1.0 gm MgH2 powder + 4.0 gm activated carbon CAII300) ball mill + 1.6 gm TeO2. The input energy (Ein) is 110 kJ. The output energy (dE) is 16 kJ. Temperature gradient jump at 190 ° C. Maximum temperature (Tmax) to 400 ° C. Theoretically, 9.67 kJ. Gain is 1.65 times.

1.66 gm KH + 1.0 gm MgH2 powder + 4.0 gm activated carbon CAII300) ball mill + 1.6 gm TeO2. The input energy (Ein) is 119 kJ. The output energy (dE) is 19 kJ. Temperature gradient jump at 340 ° C. Maximum temperature (Tmax) to 570 ° C. Theoretically, 9.67 kJ. Gain is doubled.

4 g CAIII-300 + 1 g NaH + 1.6 g TeO2. Input energy (Ein) is 116.0 kJ. The output energy (dE) is 11.0 kJ. Rapid temperature increase (TSC): 207-352 ° C. Maximum temperature (Tmax): 381 ° C. Theoretically, it is 6.6 kJ. Gain is 1.67 times.

1.66 gm KH + 1.0 gm MgH2 powder + 4.0 gm TiC + 1.6 gm TeO2. Input energy (Ein) is 133 kJ. The output energy (dE) is 15 kJ. Temperature gradient jump is 280 ° C. Maximum temperature (Tmax) to 460 ° C. Theoretically, 8.64 kJ. Gain is 1.745 times.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 1.60 g TeO2. The experimental output energy (dE) is -17.0 kJ. The following reaction is considered: TeO2 (c) + 3Mg (c) + 2NaH (c) = 2MgO (c) + Na2Te (c) + MgH2 (c) Q = −1192.7 kJ / reaction. The theoretical chemical reaction energy is −11.9 kJ. Excess heat is -5.1 kJ. 1.43X excess heat.

P2O5
-1.66 g KH, 2 g P2O5, and 1 g MgH2, and 4 g CA-III300 activated carbon powder (dried at 300 <0> C) in a 1 inch very rugged cell. The energy gain is 21.2kJ. The rapid rise in temperature is 242 ° C (299-541 ° C). Maximum cell temperature is 549 ° C. Theoretically 10.8 kJ. The excess is 10.35 kJ. Gain is 1.96 times.
032609 GC4: 031909 RCWF4 / 1.66 g KH + 2 g P2O5 + 1 g MgH2 + DMF-d7 in 4 g CAIII-300 (as received). Strong -3.86 ppm peak.

4 g CAIII-300 + 1 g MgH2 + 1.66 g KH + 2 g P2O5. Input energy (Ein) is 138.0 kJ. The output energy (dE) is 21.6 kJ. Rapid increase in temperature (TSC) is present at 320-616 ° C. Maximum temperature (Tmax): 616 ° C. Theoretically 11.5 kJ. The excess is 10.1 kJ. Gain is 1.9 times.

-8.3 gm KH + 5.0 gm MgH2 powder + 20 gm activated carbon CAII300) ball mill + 10.0 gm P2O5. The input energy (Ein) is 272 kJ. The output energy (dE) is 98 kJ. Jump at 250 ° C. Maximum temperature (Tmax) to 450 ° C. Theoretically 54 kJ. Gain is 1.81 times.

1.66 gm KH + 1.0 gm MgH2 powder + 4 gm activated carbon CAII300) ball mill + 2.0 gm P2O5. Input energy (Ein) is 130 kJ. The output energy (dE) is 21 kJ. Jumpup 300 ° C. with maximum temperature (Tmax) to 550 ° C. Theoretically 10.8 kJ. Gain is 1.94 times.

1.66 gm KH + 1.0 gm MgH2 powder + 4.0 gm TiC + 2.0 gm P2O5. Input energy (Ein) is 129 kJ. The output energy (dE) is 21 kJ. Temperature gradient jump is 270 ° C. Maximum temperature (Tmax) to 600 ° C. Theoretically 10.8 kJ. Gain is 1.95 times.

NaMnO4
4 g CAIII-300 + 1 g Si + 1 g NaH + 3.5 g NaMnO4. The input energy (Ein) is 123.0 kJ. The output energy (dE) is 26.25 kJ. Rapid increase in temperature (TSC) at 45-330 ° C. Maximum temperature (Tmax): 465 ° C. Theoretically 17.6 kJ. Gain is 1.5 times.

4 g CAIII-300 + 1 g Al + 1 g NaH + 3.5 g NaMnO4. The input energy (Ein) is 120.0 kJ. The output energy (dE) is 32.41 kJ. Rapid increase in temperature (TSC) at 44-373 ° C. Maximum temperature (Tmax): 433 ° C. Theoretically 20.5kJ. The excess is 7.7 kJ. Gain is 1.58 times.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 3.5 g NaMnO 4; input energy (Ein) is 66.0 kJ. The output energy (dE) is 32.27 kJ. Rapid temperature increase (TSC) is 74-430 ° C. Maximum temperature (Tmax): 430 ° C. Theoretically 17.4 kJ. The excess is 14.9 kJ. Gain is 1.85 times.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 3.5 g NaMnO4. The input energy (Ein) is 72.0 kJ. The output energy (dE) is 34.1 kJ. Rapid increase in temperature (TSC) at 49-362 ° C. Maximum temperature (Tmax): 364 ° C. Theoretically 17.4 kJ. The excess is 16.7 kJ. Gain is doubled.

8.3 gm KH + 5.0 gm Mg powder + 20 gm activated carbon CAII300) ball mill + 17.5 gm NaMnO4. Input energy (Ein) is 130 kJ. The output energy (dE) is 160 kJ. Temperature gradient jump is 70 ° C. Maximum temperature (Tmax) to 350 ° C. It is 87kJ in theory. Gain is 1.84 times.

8.3 gm KH + 5.0 gm Al powder + 20 gm activated carbon CAII300) ball mill + 17.5 gm NaMnO4. The input energy (Ein) is 134 kJ. The output energy (dE) is 171 kJ. Temperature gradient jump at 50 ° C. Maximum temperature (Tmax) to 350 ° C. Theoretically 102.5 kJ. Gain is 1.66 times.

1.0 gm NaH + 1.0 gm Mg powder + 4.0 gm activated carbon CAII300) ball mill + 3.5 gm NaMnO 4 (theoretical ˜17.4 kJ). Input energy (Ein) is 54 kJ. The output energy (dE) is 32 kJ. Temperature gradient jump at 60 ° C. Maximum temperature (Tmax) to 450 ° C. Theoretically 17.4 kJ. Gain is 1.8 times.

1.66 gm KH + 1.0 gm Mg powder + 4.0 gm TiC + 3.5 gm NaMnO4. Input energy (Ein) is 65 kJ. The output energy (dE) is 30 kJ. Temperature gradient jump is 70 ° C. Maximum temperature (Tmax) to 410 ° C. Theoretically 17.4 kJ. Gain is 1.7 times.

Nitrate
In a 1 inch cell, 2. A mixture of g NaH, 3 g NaNO 3, and 1 g Ti powder and 4 g activated carbon powder (dried at 300 ° C.). The energy gain is 33.2kJ. And there is a sudden rise in temperature at 418 ° C (110-528 ° C). Maximum cell temperature is 530 ° C. Theoretically 24.8 kJ. The excess is 8.4 kJ. Gain is 1.3 times.

In a 1-inch cell, 3. A mixture of g NaH, 3 g NaNO 3, and 1 g Al nanopowder and 4 g activated carbon powder (dried at 300 ° C.). The energy gain is 42.3 kJ. And there is a sudden rise in temperature at 384 ° C (150-534 ° C). Maximum cell temperature is 540 ° C. Theoretically 33.3 kJ. The excess is 9 kJ. Gain is 1.27 times.

A mixture of 2,1 g NaH, 3 g NaNO 3 and 1 g MgH 2 and 4 g activated carbon powder (dried at 300 ° C.) in a 1 inch cell. The energy gain is 43.4kJ. And there is a sudden rise in temperature at 382 ° C (67-449 ° C). Maximum cell temperature is 451 ° C. Theoretically 28.6 kJ. The excess is 14.8 kJ. The gain is 1.527 times.

A mixture of 0.33 g LiH, 1.7 g LiNO 3, and 1 g MgH 2 and 4 g activated carbon powder (dried at 300 ° C.) in a very sturdy cell of 1 inch. The energy gain is 40.1kJ. And there is a sudden rise in temperature at 337 ° C (92-429 ° C). Maximum cell temperature is 431 ° C. Theoretically 21.6 kJ. The excess is 18.5 kJ. Gain is 1.86 times.

A mixture of 0.33 g LiH, 1.7 g LiNO3, and 1 g Ti and 4 g activated carbon powder (dried at 300 ° C.) in a 1 inch cell. The energy gain is 36.5 kJ. And there is a sudden rise in temperature at 319 ° C (83-402 ° C). Maximum cell temperature is 450 ° C. Theoretically, it is 18.4kJ. The excess is 18 kJ. Gain is doubled.

4 g CAIII-300 + 1 g MgH2 + 1 g NaH + 2.42 g LiNO3. Input energy (Ein) is 75.0 kJ. The output energy (dE) is 39.01 kJ. Rapid increase in temperature (TSC) at 57-492 ° C. Maximum temperature (Tmax): 492 ° C. Theoretically 28.5 kJ. The excess is 10.5 kJ. Gain is 1.37 times.

4 g CAIII-300 + 1 g Al + 1 g NaH + 2.42 g LiNO3. Input energy (Ein) is 81.2kJ. The output energy (dE) is 41.89 kJ. Rapid increase in temperature (TSC) at 73-528 ° C. Maximum temperature (Tmax): 528 ° C. Theoretically 34.6 kJ. The excess is 7.3 kJ. Gain is 1.21 times.

ClO4
4 g CAIII-300 + 1 g MgH2 + 2 g NaClO4 + 1 g NaH. Input energy (Ein) is 86.0 kJ. The output energy (dE) is 38.88 kJ. Rapid increase in temperature (TSC) at 130-551 ° C. Maximum temperature (Tmax): 551 ° C. Theoretically 30.7 kJ. The excess is 8.2 kJ. Gain is 1.27 times.

4 g CAIII-300 + 1 g Al + 1 g NaH + 4.29 g NaClO4. Input energy (Ein) is 88.0 kJ. The output energy (dE) is 58.24 kJ. There is a rapid temperature rise (TSC) at 119-615 ° C. Maximum temperature (Tmax): 615 ° C. Theoretically 47.1 kJ. The excess is 11.14 kJ. The gain is 1.23 times.

4 g CAIII-300 + 1 g MgH 2 + 1 g NaH + 4.29 g NaClO 4. Input energy (Ein) is 98.0 kJ. The output energy (dE) is 56.26 kJ. Rapid increase in temperature (TSC) at 113-571 ° C. Maximum temperature (Tmax): 571 ° C. In theory, it is 36.2 kJ. The excess is 20.1 kJ. Gain is 1.55 times.

K2S2O8
4 g CAIII-300 + 1 g MgH2 + 1.66 g KH + 2.7 g K2S2O8. The input energy (Ein) is 121.0 kJ. The output energy (dE) is 27.4 kJ. Rapid increase in temperature (TSC) at 178-462 ° C. Maximum temperature (Tmax): 468 ° C. Theoretically 19.6 kJ. The excess is 7.8 kJ. Gain is 1.40 times.

SO2
4 g CAIII-300 + 1 g MgH2 + 1 g NaH + 0.0146 mol SO2. Input energy (Ein) is 58.0 kJ. The output energy (dE) is 20.7 kJ. There is a rapid temperature rise (TSC) at 42-287 ° C. Maximum temperature (Tmax): 309 ° C. In theory, it is 15 kJ. The excess is 5.7 kJ. The gain is 1.38 times.

S
4 g CAIII-300 + 1 g MgH 2 + 1 g NaH + 3.2 g S. Input energy (Ein) is 67.0 kJ. The output energy (dE) is 22.7 kJ. There is a rapid temperature rise (TSC) at 49-356 ° C. Maximum temperature (Tmax): 366 ° C. In theory, it is 17.9 kJ. The excess is 4.8 kJ. Gain is 1.27 times.

• 1.3 g S powder, 1.66 g KH, 1 g Si powder, and 4 g CA-III300 activated carbon powder (dried at 300 ° C.) in a very sturdy cell of 1 inch. The energy gain is 13.7 kJ. And there is a rapid increase in temperature at 129 ° C (66-195 ° C). Maximum cell temperature is 415 ° C. Theoretically 7.5 kJ. The excess is 1.82 times.

• 3.2 g S powder, 0.33 g LiH, 1 g Al powder, and 4 g CA-IV300 activated carbon powder (dried at 300 ° C.) in a 1 inch very sturdy cell. The energy gain is 27.1 kJ. And there is a sharp rise in temperature at 301 ° C (163-464 ° C). Maximum cell temperature is 484 ° C. Theoretically 20.9kJ. The excess is 6.2 kJ. Gain is 1.3 times.

• 3.2 g of S powder, 0.33 g of LiH, 1 g of Si powder, and 4 g of CA-IV300 activated carbon powder (dried at 300 ° C.) in a very sturdy cell of 1 inch. The energy gain is 17.7 kJ. And there is a rapid rise in temperature at 233 ° C (212-445 ° C). Maximum cell temperature is 451 ° C. In theory, it is 13.7 kJ. The excess is 4kJ. Gain is 1.3 times.

4 g CAIII-300 + 1 g Si + 1.66 g KH + 1.3 g S. The input energy (Ein) is 81.0 kJ. The output energy (dE) is 10.8 kJ. There is a rapid temperature rise (TSC) at 52-196 ° C. Maximum temperature (Tmax): 326 ° C. 7.4 kJ in theory. Gain is 1.45 times.

SnF4
4 g CAIII-300 + 1 g Mg + 1 g NaH + 1.95 g SnF4. The input energy (Ein) is 130.2 kJ. The output energy (dE) is 13.89 kJ. Rapid increase in temperature (TSC) at 375-520 ° C. Maximum temperature (Tmax): 525 ° C. 9.3 kJ in theory. Gain is 1.5 times.

4 g CAIII-300 + 1 g Mg + 1 g NaH + 1.95 g SnF4. The input energy (Ein) is 130.2 kJ. The output energy (dE) is 13.89 kJ. Rapid increase in temperature (TSC) at 375-520 ° C. Maximum temperature (Tmax): 525 ° C. 9.3 kJ in theory. Gain is 1.5 times.

SeO2
4 g CAIII-300 + 2 g MgH2 + 2 g NaH + 2.2 g SeO2. Input energy (Ein) is 82.0 kJ. The output energy (dE) is 29.5 kJ. Excessive temperature rise (TSC) is 99-388 ° C. Maximum temperature (Tmax): 393 ° C. Theoretically 20.5kJ. Gain is 1.4 times.

CS2
• 1.2 g of CS2 in 1.0 gm NaH + (1.0 gm Al powder + 4 gm activated carbon CAII300) ball mill + PP vial. Input energy (Ein) is 72kJ. The output energy (dE) is 18 kJ. Temperature gradient jump is ~ 80 ° C. Maximum temperature (Tmax) to 320 ° C. In theory, it is 11.4kJ. Gain is 1.58 times.

1.0 gm NaH + 1.0 gm MgH2 powder + 4 gm activated carbon CAII300) 1.2 ml CS2 in a vial of ball mill + PP. Input energy (Ein) is 82 kJ. The output energy (dE) is 18 kJ. Temperature gradient jump is available at ~ 80 ° C. Maximum temperature (Tmax) to 330 ° C. Theoretically 12.6 kJ. Gain is 1.4 times.

CO2
4 g CAIII-300 + 1 g MgH 2 + 1 g NaH + 0.00953 mol CO 2 (cell temperature rises to 45 ° C. when CO 2 is met). Input energy (Ein) is 188.4kJ. The output energy (dE) is 10.37 kJ. There is a rapid temperature rise (TSC) at 80-120 ° C. Maximum temperature (Tmax): 508 ° C. 6.3 kJ in theory. Gain is 1.65 times.

PF5
4 g CAIII-300 + 1 g Al + 1 g NaH + 0.010 mol PF5. Input energy (Ein) is 127.0 kJ. The output energy (dE) is 15.65 kJ. There is a rapid temperature rise (TSC) at 210-371 ° C. Maximum temperature (Tmax): 371 ° C. 10kJ in theory. The excess is 6.45 kJ. Gain is 1.57 times.

4 g CAIII-300 + 1 g Al + 1 g NaH + 0.01 mol PF5. The input energy (Ein) is 101.0 kJ. The output energy (dE) is 15.7 kJ. Rapid increase in temperature (TSC) at 178-370 ° C. Maximum temperature (Tmax): 391 ° C. 10kJ in theory. Gain is 1.57 times.

NF3
1.0 gm NaH + (1.0 gm Mg powder + 4 gm activated carbon CAII-300) ball mill + 0.011 mole NF3. And the theoretical energy is ~ kJ). The input energy (Ein) is 136 kJ. The output energy (dE) is 28 kJ. Temperature gradient jump is 70 ° C. Maximum temperature (Tmax) to 470 ° C. Theoretically 19.6 kJ. Gain is 1.4 times.

PCl5
4 g CAIII-300 + 1 g MgH2 + 2.08 g PCl5 + 1 g NaH. Input energy (Ein) is 90.0 kJ. The output energy (dE) is 20.29 kJ. There is a rapid temperature rise (TSC) at 180-379 ° C. Maximum temperature (Tmax): 391 ° C. Theoretically, 13.92 kJ. Gain is 1.45 times.

P2S5
4 g CAIII-300 + 1 g MgH2 + 1 g NaH + 2.22 g P2S5. The input energy (Ein) is 105.0 kJ. The output energy (dE) is 13.79 kJ. There is a rapid temperature rise (TSC) at 150-363 ° C. Maximum temperature (Tmax): 398 ° C. Theoretically 10.5kJ. The excess is 3.3 kJ. Gain is 1.3 times.

1.0 gm NaH + 1.0 gm Al powder + 4 gm activated carbon CAII 300) Ball mill + 2.22 gm P2S5). The input energy (Ein) is 110 kJ. The output energy (dE) is 14 kJ. Temp. Slopejumpat-170 ° C with maximum temperature (Tmax)-425 ° C. Theoretically 10.1 kJ. Gain is 1.39 times.

Oxide
4 g AC + 1 g MgH2 + 1.66 g KH + 1.35 g KO2. Input energy (Ein) is 86.0 kJ. The output energy (dE) is 21.0 kJ. Rapid increase in temperature (TSC) at 157-408 ° C. Maximum temperature (Tmax): 416 ° C. Theoretically 15.4 kJ. Gain is 1.36 times.

MnO4
4 g CAIII-300 + 1 g Mg + 1 g NaH + 3.5 g MnO2. Input energy (Ein) is 108.0 kJ. The output energy (dE) is 22.11 kJ. Rapid increase in temperature (TSC) is 170-498 ° C. Maximum temperature (Tmax): 498 ° C. Theoretically, it is 18.4kJ. The excess is 3.7 kJ. Gain is 1.2 times.

N2O
4 g Pt / C + 1 g Mg + 1 g NaH + 0.0198 mol N2O. The input energy (Ein) is 72.0 kJ. The output energy (dE) is 22.2 kJ. Rapid increase in temperature (TSC) at 73-346 ° C. Maximum temperature (Tmax): 361 ° C. Theoretically, it is 16.2 kJ. Gain is 1.37 times.

HFB
1.0 gm NaH + ball milled (1 gm Aluminum nanopowder + 5 gm activated carbon (AC)) + 1 ml HFB. The input energy (Ein) is 108 kJ. The output energy (dE) is 35 kJ. 450 ° C temperature jump at 90 ° C.

1.0 gm NaH + ball milled (5 gm La + 5 gm activated carbon) +1 ml hexafluorobenzene. The input energy (Ein) is 109kJ. The output energy (dE) is 38 kJ. Temperature jump at 400 ° C is 90 ° C.

Ball milled (4 g activated carbon (AC) +1 g MgH ₂ ) +1 ml HFB + 1 g NaH. Input energy (Ein) is 150.0 kJ. The output energy (dE) is 45.1 kJ. Rapid rise in temperature (TSC) is present at ~ 50-240. Maximum temperature (Tmax) to 250 ° C.

Blend (4 g AC + 1 g MgH ₂ ) +1 ml HFB + 1 g NaH. Input energy (Ein) is 150.0 kJ. The output energy (dE) is 35.0 kJ. Rapid increase in temperature (TSC) at 54-255 ° C. 45-241 ° C., 48-199 ° C .; maximum temperature (Tmax): 258 ° C., 247 ° C., 206 ° C. (triple cell).

A mixture of 1.66 g KH, 1 ml hexadecafluoroheptane (HDFH), 4 g activated carbon powder, and 1 g MgH 2 in a 1 inch cell. The output energy (dE) is 34.3 kJ. The rapid rise in temperature is 419 ° C (145-564 ° C). Maximum temperature (Tmax) to 575 ° C.

B. Solution NMR
A typical reaction mixture for forming hydrinos includes (i) at least one catalyst such as one selected from LiH, KH, and NaH, and (ii) NiBr ₂ , MnI ₂ , AgCl, EuBr ₂ , At least one oxidizing agent such as one selected from SF ₆ , S, CF ₄ , NF ₃ , LiNO ₃ , M ₂ S ₂ O ₈ with Ag, and P ₂ O ₅ , and (iii) Mg powder, Or at least one reducing agent such as one selected from MgH ₂ , Al powder or aluminum nanopowder (AlNP), Sr and Ca, and (iv) one selected from AC and TiC And at least one support. 50 mg reaction product of the reaction mixture was added to 1.5 ml of deuterated N, N-dimethylformamide-d7 (DCON (CD ₃ ) ₂ , DMF-d7, (99.5%, Cambridge isotope) in a vial. This was sealed with a glass polytetrafluoroethylene (TEFLON®) valve, stirred, and dissolved in a glove box under an argon atmosphere for 12 hours. The solution in the absence of any solid was transferred to an NMR tube (outer diameter 5 mm, length 23 cm, manufactured by Wilmad) by a gas-tight connection, and the tube was sealed with a flame. Recorded on a 500 MHz Bruker NMR spectrometer (locked with deuterium). Relatively silane (TMS), referenced in a solvent frequencies such as DMF-d7 in 8.03Ppm.

The hydrino hydride ion H ⁻ (1/4) is expected to be observed at about −3.86 ppm, and the molecular hydrino H ₂ (1/4) is observed at 1.25 ppm compared to TMS. It was predicted. The location of the occurrence of these peaks due to the shift and the intensity for a particular reaction mixture are given in Table 4.

Claims (25)

A reaction cell for the catalysis of atomic hydrogen to form a hydrogen species having a total energy that is more stable and more negative than the non-catalytic hydrogen species and a composition comprising hydrogen species;
A reaction vessel;
A vacuum pump,
A source of atomic hydrogen from a source in communication with the reaction vessel;
A source of hydrogen catalyst in communication with the reaction vessel;
At least one source of the source of atomic hydrogen and the source of hydrogen catalyst comprises a reaction mixture comprising at least one reactant comprising an element that forms at least one of atomic hydrogen and a hydrogen catalyst and at least one other element. Wherein at least one of atomic hydrogen and a hydrogen catalyst is formed from the source,
At least one other reactant that causes catalysis by performing at least one function of activating and propagating the catalyst;
Initiating the formation of at least one of hydrogen catalyst and atomic hydrogen in the reaction vessel so that during hydrogen catalysis, atomic hydrogen releases energy in an amount greater than about 300 kJ per mole of hydrogen. A heater for the container that initiates the reaction that causes catalysis, and
A power source characterized by comprising: The reaction that causes the catalytic reaction
(i) an exothermic reaction that supplies activation energy for the catalytic reaction;
(ii) a conjugation reaction fed to at least one of a catalyst or a source of atomic hydrogen that supports the catalysis reaction;
(iii) a free radical reaction that functions as an electron acceptor from the catalyst during the catalysis reaction;
(iv) a redox reaction that functions as an electron acceptor from the catalyst during the catalysis reaction;
(v) an exchange reaction that accepts energy from atomic hydrogen to form the hydrogen species to facilitate the activity of the ionized catalyst; and
(vi) getter, support, matrix-assisted catalytic reaction,
The power source according to claim 1, comprising a reaction selected from:   2. A power source according to claim 1, wherein the reaction mixture comprises a conductive support so as to allow a catalytic reaction.   2. The power source according to claim 1, wherein the reaction mixture comprises a solid, liquid or heterogeneous catalytic reaction mixture. A reaction mixture comprising a redox reaction that causes a catalytic reaction,
(I) at least one catalyst selected from Li, LiH, K, KH, NaH, Rb, RbH, Cs, and CsH;
(Ii) H ₂ gas, a source of H ₂ gas, or a hydride;
(Iii) at least one oxidizing agent selected from:
Halide, phosphide, boride, oxide, hydroxide, silicide, nitrogen compound, arsenide, selenide, telluride, antimonide, carbide, sulfide, hydride, carbonate, bicarbonate, sulfate, sulfuric acid Hydrogen salt, phosphate, hydrogen phosphate, dihydrogen phosphate, nitrate, nitrite, permanganate, chlorate, perchlorate, chlorite, perchlorite, hypochlorite Acid salt, bromate, perbromate, perbromites, perbromites, iodate, periodate, iodoites, periodites, chromate, Dichromate, tellurate, selenate, arsenate, silicate, borate, cobalt oxide, tellurium oxide and halogen oxyanions, P, B, Si, N, As, S, Te, Sb, C, S, P, Mn, Cr, Co, and A metal compound comprising Te;
Transition metals, Sn, Ga, In, lead, germanium, alkali metals and alkaline earth metal compounds;
GeF ₂ , GeCl ₂ , GeBr ₂ , GeI ₂ , GeO, GeP, GeS, GeI ₄ , and GeCl ₄ , fluorocarbon, CF ₄ , ClCF ₃ , chlorocarbon, CCl ₄ , O ₂ , MHO ₃ , MClO ₄ , MO ₂ , NF ₃ , N ₂ O, NO, NO ₂ , boron-nitrogen compounds such as B ₃ N ₃ H ₆ , sulfur compounds such as SF ₆ , S, SO ₂ , SO ₃ , S ₂ O ₅ Cl ₂ , F ₅ SOF, M ₂ S ₂ O ₈ , S _x X _y , for example, S ₂ Cl ₂ , SCl ₂ , S ₂ Br ₂ , or S ₂ F ₂ , CS ₂ , SO _x X _y , SOCl ₂ , _{SOF 2, SO 2 F 2,} SOBr 2, X x X 'y, ClF 5, X x X' y O z, ClO 2 F, ClO 2 F 2, ClOF 3, ClO 3 F, ClO 2 F Boron - nitrogen _{compounds, B 3 N 3 H 6,} Se, Te, Bi, As, Sb, Bi, TeX x, TeF 4, TeF 6, TeO x, TeO 2, TeO 3, SeX x, SeF 6, SeO _x, SeO _2, or, SeO _3, tellurium oxide, halide, tellurium _{compounds, TeO 2, TeO 3, Te} (OH) 6, TeBr 2, TeCl 2, TeBr 4, TeCl 4, TeF 4, TeI 4, TeF _6, cote, or, NITE, selenium compounds, selenium oxide, halogenated selenium, selenium _{sulfide, SeO 2, SeO 3, Se} 2 Br 2, Se 2 Cl 2, SeBr 4, SeCl 4, SeF 4, SeF 6, SeOBr _{2, SeOCl 2, SeOF 2,} SeO 2 F 2, SeS 2, Se 2 S 6, Se 4 S 4, also _{, Se 6 S 2, P,} P 2 O 5, P 2 S 5, P x X y, PF 3, PCl 3, PBr 3, PI 3, PF 5, PCl 5, PBr 4 F, PCl 4 F, PO _{x X y, POBr 3, POI} 3, POCl 3, _{or, POF 3, PS x X y} , (M is an alkali metal .x, y, and, z is an integer .X and X 'is a halogen), pSBr _3, PSF ₃ , PSCl ₃ , nitrogen phosphite compound, P ₃ N ₅ , (Cl ₂ PN) ₃ , (Cl ₂ PN) ₄ , (Br ₂ PN) _x , arsenic compound, arsenic oxide, arsenic halide, arsenic sulfide , Arsenic selenide, arsenic telluride, AlAs, As ₂ I ₄ , As ₂ Se, As ₄ S ₄ , AsBr ₃ , AsCl ₃ , AsF ₃ , AsI ₃ , As ₂ O ₃ , As ₂ Se ₃ , As ₂ S _3, As _{2 e 3, AsCl 5, AsF 5} , As 2 O 5, As 2 Se 5, As 2 S 5, antimony compounds, antimony oxide, antimony halide, antimony sulfide, antimony sulfate, antimony selenide, antimony arsenide, _{SbAs, SbBr 3, SbCl 3,} SbF 3, SbI 3, Sb 2 O 3, SbOCl, Sb 2 Se 3, Sb 2 (SO4) 3, Sb 2 S 3, Sb 2 Te 3, Sb 2 O 4, SbCl 5 _{, SbF 5, SbCl 2 F 3} , Sb 2 O 5, Sb 2 S 5, bismuth compounds, bismuth oxide, halogenated bismuth, bismuth sulfide, bismuth _{selenide, BiAsO4, BiBr 3, BiCl 3} , BiF 3, BiF 5 _{, Bi (OH) 3, BiI} 3, Bi 2 O 3, BiOBr, BiO _{l, BiOI, Bi 2 Se 3} , Bi 2 S 3, Bi 2 Te 3, Bi 2 O 4, SiCl 4, SiBr 4, transition metal _{halides, CrCl 3, ZnF 2, ZnBr} 2, ZnI 2, MnCl 2, MnBr ₂ , MnI ₂ , CoBr ₂ , CoI ₂ , CoCl ₂ , NiCl ₂ , NiBr ₂ , NiF ₂ , FeF ₂ , FeCl ₂ , FeBr ₂ , FeCl ₃ , TiF ₃ , CuBr, CuBr ₂ , VF ₃ , CuCl ₂ , Metal halide, SnF ₂ , SnCl ₂ , SnBr ₂ , SnI ₂ , SnF ₄ , SnCl ₄ , SnBr ₄ , SnI ₄ , InF, InCl, InBr, InI, AgCl, AgI, AlF ₃ , AlBr ₃ , AlF ₃ , AlF ₃ , AlI _{3 3, CdCl 2, CdBr 2,} CdI 2, InCl 3, _{rCl 4, NbF 5, TaCl 5} , MoCl 3, MoCl 5, NbCl 5, AsCl 3, TiBr 4, SeCl 2, SeCl 4, InF 3, InCl 3, PbF 4, TeI 4, WCl 6, OsCl 3, GaCl 3 , PtCl ₃ , ReCl ₃ , RhCl ₃ , RuCl ₃ , metal oxide, metal hydroxide, Y ₂ O ₃ , FeO, Fe ₂ O ₃ , or NbO, NiO, Ni ₂ O ₃ , SnO, SnO ₂ , Ag ₂ O, AgO, Ga ₂ O, As ₂ O ₃ , SeO ₂ , TeO ₂ , In (OH) ₃ , Sn (OH) ₂ , In (OH) ₃ , Ga (OH) ₃ , Bi (OH) _{3 , CO 2, As 2 Se 3} , SF 6, S, SbF 3, CF 4, NF 3, metal _{permanganate, KMnO 4, NaMnO 4, P} 2 O ₅ , metal nitrate, LiNO ₃ , NaNO ₃ , KNO ₃ , boron halide, BBr ₃ , BI ₃ , Group 13 element halide, indium halide, InBr ₂ , InCl ₂ , InI ₃ , silver halide, AgCl, AgI, lead halide, cadmium halide, zirconium halide, transition metal oxide, transition metal sulfide, or transition metal halide (Sc, Ti, V, Cr, Mn, Fe, Co, Ni, Cu, or , Zn, F, Cl, Br, or I), second or third transition metal halide, YF ₃ , second or third transition metal oxide, second or third transition metal sulfide, Y _{2 S 3 ,, Y, Zr,} Nb, Mo, Tc, Ag, Cd, Hf, Ta, W, Os halides, _e.g., NBX 3, NBX _5, or, _TaX 5, _{i 2 S, ZnS, FeS,} NiS, MnS, Cu 2 S, CuS, SnS, alkaline earth _{halides, BaBr 2, BaCl 2, BaI} 2, SrBr 2, SrI 2, CaBr 2, CaI 2, MgBr 2, Or MgI ₂ , rare earth element halide, EuBr ₃ , LaF ₃ , LaBr ₃ , CeBr ₃ , GdF ₃ , GdBr ₃ , rare earth element halide, divalent metal, CeI ₂ , EuF ₂ , EuCl ₂ , EuBr _{2, EuI 2, DyI 2,} NdI 2, SmI 2, YbI 2, and, TmI _2, metal borides, europium boride, MB _{2 borides, CrB 2, TiB 2, MgB} 2, ZrB 2, GdB 2 , Alkali halides, LiCl, RbCl, or CsI, metal phosphides, such as Ca ₃ P ₂ , noble metal halide, noble metal oxide, noble metal sulfide, PtCl ₂ , PtBr ₂ , PtI ₂ , PtCl ₄ , PdCl ₂ , PbBr ₂ , PbI ₂ , rare earth element sulfide, CeS, La halide, Gd Halide, metal and anion, Na ₂ TeO ₄ , Na ₂ TeO ₃ , Co (CN) ₂ , CoSb, CoAs, Co ₂ P, CoO, CoSe, CoTe, NiSb, NiAs, NiSe, Ni ₂ Si, MgSe, rare earth Element telluride, EuTe, rare earth selenide, EuSe, rare earth nitrogen compound, EuN, metal nitride, AlN, GdN, Mg ₃ N ₂ , a compound containing at least two selected from oxygen and different halogen atoms, F _{2 O, Cl 2 O, ClO 2} , Cl 2 O 6, Cl 2 O 7, Cl _{, ClF 3, ClOF 3, ClF} 5, ClO 2 F, ClO 2 F 3, ClO 3 F, BrF 3, BrF5, I 2 O 5, IBr, ICl, ICl 3, IF, IF 3, IF 5, IF 7 , Second or third transition metal halide, OsF ₆ , PtF ₆ , or IrF ₆ , a compound that forms a metal by reduction, a metal hydride, a rare earth element hydride, an alkaline earth hydride, or an alkali hydride ;
(Iv) metals, alkalis, alkaline earths, transition metals, second and third transition metals, and rare earth metals, Al, Mg, MgH ₂ , Si, La, B, Zr, Ti powder, and H ₂ , at least one reducing agent selected from
(V) at least one electrically conductive support selected from AC, 1% Pt or Pd on carbon (Pt / C, Pd / C), carbides, TiC, and WC;
The power source of claim 2 comprising: A reaction mixture comprising a redox reaction that causes a catalytic reaction,
(I) at least one source or catalyst comprising a metal or hydride from a Group 1 element;
(Ii) at least one of a source of H ₂ gas or hydride, or a source of hydrogen containing H ₂ gas;
(Iii) selected from F, Cl, Br, I, B, C, N, O, Al, Si, P, S, Se, and Te; Group 13, Group 14, Group 15, Group 16 At least one oxidant comprising a compound, an ion or an atom comprising at least one of the elements from the group and group 17;
_{(iv) Mg, MgH 2,} Al, Si, B, Zr, and at least one reducing agent comprises a hydride or an element selected from rare earth metals; and
(v) at least one of electrically conductive supports selected from carbon, AC, graphene, metal-impregnated carbon, Pt / C, Pd / C, carbide, TiC, and WC;
The power source according to claim 2, comprising: The reaction mixture comprising a redox reaction to cause a catalysis reaction is (i) at least one of a catalyst or a source of catalysts comprising a metal or hydride from a Group 1 element;
(Ii) _{H 2} gas, or a source of _{H 2} gas, or, at least one source of hydrogen including hydrides. ;
(Iii) Group IA, IIA, 3d, 4d, 5d, 6d, 7d, 8d, 9d, 10d, 11d, 12d, and halides, oxides or sulfides of elements selected from lanthanides At least one of the oxidizing agents comprising:
_{(Iv) Mg, MgH 2,} Al, Si, B, Zr, and at least one reducing agent containing an element or hydride is selected from rare earth metals; and (v) carbon, AC, graphene, Pt / C Or at least one of electrically conductive supports selected from metal-impregnated carbon such as Pd / C, carbide, TiC, and WC;
The power source according to claim 2, comprising:   The exchange reaction that causes a catalytic reaction includes an anion exchange between at least two of the oxidant, the reducing agent, and the catalyst, where the anion is a halide, hydride, oxide, sulfide, nitrogen compound, Boride, carbide, silicide, arsenide, selenide, telluride, phosphide, nitrate, hydrogen sulfide, carbonate, sulfate, hydrogensulfate, phosphate, hydrogenphosphate, dihydrogenphosphate, perchlorine 3. Power source according to claim 2, characterized in that it is selected from acid salts, chromates, dichromates, cobalt oxides and oxyanions.   9. Power source according to claim 8, characterized in that the exchange reaction that causes catalysis is thermally reversible so as to regenerate the original exchange reaction. The thermally regenerated reactant is
(I) at least one catalyst or catalyst source selected from NaH and KH;
(Ii) a source of hydrogen selected from NaH, KH, and MgH ₂ ;
(Iii) at least one oxidizing agent _{(a) BaBr 2, BaCl 2} , BaI 2, CaBr 2, MgBr 2, and alkaline earth halide selected from MgI ₂ selected from the following;
_{(B) EuBr 2, EuBr 3} , EuF 3, DyI 2, LaF 3 and a rare earth halide selected from GdF _3;
(C) a second or third row transition metal halide selected from YF ₃ ;
(D) a metal boride selected from CrB ₂ and TiB ₂ ;
(E) an alkali halide selected from LiCl, RbCl, and CsI;
(F) a metal sulfide selected from Li ₂ S, ZnS, and Y ₂ S ₃ ;
(H) a metal oxide selected from Y ₂ O ₃ ;
(I) a metal phosphide selected from Ca ₃ P ₂ (iv) at least one reducing agent selected from Mg and MgH ₂ ; and (v) a support selected from AC, TiC and WC;
The power source according to claim 9, comprising:   A getter, support, or matrix-assisted catalysis reaction that causes a catalysis reaction provides at least one chemical environment for the catalysis reaction, moves electrons to promote H catalyst function Binding to the hydrogen species product so as to increase at least one of the rate or degree of catalysis reaction, through a reversible phase or other physical change or change in electronic state, The power source according to claim 2, comprising:   The power source of claim 11, wherein the getter, support, or matrix-assisted catalysis reaction can be thermally reversed to regenerate the initial exchange reactant. A getter, support, or matrix-assisted catalytic mixture
(I) at least one catalyst or catalyst source selected from NaH and KH;
(Ii) a source of hydrogen selected from NaH, KH, and MgH ₂ ;
(Iii) at least one oxidizing agent selected from the following two;
(A) a metal arsenide selected from Mg ₃ As ₂ ; and (b) a metal nitride selected from Mg ₃ N ₂ and AlN;
(Iv) at least one reducing agent selected from Mg and MgH ₂ ; and (v) at least one support selected from AC, TiC, and WC;
The power source of claim 12 comprising:   A reaction mixture that causes a catalytic reaction comprising a catalyst comprising an alkali metal is regenerated from the product by regenerating the alkali metal by electrolysis and separating one or more components. 1 power source. A reaction cell for the catalysis of atomic hydrogen to form a hydrogen species having a total energy that is more stable and more negative than the non-catalytic hydrogen species and a composition comprising hydrogen species;
A reaction vessel;
A vacuum pump,
A source of atomic hydrogen from a source in communication with the reaction vessel;
A source of hydrogen catalyst from a source in communication with the reaction vessel;
At least one source of the source of atomic hydrogen and the source of hydrogen catalyst comprises a reaction mixture comprising at least one reactant comprising an element that forms at least one of atomic hydrogen and a hydrogen catalyst and at least one other element. Wherein at least one of atomic hydrogen and a hydrogen catalyst is formed from the source,
At least one other reactant that causes catalysis by performing at least one function of activating and propagating the catalyst;
Initiating the formation of at least one of hydrogen catalyst and atomic hydrogen in the reaction vessel such that during hydrogen atom catalysis, atomic hydrogen releases energy in an amount greater than about 300 kJ per mole of hydrogen. A hydride reactor comprising: a heater for a vessel that initiates a reaction that causes catalysis. A reaction mixture for the synthesis of the compound is
(I)-(v): (i) a catalyst, (ii) a source of hydrogen, (iii) an oxidizing agent, (iv) a reducing agent, and (v) a support,
16. The hydride reactor of claim 15, comprising at least two selected from the genus. The oxidizing agent is sulfur, phosphorus, oxygen, SF ₆ , S, SO ₂ , SO ₃ , S ₂ O ₅ Cl ₂ , F ₅ SOF, M ₂ S ₂ O ₈ , S _x X _y S ₂ Cl ₂ , SCl _2. , S ₂ Br ₂ , S ₂ F ₂ , CS ₂ , Sb ₂ S ₅ , SO _x X _y , SOCl ₂ , SOF ₂ , SO ₂ F ₂ , SOBr ₂ , P, P ₂ O ₅ , P ₂ S ₅ , _{P x X y, PF 3,} PCl 3, PBr 3, PI 3, PF 5, PCl 5, PBr 4 F, PCl 4 F, PO x X y, POBr 3, POI 3, POCl 3, POF 3, PS x _{X y, pSBr 3, PSF 3} , PSCl 3, Rin nitrogen _{compounds, P 3 N 5, (Cl} 2 PN) 3, _{or, (Cl2PN) 4, (Br} 2 PN) x (M is an alkali metal .x and y integer .X is halogen.), O , _N 2 O, and, TeO _{2, halide, CF 4, NF 3, CrF} 2, a source of phosphorus, a source of sulfur, MgS, MHS (M is an alkali metal) claims characterized in that it is selected from Item 16. The hydride reactor according to item 16.   The reaction mixture is for catalyzed hydrogen and is selected from compounds containing the elements S, P, O, Se, and Te, as well as S, P, O, Se, and Te. The hydrogenation reactor according to claim 17, further comprising a getter. The catalyst is about 27.2 eV ± 0.5 eV and 27.2 / 2 eV. ± 2. The power source according to claim 1, wherein energy can be received from a hydrogen atom with one of 0.5 eV as an integer unit. When the catalyst contains atoms or ions M and t electrons are ionized from these atoms or ions M to a continuous energy level, the total ionization energy of t electrons is approximately m · 27.2 eV, where m is an integer. And m · 27.2 / 2 eV. 1. The power source according to claim 1. The catalyst contains the diatomic molecule MH, and the sum of the bond energy and the ionization energy of the t-electron is approximately m × 27.m in the MH bond breakage and the t-electron ionization from the atom M to the continuous energy level. 2. The power source according to claim 1, wherein the power source is 2 eV and m · 27.2 / 2 eV ₍ m is an integer). Catalyst, AlH, BiH, ClH, CoH , GeH, InH, NaH, RuH, SbH, SeH, SiH, SnH, C 2, N 2, O 2, CO 2, NO 2, and the molecules of NO _3, and , Li, Be, K, Ca, Ti, V, Cr, Mn, Fe, Co, Ni, Cu, Zn, As, Se, Kr, Rb, Sr, Nb, Mo, Pd, Sn, Te, Cs, Ce , Pr, Sm, Gd, Dy, Pb, Pt, Kr, 2K ⁺ , He ⁺ , Ti2 ⁺ , Na ⁺ , Rb ⁺ , Sr ⁺ , Fe3 ⁺ , Mo2 ⁺ , Mo4 ⁺ , In3 ⁺ , He ⁺ , Ar ⁺ The power source according to claim 1, comprising atoms, ions and / or molecules selected from:, Xe ⁺ , Ar ²⁺ and H ⁺ , and Ne ⁺ and H ⁺ atoms or ions.   The power source of claim 1, which is operated continuously so that power production and regeneration are maintained in synchrony using electrolysis or heat regeneration reactions.   The power source of claim 1 further comprising a power converter. The power source according to claim 24, wherein the converter comprises a steam generator in communication with the reaction vessel, a steam turbine in communication with the steam generator, and a power generator in communication with the steam turbine.

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