MX2011001061A

MX2011001061A - Heterogeneous hydrogen-catalyst reactor.

Info

Publication number: MX2011001061A
Application number: MX2011001061A
Authority: MX
Inventors: Randell L Mills
Original assignee: Blacklight Power Inc
Priority date: 2008-07-30
Filing date: 2009-07-29
Publication date: 2011-03-24
Also published as: CA2730712A1; AU2009276601B2; MX351888B; KR20110063745A; WO2010014684A8; WO2010014684A2; ZA201100321B; CN102164849A; CN102164849B; AP2011005548A0; WO2010014684A3; IL210844A0; EP2318307A2; BRPI0916743A2; US20110114075A1; KR101728176B1; EA201100279A1; EA031711B1; AU2009276601A1; AP3363A

Abstract

A power source and hydride reactor is provided comprising a reaction cell for the catalysis of atomic hydrogen to form hydrinos, a source of atomic hydrogen, a source of a hydrogen catalyst comprising a solid, liquid, or heterogeneous catalyst reaction mixture. The catalysis reaction is activated or initiated and propagated by one or more chemical other reactions. These reactions maintained on a electrically conductive support can be of several classes such as (i) exothermic reactions which provide the activation energy for the hydrino catalysis reaction, (ii) coupled reactions that provide for at least one of a source of catalyst or atomic hydrogen to support the hydrino catalyst reaction, (iii) free radical reactions that serve as an acceptor of electrons from the catalyst during the hydrino catalysis reaction, (iv) oxidation-reduction reactions that, in an embodiment, serve as an acceptor of electrons from the catalyst during the hydrino catalysis reaction, (v) exchange reactions such as anion exchange that facilitate the action of the catalyst to become ionized as it accepts energy from atomic hydrogen to form hydrinos, and (vi) getter, support, or matrix-assisted hydrino reaction that may provide at least one of a chemical environment for the hydrino reaction, act to transfer electrons to facilitate the H catalyst function, undergoes a reversible phase or other physical change or change in its electronic state, and binds a lower-energy hydrogen product to increase at least one of the extent or rate of the hydrino reaction. Power and chemical plants that can be operated continuously using electrolysis or thermal regeneration reactions maintained in synchrony with at least one of power and lower-energy-hydrogen chemical production.

Description

HYDROGEN REACTOR-CATHETER HETEROGÉNEO BRIEF DESCRIPTION OF THE MODALITIES REVEALED The present disclosure is concerned with catalyst systems comprising a hydrogen catalyst capable of causing the atomic H in its n = 1 state to form a lower energy state, a source. of atomic hydrogen and other species capable of initiating and propagating the reaction to form lower energy hydrogen. In certain embodiments, the present disclosure is concerned with a reaction mixture comprising. at least one source of atomic hydrogen and a catalyst or catalyst source to support the hydrogen catalysis to form hydrins. The reagents and reactions disclosed herein for solid and liquid fuels are also reactants and reactions of heterogeneous fuels comprising a mixture of phases. The reaction mixture comprises at least two chosen components of a hydrogen catalyst or source of hydrogen catalyst and a source of atomic hydrogen, wherein at least one of the atomic hydrogen and the hydrogen catalyst can be formed by a reaction of the reaction mixture. In further embodiments, the reaction mixture further comprises a support, which in certain embodiments can be electrically conductive, a solvent such as an organic solvent or inorganic solvent that includes a molten salt, a and at least one reagent which by virtue of suffering a reaction causes the catalysis to be active.

The reaction to form hydrinqs can be activated or initiated and propagated by one or more chemical reactions. These reactions can be chosen from (i) exothermic reactions, which provide the activation energy for the hydrino reaction, (ii) coupled reactions, which provide at least one of a catalyst source or atomic hydrogen to support the hydrino reaction , (iii) reactions of free radicals, which in certain embodiments serve as an electron acceptor of the catalyst during the hydrino reaction, (iv). oxidation-reduction reactions, which in certain embodiments serve as an electron acceptor of the catalyst during the hydrino reaction, (v) exchange reactions, such as anion exchange, in which halide, sulfide, hydride, arsenide, oxide, phosphide and nitride that in one modality facilitate the action of the catalyst to become ionized as it accepts energy from atomic hydrogen to form hydrines and (vi) hydrino reactions aided by the rarefactor, support or matrix, which provides at least one of a chemical environment for the hydrino reaction, act to transfer electrons to facilitate the function of the H catalyst, undergo a reversible phase change or other physical change or change in its electronic state and bind to a more energy hydrogen product low to increase at least one of the extent or speed of the hydrino reaction. In certain embodiments, the electrically conductive support enables the activation reaction.

In further embodiments, the present disclosure is concerned with an energy system comprising at least two components chosen from: a catalyst or catalyst source; atomic hydrogen or a source of atomic hydrogen; reagents to form the catalyst or. source of the catalyst and atomic hydrogen or a source of atomic hydrogen; one or more reagents for initiating atomic hydrogen catalysis and a support for enabling the catalyst, wherein the energy system may further comprise any of a reaction vessel, a vacuum pump, an energy converter and systems such as separator, an electrolyser, thermal systems to reverse an exchange reaction and chemical synthesis reactors to regenerate the fuel from the reaction products.

In further embodiments, the present disclosure is concerned with a system for forming compounds having hydrogen at lower energy states comprising at least two components chosen from: a catalyst or catalyst source; atomic hydrogen or a source of atomic hydrogen; reagents to form the catalyst or catalyst source and a source of atomic hydrogen or atomic hydrogen; one or more reagents for initiating atomic hydrogen catalysis and a support for enabling the catalyst, wherein the system for forming compounds having hydrogen at lower energy states may further comprise any one of a reaction vessel, a vacuum pump and systems such as separator systems, an electrolyser, thermal systems for reversing an exchange reaction and chemical synthesis reactors to regenerate the fuel from the reaction products.

Other embodiments of the present disclosure are concerned with a battery or fuel cell system for forming compounds having hydrogen in a lower energy state comprising at least two chosen components of: a. catalyst or catalyst source; atomic hydrogen or a source of atomic hydrogen; reagents to form the catalyst or source of the catalyst and atomic hydrogen or a source of atomic hydrogen; one or more reagents to start atomic hydrogen catalysis and a support to enable the catalyst, wherein the battery or fuel cell system for forming compounds having hydrogen in lower energy states can further comprise any of a reaction vessel, a vacuum pump and systems such as separator systems, an electrolyser, thermal systems for invest an exchange reaction and chemical synthesis reactors to regenerate the fuel from the reaction products.

BRIEF DESCRIPTION OF THE FIGURES Figure 1 is a schematic drawing of an energy reactor and power plant according to the present disclosure.

Figure 2 is a schematic drawing of an energy reactor and power plant for recycling or regenerating the fuel according to the present disclosure.

Figure 3 is a schematic drawing of an energy reactor according to the present disclosure.

Figure 4 is a schematic drawing of a system for recycling or regenerating fuel according to the present disclosure.

Figure 5 is a schematic drawing of a discharge and plasma and reactor energy cell according to the present disclosure.

Figure 6 is a schematic drawing of a battery and fuel cell according to the present disclosure.

DETAILED DESCRIPTION OF THE MODALITIES OF THE REVELATION The present disclosure is concerned with catalyst systems for releasing atomic hydrogen energy to form lower energy states, wherein the electron shell is in a closer position in relation to the core. The released energy is provided for the assimilation of energy and additionally new species of hydrogen and compounds are desirable products. These energy states are predicted by the laws of classical physics and require a catalyst to accept energy from hydrogen in order to undergo the corresponding energy release transition.

Classical physics gives closed-form solutions of the atom, of hydrogen, the hydride ion, the molecular ion of hydrogen, and the hydrogen molecule and predicts which corresponding species have major fractional quantum numbers. Using the Maxwell equations, the structure of the electron was derived as a. boundary-value problem where the electron comprises the source current of time-varying electromagnetic fields during transitions with the restriction that the linked n = 1 bound state electron can not radiate energy. A reaction predicted by the H atom solution involves a transfer of resonant non-radiating energy from atomic hydrogen otherwise stable to a catalyst capable of accepting energy to form hydrogen at lower energy states than previously. I thought possible. Specifically, classical physics predicts that atomic hydrogen can undergo a catalytic reaction with certain atoms, excimers, ions, and diatomic hydrides that provide a reaction with a net enthalpy of an integral multiple of atomic hydrogen potential energy, Eh = 27.2 eV in where Ehes a Hartree. Specific species (for example He +, Ar +, Sr +, K, Li, HC1, and NaH) identifiable. based on their known electronic energy levels they are required to be present with atomic hydrogen to catalyze the process. The reaction involves a transfer of non-radiant energy followed by continuous emission q. 13.6 eV or transfer of q. 13.6 eV to H to form H of extraordinarily hot excited state and a hydrogen atom that is lower energy than the unreacted atomic hydrogen corresponding to a fractional main quantum number. That is, in- the formula for the main energy levels of the hydrogen atom: «= 1,2,3, ... (2) where h is the radius Bohr for the hydrogen atom (52.947 pm), e is the magnitude of the charge of the electron and e? is the permissiveness to vacuum, fractional quantum numbers: where p = 137 is a whole number it replaces the well-known parameter n = integer in the Rydberg equation for the excited hydrogen states and represents hydrogen atoms of lower energy status called "hydrinos". The state n = · 1 of hydrogen and the hydrogen states are non-radioactive, without = ---: go a whole transition between two non-radioactive states, ie n = l a n = l / 2, is possible via a non-radiant energy transfer. Hydrogen is a special case of the stable states given by equations (1) and (3) where the corresponding radius of the hydrogen or hydrino atom is given by: P where p = 1, 2, 3, ... In order to conserve energy, the energy must be transferred from the hydrogen atom to the catalyst in units of an integer of the potential energy of the hydrogen atom in the n = state 1 normal and radio transitions to ---. Hydrinos are formed at m + p reacting an ordinary hydrogen atom with an appropriate catalyst having a net enthalpy of reaction of m. 27.2 eV (5) where m is a whole number. It is believed that the rate of catalysis is increased as the net enthalpy of the reaction is more closely matched to m. 27.2 eV. It has been found that catalysts that have a net enthalpy of reaction within. ± 10%, preferably ± 5%, of m. 27.2 eV are appropriate for most applications.

The reactions of the catalyst involve two energy release stages: a transfer of non-radiant energy to the catalyst followed by release of additional energy as the radius decreases to the corresponding stable end state. 'Thus, the general reaction is given by: m - 27.2 eV + Caf * + H? Cat. { q * '+ re + H m - 27.2 eV (6) H H + \ (P + mf-p2] - 13.6 eV-m- 27.2 eV (m + p) (8) Cat (q + r) + + re? Catq + + m - 27.2 eV the overall reaction is has the radius of the hydrogen atom (corresponding to 1 in the denominator) and a central field equivalent to (m + p) times that a proton and H (m + p) is the corresponding stable state with the radius of (m + p) that of H. As the electron undergoes radial acceleration of the radius of the hydrogen atom at a radius of - (m + p) distance, the energy is released as characteristic light emission or as third body kinetic energy. The emission may be in the form of an extreme ultraviolet continuous radiation that has an edge in and that extends to longer wavelengths. In addition to radiation, a transfer of resonant kinetic energy to form H fast can occur. The subsequent excitation of these fast H atoms (n = 1) or conditions with the background H2 followed by the emission of the corresponding fast H atoms (n = 3) gives rise to the extended Balmer emission. The extraordinary Balmer line widening (> 100 eV) is observed consistent with the predictions.

Therefore, an appropriate catalyst can provide a net positive reaction enthalpy of m. 27.2 eV. That is, the catalyst resonantly accepts the transfer of non-radiant energy from the hydrogen atoms and releases the energy to the surroundings to affect electronic transitions, at fractional quantum energy levels. As a consequence of the transfer of nonradiating energy, the hydrogen atom becomes unstable and emits additional energy until it obtains a non-radiating state of lower energy having a main energy level given by equations (1) and ( 3). Thus, catalysis releases energy from the hydrogen atom with a commensurate decrease in the size of the hydrogen atom, rn = naH where n is given by equation (3). For example, the catalysis of H (n = 1) to H (n = 1/4) releases 204 eV and the radius of hydrogen decreases from aH to 1/4 of aH. The product of the catalyst, H (1 / p), can also react with an electron to form a hydride hydride ion H "(1 / p) or two H (1 / p) can react to form the corresponding molecular hydrino H2 (1 p) . Specifically, the catalytic product, H (1 / p), can also react with an electron to form a new hydride ion H "(1 / p) with an EB bonding energy: where p = integer > 1, s = 1/2, ¾ is the Planck constant, μ0 is the permeability of the vacuum, rrie is the mass of the electron, μß is the reduced electronic mass given by where mp is the mass of the proton, a0 is the radius of Bohr and the ionic radius From equation (10), the calculated ionization energy of the hydride ion is 0.75418 eV and the experimental value is 6082.99 ± 0.15 cm "1 (0.75418 eV).

The NMR peaks displaced upward are direct evidence of the existence of lower energy state hydrogen with a reduced radius relative to the ordinary hydride ion and having an increase in the proton's diamagnetic shield. The displacement is given by the sum of that of an ordinary hydride ion H "and a component due to the lowest energy state: where for H p = 0 and p = integer > 1 for H (1 / p) and a is the fine structure constant.

H (1 / p) can react with a proton and two H (1 / p) can react to form H2 (1 / p) + and H2 (1 / p), respectively. The molecular hydrogen ion and molecular charge and current density functions, bond distances and energies are resolved from the Laplacian in ellipsoidal coordinates with the restriction of non-radiation. (7-0R ¿(R #)? -?) ?? A- (R É) +. { ? -?) ?? - (R.-) = 0. '? d? ? ?? ? d? ? 3? ? d? ? d? (12) The total energy? T of the molecular hydrogen ion having a central field of + pe in each focus of the molecular spherical orbital prolate is = - /? 216.13392 eV - 30.118755 eV where p is an integer, c is the speed of light in vacuum and μ is the reduced nuclear mass. The total energy of the hydrogen molecule that has a central field of + pe in each focus of the molecular spherical orbital prolate is 231. 35 leV-p * 0.326469 eV The bond dissociation energy ED (from the hydrogen molecule H2 (1 / p) is the difference between the total energy of the corresponding hydrogen atoms and ET ED = E (2H (1 lp)) - ET (15) where E (2H (1 / p)) = -p227.20 eV (16) ED is given by equations (15-16) (14) • ED = -p227.20 eV-ET = -p227.2 eV - (- p231351eV-p30.326469eV). (17) = / > 24,151 eV + p30.326469 eV The calculated and experimental parameters of H2, D2, H2 + and D2 + are given in Table 1.

Table 1. Parameters calculated experimentally Maxwellianay of H2, D2, H2 + and D2 +.

Calculated Experimental Parameter Ff link power, 4,478 cV 4,478 eV Link power of D-l 4.556 eV 4.556 eV Link power of / * 2.IS4 eV 2.651 eV Link power of Q * 2,696 eV 2,691 eV Total energy H-31,677 eV 31,675 eV Total energy) -, 31,760 eV. 31,760 «V FnpTgía tle ionization ff ^ 15,425 cV 15.426 «V Ionization energy £ > 2 15,463 cV 15-466 eV Ionization energy 16. 253 eV 16,250 eV Ionization energy £} * 16. 299 cV 16.294 eV Magnetic moment * 9.274 X W JT ~ X (μ ") 9.274 X WN JT" (μß Displacement of R N -28.0 ppm -28.0 ppMi in gas phase of M.}. absolute 0. 748 A 0,741 Distant rnuclear of H A Runtime distance of 0.741 A Rntemuclear distance of //, 1.06 A 3 1,058 Á Integral distance of D '1.0559 A 2 «0 Viral energy of f / z 0_S} 7 eV O.S I6 cV Braoonal energy of 0.371 eV 0.371 eV 120. 4 m '% 121.33 ew "' Dz &txt 60.93 cm i 61. &2 cm ~ l Vibrational energy of Hj 0.270 cV 0.271 cV Viral energy of 0.193 eV 0.196 eV 0. 0148 eV 0.01509 cV Rotational energy of Ja 1 to J = 0 J¾ Rotational energy of Ja] a J = ü 0.00741 eV 0.00755 eV Hj Rotational energy of Ja 1 to J = Q O.QQ740eV 0.00739 eV to Dj Rotational energy of Ja] a J = 0 0.00370 «V 0.003723 eV, Not corrected by the slight reduction in internuclear distance due to £. · The NMR of the catalyst gas - product provides a definitive proof of the theoretically predicted chemical shift of H2 (1/4). In general, the 1H NMR resonance of H2 (1 / p) is predicted to be upfield from that of H2 due to the fractional radius in elliptical coordinates, where the electrons are significantly closer to the nuclei. The predicted displacement, - AB for H2 (1 / p) is B given by the sum of that of H2 and a term that depends on p = integer > 1 for H2 (1 / p): where for H2 p = 0. The gaseous resonance displacement of experimental absolute H2 of -28.0 ppm is in excellent agreement with the predicted absolute gas phase shift of -28.01 ppm (equation 19).

The vibrational energies, Evib, for the transition from v = 0 to? = 1 of H2 hydrogen molecules (1 / p) are Evib = / > 20.515902 eV (20) where p is an integer. The rotational energies, Erot / for the transition from J to J + 1 of H2 hydrogen molecules (1 / p) are ? G0? =?, +? +?] =? 2 (? +1) 0.01509 eV (21) where p is an integer, I is the moment of inertia.

The dependence of p2 on the rotational energies results from an inverse p dependence of the internuclear distance and the corresponding impact on the moment of inertia I. The predicted internuclear distance 2c 'for H2 (1 / p) is 2c '= a ° ^, < 22 > P Data from a broad spectrum of research techniques strongly and consistently indicate that hydrogen can exist at a lower energy state than previously thought possible. These data support the existence of these lower energy states called hydrino, by "small hydrogen" and the corresponding hydride and hydrino molecular ions. Some of these previous related studies support the possibility of a new atomic hydrogen reaction, which produces hydrogen in fractional quantum states that are at lower energies than the traditional "basal" state (n = 1), include extreme ultraviolet spectroscopy (EUV) , characteristic emission of catalysts and hydride ion products, lower energy hydrogen emission, chemically formed plasmas, Balmer line widening, H line population reversal, high electron temperature, plasma phosphorescence duration anomalous, generation of energy and analysis of new chemical compounds.

The lower catalytic energy hydrogen transitions of the present disclosure require a catalyst which may be in the form of an endothermic chemical reaction of an integer m of the potential energy of the uncatalyzed atomic hydrogen, 27. 2 eV, which accepts the energy of atomic H to cause the transition. The endothermic catalytic reaction may be the ionization of one or more electrons of a species such as an atom or ion (for example m = 3 for Li? Li2 +) and may further comprise the concerted reaction of an ionization bond cleavage of one or more electrons from one or more partners of the initial bond (eg, m = 2 for NaH? Na2 + + H). He + satisfies the catalyst criterion - a chemical or physical process with an enthalpy change equal to an integer multiple of '27. 2 eV since it is ionized to 54. 417 eV, which is 2. 27 2 eV. Two hydrogen atoms can also serve as the catalyst for the same enthalpy. The hydrogen atoms H (1 / p) p = 1, 2, 3, .... 137 may undergo additional transitions to lower energy states given by equations (1) and (3), where the transition of an atom is catalyzed by a second that accepts resonant and not reactive m. 27 2 eV with a concomitant opposite change in its potential energy. The overall general equation for the transition from H (1 / p) to H (1 / (p + m)) induced by a resonance transfer of m. 27 2 eV to H (1 / p ') is represented by H (l / p ') + H (l / p)? H + H (l / (p + m)) + [2pm + m2-p + l] -13.6eV. (2. 3) Hydrogen atoms can serve as a catalyst where m = 1 and m = 2 for one and two atoms, respectively, which act as a catalyst to each other. The speed for the two-atom catalyst, 2H, can be high when extraordinarily fast H hits a molecule to form 2H, where two atoms accept resonant and non-reactive 54.4 eV of a third hydrogen atom from the partners. of collision.

With m = 2, the product of the catalysts is He + and 2H is H (1/3) which reacts rapidly to form H (1/4), then the molecular hydrino, H2 (1/4) as a preferred state. Specifically, in the case of a high concentration of hydrogen atom, the additional transition given by equation (23) of H (1/3) (p = 3) to H (l / 4) (p + m = 4 ) with H as the catalyst (p '= 1; m = 1) can be fast: H (l / 3) - H? H (1/4) +95.2 eV. (24) The corresponding molecular hydride H2 (1/4) and hydride hydride ion H "(1/4) are final products consistent with observation, since the quantum state p = 4 has a multi-polarity greater than that which a picture-pole that gives H (1/4) a long theoretical lifetime for additional catalysis.

The transfer of non-radioactive energy to the catalysts, He + and 2H is predicted to pump the energy levels of the He + ion and increase the electronic excitation temperature of H in helium-hydrogen and hydrogen plasmas, respectively. For both catalysts, the intermediary H * | _2 + 1_ equation (6) with m = 6) has the radius of the hydrogen atom (corresponding to 1 in the denominator) and a central field equivalent to three times that of a proton and to 3 is the corresponding stable state with the radius of 1/3 that of H. Since the electron undergoes radial acceleration of the * radius of the hydrogen atom at a radius of 1/3 of this distance, the energy is. released as characteristic light emission or as third body kinetic energy. The emission may be in the form of an extreme ultraviolet continuous radiation having an edge at 54.4 eV (22.8 nm) and extending to longer wavelengths. The emission may be in the form of an extreme ultraviolet continuous radiation having an edge at 54.4 eV (22.8 nm) and extending to longer wavelengths. Alternatively, the fast H is predicted due to a transfer of resonant kinetic energy. A secondary continuous band is predicted to arise from the subsequently rapid transition of the catalytic product (equations (4-7) and (23)) to the state where atomic hydrogen accepts 27.2 eV of Extreme ultraviolet spectroscopy (EUV) and high resolution visible spectroscopy were recorded in microwave discharges and helium pulsed and lightening discharges with hydrogen and hydrogen only providing the He + and 2H catalysts, respectively. The pumping of the He + ion line occurred with the addition of hydrogen and the excitation temperature of the hydrogen plasmas under certain conditions was very high. The EUV continuums at both 22.8 nm and 40.8 nm were observed and Balmer line a widening (> 50 eV) was observed. H2 (1/4) was observed by MR in solution at 1.25 ppm in gases collected from helium plasmas-hydrogen, hydrogen and hydrogen plasmas aided by water vapor and dissolved in CDC13.

Similarly, the reaction of Ar + to Ar2 + has a net reaction enthalpy of 27.63 eV, which is equivalent to m = 1 in equations (4-7). When Ar + served as the catalyst, its predicted 91.2 nm and 45.6 nm continuums were observed, as well as the other signature hydride transitions, pumping excited states of the catalyst, - H fast and predicted hydrogen hydride producer H2 ( 1/4) that was observed by NMR. in solution at 1.25 ppm. Considering these results and those of the helium plasmas, the continuous ones of q. 13.6 ev with thresholds at 54.4 eV (q = 4) and 40.8 eV (q = 3) for the He + catalyst and at 27.2 eV (q = 2) and 13.6 eV (q = 1) for the Ar + catalyst have been observed. Much higher values of q are possible with transitions from hydrinos to lower states giving rise 1 to continuous high energy radiation in a broad spectral region.

In studies of power generation and characterization of recent products, atomic lithium and molecular NaH served as catalysts, since they meet the criteria of the catalyst - a chemical or physical process with an enthalpy change equal to an integral multiple of m of the potential energy of atomic hydrogen, 27.2 eV (for example m = 3 for Li and m = 2 for NaH). Specific predictions based on closed-form equations for energy levels of the corresponding hydride hydride ions H "(1/4) of new new alkyl halide hydride hydride compounds (MH * X; M = Li or Na, X = halide) and hydrino molecular H2 (1/4) were tested using chemically generated catalyst reagents.

First, Li's catalyst was tested. Li and LiNH2 were used as a source of atomic lithium and hydrogen atoms. Using batch calorimetry, with water flow, the measured energy of 1 g Li, 0.5 g LiNH2, 10 g LiBr, and 15 g Pd / Al203 was give approximately 160 W with an energy balance of ?? = -19.1 kJ. The observed energy balance was 4.4 times the theoretical maximum based on the known chemistry. Next, Raney nickel (R-Ni) served as a dissociator when the energy reaction mixture was used in chemical synthesis, where LiBr acted as the catalyst of the catalytic product H (1/4) to form LiH * X as well as for trap H2 (1/4) in the crystal. The ToF-SIM showed LiH * X peaks. The MAS 1H NMRs of LiH * Br and LiH * 1 showed a distinct large upward field resonance at approximately - 2.5 ppm which coincided with H "(1/4) in one LiX matrix An NMR peak at 1.13 ppm coincided with H2 (1/4) interstitial and, the rotation frequency of H2 (1/4) of 42 times that of ordinary H2 was observed at 1989 cm "1 in the spectrum of FTIR. The XPS spectrum recorded in the LiH * Br crystals showed peaks at approximately 9.5 eV and 12.3 eV which could not be assigned to any known elements based on the absence of any other peaks of primary elements, but coincided with the binding energy of H ~ (1/4) in two chemical environments. An additional signature of the energy process was the observation of the formation of a plasma called a resonant transfer or rt plasma at low temperatures (for example * 103 K) and very low field strengths of approximately 1-2 V / cm when atomic Li it is present with atomic hydrogen. The time-dependent line broadening of the Balmer line a of H was observed corresponding to the extraordinarily fast H (> 40 eV).

A compound of the present disclosure such as MH comprising hydrogen and at least one M element other than hydrogen serves as a source of hydrogen and a catalyst source to form hydrins. A catalytic reaction is provided by the breaking of the bond. M - H plus the ionization of t electrons of the M atom, each at a continuous energy level, such that the sum of the bond energy and ionization energy of the t electrons is approximately m. 27.2 eV, where m is an integer. One such catalyst system involves sodium. The binding energy of NaH is 1.9245 eV and the first and second ionization energies of Na are 5.13908 eV and 47.2864 eV, respectively. Based on these energies, the NaH molecule can serve as a catalyst and source of H, since the binding energy of NaH plus the double ionization (t = 2) of Na to Na2 + is 54.35 eV (2.27.2 eV) . The catalytic reactions are given by: (25) 54. 35 eV + NaH? Na1 + + 2e ~ 4- H + [32-l2] 13.6 eV Na2 + + 2e ~ + H? NaH +54.35 eV. (26) And the global reaction is .

H? H + [3 -I2] · 13.6 eV. (27) The product ? (1/3) reacts quickly to form? (1/4), then molecular hydrino,? 2 (1/4), as a preferred state (equation (24)). The catalytic reactions of NaH can be concerted, since the sum of the NaH binding energy, the double ionization (t = 2) of Na to Na2 + and the potential energy of H is 81.56 eV- (3.27.2 eV) . The catalytic reactions are given by: 81. 56 eV + NaH + H? Na2 * + 2e ~ + H1"+ e ~ + H + (42-l2l-13.6e (28) M.2 ++ 2e - +. H + Hrá * pi.do + e "~> NaH + H +81.56 eV. (29) And the global reaction is' H? H + [42-l2] 13.6 eV, (30) where H + fast is a fast hydrogen atom, which has at least 13.6 eV of kinetic energy. H "(1/4) halide forms stable hydrides and is a favored product together with the corresponding molecule formed by the reactions 2H (1/4) - H2 (1/4) and H" (1/4) + H +? H2 (1/4) - Sodium hydride is commonly in the form of an ionic crystalline compound formed by the reaction of gaseous hydrogen with metallic sodium. Furthermore, in the gaseous state, sodium comprises covalent Na2 molecules with a binding energy of 74.8048 kJ / mol. It was found that when NaH (s) -was heated at a very slow temperature rise rate (0.1 ° C / min) under a helium atmosphere to form NaH (g), the predicted exothermic reaction given by the equations (25- 27) was observed at high temperature by differential scanning calorimetry (DSC). To obtain high energy, a chemical system was designed to greatly increase the amount and speed of formation of NaH (g). The reaction of NaOH and Na to Na20 and NaH (s) calculated from the heats of formation releases ?? = -44.7 kJ / mol NaOH: NaOH + 2Na? Na20 + NaH (s) ?? = -44.7 kJ / mol NaOH (31) This exothermic reaction can promote the formation of NaH (g) and was used to promote the very exothermic reaction given by the equations (25-27). The regenerative reaction in the presence of atomic hydrogen is Na20 + H? NaOH + Na ?? = '- 11.6 kJ / mol. of NaOH ^,) NaH? Na + H (l / 3) AH = -10,500 kJ / mol of H (33) Y NaH? Na + H (1/4) ?? = -19,700 kJ / mol of H. (34) NaH obtains, in a uniquely high kinetics since the catalytic reaction depends on the release of intrinsic H, which concomitantly undergoes the transition to form H (1/3) that reacts additionally to form H (1/4). High temperature differential scanning calorimetry (DSC) was performed on ionic NaH under a helium atmosphere at an extremely slow temperature rise rate (0.1 ° C / min) to increase the amount of molecular NaH formation. A new exothermic effect of -177 kJ / mol of NaH was observed in the temperature range of 640 ° C to 825 ° C. To obtain high potency, R-Ni having a surface area of about 100 m2 / g was coated on the surface with NaOH and reacted with Na metal to form NaH. Using batch calorimetry of water flow, the measured energy of 15 g of R-Ni was approximately 0.5 kW with an energy balance of ?? = -36 kJ compared to ?? «0 kJ of the R-Ni starting material, R-NiAl alloy when it reacts with the Na metal. The observed energy balance of NaH reaction was -1.6 X 104 KJ / mol H2, more than 66 times the combustion enthalpy of -241.8 KJ / mol H2. With an increase in the impurification of NaOH at 0.5% by weight, the Al of the intermetal R-Ni served to replace the Na metal as a reducer to generate the NaH catalyst. When heated to 60 ° C, 15 g of the composite catalytic material did not require additive to release 11.7 KJ of excess energy and. they developed the energy of 0.25 KW. The NMR in solution on gases dissolved in DMF-d7 showed H2 (1/4) at 1.2 ppm.

The ToF-SlM showed sodium hydride hydride, NaHx peaks. The NMR spectra of MAS from ?? of NaH * Br and NaH * Cl showed distinct large upward field resonance at -3.6 ppm and -4 ppm, respectively, which coincided with H "(1/4) and an NMR peak at 1.1 ppm coinciding with H2 ( 1/4) The NaH * Cl reaction of NaCl and the solid acid KHS04 as the sole source of hydrogen comprised two fractional hydrogen states.The NMR peak of H "'(1/4) was observed at -3.97 ppm and the peak of H "(1/3) was also present at -3.15 ppm The corresponding" peaks of H2 (1/4) and H2 (1/3) were observed at 1.15 ppm and 1.7 ppm, respectively. XH NMR of NaH * F dissolved in DMF-d7 showed H2 (1/4) and H "(1/4) at 1.2 ppm and -3.86 ppm, respectively, where the absence of any effect of solid matrix or possibly from alternative assignments confirmed solid NMR assignments The XPS spectrum recorded on NaH * Br showed the peaks of H "(1/4) at approximately 9.5 eV and 12.3 eV which coincided with the results of LiH * Br and KH * I; while the sodium hydride hydride showed two fractional hydrogen states that additionally have the XPS peak of H "(1/3) at 6 eV in the absence of a halide peak.The predicted rotational predictions have energies of 42 Sometimes those of the ordinary H2 were also observed from H2 (1/4) that was excited using an electron beam of 12.5 keV.

These data, such as RN displacement, ToF-SIM masses, XPS binding energies, FTIR and emission spectrum are characteristic of and identify hydrine products of the catalyst systems comprising an aspect of the present disclosure.

I. Hydrinos A hydrogen atom that has a binding energy given by: Link energy (35) wherein p is' an integer greater than 1, preferably from 2 to 137, is the product of the H catalysis reaction of the present disclosure. The binding energy of an atom, ion or molecule, also known as ionization energy, is the energy required to remove an electron from the atom, ion or molecule. A hydrogen atom having the bond energy given in equation (35) is hereinafter referred to as a "hydrino atom" or "hydrino". The designation for a radio hydrino P where aH is the radius of an ordinary hydrogen atom and p is an integer, is A hydrogen atom with a radius aH is subsequently referred to herein as "ordinary hydrogen atom" or "normal hydrogen atom". Ordinary atomic hydrogen is characterized by its binding energy of 13.6 eV.

Hydrins are formed by reacting an ordinary hydrogen atom with an appropriate catalyst. that has a net reaction enthalpy of m. 27.2 eV (36) where m is a whole number. It is believed that the rate of catalysis is increased as the net reaction enthalpy coincides m. 27.2 eV. It has been found that catalysts having a net reaction enthalpy within ± 10%, preferably ± 5% of m. 27.2 eV are appropriate for most applications.

This catalysis releases energy from the hydrogen atom with a commensurate decrease in the size of the hydrogen atom, rn = naH. For example, the catalysis of H (n = 1) to H (n = 1/2). Releases 40.8 eV and the radius of hydrogen decreases from aH to 1/2 of aH. A catalytic system is provided by the ionization of t electrons of an atom each at a continuous energy level, such that the sum of the ionization energies of the t electrons is approximately m. 27.2 eV where m is a whole number.

An additional example to such catalyst systems given supra (equations (6-9)) involves lithium metal. The first and second lithium ionization energies are 5.39172 eV and 75.64018 eV. The double ionization reaction '(t = 2) from Li to LI2 +, then, has a net reaction enthalpy of 81.0319 eV, which is equivalent to m = 3 in equation (36). 81. 0319 eV + Li (m) + H? Li2 + + 2e- + H + \ (P + 3f - p21-13.6 eV (+ 3) (37) Li2 + + 2e-? Li (m) + 81.0319 eV. (38) And the global reaction H + 3) 2 - / > 2] -13.6 eV (39) In another modality, the catalytic system involves cesium. The first and second cesium ionization energies are 3.89390 eV and 23.15745 eV, respectively. The double ionization reaction (t = 2) from Cs to Cs2 +, then, has a net reaction enthalpy of 27.05135 eV, which is equivalent to m = 1 in equation (36). (40) Cs2 + + 2e? Cs (m) + 27.05135 eV (41) And the global reaction is H An additional catalytic system involves the potassium metal. The first, second and third potassium ionization energies are 4.34066 eV, 31.63 eV, 45.806 eV, respectively. The triple ionization reaction (t = 3) from K to K3 +, then, has a net reaction enthalpy of 81.7767 eV, which is equivalent to m = 3 in equation (36). 81. 7767 eV + K (m) + H (43) ? AT (m) +81.7426 eV (44) And the global reaction is H H L (/ > + + f (/ > +3) 2 - 1-13.6 eV. 3). (Four. Five) As an energy source, the energy released during the catalysis is much greater than the energy lost to the catalyst. The energy released is great compared to conventional chemical reactions. For example, when hydrogen and oxygen gases undergo combustion to form water The enthalpy of known water formation is AHf = -286 KJ / mol or 1.48 eV per hydrogen atom. In contrast, each ordinary hydrogen atom (n - 1) undergoes catalysis liberates 40.8 eV net. In addition, additional catalytic transitions may occur: n l > -i, -l -i, l í 2 3 3 4 4 5 and so on. Once the catalysis begins, the hydrinos further self-catalyze in a process called de-provisioning. This mechanism is similar to that of an inorganic ion catalysis. However, hydrine catalysis must have a higher reaction rate than that of the inorganic ion catalyst due to the better coincidence of the enthalpy to m. 27.2 eV.

The hydride hydride ion of the present disclosure can be formed by the action of an electron source with a hydrino, that is, a hydrogen atom having a binding energy of about 13. 6 eV n where n = - P and p is an integer greater than 1. The hydride hydride ion is represented by H "(n = 1 / p) or H" (1 / p): H + e ~? H ~ (n = \ lp) (47) H + e ~? H - (\ lp). (48) The hydride hydride ion is distinguished from an ordinary hydride ion comprising an ordinary hydrogen nucleus and two electrons having a binding energy of about 0.8 eV. The latter is referred to herein as "ordinary hydride ion" or "normal hydride ion". The hydride hydride ion comprises a hydrogen nucleus that includes protein, deuterium or tritium and two electrons indistinguishable at a binding energy according to equations (49-50).

The binding energy of a hydride hydride ion can be represented by the following formula: Link energy (49) m: 1 + yJsjS + t) 8 / IA * P P where p is an integer greater than 1, s = 1/2, n is pi, h is the constant of 'Planck with bar, μ0 is the permeability of vacuum, me is the mass of the electron and is the mass of the electron reduced given by g p where, mp is the mass of the proton, aH is the radius of the hydrogen atom, a0 is a radius of Bohr and e is the elementary charge. The radios are given by The binding energies of the hydride hydride ion, H "(n = 1 / p) as a function of p, where p is a whole number, are given in Table 2.

Table 2. The binding energy representative of the hydride hydride ion H (n = 1 / p) as a function of p, equation (49).

Hydride ion A Bond energy Wavelength (eV) * > (nm) H ~ ("= 1) 1.8660 0-7542 1644 H ~ (n = l / 2) 0.9330 3047 406.9 fí- (fl = l / 3) 0.6220 6.610 187.6 H "(« = 1/4) 0.4665 11.23 110.4 H "(n = l / 5). 0.3732 16.70 74.23 H "(« = 1/7) 0.2666 29.34 42.25 fí "(« = 1/8) 0,2333 36.09 34.46 H "(« = 1/9) 0.2073 42.84 28.94 H "(« = 1/10) 0.1866 49.38 25.11 H ~ («= 1/11) 0.1696 55.50 22.34 H ~ (? = 1/12) 0.1555 60.98 20.33 - (rt = l / 13) 0.1435 65.63 18.89 ~ (? = 1/14) 0.1333 69.22 17.91 H- («= 1/15) 0.1244 71.55 17.33 H \ (? = 1 /? 6) 0,1166 72.40 17.12 H \ (n = l / 17) 0.1098 71.56 1733 \ (t = l / 18) 0.1037 68J3 18.01 H \ (? = 1/19) 0.0982 63.98 19.38 ?? («= L / 20) 0.0933 56.81 21.82 H \ (n = l / 2i) 0.0889 47.11 26.32 H. { (n = l / 22) 0.0848 34.66 35.76 H \ «= 1/23) 0.0811 19.26 64.36 ?? = l / 24) 0.0778 0.6945 1785 to Eq. (fifty) b Eq. (49) According to the present disclosure, a hydride hydride ion (H ~) having a binding energy according to equations (49-50) which is greater than the ordinary hydride ion bond (about 0.75 eV) for p = 2 to 23 and less for p = 24 (H ") is provided. ' For p = 2 ap = 24 of equations (49-50), the binding energies of the hydride ion are respectively 3, 6.6, 11.2, 16.7, 22.8 ', 29.3, 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 Exemplary compositions comprising the new hydride ion are also provided herein.

Exemplary compounds are also provided which comprise one or more hydride hydride ions and one or more other elements. Such a compound is referred to as "hydride hydride compound".

Ordinary hydrogen species are characterized by the following binding energies (a) hydride ion, 0.754 eV ("ordinary hydride ion"); (b) hydrogen atom ("ordinary hydrogen atom") 13.6 eV; (c) di-atomic hydrogen molecule, 15.3 eV ("ordinary hydrogen molecule"); (d) molecular hydrogen ion, 16.3 eV ("ordinary hydrogen molecular ion") and (e) H3 +, 22.6 eV ("ordinary tri-hydrogen molecular ion"). In the present, with reference to the forms of hydrogen, "normal" and "ordinary" are synonymous.

According to a further embodiment of the present disclosure, there is provided a compound comprising at least one hydrogen species of increased binding energy, such as (a) a hydrogen atom having a binding energy of about, 13. 6 ev 77 † "' P such as within a range of approximately 0.9 to 1.1 times 13. 6 eV where p is an integer number from 2 to 137; (b) a hydride ion (H ~) having a binding energy of approximately: Enlighten Energy = | a "3 «O3 P P such as within a range of approximately 0.9 to 1.1 times binding energy Link energy where p is an integer from 2 to 24; (c) H + (1 / p); (d) a tri-hydrino molecular ion H3 + (1 / p), which has a binding energy of about such as within a range of approximately 0.9 to 1.1 times 22.6 eV where p is an integer from 2 to 137; (e) a di-hydr that has a binding energy of about 15. 3 eV such as within a range of approximately 0.9 to 1.1 times 15-3 eV where p is an integer from 2 to 137; (f) a hydrino molecular ion with a binding energy of approximately such as within a range of approximately 0.9 to 1.1 times wherein p is an integer, preferably an integer from 2 to 137.

According to a further embodiment of the present disclosure, there is provided a compound comprising at least one hydrogen species of increased binding energy, such as (a) a hydrino-molecular ion having a total energy of about 216. 13392 ^ - s30.118755 eV such as inside, from an interval of approximately 0.9 to 1.1 times 216. 13392 eV - 30.118755 eV where p is an integer, h is Planck's constanté with bar, is the mass of the electron, c is the speed of light in vacuum and μ is the reduced nuclear mass and (b) a hydrinogen molecule that It has a total energy of approximately = -p231.351 eV - / > 30.326469 eV such as within a range of approximately 0.9 to 1.1 times = - 31.351 eV - p30.326469 eV where p is an integer and a0 is the radius of Bohr.

According to one embodiment of the present disclosure, wherein the compound comprises a hydrogen species of increased, negatively charged binding energy, the compound further comprises one or more cations, such as a proton, ordinary H 2+ or ordinary H 3 +.

A method is provided herein to prepare compounds comprising at least one hydride hydride ion. Such compounds are referred to herein as "hydride hydride compounds." The method comprises reacting atomic hydrogen with a catalyst having a net reaction enthalpy of about ^ - 27 eV, 2 wherein m is an integer greater than 1, preferably an integer less than 400, to produce a hydrogen atom of increased binding energy having a binding energy of about 13. 6 eV where p is an integer, preferably an integer from 2 to 137. An additional product of the catalysis is energy. The hydrogen atom of increased binding energy can be reacted with an electron source to produce an increased binding energy hydride ion. The hydride ion of increased binding energy can be reacted with one or more cations to produce a compound comprising at least one hydride ion of increased binding energy.

The new compositions of hydrogen matter may comprise: (a) at least one kind of neutral, positive or negative hydrogen (hereinafter referred to as the "hydrogen species of increased binding energy"), which has a binding energy: (i) greater than the binding energy of the corresponding ordinary hydrogen species or (ii) greater than the binding energy of any species of hydrogen for which the corresponding ordinary hydrogen species is unstable or is not observed because the binding energy of the ordinary hydrogen species is less than the thermal energy at conditions environmental (standard temperature and pressure, STP) or is negative and (b) at least one other element. The compounds of the present disclosure are referred to herein as "hydrogen compounds of increased binding energy".

"Another element" in "this context means an element different from a kind of hydrogen, of increased bonding energy. Thus, the 'other element can be a kind of ordinary hydrogen or any element other than hydrogen. In a group of compounds, the other element y. the increased hydrogen bonding species of hydrogen are neutral. In another group of compounds, the other element and the hydrogen species of increased binding energy are charged in such a way that the other element provides the charge equilibrium to form a neutral compound. The above group of compounds is characterized by molecular and coordinated bonding; the last group is characterized by ionic bonding.

New compounds and molecular ions are also provided which comprise: (a) at least one kind of neutral hydrogen, positive or negative (hereinafter, in the present "hydrogen species of increased binding energy") having a total energy: (i) greater than the total energy of the corresponding ordinary hydrogen species or (ii) greater than the total energy of any species of hydrogen for which the corresponding ordinary hydrogen species is unstable or is not observed because the total energy of the ordinary hydrogen species is less than the thermal energy at ambient conditions or it is negative and (b) at least one other element.

The total energy of the hydrogen species is the sum of the energies to remove all the electrons from the hydrogen species. The hydrogen species according to the present disclosure has a total energy greater than the total energy of the corresponding ordinary hydrogen species. The species of hydrogen that has a total energy increased according to the present disclosure is also referred to as a "hydrogen species of increased binding energy" although some embodiments of the hydrogen species having an increased total energy may have a first electron bond energy less than the first electron bond energy of the corresponding ordinary hydrogen species. For example, the hydride ion of equations (49-50) for p = 24 has a first binding energy that is smaller than the first binding energy of the ordinary hydride ion, while the total energy of the hydride ion of the equations (49-50) for p = 24 is much greater than the total energy of the corresponding ordinary hydride ion.

New compounds and molecular ions are also provided herein which comprise: (a) a neutral, positive or negative hydrogen species (hereinafter referred to as "hydrogen species of increased binding energy") having a binding energy: (i) greater than the binding energy of the corresponding ordinary hydrogen species or (ii) greater than the binding energy of any species of hydrogen for which the corresponding ordinary hydrogen species is unstable or is not observed because the binding energy of the ordinary hydrogen species is less than the thermal energy at conditions environmental or is negative and (b) optionally another element. The compounds of the present disclosure are referred to herein as "hydrogen compounds of increased binding energy".

The hydrogen species of increased binding energy can be formed by reacting one or more hydrino atoms with one or more than one. electron, hydrino atom, a compound containing at least one of the hydrogen species of increased binding energy and at least one other atom, molecule or ion other than a hydrogen species of increased binding energy.

Also provided are new compounds and molecular ions that comprise: (a) a plurality of neutral, positive or negative hydrogen species (hereinafter referred to as the "hydrogen species of increased binding energy") having a total energy: (i) greater than the total energy of the ordinary molecular hydrogen or (ii) greater than the total energy of any species of hydrogen for which the corresponding ordinary hydrogen species is unstable or is not observed because the total energy of the ordinary hydrogen species is less than the thermal energies at ambient conditions or is negative and (b) optionally another element. The compounds of the present disclosure are referred to herein as "hydrogen compounds of increased binding energy".

In one embodiment, a compound is provided comprising at least one hydrogen species of increased binding energy chosen from (a) a hydride ion having a binding energy in accordance with equations (49-50) that is greater than the bond of the ordinary hydride ion (approximately 0.8 eV) for p = 2 to 23 and lower for p = 24 ("increased binding energy hydride ion" or "hydride hydride ion"); (b) a hydrogen atom having a binding energy greater than the binding energy of the ordinary hydrogen atom (about 13.6 eV) ("hydrogen atom of increased binding energy" or "hydrino"); (c) a hydrogen molecule having a first binding energy greater than about 15.3 eV ("hydrogen molecule of increased binding energy" or "di-hydrino") and (d) a molecular hydrogen ion having an energy of binding greater than about 16.3 eV ("increased binding energy molecular hydrogen ion" or "di-hydrino molecular ion").

II. Reactor and power system According to another embodiment of the present disclosure, a hydrogen catalyst reactor is provided to produce a lower energy and hydrogen species of energy. As shown in Figure 1, a hydrogen catalyst reactor 70 comprises a vessel 72 containing an energy reaction mixture 74, a heat exchanger 80 and a power converter, such as a steam generator 82 and turbine 90 . In one embodiment, the catalysis involves reacting atomic hydrogen from the source 76 with the catalyst 78 to form "idrins" of lower energy hydrogen and producing power. The heat exchanger 80 absorbs the heat released by the catalysis reaction, when the reaction mixture, consisting of hydrogen and a catalyst, reacts to form hydrogen of lower energy. The heat exchanger exchanges heat with the steam generator 82 which absorbs heat from the exchanger 80 and produces steam. The power reactor 70 further comprises a turbine 90 which receives steam from the steam generator 82 and supplies mechanical energy to an energy generator 100 which converts the energy of the steam to electrical energy, which can be received by a load 110 to produce work or for dissipation.

In one embodiment, the energy reaction mixture 74 comprises any energy releasing material 76, such as a fuel supplied via the supply passage 62. The reaction mixture may comprise a source of hydrogen isotope atoms or a source of molecular hydrogen isotope and a source of catalyst 78 that resonantly remove approximately m. 27 2 eV to form low-energy atomic hydrogen, wherein m is an integer, preferably an integer less than 400, wherein the reaction to lower energy states of hydrogen occurs by contact of the hydrogen with the catalyst. The catalyst can be in the molten, liquid, gaseous or solid state. Catalysis releases energy in the form of heat and forms at least one of the lowest energy hydrogen isotope atom, lowest energy hydrogen molecule, hydride ions, and lower energy hydrogen compounds. Thus, the energy cell also comprises a lower energy hydrogen chemical reactor.

The hydrogen source can be hydrogen gas, water dissociation including thermal dissociation, water electrolysis, hydride hydrogen or hydrogen from metal-hydrogen solutions. In another embodiment, the molecular hydrogen of the energy releasing material 76 is dissociated into atomic hydrogen by a molecular hydrogen dissociation catalyst of the mixture 74. Such dissociation catalysts or dissociators can also absorb hydrogen, deuterium or atoms and / or molecules of tritium and include, for example, an element, compound, alloy or mixture of noble metals such as palladium and platinum, refractory metals such as molybdenum and tungsten, transition metals such as nickel and titanium, and internal transition metals such as niobium and zirconium. Preferably, the dissociant has a high surface area such as a noble metal such as Pt, Pd, Ru, Ir, Re or Rh, or Ni on Al203, SiO2 or combinations thereof.

In one embodiment, a catalyst is provided by the ionization of t electrons from an atom or ion at a continuous energy level, such that the sum of the ionization energies of the t electrons is approximately m »27.2 eV where t and m they are each a whole number. A catalyst can also be provided by the transfer of t electrons between the participating ions. The transfer of t electrons from one ion to another ion provides a net reaction enthalpy, whereby the sum of the t ionization energies of the electron donor ion minus the ionization energies of t electrons of the electron acceptor ion is equal to approximately m »21.2 eV where t and m are each a whole number. In another embodiment, the catalyst comprises MH such as NaH having a Vf atom bound to hydrogen, and the enthalpy of m «27.2 eV is provided by the sum of the MH bond energy and the ionization energies of the t electrons .

In one embodiment, a catalyst source comprises a catalytic material 78 supplied through the catalyst supply passage 61, which commonly provides a net enthalpy of approximately. + -. 2.e.sup.-eV plus or minus 1 eV. The catalysts comprise atoms, ions, molecules, and hydrinoids that accept atomic hydrogen energy and hydrinos.

In some embodiments, the catalyst may comprise at least one chosen species of molecules of AlH, BiH, ClH, CoH, GeH, InH, NaH, RuH, SbH, SeH, SiH, SnH, C2, N2 02, C02, N02 and NO3 and atoms or ions of 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 +, ln3 +, He +, Ar +, Xe +, Ar2 + and H +, and Ne + and H +.

In one embodiment of an energy system, the heat is removed by a heat exchanger having a heat exchange medium. The heat exchanger can be a wall of water and the medium can be water. The heat can be transferred directly for heating space and process. Alternatively, the heat exchanger means such as water undergoes a phase change such as steam conversion. This conversion can occur in a steam generator. The steam can be used to generate electricity in a heat engine such as a steam turbine and a generator.

One embodiment of a reactor producing hydrogen species of hydrogen energy and of lower energy 5, for recycling or regeneration of fuel according to the present disclosure, is shown in Figure 2 and comprises a kettle 10 containing a fuel reaction mixture 11 which can be a mixture of a source of hydrogen, a source of catalyst, and optionally a solvent that can be vaporized, a source of hydrogen 12, steam tubes and steam generator 13, a converter of energy such as a turbine 14, a water condenser 16, a water compensation source 17, a fuel recycler 18, and a hydrogen-dihydrine gas separator 19. In Step 1, the fuel, such as one that is gaseous, liquid, solid or a heterogeneous mixture comprising multiple phases, comprising a source of catalyst and a source of hydrogen It reacts to form hydrinos and lower energy hydrogen products. In Step 2, the spent fuel is reprocessed to re-supply the kettle 10 to maintain the generation of thermal energy. The heat generated in the boiler 10 forms steam in the tubes and steam generator 13 which is fed to the turbine 14 which in turn generates electricity by energizing a generator. In Step 3, the water is condensed by the water condenser 16. Any water loss can be compensated by the water source 17 to complete the cycle to maintain the conversion of thermal to electrical energy. In Step 4, the lower energy hydrogen products such as hydride hydride compounds and dihydride gas can be removed, and the unreacted hydrogen can be returned to the fuel recycler 18 or hydrogen source 12 to be re-added to spent fuel to compensate for the recycled fuel. The unreacted gas and hydrogen products can be separated by. the hydrogen-dihydrine gas separator 19.

Any hydride hydride compounds produced can be separated and removed using the fuel recycler 18. Processing can be done in the boiler or externally to the boiler with the returned fuel. Thus, the system can also comprise at least one of gas and mass conveyors to move the reactants and products to achieve the removal, regeneration and re-supply of spent fuel. Hydrogen compensation for that exhausted in hydrine formation is added from source 12 during fuel reprocessing and may involve recycled hydrogen, without consuming. The recycled fuel maintains the production of thermal energy to drive the power plant to generate electricity.

The reactor can operate in a continuous mode with the addition of hydrogen and with separation and addition or replacement to counteract the minimal degradation of the reactants. Alternatively, the fuel that reacted is continuously regenerated from the products. In one embodiment of the latter scheme, the reaction mixture comprises species that can generate atomic or molecular catalyst reagents and atomic hydrogen which additionally reacts to form hydrins, and the produced species formed by the generation of catalyst and atomic hydrogen can be regenerated by at least the step of reacting the products with hydrogen. In one embodiment, the reactor comprises a moving bed reactor which may further comprise a fluidized reactor section, wherein reagents are continuously supplied and byproducts are removed and regenerated and returned to the reactor. In one embodiment, lower energy hydrogen products such as hydride hydride compounds or dihydrine molecules are collected as the reagents are regenerated. In addition, the hydride hydride ions can be formed to other compounds or converted to dihydrine molecules during the regeneration of the reactants.

The reactor may further comprise a separator for separating components from a mixture of products such as by evaporation of the solvent if one is present. The separator may comprise, for example, screens to be mechanically separated by differences in physical properties such as size. The separator can also be a separator that takes advantage of differences in density of the component of the mixture, such as a cyclone separator. For example, at least two of the chosen carbon groups, a metal such as Eu, and an inorganic product such as KBr can be separated based on differences in density in an appropriate medium medium, such as forced inert gas and also by centrifugal forces. The separation of the components can also be based on the differential of the dielectric constant and load capacity.

For example, the carbon can be separated from the metal based on the application of an electrostatic charge to the first one with removal of the mixture by an electric field. In the case that one or more components of a mixture are magnetic, the separation can be obtained using magnets. The mixture can be stirred on a series of strong magnets alone or in combination with one or more screens to cause at least one base separation of the adhesion or attraction of the magnetic particles to the magnet and a difference in size of the two kinds of particles. In one embodiment of the use of sieves and an applied magnetic field, the latter adds an additional force to that of gravity to attract the smaller magnetic particles through the sieve while the other particles of the mixture retained on the sieve due to its largest size.

The reactor may further comprise a separator for separating one or more components based on a differential phase change or reaction. In one embodiment, the phase change comprises fusion using a heater, Y. the liquid is separated from the solid by methods known in the art such as filtration by gravity, filtration using a pressurized gas assist, centrifugation, and by applying vacuum. The reaction may comprise decomposition such as hydride decomposition or reaction to form a hydride, and separations may be obtained by melting the corresponding metal followed by its separation and by mechanically separating the hydride powder, respectively. The latter can be obtained by sieving In one embodiment, the phase change or reaction can produce a desired or intermediate reagent. In certain embodiments, the regeneration includes any separation steps that may occur inside or outside the reactor.

Other methods known to those skilled in the art may be applied to the separations of the present disclosure by application of routine experimentation. In general, the mechanical separations can be divided into four groups: sedimentation, centrifugal separation, filtration and sieving. In one embodiment, the separation of the particles is obtained by at least one screening and use of classifiers. The size and shape of the particles can be chosen in the starting materials to obtain the desired separation of the products.

The power system may further comprise a catalytic condenser to maintain the vapor pressure of the catalyst by a temperature control which controls the temperature of the surface to a value lower than that of the reaction cell. The surface temperature is maintained at a desired value which provides the desired vapor pressure of the catalyst. In one embodiment, the catalytic condenser is a grid of tubes in the cells. In an embodiment with a heat exchanger, the flow rate of the heat transfer medium can be controlled at a rate that keeps the condenser at the desired lower temperature than the main heat exchanger. In one embodiment, the working medium is water and the flow rate is higher in the condenser than the water wall such that the condenser is at the lowest desired temperature. Separate streams of the working medium can be recombined and transferred for space and process heating or for steam conversion.

The cells of the present disclosure comprise the catalysts, mixtures, reaction, methods and systems disclosed herein wherein the particular cell serves as a reactor and at least one component for activating, initiating, propagating and / or maintaining the reaction and regenerating the reagents. According to the present disclosure, the cells comprise by. at least one catalyst or catalyst source, at least one source of atomic hydrogen and one container. The cells and systems for their operation are known to those skilled in the art. The electrolytic cell energy reactor such as eutectic salt electrolysis cell, plasma electrolysis reactor, barrier electrode reactor, RF plasma reactor, pressurized gas energy reactor, gas discharge energy reactor, preferably pulsed discharge and more preferably discharge of pulsed pressed plasma, microwave cell energy reactor, and a combination of a brightness discharge cell and a microwave reactor and / or RF plasma reactor of the present disclosure comprises: a source of hydrogen; one of a solid, molten, liquid, gaseous and heterogeneous source of catalyst or reagents in any of these states to cause the hydrino reaction by a reaction between the reactants; a reagent container or at least one containing hydrogen and the catalyst wherein the reaction to form lower energy hydrogen occurs by hydrogen contact with the catalyst or by reaction of the MH catalyst; and optionally a component for removing the lower energy hydrogen product. In one embodiment, the reaction to form lower energy state hydrogen is facilitated by an oxidation reaction. The oxidation reaction can increase the reaction rate to form hydrinos by at least one of accepting electrons from the catalyst and neutralizing the highly charged cation formed by accepting atomic hydrogen energy. Thus, these cells can be put into operation in a way that provides such oxidation reaction. In one embodiment, the electrolysis or plasma cell can provide an oxidation reaction at the anode, wherein the hydrogen provided by a method such as bubbling and catalyst react to form hydrinos via the participant oxidation reaction.

In a liquid fuel mode, the cell is operated at a temperature where the decomposition rate of the solvent is negligible with respect to the energy to regenerate it in relation to the energy of the cell. In the case that the temperature is below that at which a satisfactory efficiency of energy conversion can be obtained by more conventional methods, such as those using a steam cycle, a working medium of boiling point can be used. lower. In another embodiment, the temperature of the working medium can be increased using a heat pump. Thus, the heating of space and process can be supplied using the energy cell that operates at a temperature above the ambient, where. a working medium is increased in temperature with a component such as a heat pump. With sufficient temperature rise, a phase transition from liquid to gas can occur, and the gas can be used for volume pressure (PV) work. PV's work can include energizing a generator to produce electricity. Then, the medium can be condensed and the condensed working medium can be returned to the reactor cell to be reheated and recirculated in the cycle or power loop.

In one embodiment of the reactor, a heterogeneous catalyst mixture comprising a liquid phase and a solid phase is flowed through the reactor. The flow can be obtained by pumping. The mixture can be a suspension. The mixture can be heated in a hot zone to cause catalysis of hydrogen to hydrinos to release heat to maintain the hot zone. The products can be made to flow out. The heat zone and the reagent mixture can be regenerated from the products. In another embodiment, at least one solid of a heterogeneous mixture can be flowed into the reactor by gravity feed. A solvent can be made to flow to the reactor separately or in combination with one or more solids. The reagent mixture may comprise at least one of the group of a dissociator, a high surface area material (HSA), R-Ni, Ni, NaH, Na, NaOH, and a solvent.

In one embodiment, one or more reagents, preferably a source of halogen, halogen gas, oxygen source or solvent, are injected into a mixture of the other reagents. The injection is controlled to optimize the excess energy and energy of the hydrine formation reaction. The temperature of the cell in the injection and speed of injection. Can be controlled to obtain the optimization. Other process and mixing parameters can be controlled for further optimization using methods known to those experienced in the art of process design.

For energy conversion, each type of cell can be interconnected with any of the known converters of thermal energy or plasma a. mechanical or electrical energy including, for example, a heat engine, steam or gas turbine system, Sterling motor or thermionic or thermoelectric converters. Additional plasma converters comprise the magnetic mirror magnetohydrodynamic energy converter, plasmadynamic energy converter, gyrotron, photon stacking microwave energy converter, charge displacement energy or photoelectric converter. In one embodiment, the cell comprises at least one cylinder of an internal combustion engine.

III. Hydrogen Gas Cell and Solid Fuel Reactor, Liquid and Heterogeneous In accordance with one embodiment of the present disclosure, a reactor for producing hydrines and energy can take the form of a reactor cell. A reactor of the present disclosure is shown in Figure 3. The reactive hydrins are provided by a catalytic reaction with the catalyst. Catalysis can occur in the gas phase or in the solid or liquid state.

The reactor of Figure 3 comprises a reaction vessel 207 having a chamber 200 capable of containing a vacuum or pressures greater than atmospheric. A source of hydrogen 221 communicating with the chamber 200 feeds hydrogen into the chamber through the hydrogen supply passage 242. A controller 222 is positioned to control the pressure and flow of hydrogen to the container through the hydrogen supply passage. 242. A pressure detector 223 monitors the pressure in the container. A vacuum pump 256 is used to evacuate the chamber through a vacuum line 257.

In one embodiment, the catalysis occurs in the gas phase. The catalyst can be made gaseous by maintaining the temperature of the cell at an elevated temperature which, in turn, determines the vapor pressure of the catalyst. The atomic and / or molecular hydrogen reagent is also maintained at a desired pressure that can be in any pressure range. In one embodiment, the pressure is less than atmospheric, preferably in the range of about 10 millitorricelis to about 100 Torr. In another embodiment, the pressure is determined by maintaining a source mixture of the catalyst, such as a metal furnace and the corresponding hydride, such as a metal hydride in the cell maintained at the desired operating temperature.

A suitable catalyst source 250 for generating hydrino atoms can be placed in a reservoir of the catalyst 295, and the gaseous catalyst can be formed by heating. The reaction vessel 207 has a catalyst supply passage 241 for the passage of the gaseous catalyst from the catalyst tank 295 into the reaction chamber 200. Alternatively, the catalyst can be placed in a chemically resistant open vessel, such as a canister, inside the reaction vessel.

The source of hydrogen can be hydrogen gas and molecular hydrogen. The 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), precious or noble metals and a precious or noble metal on a support. The precious or noble metal can be Pt, Pd, Ru, Ir, and Rh, and the support can be at least one of Ti, b, AI2O3, SiO2 and combinations thereof. Additional dissociators are Pt or Pd on carbon which may comprise a hydrogen spill catalyst, nickel fiber mat, Pd sheet, Ti sponge, Pt or Pd electrodeposited on Ti or Ni sponge, TiH, Pt black, and Pd black, refractory metals such as molybdenum and tungsten, transition metals such as nickel and titanium, internal transition metals such as niobium and zirconium, and other such materials known to those skilled in the art. In one embodiment, the hydrogen is dissociated over Pt or Pd. The Pt or Pd can be coated on a support material such as titanium or Al203. In another embodiment, the dissociator is a refractory metal such as tungsten or molybdenum, and the dissociation material can be maintained at an elevated temperature by the temperature control component 230, which can take the form of a heating coil as shown in FIG. cross section in Figure 3. The heating coil is energized by a power source 225. Preferably, the dissociation material is maintained at the operating temperature of the cell. The catalyst can be operated further at a temperature above the temperature of the cell to dissociate more effectively, and the elevated temperature can prevent the catalyst from condensing on the dissociator. The hydrogen dissociator may also be provided by a hot filament such as 280 energized by the power source 285.

In one embodiment, the dissociation of hydrogen occurs in such a manner that the dissociated hydrogen atoms are brought into contact with the gaseous catalyst to produce hydrino atoms. The vapor pressure of the catalyst is maintained at the desired pressure by controlling the temperature of the catalyst tank 295 with a heater from the catalyst tank 298 energized by the power source 272. When the catalyst is contained in a canister inside the reactor, the vapor pressure of the catalyst is maintained at the desired value by controlling the temperature of the catalyst canister, by adjusting the power source of the canister. The temperature of the cell can be controlled at the desired operating temperature by the heating coil 230 which is energized by the power source 225. The cell (called a permeation cell) can further comprise an internal reaction chamber 200 and an external hydrogen tank 290, in such a way that the hydrogen can be supplied to the cell by diffusion of hydrogen through the wall 291 that separates the two chambers. The temperature of the wall can be controlled with a heater to control the speed of diffusion. The diffusion rate can be further controlled by controlling the hydrogen pressure in the hydrogen tank.

To maintain the catalyst pressure at the desired level, the cell having permeation as the source of hydrogen can be sealed. Alternatively, the cell further comprises high temperature valves at each inlet or outlet, such that the valve that contacting the reaction gas mixture is maintained at the desired temperature. The cell may further comprise a rarefactor or trap 255 for selectively collecting the lower energy hydrogen species and / or hydrogen compounds of increased binding energy and may further comprise a selective valve 206 for releasing the dihydrino gas product.

In one embodiment, reagents such as the solid fuel or heterogeneous catalyst fuel mixture 260 are reacted in vessel 200 by heating with heaters 230. Such an additional added reagent. as at least one of an exothermic reagent, which preferably has rapid kinetics, can be flowed to cell 200 through control valve 232 and connection 233. The added reagent can be a source of halogen, halogen, source of oxygen, . or solvent. Reagent 260 may comprise a species that reacts with the added reagent. A halogen can be added to form a halide with reagent 260 or an oxygen source can be added to reagent 260 to form an oxide, for example.

The catalyst may be at least one of the group of lithium, potassium or atomic cesium, molecule of NaH, 2H and hydrino atoms, wherein the catalysis comprises a dismutation reaction. The lithium catalyst can be made gaseous by maintaining the temperature of the cell in approximately the range of 500-1000 ° C. Preferably, the cell is maintained in the range of about 500-750 ° C. The cell pressure can be maintained at less than atmospheric pressure, preferably in the range of about 10 millitor to about 100 millimeter. More preferably, at least one of the catalyst and hydrogen pressure is determined by maintaining a mixture of catalytic metal and the corresponding hydride such as lithium and lithium hydride, potassium hydride and potassium hydride, sodium and sodium hydride, and cesium and cesium hydride in the cell maintained at the desired operating temperature. The gas phase catalyst may comprise lithium atoms of the metal or a source of lithium metal. Preferably, the lithium catalyst is maintained at the pressure determined by a mixture of lithium metal and lithium hydride at the operating temperature range of about 500-1000 ° C and more preferably, the pressure with the cell at the temperature range of : operation of approximately 500-750 ° C. In other modalities, K, Cs and Na replace the Li, where the catalyst is atomic K, atomic Cs and molecular NaH.

In a gas cell reactor embodiment comprising a catalyst or canister reservoir, gaseous Na, NaH catalyst, or gaseous catalyst such as Li, K and Cs vapor is maintained in a superheated condition in the cell in relation to the steam in the tank or boat that is the steam source of the cell. In one embodiment, the superheated vapor reduces the condensation of the catalyst on the hydrogen dissociator or the dissociator of at least one of metal and metal hydride molecules disclosed infra. In a mode comprising Li as the catalyst of a tank or canister, the tank or canister is maintained at a temperature at which Li vaporizes. The H2 can be maintained at a pressure that is lower than that which forms a significant mole fraction of LiH at the tank temperature. The pressures and temperatures that obtain this condition can be determined from the graphs of data of the pressure of H2 against the mole fraction of LiH to given isotherms that are known in the art. In one embodiment, the reaction chamber of the cell containing a dissociator is put into operation at a higher temperature, in such a way that the Li does not condense on the walls or the dissociator. The H2 can flow from the reservoir to the cell to increase the transport rate of the catalyst. The flow such as from the catalyst deposit to the cell and then out of the cell is a method to remove the hydrino product to prevent inhibiting the hydrino product from the reaction. In other modalities, K, Cs and Na replace Li where the catalyst is atomic K, atomic Cs and molecular NaH.

Hydrogen is supplied to the reaction of a source of hydrogen. For example, hydrogen is supplied by permeation of a hydrogen deposit. The pressure of the hydrogen tank can be in the range of 10 Torr to 10,000 Torr, preferably 100 Torr to 1000 Torr, and more preferably around atmospheric pressure., The cell can be put into operation in the temperature range of about 100. ° C to 3000 ° C, preferably in the temperature range of about 100 ° C to 1500 ° C, and more preferably in the temperature range of about 500 ° C to 800 ° C.

The hydrogen source can be from the decomposition of an added hydride. A cell design that delivers H2 by permeation is one that comprises an internal metal hydride placed in a sealed container, where the atomic H permeates at high temperature. The container may comprise Pd, Ni, Ti or N. In one embodiment, the hydride is placed in a sealed tube, such as an Nb tube containing a hydride and sealed at both ends with seals such as upset closures. In the sealed case, the hydride could be an alkaline or alkaline earth hydride. Alternatively, in this, also as in the case of the internal hydride reagent, the hydride could be at least one of the group of saline hydrides, titanium hydride, vanadium, niobium, and hydrides of tantalum, zirconium and hafnium hydrides, hydrides of rare earths, yttrium and scandium hydride, transition element hydrides, intermetallic hydrides, and their alloys.

In one embodiment, the hydride and the operating temperature of ± 200 ° C, based on each hydride decomposition temperature, is chosen from at least one of the list of: a rare earth hydride with an operating temperature of about 800 ° C; lanthanum hydride with an operating temperature of approximately 700 ° C; gadolinium hydride with an operating temperature of about 750 ° C; Neodymium hydride with an operating temperature of about 750 ° C; yttrium hydride with an operating temperature of about 800 ° C; scandium hydride with an operating temperature of approximately 800 ° C; ytterbium hydride with an operating temperature of about 850-900 ° C; titanium hydride with an operating temperature of approximately 450 ° C; cerium hydride with an operating temperature of approximately 950 ° C; praseodymium hydride with an operating temperature of approximately 700 ° C; zirconium-titanium hydride (50% / 50%) with an operating temperature of approximately 600 ° C; an alkali metal / alkali metal hydride mixture such as Rb / RbH or K / KH with an operating temperature of about 450 ° C; and a mixture of alkaline earth metal / alkaline earth metal hydride such as Ba / BaH2 at an operating temperature of about 900-1000 ° C.

Gaseous metals can comprise diatomic covalent molecules. An objective of the present disclosure is to provide an atomic catalyst such as Li also as K and Cs-. Thus, the reactor may further comprise a dissociator of at least one of metal molecules ("MM") and metal hydride ("MH") molecules. Preferably, the source of the catalyst, the source of H 2, and the dissociator of MM, MH, and HH, where M 'is the atomic catalyst, are matched to be put into operation at the desired cell conditions of temperature and concentrations of reactive, for example. In the case that a source of H2 hydride is used, in one embodiment, its decomposition temperature is at. the temperature range that produces the desired vapor pressure of the catalyst. In case the source of hydrogen is permeation of a hydrogen deposit to the reaction chamber, preferred sources of catalysts for continuous operation are metals of Sr and Li since each of their vapor pressures may be in the range desired from 0.01 to 100 Torr at the temperatures for which the permeation occurs. In other embodiments of the permeation cell, the cell is operated at a high permissive permeation temperature, then the cell temperature is lowered to a temperature that maintains the vapor pressure of the volatile catalyst at the desired pressure.

In one embodiment of a gas cell, a dissociator comprises a component for generating the catalyst and H of the sources. Surface catalysts such as Pt on Ti or Pd, iridium or rhodium alone or on a substrate such as Ti can also serve for the role of dissociating molecules of catalyst combinations and hydrogen atoms. Preferably, the dissociator has a high surface area such as Pt / Al203 or Pd / Al203.

The source of H2 can also be H2 gas. In this mode, the pressure can be monitored and controlled. This is possible with the catalyst and catalyst sources such as K or metal of Cs and LiNH2, respectively, since they are volatile at low temperature which is permissive to use a high temperature valve. The Li H2 also lowers the necessary operating temperature of the Li cell and is less corrosive which is permissive of long-term operation using a feed in the case of the plasma and filament cells where a filament serves. as a hydrogen dissociator.

Additional embodiments of the gas cell hydrogen reactor having NaH as the catalyst comprise a filament with a dissociator in the reactor cell and Na in the reservoir. The H2 can be flowed through the reservoir to the main chamber. The energy can be controlled by controlling the gas flow velocity, H2 pressure, and Na vapor pressure. The latter can be controlled by controlling the tank temperature. In another embodiment, the hydrino reaction is initiated by heating with the external heater and atomic H is provided by a dissociator.

The reaction mixture can be stirred by methods known in the art such as mechanical stirring or mixing. The agitation system may comprise one or more piezoelectric transducers. Each piezoelectric transducer can provide ultrasonic agitation. The reaction cell can be. further vibrating and containing stirring elements such as stainless steel balls or tungsten which are vibrated to stir the reaction mixture. In another embodiment, the mechanical agitation comprises ball mill. The reagent can also be mixed using these methods, preferably by ball mill: In one embodiment, the catalyst is formed by mechanical agitation such as, for example, at least one of vibration with stirring elements, ultrasonic agitation, and ball mill. The mechanical impact or compression of sound waves such as ultrasound can cause a reaction or a physical change in the reagents to cause catalyst formation, preferably NaH molecules. The reagent mixture may or may not comprise a solvent. The reactants can be solids such as solid NaH which is mechanically stirred to form NaH molecules. Alternatively, the reaction mixture may comprise a liquid. The mixture can have at least one Na species. The Na species can be a component of a liquid mixture, or it can be in solution. In one embodiment, the sodium metal is dispersed by high-speed stirring of a suspension of the metal in a solvent such as an ether, hydrocarbon, fluorinated hydrocarbon, aromatic sol or heterocyclic aromatic solvent. The temperature of the solvent can be maintained just above the melting point of the metal.

IV. Types of Fuels One embodiment of the present disclosure is concerned with a fuel comprising a reaction mixture of at least one source of hydrogen and a source of catalyst to support the catalysis of hydrogen to form hydrins in at least one of gaseous, liquid and solid of a possible mixture of phases. The reagents and reactions given herein for solid and liquid fuels are also reactants and reactions of heterogeneous fuels comprising a mixture of phases.

An objective of the present disclosure is to provide atomic catalysts. such as Li also as K and Cs and NaH molecular catalyst. Metals form diatomic covalent molecules. Thus, in forms of solid fuels, liquid fuels and heterogeneous fuels, the reactants comprise alloys, complexes, sources of complexes, mixtures, suspensions and solutions that can be reversibly formed with a metal M catalyst and decomposed or reacted to provide such a catalyst. as Li or NaH. In another embodiment, at least one of the catalyst source and source of atomic hydrogen further comprises at least one reagent that reacts to form at least one of the catalyst and atomic hydrogen. In another embodiment, the reaction mixture comprises a NaH catalyst or a source of NaH catalyst or another catalyst such as Li or K which can be formed via the reaction of one or more reactants or species of the reaction mixture or can be form through a physical transformation. The transformation can be solvation with an appropriate solvent.

The reaction mixture may further comprise a solid to support the catalysis reaction on a surface. The catalyst or a catalyst source such as NaH can be coated on the surface. The coating can be obtained by mixing a support such as activated carbon, Tic, WC, R-Ni with NaH by methods such as ball mill grinding. The reaction mixture may comprise a heterogeneous catalyst or a heterogeneous catalyst source. In one embodiment, the catalyst such as NaH is coated on the support such as activated carbon, Tic, WC or a polymer by the incipient wetting method, preferably by using an aprotic solvent such as an ether. The support can also comprise an inorganic compound such as an alkaline halide, preferably at least one of NaF and HNaF2 wherein NaH serves as the catalyst and a fluorinated solvent is used.

In one embodiment of a liquid fuel, the reaction mixture comprises at least one of a catalyst source, a catalyst, a source of hydrogen and a solvent for the catalyst. In other embodiments, the present disclosure of a solid fuel and a liquid fuel further comprises combinations of both and also comprises gaseous phases as well. Catalysis with reagents, such as the catalyst and atomic hydrogen and sources thereof in multiple phases is called a heterogeneous reaction mixture and the fuel is called a heterogeneous fuel. Thus, the fuel comprises a reaction mixture of at least one source of hydrogen to undergo transition to hydrinos, states given by Equation (35), and a catalyst to cause the transitions having the reactants in at least one of liquid, solid and gaseous phase. Catalysis with the catalyst at a different stage from the reactants is generally known in the art as heterogeneous catalysis which is a modality of the present disclosure. The heterogeneous catalysts provide a surface for the chemical reaction to take place and comprise embodiments of the present disclosure. The reagents and reactions given herein for solid and liquid fuels are also reactants and heterogeneous fuel reactions.

For any fuel of the present disclosure, the catalyst or catalyst source such as NaH can be mixed with other components of the reaction mixture, such as a support such as HSA material by methods such as mechanical mixing or by ball milling. In all cases additional hydrogen can be added to maintain the reaction to form hydrinos. The hydrogen gas can be at any desired pressure, preferably in the range of 0.1 to 200 atm. Alternative sources of hydrogen comprise at least one of the group of NH4X (X is an anion, preferably a halide), NaBH4, NaAlH4, a borane, and a metal hydride such as an alkali metal hydride, alkaline earth metal hydride, preferably MgH2, and a rare earth metal hydride, preferably LaH2 and GdH2.

A. Support In certain embodiments, the solid, liquid and heterogeneous fuels of the present disclosure comprise a support. The support comprises specific properties for its function. For example, in the case where the support functions as an electron analyzer or conduit, the support is preferably conductive. Additionally, in the case that the support disperses the reagents, the support preferably has a high surface area. In the first case, the support such as an HSA support may comprise a conductive polymer such as activated carbon, graphene, and heterocyclic polycyclic aromatic hydrocarbons which may be macromolecular. The carbon may preferably comprise activated carbon (AC), but may also comprise other forms such as mesoporous carbon, glassy carbon, coke, graphite carbon, carbon with a dissociating metal such as Pt or Can, wherein the weight percent is 0.1 to 5 weight percent, transition metal powders preferably having from one to ten layers of carbon and more preferably three layers, and one carbon coated with metal or alloy, preferably nanopowder, such as a transition metal, preferably per the least carbon coated with Ni, Co and Mn. A metal can be intercalated with carbon. In the case that the intercalated metal is Na and the catalyst is NaH, preferably the intercalation of Na is saturated. Preferably, the support has a high surface area. Common classes of organic conductive polymers that can serve as the support are at least one of the group of poly (acetylene) s, poly (pyrrole) s, poly (thiophenes), poly (anilines) s, poly (fluorenes) s, poly (3-alkylthiophene) s, polytetrathiafulvalenes, polinaphthalenes, poly (p-phenylene sulfide), and poly (para-phenylene vinylene) s. These linear base chain polymers are commonly known in the art as polyacetylene, polyaniline, etc. "blacks" or "melanins". The support can be a mixed copolymer such as one of polyacetylene, polypyrrole and polyaniline. Preferably, the conductive polymer carrier is at least one commonly derived from polyacetylene, polyaniline and pilipyrrole. Another support comprises other elements than carbon such as the polythiazyl conducting polymer ((S-N) x).

In another modality, the support is a semiconductor. The support can be an element of Column IV such as carbon, silicon, germanium and alpha-gray tin. In addition to elemental materials such as silicon and germanium, the semiconductor support comprises a composite material such as gallium arsenide and indium phosphide or alloys such as silicon germanium or aluminum arsenide. Conduction in materials such as silicon and germanium crystals can be improved in one embodiment by adding small amounts (eg, 1-10 parts per million) of dopants such as boron or phosphorus as the crystals are grown. The doped semiconductor can be ground to a powder to serve as a support.

In certain embodiments, the HSA support is a metal such as a transition metal, noble metal, intermetallic, rare earth, actinide, lanthanide, preferably one of La, Pr, Nd, and Sm, Al, Ga, In, Ti, Sn, Pb ,, metalloids, Si, Ge, As, Sb, Te, Y, Zr, Nb, Mo, Te, Ru, Rh, Pd, Ag, Cd, Hf, Ta, W, Re, Os, Go, Pt , Au, Hg, alkali metal, alkaline earth metal, and an alloy comprising at least two metals or elements of this group such as a lanthanide alloy, preferably LaNi5 and Y-Ni. The support can 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).

In other embodiments, the HSA material comprises at least one of cubic boron nitride, hexagonal boron nitride, boron nitride powder of wurtzite, heterodiame, boron nitride nanotubes, silicon nitride, aluminum nitride, titanium nitride (TiN), titanium aluminum nitride (TiAlN), tungsten nitride, a metal or alloy, preferably nano-powder, coated with carbon 'such as at least one of Co, Ni, Fe, Mn and other powders of transition metals preferably having one to ten layers of carbon and more preferably three layers, carbon coated with metal or alloy, preferably nanopowder, such as a transition metal preferably at least one carbon coated with Ni, Co and Mn, a carbide, preferably a powder, beryllium oxide powder (BeO), rare earth oxide powder such as La2C >; 3, Zr203, 'AI2O3, sodium aluminate, and carbon such as fullerene, graphene or nanotubes, preferably single-walled.

The carbide may comprise one or more of the. linkage types: salt-like such as calcium carbide (CaC2), covalent compounds such as silicon carbide (SiC) and boron carbide (B4C or BC3), and interstitial compounds such as tungsten carbide. The carbide can be an acetylide such as Au2C2, ZnC2 and CdC2 or a methanide such as Be2C, aluminum carbide (Al4C3), and carbides of the type A3MC, where A is mostly a rare earth metal or transition metal such as Se, Y, La-Na, Gd-Lu, and M is an element of the metallic or semi-metallic main group such as Al, Ge, In, Ti, Sn and Pb. The carbide having C22 ~ ions can comprise at least one of the M12C2 carbides with the cation M1 comprising an alkali metal or one of the coining metals, M2 C2 carbides with the cation M11 comprising an alkaline earth metal, and preferably carbides? 21? 1 (C2) 3 with the cation M111 comprising Al, La, Pr, or Tb. The carbide may comprise an ion other than C22 ~ such as those from the group of YC2, TbC2 > YbC2, UC2, Ce2C3, Pr2C3 and Tb2C3. The carbide may comprise a sesquicarbide such as Mg2C3, SC3C4 and LÍ4C3. The carbide may comprise a tertiary carbide such as those containing lanthanide metals and transition metals which may further comprise C2 units such as Ln3M (C¿) 2, wherein M is Fe, Co, Ni, Ru, Rh, Os and Ir, Dy12Mn5Ci5, Ln3.'67FeC6, Ln3Mn (C2) 2 (Ln = Gd and Tb), and ScCrC2. The carbide can also be of the "intermediate" transition metal carbide classification such as iron carbide (Fe3C or FeC2: Fe). The carbide may be at least one of the group of lanthanides (MC2 and M2C3) such as lanthanum carbide (LaC2 or La2C3), yttrium carbide, carbides, actinide, transition metal carbides such as scandium carbide, carbide titanium (TiC), vanadium carbide, chromium carbide, manganese carbide and cobalt carbide, niobium carbide, molybdenum carbide, tantalum carbide, zirconium carbide, and hafnium carbide. Additional suitable carbides comprise at least one of Ln2FeG4, Sc3CoC4, Ln3MC4 (M = Fe, Co, Ni, Ru, Rh, Os, Ir), Ln3Mn2C6, Eu3.i6NiC6, ScCrC2, Th2NiC2, Y2ReC2, Lni2M5Ci5 (M = Mn, Re), YCoC, Y2ReC2, and other carbides known in the art.

In one embodiment, the support is an electrically conductive carbide such as TiC or WC and HfC, Mo2C, TaC, YC2, ZrC, Al c3 and B4C. The support can be a metal boride such as MB2 borides inclusive. The support or material of HSA can be a boride, preferably a two-dimensional network boride which can be conductive such as MB2 where M is a metal such as at least one of Cr, Ti, Mg, Zr and Gd (CrB2, TiB2 , gB2, ZrB2, GdB2).

In a modality of carbon HSA material, Na does not intercalate to carbon support or form an acetylide by reacting with carbon. In one embodiment, the catalyst or catalyst source, preferably NaH, is incorporated into the interior of the HSA material such as fullerene, nanotubes. of carbon and zeolite. The HSA material may further comprise graphite, graphene, diamond-like carbon (DLC), hydrogenated diamond-like carbon (HDLC), diamond powder, graphite carbon, glassy carbon, and carbon with other metals such as at least one of Co, Ni, Mn, Fe, Y, Pd and Pt, or impurifiers comprising other elements such as fluorinated carbon, preferably fluorinated graphite, fluorinated diamond or tetracarbon fluoride (C4F).

Preferably the metals are a mixture of such a mixture of Co, 'Ni, Mn. The metals can be in any proportion of weight percent. Preferably, the composition and proportions of percent by weight (%) are about 20 to 25% Ni, 60% to 70% Co, and 5 to 15% Mn. The HSA material can be passivated by fluoride such as metal or carbon coated with fluoride or comprise a fluoride such as a metal fluoride, preferably an alkaline fluoride or alkaline earth fluoride.

In another embodiment, the support has a pore size or interlayer spacing that will accommodate only a catalyst radius such as the atomic radius in the case of Li or K and. the molecular dimensions in the case of NaH. In the case of Li, the pore size or inter-layer spacing is ideally between about 1.35 A and 3 A. In the case of K, the pore size or inter-layer spacing is ideally between about 1.1 A and 3.5A. In the case of NaH, the pore size or inter-layer spacing is ideally between about 1.5 A and 5 A. In one embodiment, the support provides an atomic catalyst such as Li or K and single catalyst molecules such as as NaH based on discrimination and size selection. A suitable support having a large surface area and an interlayer separation distance of about 25 Á is activated carbon. Activated carbon can be activated or reactivated by physical or chemical activation. The first activation may comprise carbonization or oxidation, and the last activation may comprise impregnation with chemicals.

The reaction mixture may further comprise a support such as a polymeric support. The polymeric support can be chosen from poly (tetrafluoroethylene) such as TEFLON ™, polyvinyl ferrocene, polystyrene, polypropylene, polyethylene, polyisoprene, poly (aminophosphazene), a polymer comprising ether units such as polyethylene glycol or polyethylene oxide and polypropylene glycol or polypropylene, preferably aryl ether, a polyether polyol such as poly (tetramethylene ether) glycol (PTMEG, polytetrahydrofuran, "tetene", "polyTHF"), polyvinyl formal, and those from the reaction of epoxides such as polyethylene oxide and polypropylene oxide. In one embodiment, the HSA comprises fluorine. Exemplary fluorinated HSAs are TEFLON ™, TEFLON ™ -PFA, polyvinyl fluoride, PVF, poly (vinylidene fluoride), poly (vinylidene-co-hexafluoropropylene fluoride), and perfluoroalkoxy polymers. | B. Solid Fuels The solid fuel comprises a catalyst or catalyst source to form hydrins, such as at least one catalyst chosen from LiH, Li, NaH, Na, KH, K, RbH, Rb, and CsH, a source of atomic hydrogen, and others solid chemical reagents that perform one or more of the following functions (i) the reactants form the catalyst or atomic hydrogen by undergoing a reaction such as one between one or more components of the reaction mixture or undergoing a physical or chemical change of at least one component of the reaction mixture and (ii) the reactants initiate, propagate and maintain the catalysis reaction to form hydrinos. The many examples of solid fuels given in the present disclosure include reaction mixtures of liquid fuels comprising a solvent, except with the exception of the solvent not intended to be exhaustive. Based on the present disclosure, other reaction mixtures are taught to those skilled in the art.

In a solid fuel embodiment, the reaction mixture comprises a catalyst, a source of hydrogen and at least one of a HSA support, a rarefactor, a dispersant, and an inert gas. The catalyst can be NaH. The inert gas can be at least one of a noble gas and nitrogen. Preferably the inert gas is a mixture of Ne and N2, more. preferably, the mixture is. of approximately 50% Ne and 50% N2. The pressure may preferably be in the range of about 1 Torr to 100 atmospheres. Preferred ementer, the pressure of the Ne-N2 mixture is from one atmosphere. The reaction temperature is preferably in the range of about 100 ° to 900 ° C. The reaction mixture may further comprise at least one of Na and NaOH, and additionally a reductant such as NaH, Sn, Zn, Fe, and an alkali metal. In the event that the reaction mixture comprises NaOH, preferably H2 is also supplied and H2 comprises a gas of any mixture in the event that the reaction mixture comprises one or more inert gas. The hydrogen source may comprise hydrogen or a hydride and a dissociator such as Pt / Ti, PtATi in hydride, Pd, Pt, or Ru / Al203, Ni, Ti, or Nb powder. At least one of the HSA support, rarefactor and dispersant may comprise at least one of the group of a metal powder such as Ni, Ti, or powder of Nb, R-Ni, Zr02, A1203, NaX (X = F, Cl, Br, I), Na20, NaOH, and Na2C03. In one embodiment, a metal catalyzes the formation of NaH molecules from a source such as a Na species and a source of H. The metal can be a transition metal, noble metal, intermetallic, rare earth, lanthanide and metal of actinide, as well as others such as aluminum and tin.

C. Hydrino Reaction Activators The hydrino reaction can be activated or initiated and propagated by one or more other chemical reactions. These reactions can be of various kinds such as (i) exothermic reactions that provide the activation energy for the hydrino reaction, (ii) coupled reactions that provide at least one of a catalyst source or atomic hydrogen to support the reaction of hydrino, (iii) free radical reactions which, in one embodiment, serve as an electron acceptor of the catalyst during the hydrino reaction, (iv) oxidation-reduction reaction which, in one embodiment, serve as an electron acceptor of the catalyst during the hydrino reaction, (v) exchange reactions, such as anion exchange in which are included exchange of halide, sulfide, hydride, arsenide, oxide, phosphide and nitride that in one embodiment, facilitate the action of the catalyst to become ionized as it accepts atomic hydrogen energy to form hydrinos, and (vi) hydrino reaction aided by rarefactor, support or matrix that can eer at least one of a chemical environment for the hydrino reaction, act to transfer electrons to facilitate the H catalyst function, undergo a reversible change or other physical change or change in its electronic state and bind to a hydrogen product of lower energy to increase at least one of the extent or speed of the hydrino reaction. In one embodiment, the reaction mixture comprises a support, preferably an electrically conductive support, for enabling the activation reaction.

In one embodiment, a catalyst such as Li, K and NaH serves to form hydrins at a high speed by accelerating the rate limiting step, the removal of electrons from the catalyst as it is ionized upon accepting the non-radiant resonant energy transfer. of atomic hydrogen to form hydrinos. The typical metallic form of Li and K can be converted to the atomic form and the ionic form of NaH can be converted to the molecular form by using the support or HSA material such as activated carbon (AC), Pt / C, Pd / C, Tic, or WC to disperse the catalyst such as Li and K atoms and NaH molecules, respectively. Preferably, the support has a high surface area and conductivity considering the surface modification after the reaction with other species of the reaction mixture. The reaction to cause an atomic hydrogen transition to form hydrins requires a catalyst such as Li, K or NaH and atomic hydrogen where NaH serves as a catalyst and source of atomic hydrogen in a concerted reaction. The reaction step of a non-radiant energy transfer of an integral multiple of 27.2 eV of atomic hydrogen to the catalyst results in ionized catalyst and free electrons which cause the reaction to cease rapidly due to charge buildup. The support such as activated carbon can also act as a conductive electron acceptor and final electron acceptor reagents comprising an oxidant, free radicals or a source thereof, are added to the reaction mixture to finally purge electrons released from the reaction of catalysis to form hydrinos. In addition a reducer can be added to the reaction mixture to facilitate the oxidation reaction. The concerted electron acceptor reaction is preferably exothermic to heat the reactants and improve the rates. The activation energy and propagation reaction can be provided by rapid oxidation, exothermic or reaction of free radicals such as those of 02 or CF4 with Mg or Al where radicals such as CFX and F and 02 and 0 serve to accept electrons finally of the catalyst via support such as activated carbon. Other oxidants or radical sources individually or in combination can be chosen from the group of 02, 03, N20, NF3, M2S208 (M is an alkali metal), S, CS2, and S02, Mnl2, EuBr2, AgCl, and other dies in the Electron Acceptor Reaction section.

Preferably, the oxidant accepts at least two electrons. The corresponding anion can be 022 ~, S2", C2S42 ~ (tetrathiooxalate anion), S032 ~, and S042". The two electrons can be accepted from a catalyst that becomes doubly ionized during such catalysis. as NaH and Li (Equations (25-27) and (37-39)). The addition of an electron acceptor to the reaction mixture or reactor is applied to all cell embodiments of the present disclosure, such as the solid fuel and heterogeneous catalyst embodiments, as well as electrolysis cells and plasma cells such as discharge. luminescent, RF, microwave and plasma cells of electrode barrier and plasma electrolysis cells put into operation continuously or in a pulsed mode. An electrically conductive support, preferably non-reactive, such as activated carbon can also be added to the reagents of each of these cell modalities. One embodiment of the microwave plasma cell comprises a hydrogen dissociator such as a metal surface inside the plasma chamber to support hydrogen atoms.

In embodiments, mixtures of species, compounds or materials of the reaction mixture, such as a source of catalyst, a source of an energy reaction such as a metal, and at least one of an oxygen source, a source of halogen and a source of free radicals and a support can be used in combinations. Reactive elements of compounds or materials of the reaction mixture can also be used in combinations. For example, the fluorine or chlorine source can be a mixture of NxFy and NxCly, or the halogen can be intermixed such as in the compound NxFyClr. The combinations could be determined by routine experimentation by those experienced in the art. to. Exothermic Reactions In one embodiment, the reaction mixture comprises a catalyst or catalyst source such as at least one of NaH, K, and Li and hydrogen or a source of hydrogen and at least one species undergoing reaction. The reaction is preferably very exothermic and preferably has rapid kinetics, in such a way that it provides the activation energy to the reaction of the hydride catalyst. The reaction can be an oxidation reaction. Suitable oxidation reactions are the reaction of oxygen-comprising species such as the solvent, preferably an ether solvent, with a metal such as at least one of Al, Ti, Ser, Si, P, rare earth metals, alkali metals and alkaline earth metals. More preferably, the exothermic reaction forms an alkaline or alkaline earth halide, preferably MgF2 or halides of Al, Si, P, and rare earth metals. Suitable halide reactions are the reaction of a species comprising a halide such as the solvent, preferably a fluorinatedcarbon solvent, with at least one of a metal and a metal hydride such as at least one of Al, metals of rare earths, alkaline metals and. alkaline earth metals. The metal or metal hydride can be the catalyst or a catalyst source such as NaH, or Li. The reaction mixture may comprise at least NaH and NaAlCl4 or NaAlF4 having the NaCl and NaF products, respectively. The reaction mixture may comprise at least one NaH, a fluorosolvent having the product NaF.

In general, the product of the exothermic reaction to provide the activation energy to the hydrino reaction can be a metal oxide or a metal halide, preferably a fluoride. Suitable products are Al203 (M203 (M = rare earth metal), Ti02, Ti203, Si02, PF3 or PF5, A1F3, MgF2, MF3 (M = rare earth metal), NaF, NaHF2, KF, KHF2, LiF, and LiHF2 In one embodiment, where Ti undergoes the exothermic reaction, the catalyst is Ti2 + having a second ionization energy of 27.2 ev (m = l in Equation (5).) The reaction mixture may comprise at least two of NaH, Na, NaNH2, NaOH, Teflon, carbon · fluorinated, and: a Ti source such as Pt / Ti or Pd / Ti. In one embodiment, where Al undergoes the exothermic reaction, the catalyst is AlH as given in Table 3. The reaction mixture may comprise at least two of NaH, Al, carbon powder, a fluorocarbon, preferably a solvent such as hexafluorobenzene or perfluoroheptane, Na, NaOH, Li, LiH, K, KH, and R-Ni. Preferably, the products of the exothermic reaction to provide the activation energy are regenerated to form the reagents for another cycle for hydrine formation and release of the corresponding energy. Preferably, the metal fluoride products are regenerated to metals and fluorine gas by electrolysis. The electrolyte may comprise a eutectic mixture. The metal can be hydride and the carbon product and any CH4 and hydrocarbon products can be fluorinated to form the initial metal hydride and fluorocarbon solvent, respectively.

E h embodiments of the exothermic reaction for activating the transition reaction of hydrino to at least one of the group of a rare earth metal (M), Al, Ti, and Si is oxidized to the corresponding oxide such as M203, Al203, Ti203, and Si02, respectively. The oxidant may be an ether solvent such as 1,4-benzodioxane (BDO) and may further comprise a fluorocarbon such as hexafluorobenzene (HFB) or perfluoroheptane to accelerate the oxidation reaction. In an exemplary reaction, the mixture comprises 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 reducer, the product Si02 can be regenerated to Si by reducing H2 at high temperature or by reaction with carbon to form Si and CO and C02. A certain embodiment of the reaction mixture to form hydrins comprises a catalyst or a catalyst source such as at least one of Na, NaH, K, KH, Li, and LiH, a source of exothermic reactants or exothermic reactants, preferably they have a fast kinetics, which activate the catalysis reaction of H to form hydrinos and a support. Exothermic reagents can comprise an oxygen source and a species that reacts with oxygen to form an oxide. For x and y which are integers, preferably the oxygen source is H20, 02 / H202, Mn02, an oxide, a carbon oxide, preferably CO or C02, a nitrogen oxide, Nx0y such as N20 and, N02, an oxide of sulfur, Sx0y, preferably an oxidant such as M2SxOy (M is an alkali metal) which may optionally be used with an oxidation catalyst such as silver ion, ClxOy such as C120 and C102, preferably NaCl02; Concentrated acids and their mixtures such as H 02, HN03, H2SO4, H2SO3, HCl and HF, preferably, the acid forms nitronium ion (N02 +), NaOCl, IxOy, preferably? 205, Px0y, SxOy, an oxyanion of an inorganic compound such as one of nitrite, nitrate, chlorate, sulfate, phosphate, a metal oxide such as cobalt oxide, and oxide. or catalyst hydroxide such as NaOH, and perchlorate, wherein the cation is a catalyst source such as Na, K, and Li, an oxygen-containing functional group of an organic compound such as an ether, preferably one of dimethoxyethane, dioxane , and 1,4-benzodioxane (BDO), and the reactive species can comprise at least one of the group of a rare earth metal (M), Al, Ti, and Si, and the corresponding oxide is M203, Al203, Ti203 , and Si02, respectively. The reactive species may comprise the metal or element of the oxide products of at least one of the group of aluminum oxide Al203, lanthanum oxide 203, magnesium oxide MgO, titanium oxide Ti203, dysprosium oxide Dy203, erbium oxide Er203, europium oxide Eu203, lithium hydroxide LiOH, holmium oxide Ho203, lithium oxide Li20, lutetium oxide Lu203, niobium oxide Nb20s, neodymium oxide Nd203, silicon oxide Si02, praseodymium oxide Pr203, scandium oxide Sc203, strontium metasilicate SrSi03í samarium oxide Sm203, terbium oxide Tb203, thulium oxide Tm203, yttrium oxide Y203, and tantalum oxide Ta20s, boron oxide B203, and zirconium oxide. The support may comprise carbon, preferably activated carbon. The metal or element can be at least one of Al, La, Mg, Ti, Dy, Er, Eu, Li, Ho, Lu, b, Nd, Si, Pr, Se, Sr, Sm, Tb, Tm, Y , Ta, B, Zr, S, P, C, and their hydrides.

In another embodiment, the oxygen source may be at least one of an oxide such as M20, wherein M is an alkali metal, preferably Li20, Na20, and K20, a peroxide such as M202, wherein M is an alkali metal , preferably Li202, Na202, and K202, and a superoxide such as M02, wherein M is an alkali metal, preferably Li202, Na202, and K202. The ionic peroxides may further comprise those of Ca, Sr, or Ba.

In another embodiment, at least one of the oxygen source and the source of exothermic reagents or exothermic reagents, which preferably have rapid kinetics, which activate the catalysis reaction of H to form hydrins comprising one or more of the group of MN03, MNO, MN02, M3N, M2H, MNH2, MX, NH3, MBH, MAH4, M3AlH6, MOH, M2S, MHS, MFeSi, M2C03, MHC03, M2S04, MHS04, M3P04, M2HP04, MH2P04, M2Mo0, MNb03, M2B407 (lithium tetraborate), B02, M2W0, MAlCl4, MGaCl, M2Cr04, M2Cr207, M2Ti03, MZr03, MA102, MCo02 , MGa02, M2Ge03, MMn204, M4Si0, M2Si03, MTa03, MCuCl4, MPdCl4, MV03, MI03, MFe02, MI043MC10, MScOn, MTiOn, MVOn, MCrOn, MCr2On, MMn2On, MFeOn, MCoOn, MNiOn, MNi2On, MCuOn, and MZnOn, wherein M is Li, Na or K and n = 1, 2, 3 or 4, an oxyanion, an oxyanion of a strong acid, an oxidant, a molecular oxidant such as V203, I2O5, Mn02, Re207, Cr03i Ru02, AgO, PdO, Pd02, PtO, Pt02, I20, I205, I209í S02, S03, C02, N20, NO, N02, N203 / N204, N205, C120, Cl02, C1203, Cl206, C1207, P02, P2O3, and P205, NH4X, wherein X is a nitrate or other appropriate anion known to those experienced and n the art, such as one of the group comprising F ", Cl", Br ~, I ", N03", N02", S042", HSO4", Co02", I03", I04", Ti03", Cr04", Fe02", P043 ~, HPO42", H2P04", V03", CIO4"and Cr2072 ~ and other anions of. the reagents. The reaction mixture may additionally comprise a reductant. In one embodiment, the 20s is formed from a reaction of a mixture of reactants such as HN03 and P205 which reacts according to 2P205 + 12 HN03 to 4H3P04 + 6N205.

In one embodiment, wherein the oxygen or a compound comprising oxygen participates in the exothermic reaction, 02 can serve as a catalyst or catalyst source. The binding energy of the oxygen molecule is 5,165 eV, and the first, second and third ionization energies of an oxygen atom are 13.61806 eV, 35.11730 eV, and 54.9355 eV, respectively. The reactions 02? 0 + 02+, 02? 0 + 03+, and 20? 20+ provide a net enthalpy of. about 2, 4, and 1 times Eh, respectively, and comprise catalyst reactions to form hydrino by accepting these H energies to cause the formation of hydrinos.

Additionally, the source of an exothermic reaction for activating the hydrino reaction can be a metal alloy formation reaction, preferably between Pd and Al initiated by melting Al. The exothermic reaction preferably causes the energetic particles to activate the formation reaction of hydrino The reagents can be a pyrogen or pyrotechnic composition. In another embodiment, the activation energy can be provided by putting the reactants into operation at a very high temperature, such as in the range of about 1000-5000 ° C, preferably in the range of about> 1500-2500 ° C. The reaction vessel may comprise a high temperature stainless steel alloy, a metal or refractory alloy, alumina or carbon. The elevated reagent temperature can be obtained by heating the reactor or by exothermic retraction.

Exothermic reagents may comprise a halogen, preferably fluorine or chlorine, and a species which reacts with fluorine or chlorine to form a fluoride or chloride, respectively. Suitable fluorine sources are fluorocarbons such as CF4, hexafluorobenzene and hexadecafluoroheptane, xenon fluorides such as XeF2, XeF4, and XeF6, BxXy, preferably BF3 / B2F4, BC13 or BBr3, SFX such as fluorosilanes, fluorinated nitrogen, NXFY, preferably NF3 , NF30, SbFx, BiFx, preferably BiF5, NxCly, preferably NC13, SxXy, preferably SC12 or SxFy (X is a halogen, x and y are integers) such as SF4, SF6 or S2F10, fluorinated phosphorus, M2SiF6 wherein M is a alkali metal such as Na2SiF6 and K2SiF6, MSiF6 wherein M is an alkaline earth metal such as MgSiF6, GaF3, PF5, MPF6, wherein M is an alkali metal, HF2, wherein M is an alkali metal such as NaHF2 and KHF2, K2TaFi, KBF4 < K2MnF6 and K2ZrF6, wherein other similar compounds are anticipated such as those having another substitution of alkali metal or alkaline earth metal such as one of Li, Na or K as the alkali metal. Appropriate sources of chlorine are Cl2 gas, SbCls, and chlorocarbons such as CC14 and chloroform. The reactive species can comprise at least one of the group of a metal or alkaline or alkaline earth hydride, a rare earth metal (M), Al, Si, Ti, and P which forms the corresponding fluoride or chloride. Preferably, the reactive alkaline metal corresponds to that of the catalyst, the alkaline earth hydride is MgH2, the rare earth is La, and Al is a nanopowder. The support may comprise carbon, preferably activated carbon, mesoporous carbon, and the carbon used in lithium ion batteries. The reagents can be in any molar proportion. Preferably, the reactive species and the fluorine or chlorine are in the stoichiometric ratio as the elements of the fluorine or chlorine, the catalyst is in excess, preferably in about the same molar ratio as the element that reacts with the fluorine or chlorine and the support It is in excess.

The exothermic reagents may comprise a halogen gas, preferably chlorine or bromine, or a source of halogen gas such as HF, HCl, HBr, HI, preferably CF4 or CCI4, and a species that reacts with the halogen to form a halide. The halogen source can also be an oxygen source such as CxOyXr, where X is halogen, and x, y, and r are integers and are known in the art. The reactive species can comprise at least one of the group of an alkaline or alkaline earth metal or hydride, a rare earth metal, Al, Si, and P which forms the corresponding halide. Preferably the reactive alkali metal corresponds to that of the catalyst, the alkaline earth hydride is MgH2, the rare earth is La, and Al is a nanopowder. The support may comprise carbon, preferably activated carbon. The reagents can be in any molar proportions. Preferably, the reactive species and the halogen are in approximately equal stoichiometric ratio, the catalyst is in excess, preferably in about the same molar ratio as the element that reacts with the halogen, and the support is in excess. In one embodiment, the reagents comprise, a catalyst source or a catalyst such as Na, NaH, K, KH, Li, LiH, and (H2, a halogen gas, preferably, chlorine or bromine gas, at least one of g, MgH2, a rare earth, preferably La, Gd, or Pr, Al, and a support, preferably carbon such as activated carbon b.Free Radical Reactions In one embodiment, the exothermic reaction is a free radical reaction, preferably a free radical reaction of halide or oxygen. The source of halide radicals can be a halogen, preferably F2 or Cl2 or a fluorocarbon, preferably CF4. A source of free radicals of F is S2Fi0. The reaction mixture comprising a halogen gas may further comprise a free radical initiator. The reactor may comprise a source of ultraviolet light to form free radicals, preferably free radicals, of halogen and more preferably free radicals of chlorine or fluorine. Free radical initiators are those commonly known in the art such as peroxides, azo compounds and a source of metal ions such as a metal salt, preferably a cobalt halide such as CoCl2 which is a source of Co2 + or FeS04 which is a source of Fe2 +. The latter is preferably reacted with a kind of oxygen such as? 202 or 02. The radical can be neutral.

The oxygen source may comprise a source of atomic oxygen. Oxygen can be singlet oxygen. In one embodiment, singlet oxygen is formed from the reaction of NaOCl with H202. In one embodiment, the oxygen source comprises 02 and may further comprise a source of free radicals or a free radical initiator to propagate a free radical reaction, preferably a free radical reaction of atoms of 0. The source of free radicals or Oxygen source can be at least one of ozone or an ozonide. In one embodiment, the reactor comprises an ozone source such as an electric discharge in oxygen to provide ozone to the reaction mixture.

The source of free radicals or oxygen source may further comprise at least one of a peroxo compound, a peroxide, H202, a compound containing an azo group, N20, NaOCl, Fenton reagent, or a similar reagent, OH radical or a source thereof, permeate ion or a source thereof, such as an alkaline or alkaline earth metal perxenate, preferably, sodium perxenate (a4Xe06) or potassium perxenate (K4Xe06), xenon tetraoxide (Xe04), and perxenic acid ( HXe06), and a source of metal ions such as a metal salt. The metal salt may be at least one of FeS0, A1C13, TiCl3, and, preferably, a cobalt halide such as CoCl2 which is a source of Co2 +.

In one embodiment, free radicals such as Cl are formed, from a halogen such as Cl 2 in the reaction mixture such as NaH + MgH 2 + support such as activated carbon (AC) + halogen gas such as Cl 2. Free radicals can be formed by reaction. of a mixture of Cl2 and a hydrocarbon such as CH4 at an elevated temperature such as greater than 200 ° C. The halogen may be in a molar excess relative to the hydrocarbon. The chlorocarbon product and Cl radicals can be reacted with the reductant to provide the activation energy and path to form hydrinos. The carbon product can be regenerated using synthetic gas (synthetic gas) and Fischer-Tropsch reactions or by direct hydrogen reduction from carbon to methane. The reaction mixture may comprise a mixture of 02 and Cl 2 at an elevated temperature, such as greater than 200 ° C. The mixture can react to form ClxOy (x and y are integers) such as CIO, C120, and C102. The reaction mixture may comprise H2 and Cl2 at an elevated temperature, such as greater than 200 ° C which can react to form HCl. The reaction mixture may comprise H2 and 02 with a recombinant such as Pt / Ti, Pt / C, or Pd / C at a slightly elevated temperature such as greater than 50 ° C which can react to form H20. He . The recombiner can operate at elevated pressures, such as in the range of greater than one atmosphere, preferably in the range of about 2 to 100 atmospheres. The reaction mixture can be non-stoichiometric to promote free radical formation and singlet oxygen formation. The system can also comprise a source of ultraviolet light or plasma to form free radicals, such as an RF source, microwave, or luminescent discharge, preferably source of high voltage pulsed plasma. The reagents may further comprise a catalyst to form at least one of atomic free radicals such as Cl, 0 and H, singlet oxygen, and ozone. The catalyst can be a noble metal such as Pt. In one embodiment to form Cl radicals, the Pt catalyst is maintained at a temperature greater than the decomposition temperature of platinum chlorides such as PtCl 2, PtCl 3, and PtCl 4 having decomposition temperatures of. 581 ° C, 435 ° C, and 327 ° C, respectively. In one embodiment, the Pt can be recovered from a product mixture comprising metal halides by dissolving the metal halides in an appropriate solvent in which the Pt, Pd or its halides are not soluble and removing the solution. The solid which can comprise carbon and Pt or Pd halide can be heated to form Pt or Pd on carbon by decomposition of the corresponding halide. one mode, gas of N20, N02 or NO is added to the reaction mixture. The N20 and N02 can serve as a source of NO radicals. In another embodiment, the NO radical is produced in the cell, preferably by the oxidation of NH3. The reaction may be the reaction of NH3 with 02 on platinum or platinum-rhodium at elevated temperature. The NO, N02, and N20 can be generated by known industrial methods, such as through the Haber process followed by the Ostwald process. In one modality, the exemplary sequence of stages are: process them * NO,? ß, NQl. (53) Ostwñid Specifically, the Haber process can be used to produce NH3 from N2 and H2 at elevated temperature and pressure using a catalyst such as alpha iron containing some oxide. The Ost ald process can be used to oxidize the ammonia to NO, N02 / and N20 in a catalyst such as a hot platinum catalyst or platinum-rhodium. Alkali nitrates can be regenerated using the methods disclosed supra.

The reaction system and mixture can initiate and support a combustion reaction to provide at least one singlet oxygen and radicals. free The combustion reagents may be non-stoichiometric to favor the formation of free radical and singlet oxygen which react with the other hydrino reaction reagents. In one embodiment, an explosive reaction is suppressed to favor a prolonged stable reaction. or an explosive reaction is caused by the appropriate reagents and molar proportions to obtain the desired hydrino reaction rate. In one embodiment, the cell comprises at least one cylinder of an internal combustion engine. . c. Electron Acceptor Reactions In one embodiment, the reaction mixture further comprises an electron acceptor. The electron acceptor can act as a dissipator for the ionized electrons of the catalyst when the energy is transferred thereto from the atomic hydrogen during the catalytic reaction to form hydrinos. The electron acceptor can be at least one of a conductive polymer or metal support, an oxidant such as group VI elements, molecules and compounds, a free radical, a species that forms a stable free radical, and a species with a high affinity of electrons such as halogen atoms, 02, C, CFi > 2,3 or 4, Si, S, PxSy, CS2, SxNy and these compounds further comprise 0 and H, Au, A, AlxOy (x and y are integers), preferably Al02 which in one embodiment is an intermediate of the Al reaction. (0H) 3 with Al of R-Ni, CIO, Cl2, F2, A102, B2N, CrC2, C2H, CuCl2, CuBr2, MnX3 (X = halide), M0X3 (X = halide), Nix3 (X = halide), RuF4.5 0 6, ScX4 (X = halide), W03, and other atoms and molecules with a high affinity of electrons as are known to those skilled in the art. In one embodiment, the support acts as an electron acceptor of the catalyst as it is ionized by accepting the transfer of non-radiant resonant energy from atomic hydrogen. Preferably, the support is at least one conductor and forms stable free radicals. Appropriate supports are conductive polymers. The support can form a negative ion on a macrostructure such as carbon from lithium ion batteries to form C6 ions. In another embodiment, the support is a semiconductor, preferably doped to improve the conductivity. The reaction mixture further comprises free radicals or a source thereof such as O, OH, 02, 03, H202, F, Cl, and NO which can serve as a scavenger for the free radicals formed by the support during the catalysis. In one embodiment, the free radical such as NO can form a complex with the catalyst or catalyst source such an alkali metal. In another modality, the support has unpaired electrons. The support can be paramagnetic, such as a rare or composite earth element such as Er203. In one embodiment, the catalyst or catalyst source such as Li, NaH, K, Rb, or Cs is impregnated to the electron acceptor such as a support and the other components of the reaction mixture are added. Preferably, the support is activated carbon with NaH or Na intercalated. d. Oxidation-Reduction Reactions In one embodiment, the hydrino reaction is activated by an oxidation-reduction reaction. In an exemplary embodiment, the reaction mixture comprises at least two species from the group of a catalyst, a source of hydrogen, an oxidant, a reductant and a support. The reaction mixture may also comprise a Lewis acid such as Group 13 trihalides, preferably at least one of A1C13, BF3, BC1, and BBr3. In certain embodiments, each reaction mixture comprises at least one selected species of the following kind of components (i) - (iii). (i) A catalyst chosen from Li, LiH, K, KH, NaH, Rb, RbH, Cs, and CsH. (ii) A hydrogen source chosen from H2 gas, a H2 gas gas, or a hydride. (ii) In addition to an oxidant chosen from a metal compound such as one of halides, phosphides, borides, oxides, hydroxides, silicides, nitrides, arsenides, selenides, telluriums, antimonides, carbides, sulfides, hydrides, carbonate, hydrogen carbonate, sulfates , hydrogen sulphates, phosphates, hydrogen phosphates, dihydrogen phosphates, nitrates, nitrites, permanganates, chlorates, perchlorates, chlorites, perchlorites, hypochlorites, bromates, perbromates, bromites, perbromites, iodates, periodates, iodides, peryodites, chromates, dichromates, telurates, selenatos, arsenates, silicates, borates, cobalt oxides, tellurium oxides and other oxyanions such as those of halogens, P, B, Si, N, As, S, Te, Sb, C, S, P, Mn, Cr, Co, and Te wherein the metal preferably comprises a transition metal, Sn, Ga, In, an alkali metal or alkaline earth metal; the oxidant further comprises a lead compound such as a lead halide, a germanium compound such as a halide, oxide or sulfide such as GeF2, GeCl2, GeBr2, Gel2, GeO, GeP, GeS, Gel4, and GeCl4, fluorocarbons such as CF4 or C1CF3, such chlorocarbons ate CC14, 02, MN03, MC104, M02, NF3, N20, NO, N02, a boron-nitrogen compound such as B3 3H6, a sulfur compound such as SF6, S, S02, SO3, S20sCl2, F5SOF, M2S208, SxXy such as S2C12, SC12, S2Br2 or S2F2, CS2, SOxXy such as S0C12, SOF2, S02F2 or S0Br2, XxX'y such as ClF5 / XxX "yOz such as C102F, C102F2, C10F3, C103F, and C102F3, composed of boron-nitrogen such as B3 3H6, Se, Te, Bi, As, Sb, Bi, TeXx, preferably TeF4, TeF6, TeOx, preferably Te02 or e03, SeXx, preferably SeF6, SeOx, preferably Se02 or Se03, a tellurium oxide, halide or other tellurium compound such as Te02, Te03, Te (OH) 6, TeBr2, TeCl2> TeBr4, TeCl4, TeF4, Tel4, TeF6, CoTe, or NiTe, an oxide, halide , sulf urea of selenium, or other selenium compound such as' Se02, SeC ^, Se2Br2, Se2Cl2, SeBr, SeCl4, SeF, SeF6, SeOBr2, SeOCl2 / SeOF2, Se02F2, SeS2, Se2S6, Se4S or Se6S2, P, P205, P2S5 , PxXy such as PF3, PCI3, PBr3, PI3, PF5, PCI5, PBr4F, or PC1 F, POxXy such as POBr3, POI3, POCI3 or POF3, PSxXy (M is an alkali metal, x, yz are integers, X and X 'are halogen) such as PSBr3, PSF3, PSCI3, a phosphorus-nitrogen compound such as P3N5, (C12PN) 3, (C12PN) 4 or (Br2PN) x, an oxide, halide, sulfide, selenide or telluride of arsenic or other arsenic compound such as AlAs, AS2I4, As2Se, As4S4, AsBr3, AsCl3, AsF3, Asl3, As203, As2Se3, As2S3, As2Te3, AsCl5, AsF5, As205, As2Ses or '. As2S5, an oxide, halide, sulfide, sulfate, selenide, antimony arsenide or other antimony compound such as SbAs, SbBr3, SbCl3, SbF3, Sbl3, Sb203, SbOCl, Sb2Se3, Sb2 (S04) 3, Sb2S3, Sb2Te3, Sb204 , SbCl5, SbF-5 / SbCl2F3, Sb205 or Sb2S5, an oxide, halide, sulfide, bismuth selenide, or other bismuth compound such as BiAs0, BiBr3, BiCl3, BiF3, BiF5, Bi (OH) 3, Bil3, Bi203f BiOBr, BiOCl, BiOI, Bi2Se3, Bi2S3, Bi2Te3 or Bi204, SiCl4, SiBr4, an oxide, hydroxide, or metal halide such as a transition metal halide such as CrCl3, ZnF2, ZnBr2, Znl2, MnCl2, MnBr2) nl2, CoBr2¿ CoI2, · CoCl2, NiCl2, NiBr2, NiF2 FeF2, FeCl2, FeBr2, FeCl3, TiF3, CuBr, CuBr2, VF3, and CuCl2, a metal halide such as SnF2, SnCl2, SnBr2 >; Snl2, SnF4 (SnCl4, SnBr4 (Snl4, InF, InCl, InBr, Inl, AgCl, Agl, AlF3 (AlBr3, All3, YF3, CdCl2, CdBr2, Cdl2, InCl3, ZrCl4, NbF5, TaCl5, MoCl3, M0Cl5, NbCl5 , AsCl3, TiBr4, SeCl2, SeCl, InF3, InCl3, PbF, Tel4, WC16; • OsCl3, GaCl3, PtCl3, ReCl3 RhCl3, RuCl3, rust or metal hydroxide such as Y203, FeO, Fe203 or NbO, NiO, Ni203 , SnO, Sn02, Ag20, AgO, Ga20, As203, Se02, Te02, In (0H) 3, Sn (0H) 2, In (OH) 3, Ga (OH) 3, and Bi (OH) 3, C02, As2Se3, SF6, S, SbF3, CF4, NF3, a permanganate such as KMn0 and NaMn04, P205, a nitrate such as LiN03, NaN03 and KN03, and a boron halide such as BBr3 and BI3, a halide of group 13, preferably an indium halide such as InBr2, InCl2, and Inl3, a silver halide, preferably AgCl or Ag, a lead halide, a cadmium halide, a zirconium halide, preferably an oxide, sulfide, or transition metal halide (Se, Ti, V, Cr, Mn, Fe, Co, Ni, Cu, or Zn with F, Cl, Br or I), a second or third transitional halide, pr YF3, preferably sulfur, preferably Y2S3 or hydroxide, preferably those of Y, Zr, Nb, Mo, Te, Ag, Cd, Hf, Ta, W, O, such as b3, NbX5 or TaX5 in the case of halides, uri metal sulfide such as Li2S, ZnS, FeS, NiS, MnS, Cu2S, CuS, and SnS, an alkaline earth halide such as BaBr2, BaCl2, Bal2, SrBr2, Srl2, CaBr2, Cal2, MgBr2 or Mgl2 ,. a rare earth halide such as EuBr3f LaF3, LaBr3, CeBr3 ', GdF3, GdBr3, preferably state II such as one of Cel2, EuF2, EuCl2, EuBr2, Eul2, Dyl2, Ndl2, Sml2, Ybl2 / and Tml2, a boride of metal such as europium boride, a boride of MB2 such as CrB2, TiB2, MgB2, ZrB2, and GdB2 an alkali halide such as LiCl, RbCl, or Csl, and a metal phosphide such as Ca3P2, a halide, oxide, noble metal sulfide such as PtCl2, PtBr2í 'Ptl2, PtCl4, PdCl2, PbBr2, and Pbl2, a rare earth sulfide such as CeS, other appropriate rare earths are those of La and Gd, a metal and an anion such as Na2Te04 , Na2Te03, Co (CN) 2, CoSb, CoAs, Co2P, CoO, CoSe, CoTe, NiSb, NiAs, NiSe, Ni2Si, MgSe, a rare earth teloluro, such as EuTe, a selenium or rare earths such as EuSe, a rare earth nitride such as EuN, a metal nitride such as AlN, GdN, and. Mg3N2, a compound containing at least two oxygen group atoms and different halogen atoms such as F20, C120, C102, 01206, Cl207, C1F3, C1F3, C10F3, C1F5, C102F, C102F3, C103F, BrF3, BrF5 , I205, IBr, ICl, ICI3, 'IF, IF3, IF5, IF7, and a second or third transition metal halide such as OsF6 / PtF6 or IrF6, such an alkali metal compound. as a halide, oxide or sulfide, and a compound that can form a metal after reduction such as an alkali, alkaline earth, transition, rare earth, Group 13, preferably In, and Group 14, preferably Sn, a metal hydride as a rare earth hydride, alkaline earth hydride, or alkali hydride, wherein the catalyst or catalyst source can be a metal such as an alkali metal, when the oxidant is a hydride, preferably a metal hydride. Suitable oxidizers are halides, sulphides, oxides, hydroxides, selenides, and metal phosphides such as alkaline earth halides such as BaBr2, BaC.l2, Bal2, CaBr2, MgBr2 or Mgl2, a rare earth halide such as EuBr2, EuBr3, EuF3 , LaF3, GdF3 GdBr3, LaF3, LaBr3, CeBr3, a metal halide of second or third transition series such as YF3, a metal boride such as CrB2 or TiB2, an alkali halide such as LiCl, RbCl, or Csl, a metal sulfide such as Li2S, ZnS, Y2S3, FeS, MnS, Cu2S, CuS, and Sb2S5, a metal phosphide such as Ca3P2 (a transition metal halide such as CrCl3, ZnF2, ZnBr2, Znl2, MnCl2, MnBr2, Mnl2, CoBr2, CoI2, CoCl2, NiBr2, NiF2, FeF2, FeCl2, FeBr2, TiF3 / CuBr, VF3, and CuCl2, a metal halide such as SnBr2, Snl2, InF, InCl, InBr, Inl, AgCl, Agl, All3 YF3, GdCl, CdBr2, Cdl2, InCl3, ZrCl4, bF5, TaCl5, MoCl3, MoCl5, NbCl5, AsCl3, TiBr, SeCl2, SeCl4, InF3, PbF, and Tel4, metal oxide or hydroxide such as Y203, FeO, NbO, In (0H) 3, As203, Se02, Te02, BI3, C02, As2Se3, metal nitride such as Mg3N2 or AlN, metal phosphide such as Ca3P2, SF6, S, SbF3, CF4, NF3, KMn04, NaMn04, P205, L1NO3, NaN03, KO3 , and a metal boride such as BBr3. Suitable oxidants include at least one of the list of BaBr2, BaCl2, EuBr2, EuF3, YF3i CrB2f TiB2, LiCl, RbCl, Csl, Li2S, ZnS, Y2S3, Ca3P2, Mnl2 >; CoI2, NiBr2, ZnBr2, FeBr2, Snl2, InCl, AgCl ,. Y203, Te02, C02, SF6, S, CF4, NaMn04, P205, LiN03. Suitable oxidants include at least one of the list of EuBr2, BaBr2, CrB2, Mnl2, and AgCl. Suitable sulfide oxidizers comprise at least one of Li2S, ZnS, and Y2S3. In certain embodiments, the oxide oxidant is Y 2 O 3.

In further embodiments, each reaction mixture comprises at least one species chosen from the following genus of components (i) - (iii) described above and further comprises (iv) at least one reductant chosen from a metal such as an alkali metal, alkaline earth, transition metal, second and third transition series and rare earth metals and aluminum. Preferably the reductant is one of the group of Al, Mg, MgH2, Si, La, B, Zr, and Ti, and H2 powders.

In further embodiments, each reaction mixture comprises at least one species chosen from the following genus of components (i) - (iv) described above, and further comprises (v) a support, such as a chosen conductive support of activated carbon, % of Pt or Pd on carbon (Pt / C, Pd / C), and a carbide, preferably T.iC or WC.

The reactants can be in any molar ratio, but preferably they are in approximately equal molar proportions.

An appropriate reaction system comprising (i) a catalyst or a catalyst source, (ii) a source of hydrogen, (iii) an oxidant, (iv) a reductant, and (v) a support comprising NaH or KH as the catalyst or source of catalyst and source of H, one of BaBr2, BaCl2, MgBr2, Mgl2, CaBr2, EuBr2, EuF3, YF3i CrB2, TiB2, LiCl, RbCl, Csl, Li2S, ZnS, Y2S3, Ca3P2, Mnl2, CoI2, NiBr2, ZnBr2, FeBr2, Snl2, InCl, AgCl, Y203, TeO2. C02, SF5, S, CF, NaMn04, P05, LiN03, as the oxidant, Mg or MgH2 as the reductant, wherein MgH2 can also serve as the source of H, and activated carbon, Tic, or WC as the support. In the case that a tin halide is the oxidant, the Sn product can serve as at least one of the reductant and conductive support in the mechanism. of catalysis.

In another appropriate reaction system comprising (i) a catalyst or a source of catalyst, (ii) a source of hydrogen, (iii) an oxidant, and (iv) a support comprises NaH or KH as the catalyst or catalyst source and source of H, one of EuBr2, BaBr2, CrB2, Mnl2 > . and AgCl as the oxidant, and activated carbon, Tic, or WC as the support. The reactants may be in any molar ratio, but preferably, they are in approximately equal molar proportions.

The catalyst, the source of hydrogen, the oxidant. the reducer, and the support can be in any desired molar ratio. In an embodiment having the reactants, the catalyst comprising KH or NaH, the oxidant comprising at least one of CrB2, AgCl2, and a metal halide of the group of an alkaline earth, transition metal, p halide of rare earths , preferably a bromide or iodide, such as EuBr2, BaBr2, and Mnl2, the reductant comprising Mg or MgH2, and the support comprising activated carbon, TiC, or WC, the molar proportions are approximately the same. The rare earth halides can be formed by the direct reaction of the corresponding halogen with the metal or the hydrogen halide such as HBr. The dihalide can be formed from the trihalide by reduction of H2. > Additional oxidants are those that have a high dipole moment or form an intermediate with a high dipole moment. Preferably, the species with a high dipole moment readily accepts electrons from the catalyst during the catalysis reaction. The species can have a high affinity for electrons. In one embodiment, the electron acceptors have a half-full or approximately half-full electron envelope such as Sn, Mn, and Gd or Eu compounds that have sp3, 3d, and envelope covers. 4f half full, respectively. Representative oxidants of the latter type are metals corresponding to LaF3, LaBr3, GdF3, GdCl3, GdBr3, EuBr2, Eul2, EuCl2, EuF2, EuBr3, Eul3, EuCl3, and EuF3. In one embodiment, the oxidant comprises a non-metal compound such as at least one of P, S, Si, and C which preferably has a high oxidation state and further comprises atoms with a high electronegativity such as at least one of F, Cl or O. In another embodiment, the oxidant comprises a compound of a metal such as at least one of Sn and Fe having a low oxidation state such as II and further comprising atoms with a low electronegativity such as at least one of Br or I. A negatively charged ion individually such as Mn04 ~. C1044 ~ or N03"is favored with respect to a double negative charge such as one of C032 ~ or S02". In one embodiment, the oxidant comprises a compound such as a metal halide corresponding to a metal with a low melting point, such that it can be melted as a reaction product and removed from the cell. Suitable oxidizers of metals of low melting point are halides of In, Ga, Ag, and Sn. The reactants may be in any molar proportion, but preferably they are in approximately equal molar proportions.

In one embodiment, the reaction mixture comprises (i) a catalyst or catalyst source comprising a metal or a hydride of the elements of Group I, (ii) a source of hydrogen such as H2 gas or a gas source ¾, or a hydride, (iii) an oxidant comprising an atom or ion or a compound comprising at least one of the elements of Groups 13, 14, 15, 16 and 17; preferably chosen from the group of F, Cl, Br, I, B, C, N, or, Al, Si, P, S, Se, and Te, (iv) a reductant comprising an element or hydride, preferably one or more selected elements or hydrides of Mg, MgH2, Al, Si, B, Zr, and a rare earth metal such as La, and (v) a support that is preferably conductive and preferably does not react to form another compound with other species of the reaction mixture. Suitable supports preferably comprise carbon such as activated carbon, graphene, carbon impregnated with a metal such as Pt or Pd / C, and a carbide, preferably Tic or WC.

In one embodiment, the reaction mixture comprises (i) a catalyst or a catalyst source comprising a metal or a hydride of the elements of Group I, (ii) a source of hydrogen such as H2 gas or a gas source of H2 or a hydride, (iii) an oxidant comprising a halide, oxide or sulfide compound, preferably a metal halide, oxide or sulfide; more preferably a halide of the elements of Groups IA, IIA, 3d, 4d, 5d, 6d, 7d, 8d, 9d, 10d, lid, 12d, and lanthanides, and more preferably a transition metal halide or lanthanide halide (iv) a reducer comprising an element or hydride, preferably one or more elements or hydrides chosen from Mg, MgH2, Al, Si, B, Zr, and a rare earth metal such as La, and (v) a support which is preferably conductive and preferably does not react to form another compound with other species of the reaction mixture. Suitable supports preferably comprise carbon such as activated carbon, carbon impregnated with a metal such as Pt or Pd / C, and a carbide, preferably TiC or WC. and. Exchange Reactions, Thermally Reversible Reactions and Regeneration In one embodiment, the oxidant and at least one of the reductant, the catalyst source and the catalyst can undergo a reversible reaction. In one embodiment, the oxidant is a halide, preferably a metal halide, more preferably at least one of a transition metal, tin, indium, alkali metal, alkaline earth metal, and rare earth halide, more preferably a halogen halide. rare earths The reversible reaction is preferably a halide exchange reaction. Preferably, the. The energy of the reaction is. low, so that the halide can be reversibly exchanged between the oxidant and the at least one of the reductant, source of catalyst and catalyst at a temperature between room temperature and 3000 ° C, preferably between room temperature and 1000 ° C . The balance of the reaction can be; displaced to boost the hydrino reaction. Displacement can be by a change in temperature or change in the concentration or proportion of the reaction. The reaction can be sustained by the addition of hydrogen. In a representative reaction, the exchange is NiMox + n2McaJ / redXy (54) where ¾, n2, x, e y are integers, X is a halide, and M0x is the metal of the oxidant, Mrer / Cat is the metal of at least one of the reductant, catalyst and catalyst source. In one embodiment, one or more of the reactants is a hydride and the reaction also involves a reversible hydride exchange in addition to a halide exchange. The reversible reaction can be controlled by controlling the hydrogen pressure in addition to other reaction conditions such as temperature and reagent concentration. An exemplary reaction is njtfaJCx + n2Mau / redH njMa iG + (55) In one embodiment, the oxidant such as an alkali metal halide, alkaline earth metal halide or a rare earth halide, preferably RbCl., BaBr2, BaCl2, EuX2 or Gdx3 wherein X is halide or sulfide, more preferably EuBr2, is reacted with the catalyst or catalyst source, preferably NaH or KH, and optionally a reductant, preferably Mg or MgH2, to form M0x or M0xH2 and the halide or sulfide of the catalyst such as NaX or KX. The rare earth halide can be regenerated by selectively removing the catalyst or catalyst source and optionally the reductant. In one embodiment, M0xH2 can be thermally decomposed and the hydrogen gas removed by methods such as pumping. The halide exchange (Equations (54-55)) forms the catalyst metal. The metal can be removed as a molten liquid or as an evaporated or sublimated gas leaving the metal halide such as the alkaline earth halide or rare earth halide. The liquid can be removed, for example, by methods such as centrifugation or by a stream of pressurized inert gas. The catalyst or catalyst source may be rehydrated where appropriate to regenerate the original reagents that are recombined into the original mixture with the rare earth halide and support. In the case that Mg or Mg¾ is used as the reducer, the Mg can be removed first by forming the hydride with the addition of H2, hydride fusion, and liquid removal. In a modality wherein X = F, the product of MgF2 can be converted to MgH2 by exchange of F with the rare earth such as EuH2 where the molten MgH2 is continuously removed. The reaction can be carried out under high pressure of H2 to favor the formation and selective removal of MgH2. The reducer can be rehydrated and added to the other regenerated reagents to form the original reaction mixture. In another modality, the. The exchange reaction is between sulfides or metal oxides of the oxidant and the at least one of the reductant, catalyst and catalyst source. An exemplary system of each type is 1.66g KH + lg Mg + 2.74g Y2S3 + 4g AC and Ig NaH + Ig g '+ 2.26g Y203 + 4g AC. The selective removal of the catalyst, catalyst source or reducer can be continuous where the catalyst,. The catalyst source or the reductant can be recycled at least partially into the reactor. The reactor may further comprise a still or reflux component to remove the catalyst such as still 34 of Figure 4, catalyst source or reducer and return it to the cell. Optionally, it can be hydrated or further reacted and this product can be returned. The reaction temperature can be cycled between two ends to continuously recycle the reactants by an equilibrium shift. In one embodiment, the system heat exchanger has the ability to rapidly change the temperature of the cell between a high value and a low value to shift the balance alternately to propagate the hydrino reaction.

The regeneration reaction may comprise a catalytic reaction with an aggregated species such as hydrogen. In one embodiment, the catalyst source and H is KH and the oxidant is EuBr2. The thermally driven regeneration reaction can be 2KBr + Eu to EuBr2 + 2K (56) or 2KBr + EuH2 at EuBr2 + 2KH, (57) Alternatively, H2 can serve as catalyst for regeneration of the catalyst or catalyst source and oxidant such as KH and EuBr2, respectively: 3KBr + 1 2H2 + Eu¾ at EuBr3 + 3KH. (58) Then, EuBr2 is formed- from EuBr3 by reduction of H2. A possible route is EuBr3 + 1 / 2H2 at EuBr2 + HBr. (59) The HBr can be recycled: HBr + KH at KBr + H2 (60) The net reaction is: 2KBr + EuH2 at EuBr2 + 2KH. (61) The speed of the thermally driven regeneration reaction can be increased by using a different route with a lower energy known to those experienced in the art: 2KBr + H2 + Eu to EuBr2 + 2KH (62) 3 Br + 3 / 2H2 + Eu to EuBr3 + 3KH or (63) EuBr3 + I / 2H2 at EuBr2 + HBr. (64) The reaction given by Equation (62) is possible since there is an equilibrium between a metal and the corresponding hydride in the presence of H2 such as Eu + H2? EuH2. (65) The reaction route may involve intermediate stages of energy. lowest known to those experienced in the art, such as " 2KBr + Mg + H2 to MgBr2 + 2 H and (66) MgBr2 + Eu + H2 to EuBr2 + MgH2. (67) The KH or K metal can be removed as a molten liquid or as an evaporated or sublimated gas leaving the metal halide such as the alkaline earth or rare earth halide. The liquid can be removed by methods such as centrifugation or by a current, pressurized inert gas. In other embodiments, another catalyst or catalyst source such as NaH, LiH, RbH, CsH, Na, Li, Rb, Cs can be substituted for KH or K, and the oxidant can comprise another metal halide such as another earth halide. Rare or an alkaline earth halide, preferably BaCl2 or BaBr2. In other embodiments, the thermally reversible reaction comprises additional exchange reactions, preferably between two species each comprising at least one metal atom. The exchange can be between a metal of the catalyst, such as an alkali metal and the metal of the exchange partner, such as an oxidant. The exchange can also be between the oxidant and the reducer. The exchanged species can be an anion such as a halide, hydride, oxide, sulfide, nitride, boride, carbide, silicide, arsenide, selenide, telulide, phosphide, nitrate, hydrogen sulfide, carbonate, sulfate, hydrogen sulfate, phosphate, hydrogen phosphate, dihydrogen phosphate, perchlorate, chromate, dichromate, cobalt oxide, and other oxyanions and anions known to those skilled in the art. The at least one exchange partner may comprise an alkali metal, alkaline earth metal, transition metal, second transition metal, metal of third transition series, noble metal, rare earth metal, Al, Ga, In, Sn, As, Se, and Te. Suitable exchanged anions are halide, oxide, sulfur, nitride, phosphide and boride. Suitable metals for exchange are alkali, preferably Na or K, alkaline earth metal, preferably Mg or Ba, and a rare earth metal, preferably Eu or Dy, each as the metal or idruro. Reagents of exemplary catalysts and with an exemplary exchange reaction are given infra. These reactions are not intended to be exhaustive and additional examples would be known to those skilled in the art. | 4g AC3-3 + lg Mg + 1.66g KH + 2.5g Dyl2, Ein: 135.0 kJ, dE: 6.1 kJ, TSC: none, Tmax: 403 ° C, theoretical is 1.89 kJ, gain is 3.22 times, DyBr2 + 2K? 2KBr + Dy. (68) | 4g AC3-3 + lg Mg + lg NaH + 2.09g EuF3, Ein: 185.1 kJ, dE: 8.0 kJ, TSC: none, Tmax: 463 ° C, theoretical is 1.69 kJ, gain is 4.73 times, EuF3 + 1.5Mg? 1.5MgF2 + Eu (69) EuF3 + 3 aH ^ 3NaF + Eu ¾. (70) | KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0gm + CrB2 3.7gm, Ein: 317 kJ, dE: 19 kJ, without TSC with Tmax ~ 340 ° C, the theoretical energy is endothermic 0.05 kJ, the gain is infinite , CrB2 + g ¾ MgB2. (71) 0.70 g of TiB2, 1.66 g of KH, 1 g of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-4) was finished. The energy gain was 5.1 kJ, but no burst of cell temperature was observed. The maximum temperature of the cell was 431 ° C, the theoretical temperature is 0. '' TiB2 + Mg? MgB2. (72) 0.42 g of LiCl, 1.66 g of KH, 1 g of Mg powder and 4 g of AC3-4 was finished. The energy gain was 5.4 kJ, but no burst of cell temperature was observed. The maximum temperature of the cell was 412 ° C, the theoretical temperature is 0, the gain is infinite.

LiCl + KH? KC1 + LiH. (73) 1.21 g of RbCl, 1.66 g of KH, 1 g of Mg powder and 4 g of AC3-4, the energy gain was 6.0 kJ, but no burst of cell temperature was observed. The maximum temperature of the cell was 442 ° C, the theoretical temperature is 0.

RbCl + KH? KC1 + RbH. (74) | 4g AC3-5 + lg Mg + 1.66g KH + 0.87g LiBr; Ein: 146.0 kJ; dE: 6.24 kJ; TSC: not observed; Tmax: 439 ° C, the theoretical is endothermic, LiBr + KH? KBr + LiH (75).

| KH 8.3 girv + Mg_ 5.0 gm + CAII-300 20.0gm + YF3 7.3 gm; Ein: 320 kJ; dE: 17 kJ; without TSC with Tmax ~ 340 ° C; Energy gain ~ 4.5 X (X ~ 0.74kJ * 5 = 3.7kJ), YF3 + 1.5Mg + 2KH? 1.5MgF2 + YH2 + 2K. (76) | NaH 5.0 gm + Mg 5.0 gm + CAII-300 20.0gm + BaBr2 14.85 gm (dry); Ein: 328 kJ; dE: 16 kJ; without TSC with Tmax ~ 320 ° C; Energy gain 160X (X ~ 0.02kJ * 5 = 0.1 kJ), BaBr2 + 2 aH ¾ 2NaBr + BaH2. (77) "KH 8.3 gm + Mg 5.0 p + CAII-300 20.0gm + BaCl2 10. 4 gm; Ein: 331 kJ; dE: 18 kJ Without TSC with Tmax ~ 320 ° C. Power gain -6.9X (X ~ 0.52x5 = 2.6 kJ) BaCl2 + 2KH ¾ 2KC1 + BaH2. (78) NaH 5.0 gm + Mg 5.0 gm + CAII-300 20.0gm + Mgl2 13.9 gm; Ein: 315 kJ; dE: 16 kJ Without TSC with Tmax ~ 340 ° C. Energy gain ~ 1.8X (X ~ l .75x5 = 8.75 kJ) Mgl2 + 2 aH ¾ 2NaI + MgH2. (79) 4g AC3-2 + lg Mg + lg NaH +, 0.97g ZnS; Ein: 132. lkJ; dE: 7.5kJ; TSC: none; Tmax: 370 ° C, the theoretical is 1.4 kJ, the gain is 5.33 times, -; ZnS + 2 aH? 2NaHS + Zn (80) ZnS + Mg '¾ MgS + Zn. (81) 2.74 g of Y2S3, 1.66 g of KH, 1 g of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 5.2 kJ, but no He observed no explosion of cell temperature. The maximum temperature of the cell was 444 ° C, the theoretical temperature is 0.41 kj, the gain is 12.64 times, Y2S3 + 3 H? 3KHS + 2Y (82) Y2S3 + 6KH + 3Mg ¾ 3K2S + 2Y + 3MgH2 (83) Y2S3 + 3Mg ^ '3MgS + 2Y. (84) | 4g AC3-5 + lg Mg + 1.66g KH + 1.82g Ca3P2; Ein: 133. 0 kJ; dE: 5.8 kJ; TSC: none; Tmax: 407 ° C, the theoretical is endothermic, the gain is infinite. | 20g AC3-5 + 5g Mg + 8.3g KH + 9. lg Ca3P2, Ein: 282. lkJ, dE: 18.1 kJ, TSC: none, Tmax: 320 ° C, the theoretical is endothermic, the gain is infinite.

Ca3P2 + 3Mg ¾ Mg3P2 + 3Ca. (85) In one embodiment, the thermally regenerative reaction system comprises: (i) at least one catalyst or catalyst source chosen from NaH and KH; (ii) at least one hydrogen source chosen from NaH, KH, and MgH2; . (iii) at least one oxidant chosen from an alkaline earth halide, such as BaBr2, BaCl2, Bal2, CaBr2, MgBr2 or Mgl2, a rare earth halide such as EuBr2, EuBr3, EuF3, Dyl2, LaF3 or GdF3 (a halide metal of the second or third series of transition metal such as YF3, a metal boride such as CrB2 or TiB2, an alkali halide such as LiCl, RbCl, or Csl, a metal sulfide such as Li2S, ZnS or Y2S3 / a metal oxide such as Y203, and a metal phosphide such as Ca3P2; (iv) at least one reducer chosen from Mg and MgH2; Y (v) a chosen support of activated carbon, Tic, and WC.

F. Auxiliary Hydride Reaction by Rarefactor, Support or Matrix In one embodiment, the exchange reaction is endothermic. In such an embodiment, the metal compound can serve as at least one of a support or matrix favorable for the reaction of hydrino or rarefactor for the product to improve the hydrino reaction rate. Exemplary catalyst reagents and with an exemplary support, matrix or rarefactor are given below. These reactions are not intended to be exhaustive and additional examples would be known to those skilled in the art. 4g of AC3-5 + lg Mg + 1.66g KH + 2.23g Mg3As2, Ein: 139.0 kJ, dE: 6.5 kJ, TSC: none, Tmax: 393 ° C, the theoretical is endothermic, the gain is infinite. | 20g of AC3-5 + 5g Mg + 8.3g KH + 11.2g Mg3As2, Ein: 298.6 kJ, - dE: 21.8 kJ, TSC: none, Tmax: 315 ° C, the theoretical is endothermic, the gain is infinite. | 1.01 g of Mg3N2, 1.66 g of KH, 1 g of Mg powder and 4 g of AC3-4 in a heavy use cell of 2.5 cm (1 inch), the energy gain was 5.2 kj, but no He observed no explosion of cell temperature. The maximum temperature of the cell was 401 ° C, the theoretical temperature is 0, the gain is infinite. . | 0.41 g of AlN, 1.66 g of'KH, 1 g of Mg powder and 4 g of AC3-5 in a 2.5 cm (1 inch) heavy-use Celtic, the energy gain was 4.9 kj, but not no explosion of cell temperature was observed. The maximum temperature of the cell was 407 ° C, the theoretical temperature is endothermic.

In one embodiment, the thermally regenerative reaction system comprises at least two components chosen from (i) - (v): (i) at least one catalyst or catalyst source chosen from NaH, KH, and MgH2; (ii) at least one hydrogen source chosen from NaH and KH; (iii) at least one oxidant, matrix, second support or rarefactor chosen from a metal arsenide such as Mg3As2 and a metal nitride such as Mg3N2 or AlN; (iv) at least one reducer chosen from Mg and MgH2; And < ( (v) at least one chosen support of activated carbon, Tic, or WC.

D. Liquid Fuels: Organic Solvent Systems and Cast Additional embodiments comprise a molten solid such as a molten salt or a liquid solvent contained in the chamber 200. The liquid solvent can be vaporized by operating the cell at a temperature higher than the boiling point of the solvent. Reagents such as the catalyst can be dissolved or suspended in the solvent or. reagents that form the catalyst and H can be suspended or. dissolved in the solvent. A vaporized solvent can act as a gas with the catalyst to increase the rate of the hydrogen catalysis reaction to form hydrinos. The molten solid or vaporized solvent may be maintained by applying heat with the heater 230. The reaction mixture may further comprise a solid support such as an HSA material. The reaction may occur on the surface due to the interaction of a molten solid solvent, a liquid solvent or a gaseous solvent with the catalyst and hydrogen such as K or Li plus H or NaH. In an embodiment using a heterogeneous catalyst, a solvent in the mixture can increase the reaction rate of the catalyst.

In embodiments comprising hydrogen gas, the H2 can be bubbled through the solution. In another embodiment, the cell is pressurized to increase the concentration of dissolved ¾. In a further embodiment, the reagents are agitated, preferably at high speed and at a temperature that is around the boiling point of the organic solvent and around the melting point of the inorganic solvent.

The reaction mixture of organic solvent can be heated, preferably in the temperature range of about 26 ° C to 400 ° C, more preferably in the range of about 100 ° C to 300 ° C. The mixture of inorganic solvents can be heated to a temperature above that at which the solvent is liquid and below a temperature that causes the total decomposition of the NaH molecules. to. Organic Solvents The organic solvent may comprise. one or more of , the portions that can be modified to solvents, additional by adding functional groups. The portions may comprise at least one of a hydrocarbon such as an alkane, cyclic alkane, alkene, cyclic akene, alkyne, aromatic, heterocyclic, and combinations thereof, ether, halogenated hydrocarbon (fluoro hydrocarbon, chlorine, bromine, iodine) , preferably fluorinated, amine, sulfur, nitrile, phosphoramide (eg, OP (N (CH 3) 2) 3), and aminophosphazene. The groups may comprise at least one of alkyl, cycloalkyl, alkoxycarbonyl, cyano, carbamoyl, heterocyclic rings containing C, O, N, S, sulfo, sulfamoyl, alkoxysulfonyl, phosphono, hydroxyl, halogen, alkoxy, alkylthiol, acyloxy-, aryl, alkenyl, aliphatic, acyl, carboxyl, amino, cyanoalkoxy, diazonium, carboxyalkylcarboxamido, alkenylthio, cyanoalkoxycarbonyl, carbamoylalkoxycarbonyl, alkoxycarbonylamino, cyanoalkylamino, alkoxycarbonylalkylamino, sulfoalkylamino, alkylsulfamoylalkylamino, oxido, hydroxy alkyl, carboxy alkylcarbonyloxy, cyanoalkyl, carboxyalkylthio, arylamino, heteroarylamino ,. alkoxycarbonyl, alkylcarbonyloxy, cyanoalkoxy, alkoxycarbonylalkoxy, carbamoylalkoxy, carbamoylalkyl, carbonyloxy, sulfoalkoxy, nitro, alkoxyaryl, halogenarilo, amino aryl, alkylaminoaryl, tolyl, alkenylaryl, alilarilo, alqueniloxiarilo, aliloxiarilo, cyanoaryl, carbamoilarilo, carboxyaryl, alkoxycarbonylaryl, alkylcarbonyloxyaryl, sulfoaryl, alcoxisulfoarilo , sulfamoyilaryl and nitroaryl. Preferably, the groups comprise at least one of alkyl, cycloalkyl, alkoxy, cyano, heterocyclic rings containing C, 0, N, S, sulfo, phosphono, halogen, alkoxy, alkylthiol, aryl, alkenyl, aliphatic, acyl, alkylamino, alkenylthio, arylamino, heteroarylamino, halogenaryl, amino aryl, alkylaminoaryl, alkenylaryl, allylaryl, alkenyloxyaryl, allyloxyaryl and cyanoaryl groups.

The catalyst can be at least one of molecules of NaH, Li and K. In the latter case, LiH and KH can serve as the source of the catalyst. The solvent can be an organic solvent. The solvent may be substantially vaporized at the operating temperature of the cell which is preferably higher than the boiling point of the solvent. Preferably, the solvent is polar. The solvent can be an aprotic solvent. Polar aprotic solvents are solvents that share ion dissolving power with porous solvents such as water, methanol, ethanol, formic acid, fluoride. hydrogen and ammonia, but lack an acid hydrogen. These solvents generally have high dielectric constants and high polarity. Examples are dimethyl sulfoxide, dimethylformamide, 1,4-dioxane and hexamethylphosphoramide.

In one embodiment of the present disclosure, the solvent comprises an ether such as at least one of the group of 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, dibutyl ether of diethylene glycol, bis (2-ethylhexyl) ether, sec-butyl ethyl ether, dicyclohexyl ether, diethyl ether of diethylene glycol, 3,4-dihydro-lH-2-benzopyran, 2,2'-dimethoxybiphenyl, 1,6-dimethoxyhexane, substituted aromatic ethers such as methoxy benzene, methoxy toluene, 2,5-dimethoxy toluene, diphenoxybenzene such as 1,4-diphenoxybenzene, allyl phenyl ether, dibenzyl ether, benzyl phenyl ether , n-butyl phenyl ether, trimethoxytoluene such as 3,4,5-trimethoxytoluene, 2,2'-dinaphthyl e ter, 2- [2- (benzyloxy) ethyl] -5,5-dimethyl-1,3-dioxane, 1,3-benzodioxole, veratrol (1,2-dimethoxybenzene), anisole, bis (phenyl) ether, 1,4-dioxin, dibenzodioxin or dibenzo [1,4] dioxin, divinyl ether, coronary ethers such as dicyl exano-18-crown-6, dibenzo-18-crown-6, .15-crown-5, and 18 -Cone-6, bis (4-methylphenyl) ether, bis (2-cyanoethyl) ether, bis (2-dimethylaminoethyl) ether and bis [2- (vinyloxy) ethyl] ether. In an embodiment comprising Na and a source of hydrogen, an ether is an exemplary solvent, since Na is somewhat soluble in ether, and also stabilizes the sodium ions. These elements favor the hydrino reaction. In addition to NaH, K or Li can serve as the catalyst of a reaction mixture also comprising an ether solvent.

In one embodiment, the solvent or HSA material comprises functional groups with a high bonding moment such as C-O, C = 0, C = N and C-F. The molecules of the solvent or HSA material can have a high dipole moment. Preferably, the solvent or HSA comprises at least one of an ether, nitrile or halogenated hydrocarbons, preferably having very stable, preferably polar bonds, such as fluorinated hydrocarbons. Preferably, the fluorocarbon solvent has the formula CnF2n + 2 and may also have some H instead of F or it may be aromatic. In another embodiment, the solvent or HSA comprises at least one of the groups of fluorinated organic molecules, fluorinated hydrocarbons, fluorinated alkoxy compounds, and fluorinated ethers. Exemplary fluorinated solvents are 1,2-dimethoxy-4-fluorobenzene, hexaflorobenzene, perfluoroheptane, octafluoronaphthalene, octafluorotoluene, 2H-perfluoro-5, 8, 11, 14-tetramethyl-3, 6, 9, 12, 15-pentaoxaoctadecane, perfluoro -5, 8, 11, 14-tetramethyl-3, 6, 9, 12, 15-pentaoxaoctadecane, perfluoro (tetradecahydrophenanthrene), and perfluoro-1,3,5-.trimethylcyclohexane. Exemplary fluorinated HSAs are TEFLON ™, TEFLON ™ -PFA, polyvinyl fluoride, PVF, poly (vinylidene fluoride), poly (vinylidene-co-hexafluoropropylene fluoride), and perfluoroalkoxy polymers. A suitable reaction mixture comprises octafluoronaphthalene, NaH and a support such as activated carbon, Tic, -WC, or R-Ni. The reagents may be in any desired proportion such as octafluoronaphthalene (45 weight percent), NaH (10 weight percent), and R-Ni (45 weight percent).

Another exemplary solvent is a fluorocarbon such as one having the formula CnF2n + 2 / Y may also have some H instead of F or it may be aromatic. In one modality, the.

The fluorinated solvent comprises at least one of the group and derivatives of perfluoro-methane, perfluoro-ethane, perfluoro-propane, perfluoro-heptane, perfluoro-pentane, perfluoro-hexane, and perfluoro-cyclohexane, as well as other chain perfluoro-alkanes straight and branched 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-difluoroethane, 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'-biohenyl, 4-fluoro-1, 1'-biohenyl, 1-fluorobutane, 2-fluorobutane, fluorocyclohexane, 1-fluorocyclohexene, 1-fluorodecane, fluoroethane, fluoroethene, 1-fluoroheptane, 1-fluorohexane, fluoromethane, l-fluoro-2-methoxybenzene, 1-fluoro-3-methoxybenzene, l-fluoro-4- methoxybenzene, (fluoromethyl) benzene, 2-fluoro-2-methylpropane, 1-fluoronaphthalene, 2-fluoronaphthalene, 1-fluorooctane, 1-fluoropentane, 1-fluoropropane, 2-fluoropropane, cis-1-fluoropropene, trans-l-fluoropropene , 2-fluoropropene, 3-fluoropropene, 2-fluoropyridine, 3-fluoropyridine, 2-fluorotoluene, 3-fluorotoluene, 4-fluorot oluene, l-fluoro-2- (trifluoromethyl (benzene, 1-fluoro-3- (trifluoromethyl) benzene, 1-fluoro-4- (trifluoromethyl) benzene, 1,1,1,2,3,3,3-heptafluoro -propane, hexafluorobenzene, 1, 1, 2, 3, 4, 4-hexafluoro-1,3-butadiene, 1, 1, 4, 4, 4-hexafluoro-2-butyne, hexafluoro-cyclobutene, hexafluoroethane, , 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, perfluoro-2, 3-dimethylbutane, perfluoroethyl ethyl ether, perfluoroethyl 2,2,2-trifluoroethyl ether, perfluoroheptane, perfluoro-1-heptane, perfluorohexane, perfluoro-1-hexene, perfluoroisobutane, perfluoroisobutene, perfluoroisopropyl methyl ether, perfluoromethylcyclohexane, perfluoro- 2-methylpentane, perfluoro-3-methylpentane, perfluoronaphthalene, perfluorononane, perfluorooctane, fluoride perfluorooctylsulfonyl, perfluorooxetano, perfluoropentane, perfluoropropane, perfluoropropene, perfluoropropyl methyl ether, perfluoropiridina, perfluorotolueno, perfluorotripropylamine, 1, 1, 1, 2-tetrafluoroethane, 1, 1, 2, 2-tetrafluoroethane, 1,2,2,2-tetrafluoroethyl difluoromethyl ether, tetrafluoromethane, triflumizole, trifluoperazine, 1,2,4-trifluorobenzene, 1,3,5-trifluorobenzene, 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 r, 1,1,1-trifluoropropane, 3,3,3-trifluoropropene, 3,3,3-trifluoro-1-propyne, triflupromazine, undecafluorocyclohexane, pentafluorobenzonitrile, trifluoroacetonitrile, (trifluoromethyl) benzene, 3- (trifluoromethyl) benzonitrile, 4- (tri-fluoromethyl) -benzonitrile, trifluoro (trifluoromethyl) oxirane, and tris (per-fluorobutyl) amine.

In another embodiment, the solvent comprises a hydrocarbon such as those having functional groups for the list of straight and branched chain alkanes, alkenes, and aromatics. The hydrocarbon solvent may be at least one of or derivatives of the group comprising acenaphthene, acenaphthylene, allylbenzene, 1-alkylcyclohexene, allylcyclopentane, anthracene, benz [a] anthracene, benzene, benzo [c] chrysene, benzo [g] chrysene, benzo [b] fluoranthene, benzo [j] fluoranthene, benzo [k] fluoranthene, llH-benzo [a] fluorine, 11H-benzo [b] fluorine, benzo [ghilperylene, benzo [c] phenanthrene, benzo [a] pyrene, benzo [e] pyrene, benzo [b] triphenylene, 9,9'-biantracene, bicyclo [2.2.l] heptane, bicyclo [4.1.0] heptane, bicyclo [2, 2, 1] hept-2-ene , 1,1 '-bicyclopentyl, 1,1'-binaphthalene, 2,2' -bibphthalene, biphenyl, 1,3-bis (l-methylethyl) benzene, (trans) -1,3-butadienylbenzene, 1,3- butadiino, butane, 1-butene, cis-2-butene, t.rans-2-butene, (fcrans-l-butenyl) benzene, 2-butenylbenzene, 3-butenylbenzene, l-buten-3-yne, butylbenzene, sec -butylbenzene, (±), f-butylbenzene, 2-butyl-l, 1'-biphenyl, butylcyclohexane, sec-butylcyclohexane, tert-butylcyclohexane, b utilcyclopentane, 1-tert-butyl-3, 5-dimethylbenzene, 5-butyldocosane, 11-butyldocosane, 1-tert-butyl-4-ethylbenzene, 1-f-butyl-2-methylbenzene, 1-tert-butyl-3 methylbenzene, 1-tert-butyl-4-methylbenzene, 1-butylnaphthalene, 2-butylnaphthalene, 5-butylnonhane, camphene, (+), camphene, (-), 3 -carene, (+), α-carotene, β- carotene, ß,? -carotene,?,? -carotene,?,? - caroten-16-ol, cholestane, (5a), cholestane, (5ß), cyclobutane, cyclobutene, cyclodecane, cyclododecane, 1,5,9- cyclododecatriene, cis-cyclododecene, trvans-cyclododecene, 1,3-cycloheptadiene, cycloheptane, 1, 3, 5-cycloheptatriene, cyclohepten, 1,3-cyclohexadiene, 1,4-cyclohexadiene, cyclohexane, cyclohexene, 1-cyclohexen-1- ilbenzene, cyclohexylbenzene, cyclohexylcyclohexane, cyclononane, 1,4-cyclooctadiene, cis, cis-1,5-cyclooctadiene, cycloocatane, 1,3,5,7-cyclooctatetraene, 1,3,5-cyclooctatriene, cis-cyclooctene, trans- cyclooctene, cyclooctin, cyclopentadecane, 1,3-cyclopentadiene, cyclopentane, cyclopentene, cyclopentylbenzene, 1,3-decanediene, 1,9-decanediene, cis-decahydronaphthalene, trans-decahydronaphthalene, decane, 1-decene, cis-2-decene, trans-2 -decene, cis-5-decene, trans-5 -decene, decylbenzene, decylcyclohexane, decylcyclopentane, 11-decylheneicosane, 1-decylnaphthalene, 1-decino, 5-decino, dibenz [a, h] anthracene, dibenz [a, j] anthracene, dibenzo- [b, k] chrysene, dibenzo [a, ejpyrene, dibenzo [a, h] pyrene, dibenzo [a, ilpirene, dibenzo [a, l] pyrene, s-diethylbenzene, m-diethylbenzene, · p-diethylbenzene, 1,1-diethylcyclohexane, 1,2 -dihydrobenz [] aceanthrylene, 9, 10-dihydro-9, 10 [1 ', 2'] -benzene-anthracene, 16, 17-dihydro-15H-cyclopenta [a] phenanthrene, 2,3-dihydro-l-methyl -lH-indene, 1,2-dihydronaphthalene, 1,4- * dihydronaphthalene, 9, l-dihydrophenanthrene, 2,3-dihydro-l, 1,3-trimethyl-3-phenyl-lH-indene, 1,2-diisopropylbenzene, 1,3-diisopropylbenzene, 1,4-diisopropylbenzene, 2, 6-diisopropylnaphthalene, 7, 12-dimethylbenz [a] anthracene, 2,2'-dimethylbiphenyl, 2,3-dimethyl-1,3-butadiene, 2,2-dimethylbutane, 2,3-dimethylbutane, 2,3-dimethyl -l-butene, 3, 3-dimethyl-1-butene, 2,3-dimethyl-2-butene, 3, 3-dimethyl-l-butyne, 1,1-dimethylcyclo-exano, cis-1,3-dimethylcyclohexane, trans-1, 3-dimethylcyclohexane, cis-1,4-dimethylcyclohexane, trans-1,4-dimethylcyclohexane, 1,2-dimethylcyclohexene, 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-dimethylcycloper.tene, 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-dimethylheptane, 2,5-dimethyl-1,5-hexadiene,. 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- ene, 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-l, 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-3,1-dimethyl-1,3,6-octatriene, trans-3,7-dimethyl-1,3,6 -octarieno, 3. 7-dimethyl-1,3,7-octariene, trans, trans-2,6-dimethyl-2,4,6-octariene, trans, trans-2,6-dimethyl-2,4,6-octariene, 3, 7-dimethyl-l-octene, dimethyl-1,3-pentadiene, 2,2-dimethylpentane, 2,3-dimethylpentane, 2,4-dimethylpentane, 3,3-diraethylpentane, 2,3-dimethyl-l-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-dimethyl-2-pentene, 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, 3-butadiene, 1,4-diphenyl-1,3-butadiino, 1,1-diphenylbutane, 1,2-diphenylbutane, 1,4- diphenylbutane, 1,3-diphenyl-1-butene, 1,1-diphenylethane, 1,2-diphenylethane, 1,1-diphenylethene, 1,6-diphenyl-1,3,5-hexatriene, diphenylmethane, 1,3- diphenylpropane, 2, 2-d asenylpropane, 1,1-diphenyl-1-propene, 1,2-di (p-tolyl) ethane, o-divinylbenzene, m-divinylbenzene, p-divinylbenzene, docosane, 1-docosine, 5,7-dodecadiin, dodecane, dodecylcyclohexane, 1-dodecyl, 6-dodecyl, dotriacontane, eicosane, ergostane, (5a), ergostane, (5ß), ethane, ethylbenzene, ethylcyclohexane, 1-ethylcyclohexene, ethylcyclopentane, 1-ethylcyclopentene, l-ethyl-2,4- dimethylbenzene, l-ethyl-3, 5-dimethylbenzene, 2-ethyl-l, 3-dimethylbenzene, 3-ethyl-l, 2-dimethylbenzene, 4-ethyl-l, 2-dimethylbenzene, 3-ethyl-2, 2- dimethylpentane, 3-ethyl-2,3-dimethylpentane, 3-ethylheptane, 4-ethylheptane, 3-ethylhexane, ethylidenecyclohexane, l-ethyl-2-isopropylbenzene, 2-ethyl-3-methyl-1-butene, trans-l -ethyl-4-methylcycloexan, 1-ethyl-1-methylcyclopentane, cis-1-ethyl-2-methylcyclopentane, traris-1-ethyl-2-methylcyclopentane, cis-1-ethyl-3-methylcyclopentane, trans-1 -ethyl-3-methylcyclopentane, 3-ethyl-4-methylhexane, 4-ethyl-2-methylhexane, 3-ethyl-2-methylpentane, 3-ethyl-3-methylpentane, 3-ethyl-2-methyl-1-pentene , 1-etilnaft allene, 2-ethylnaphthalene, 3-ethyl-octane, 4-ethyl-octane, 3-ethylpentane, 2-ethyl-1-pentene, 3-ethyl-1-pentene, 3-ethyl-1-pentene, 3-ethyl-2-pentene, 2-ethylstyrene, 3-ethylstyrene, 4-ethylstyrene, 2-ethyl toluene, 3-ethyl toluene, 4-ethyl toluene, l-ethyl-2,4,5-trimethylbenzene, 2-ethyl-1,3,5-trimethylbenzene "fluoranthene, fulvene, heneicosane, hentriacontane, heptacosane, heptadecane, 1-heptadecene, heptadecylbenzene, 1,6-heptadiene, 1,6-heptadiin, 2, 2, 4, 4, 6, 8, 8-heptamethylnonano, heptane, 1-heptene, cis-2-heptene, trans-2-heptene, cis-3-heptene, trans-3-heptene, heptylcyclohexane, heptylcyclopentane, 1-heptin, 2-heptin, 3-heptin, hexacene, hexacosane, hexadecane, 1-hexadecene, hexadecylbenzene, 1-hexadecin, '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, -hexadiene, 1, 5 hexadien-3-yne, 1,5-hexadiino, 2,4-hexadino, hexaethylbenzene, cis-1, 2,3,5,6,8a-hexahydro-4,7-dimethyl-l-isopropylnaphthalene, (1S), hexamethylbenzene, 2, 6, 10, 15, 19, 23-hexamethyltetracosane, 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, , hexyl benzene, hexylcyclohexane, hexylcyclopentane, 1-hexylnaphthalene, 1-hexyl-1, 2, 3, 4-tetrahydronaphthalene, 1-hexin, 2-hexin, 3-hexin, indane, indene [1, 2, 3-cd] pyrene , isobutane, isobutene, isobutylbenzene, isobutylcyclohexane, isobutylcyclopentane, isopentane, isopentylbenzene, isopropenylbenzene, p-isopropenylizopropylbenzene, p-isopropenylstyrene, isopropylcyclohexane, 4-isopropylheptane, l-isopropyl-2-methylbenzene, l-isopropyl-3-methylbenzene, 1-isopropyl-4-methylbenzene, 5-isopropyl-2-methyl-1, 3-cyclohexadiene,, (R), 1-isopropylnaphthalene, 2-isopropylnaphthalene, d-limonene, J-limonene, [2, 2] metacyclofan, 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, l-methyl-2-benzylbenzene, l-methyl-4-benzylbenzene, 2-methylbiphenyl, 3-methylbiphenyl, 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-l-buten-3-yne, 3-methyl-l-butyne, 3-methyl-criene, 5-methyl-criene, 6-methyl-criene, 2-methyl-1,3-cyclohexadiene, 1- methylcyclohexene, 3-methylcyclohexene, (±), 4-methylcyclohexene, 1-methyl-l, 3-cyclopentadiene, methylcyclopentane, 1-methylcyclopentene , 3-methylcyclopentene, 4-methylcyclopentene, 2-methydecane, 3-methydecane, 4-methyldecane, 4-methyl-2,4-diphenyl-1-pentene, methylenecyclohexane, 3-methylene-leptan, 4-methylene-l-isopropyl-cyclohexene, - (1-methylethylidene) -1,3-cyclopentadiene, l-methyl-9H-fluorene, 9-methyl-9H-fluorene, 2-methylheptane, 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, trans-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-l-methyl-4-isopropylcyclohexane, trans-l-methyl-4-isopropylcyclohexane, l-methyl-4-isopropylcycloene, 1-methyl-7-isopropylphenanthrene, 3-methyl- 4-Methylene hexane, l-methyl-4- (5-methyl-1-methylene-4-hexenyl) cyclohexene,. (S), l-methyl-4- (1-methylvinyl) benzene, 1-methylnaphthalene, 2-methylnaphthalene, 2-methyl-nonane, 3-methyl-nonane, 4-methyl-nonane, 5-methyl-nonane, 2-methyl-l-nonene, 2 -methyl-2-norbornene, 2-methyloctane, 3-methyloctane, 4-methyloctane, 2-methyl-l-octene, 7-methyl-l-octene, cis-2-methyl-l, 3-pentadiene, 3-methyl -l, 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-tirans-2-pentene, 4-methyl-cis-2-pentene, 4-methyl-trans-2-pentene, 3-methyl -3-penten-1-yne, 4-methyl-l-pentyne, 4-methyl-2-pentyne, 1-methylphenanthrene, 3-methylphenanthrene, 4-methylphenanthrene, 2-methyl-l-propene, tetramer, cis- ( 1-methyl-1-propenyl) benzene, trans- ('1-methyl-1-propenyl) benzene, 1-methyl-2-propylbenzene, 1-methyl-3-propylbenzene, 1-methylpyrne, 2-methylpyrne, 2- methylstyrene, 3-methylstyrene, 4-methylstyrene, 2-methylundecane, 3-methylundecane, l-methyl-4-vinylcyclohexane, ß-myrcene, naphthacene, naphthalene, nonadecane, 1, 8-nonadiene, 1, 8-nonadiino, nonane, 1-nonane, nonylbenzene, nonylcyclohexane, nonylcyclopentane, 1-nonylnaphthalene, 1-nonino, octacosane, octadecahydro-crisene, octadecane, 1-oct'adecene, octadecylbenzene, octadecylcyclohexane , 1, 7-octadiene, 1,7-octadiin, 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, l-octen -3-ino, octylbenzene, octylcyclohexane, octylcyclopentane, 1-octino, 2-octino, 3-octinot 4-octino, 1,3-pentadiino, pentaethylbenzene, 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, pentafeno, pentatriacontane, 1-pentene, cis- 2-pentene, thia-2-pentene, l-penten-3-yne, 1-penten-4-yne, cis-3-penten-l-n, trans-3-penten-l-n, pentylbenzene, pentylcyclohexane, pentylcyclopentane, 1-pentylnaphthalene, 1-pentyne, 2-pentyne, perylene, α-phellandrene, β-phellandrene, phenylerene, phenylacetylene, 9-phenylanthracene, 2-phenyl-1,3-butadiene, 2-phenyl-1-butene , 1-phenyl-1H-indene, 1-phenylnaphthalene, 2-phenylnaphthalene, 5'-phenyl-1, 1 ': 3', 1"-terphenyl, pentane, propane, propene, cis-l-propenylbenzene, trans-1 -propenylbenzene, propylbenzene, propylcyclohexane, propylcyclopentane, 4-propylheptane, 1-propylnaphthalene, pyrene, 1, 1 ': 4', 1": 4", 1 '' '-cuat'erphenyl, spiro [5.5] undecane, squalene, cis-stilbene, fcrans-stilbene, styrene, o-terphenyl, m-terphenyl, p-terphenyl, α-terpinene,. ? -terpinene, tetracosane, tetradecahydrophenanthrene, tetradecane, tetradecylbenzene, tetradecylcyclohexane, 1,2,3,5-tetraethylbenzene, 1, 2, 3, 4-tetrahydro-l, 5-dimethylnaphthalene, 1,2,3,4-tetrahydro-l-methylnaphthalene, 1,2,3-tetrahydro-5-methylnaphthalene, 1,2,3,4-tetrahydro-6-methylnaphthalene, 1,2,3,4-tetrahydronaphthalene , 1, 2, 3, 4-tetrahydrophenanthrene, 1,2,3,4-tetrahydro-1,1,6-trimethylnane, 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-tetramethylcyclopentane, 1,2,2-tetramethylcyclopropane, 2, 2, 3, 3-tetramethylhexane, 2, 2, 5, 5-tetramethylhexane, 3,3,4,4-tetramethylhexane, 2, 2, 3, 3-tetramethylpentane, 2,2,3,4-tetramethylpentane, 2,, 4, 4-tetramethylpentane, 2,3,3,4-tetramethylpentane, 1, 1, 4, 4-tetraphenyl-1,3-butadiene, 1,1,2,2-tetraphenylethane, 1, 2 , 2-tetraphenylethane, tetraphenylmethane, 5, 6, 11, 12-tetraphenylnaphthacene, triacontane, tricosane, tricyclo [3.3.13'7] decane, tridecane, 1-tridecene, tridec, benzene, tridecylcyclohexane, 1-tridecyne, 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-trimethyl-bicyclo [2.2. l] hept-2-ene, 2, 2, 3-trimethylbutane, 2,3-trimethyl-1-butene, 1, 1, 2-trimethylcyclohexane, 1, 1,3-trimethyl-cyclopentane, 1a, 2a, 4β-1, 2,4-trimethylcyclopentane, 2,2,6-trimethylheptane, 2,5,5-trimethylheptane, 3,3,5-trimethylheptane, 3,4,5-trimethylheptane, 2,2,3-trimethylhexane, 2,2,4-trimethylhexane, 2,3-trimethylpentane, 2,3-trimethylpentane, 2,3-trimethyl-1-pentene, 2,4,4-trimethyl-1-pentene, 2 , 3,4-trimethyl-2-pentene, 1,1-trifenylethane, 1,1-trifenylethene, triphenylmethane, tritriacontane, 1, 10-undecadiino, undecane, 1-undecane, cis-2-undecane, trans -2-undecane, cis-4-undecane, trans-4-undecane, cis-5-undecane, trans-5-undecane, undecylbenzene, 1-undecyne, 2-undecyne, vinyl cyclohexane, 1-vinylcyclohexane, 4-vinylcyclohexane, vinylcyclopentane, 6-vinyl-6-methyl-l-isopropyl-3-l- (1-methylethylidene) cyclohexene, (S), 1-vinylnaphthalene, 2-vinylnaphthalene, 2-vinyl-5-norbornene, o-xylene, jn -xylene, p-xylene.

In another embodiment, the solvent comprises at least one of the group of amines such as tributylamine, triethylamine, triisopropylamine,?,? -dimethylaniline, tris (N, N-dimethylaniline), allyldiethyl amine, allyldimethylamine, benzo [f] quinoline, bis [4- (dimethylamino) phenyl] methane, 4,4'bis- (dimethylamino) triphenylmethane, butyldimethylamine, hydrocarbon solvents such as alkanes, alkenes and alkynes, such as pentane, hexane, heptane, octane, cyclopentane, cyclohexane, dipentene , methylcyclohexane, 2-methylpentane, octane, tetrahydrofuran (THF), pinene, styrene, terpinene and mineral oil, aromatic and heterocyclic aromatics such as toluene, o-xylene, m-xylene, p-xylene, ethylbenzene, eumeno (isopropylbenzene), p-cymene (l-methyl-4-isopropylbenzene), mesitylene (1, 3, 5 -trimethylbenzene), propylbenzene, pseudocumene (1,2,4-trimethylbenzene), naphthalene, decalin (cis and trans-decahydronaphthalene), tetralin (1, 2, 3, -tetrahydronaphthalene), pyrrole, furan, 2,5-diphenylfuran, thiophene, imidazole, pyridine, pyrimidine, pyrazine, quinoline, isoquinoline, indole, acridine, 1,2-dimethylindole, 9,9 '-dixantilidene, 2,6-lutidine (2,6-dimethylpyridine), 2-picoline (2- methylpyridine), and nitriles such as acetonitrile and propanenitrile. In one embodiment, the amino group is linked to aryl. Suitable amino solvents are α, β-dimethylaniline analogues such as N-benzyl-N-ethylaniline, preferably with multiple amino groups alkylated on an aryl such as 1, 3, 5-tris- (N, N-dimethylamino) benzene .

In another embodiment, the solvent comprises at least one of the group and derivatives of dimethylformamide (DMF), dimethylacetamide (DMA), dimethyl sulfoxide (DMSO), 1,3-dimethyl-2-imidazolidinone (DMI), hexamethylphosphoramide (HMPA), N-methyl-2-pyrrolidone (NMP), 4-dimethylaminobenzaldehyde, acetone, dimethyl acetone-1,3-dicarboxylate, 3 ', 4'-dimethylacetophenone, dimethyl methyl phosphonate, hexamethylcyclotrisiloxane, hexamethylphosphorus triamide, tributyl phosphite, tributyl borate, triethyl borate, tri-n-butyl borate, triphenylboro, triethyl phosphite, triethylphosphine, tri-n-butylphosphine, trimethyl borate, trimethylene borate, trimethyl phosphite, triphenyl phosphite, tris (phenyl) phosphine, organometallic such as ferrocene, nickelocene, organometallic, dimethyl selenium, dimethyl telulide, tetraethyl lead, ethyltrimethylphenyl , tetra-n-butylpomo, phenylthiobenzene, and diphenyl selenide, trimethyl stibin, tetra-n-butylgermanium, tetrapropyl titanate, tetrabutyl titanate, tributyl aluminate, tributyl aluminum, triethyl stibin, trimethylarsine, trimethyl indium, and trimethylstyine, sulfides of alkyl such as diethyl sulfide and bis (phenyl) sulfide, alkyl selenides such as diethyl selenides, alkyl telulides such as diethyl telluride, diethylsulfoxide, allyl ethyl ether, aluminum ethanolate, aluminum ethoxide, sec-butoxide aluminum, trimethyl borate, triethyl borate, tripropyl borate, tributyl borate, trihexyl borate, trimethylstyline, 1,3-benzodioxole, benzo furan, 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 (l-methyl-4-piperidyl) propane, bis (4-methylphenyl) ether, bis (phenyl) ether, bis (4-methylphenyl) sulfide, bis (methylthio) methane, 1,2-bis (N-morpholino) ethane , 2, 2 '-bitiofen, 1- (2-butoxyethoxy) -2-propanol, l-butoxy-4-methylbenzene, 4- [3- (4-butoxy phenoxy) propyl] morpholine, butyl ethyl ether, sec-butyl ether, t-butyl ethyl ether, sulfur butyl ethyl, t-butyl ethyl sulfide, butyl isobutyl ether, t-butyl isobutyl ether, t-butyl isopropyl ether, l-butyl-4-methoxybenzene, butyl methyl ether, sec-butyl methyl ether, butyl phenyl ether, N- butylpiperidine, butyl propyl ether, butyl vinyl ether, t-butyl vinyl ether, dibenzyl ether, 1,4-dibutoxybenzene, 1,2-dibutoxyethane, dibutoxymethane, dibutyl ether, di-sec-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-diethoxyethane, 1,2-diethoxyethane, diethoxymethane, 2- (diethoxymethyl) furan, 1,1-diethoxy pentene, 1,1-diethoxypropane, 2,2-diethoxypropane, 3,3-diethoxy-1-propene, 3,3-diethoxy-1-propyne, N, -diethylaniline, dibutyl ether of diethylene glycol, diethylene glycol diethyl ether, diethylene glycol dimethyl ether, diethyl telulide, difurfuryl ether, diheptyl ether, dihexyl ether, 2, 3-dihydro-l, 4-benzodioxine, 2,3-dihydrobenzofuran, 3. 4-dihydro-lH-2-benzopyran, 3,4-dihydro-2H-l-benzopyran, 2. 5-dihydro-2, 5-dimethoxyfuran, 2,3-dihydro-1,4-dioxin, 3,6-dihydro-4-methyl, -2H-pyran, 4,5-dihydro-2-methyltriazole, 3,4 -dihydro-2H-pyran, 3,6-dihydro-2H-pyran, diisopentyl ether, diisopropyl ether, 1,2-dimethoxybenzene, 1,3-dimethoxybenzene, 1, -dimethoxybenzene, 1,2-dimethoxyethane, 4, 8- dimethoxyfuro [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-lH-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, -diethylaniline, 2-ethoxy-3,4-dihydro-2H-pyran, 1-ethoxy-2-methoxyethane, ethyltrimethylphenyl, indolizine, 4-methoxypyridine, 6-methoxyquinoline, l-methyl-3-phenoxybenzene, l-methyl-4- (phenylthio) ene, methyltriethylpomo, 1,4-oxatiano, oxazole, oxepane, pteridine, tetraethoxygermanium, titanium n-butoxide (IV), tetrapropyl titanate, tributyl aluminate, tributyl aluminum, tributyl borate , tributyl phosphite, 1, 3, 5-triethoxybenzene, borate. of triethyl, triethylphosphine, triethyl phosphite, triethyltibine, trimethylindium, trimethyl phosphite, trimethylstyline, triphenylstymine, N- (1-cyclopenten-1-yl) pyrrolidine, cyclopentyl methyl sulfide, decamethylcyclopentasiloxane, decamethyltetrasiloxane, N, N-diallyl-2-propen -l-amine, diallyl sulphide, dibenzofuran, benzo [b] thiophene, dibenzothiophene, dibenzyl sulfide, N, -dibutylaniline, 2,6-di-tert-butylpyridine, dibutyl sulfide, di-sec-butyl sulfide, di-butyl sulfide, didecyl ether, diethylmethylamine, N, N-diethyl-2-methylaniline, N, N-diethyl-4-methylaniline, N, N-diethyl-1-naphthalenamine, N, N-diethyl-10H -phenothiazine-10-ethanamine, N, N-diethyl-a-phenylbenzenemethanamine, diethyl sulfide, diheptyl sulphide, dihexyl sulphide, 2,3-dihydrofuran, 2,5-dihydrofuran, 2,3-dihydro-2-methylbenzofuran , 2,3-dihydrothiophene, 2,5 dihydrothiophene, diisobutyl sulfide, diisopentyl sulphide, diisopropyl sulfide, 1,2-dimethoxy-4-allylbenzene, 4,7-dimethoxy-5-allyl-3, b enzodioxol, 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-dimethylanisole, 3,5 -dimethylanisole, 2,5-dimethylbenzoxazole, N, N-dimethylbenzylamine, N, N-dimethyl-N'-benzyl-N'-2-pyridinyl-l, 2-ethanediamine, 4'-dimethyl-2, 2'-bipyridine , dimethyldecylamine, dimethyl ether, (1,1-dimethylethoxy) benzene, 2,5-dimethylfuran, N, N-dimethyl-1-naphthylaraine, N, N-dimethyl-2-naphthylamine, 2,9-dimethyl-1, -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, -dimethyl-2-pyridinamine, · N, -dimethyl-4-pyridinamine, 2,3-dimethylpyridine, 2,4-dimethylpyridine, 2,5-dimethylpyridine, 2,6-dimethylpyridine, 3, -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 telulide, 2,5-dimethyl-l, 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-tridecylmorpholino, dinonyl ether, dioctyl ether, dioctyl sulfide, dipentyl ether, dipentyl sulfide, 2,5-diphenyloxazole, 1- (3, 3-diphenylpropyl) piperidine, 1,4-bis (4-methyl-5-phenyloxazol-2-yl) benzene, sulfur diphenyl, N, N- | dipropylaniline, dipropyl sulfide, 1,3-dithiane, 1,4-dithiane, 1,3-dithiolane, 1-dodecylpiperidine, dotiepine, doxepin, doxylamine, l-ethoxy-3-methylbenzene, -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, ethyl hexyl ether, 1-ethyl-lH-imidazole, ethyl isopentyl ether, ethyl isopropyl ether, N-ethyl-N-isopropyl-2-propanamine,. Ethyl isopropyl sulfide, l-ethyl-4-methoxybenzene, N-ethyl-N-methylaniline, l-ethyl-2-methyl-lH-benzimidazole, 2-ethyl-2-methyl-l, 3-dioxolane, ethyl methyl ether , 2-ethyl-5-methylpyrazine, 3-ethyl-4-methylpyridine, 4-ethyl-2-methylpyridine, ethyl methyl sulphide, N-ethylmorpholine, 1-ethylpiperidine, ethyl propyl ether, 2- (l-ethylpropyl) pyridine 4- (1-ethylpropyl) pyridine, ethyl propyl sulfide, 2-ethylpyrazine, 2-ethylpyridine, 3-ethylpyridine, 4-ethylpyridine, 1-ethyl-1H-pyrrole, 2-ethyltetrahydrofuran, (ethylthio) benzene, ethyl thiocyanate, l - ('ethyl thio) -4- methylbenzene, 2-ethylthiophene, ethyl vinyl ether, hexabutyldistanoxane, hexadecyldimethylamine, hexadecyl vinyl ether, 2, 3, 4, 6, 7, 8-hexahydropyrrolo [1,2-a] pyrimidine, hexahydro-1,3,5-triphenyl-1,3,5-triazine, hydrocotamine, hydrohydrastinine, imipramine, isobutyldimethylamine, isopropyl methyl ether, isopropyl methyl sulfide, isopropyl propyl sulfide, (isopropylthio) benzene, isopropyl vinyl ether, hydrobromoline, 2-methoxy-1, 1-biphenyl, 4-methoxy-1, -biphenyl, 1-methoxyl, 3-butadiene, 2-methoxy-l, 3-butadiene, 1-methoxy-l-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-l-methoxy-4- (2 phenylvinyl) benzene, 2-methoxy-1-propene, 3-methoxy-1-propene, tra-sl-methoxy-4- (1-propenyl) benzene, 1-methoxy-4- (2-propenyl) benzene, l-methoxy-4-propylbenzene, 2-methoxypyridine, 3-methoxypyridine, 3-methoxypyridine, (2-methoxy inyl) benzene, 2-methylanisole, 3-methylanisole, 4-methylanisole, 1-methyl-lH-benzimazole, 2- methylbenzofuran, 2-methylbenzothiazole, 2-methylbenzoxazole, 4-methyl-N, -bis (4-methylphenyl) aniline, [(3-methylbutoxy) methyl] b encene, 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-dimethylaniline, methyldioctylamine, 4-methyl-l, 3-dioxane, 2-methyl-l, 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 - . 3- (4-methyl-3-pentenyl) furan, methyl pentyl ether, methyl pentyl sulphide, methyl ter-pentyl sulphide, 10-methyl-10H-phenothiazine, N-methyl-N-phenylbenzenemethanamine, 1-methyl-N -phenyl-N-benzyl-4-piperidinamine, 2-methyl-5-phenylpyridine, 1-methylpiperidine, 4- (2-methylpropenyl) morpholine, methyl propyl ether, l-methyl-2-propylpiperidine, (S), sulfur methyl propyl, N-methyl-N-2-propynylbenzenemethanamine, 2-methylpyrazine, 1-methyl-1H-pyrazole, 3-methylpyridine, 4-methylpyridine, 2-methylpyrimidine, 4-methylpyrimidine, 5-methylpyrimidine, 1-methylpyrrole, N -methylpyrrolidine, 3- (l-methyl-2-pyrrolidinyl) pyridine, (±), 2-methylquinoline, 3-methylquinoline, 4-methylquinoline, 5-methylquinoline, 6-methylquinoline, 7-methylquinoline, 8-methylquinoline, 2-methylquinoxaline, 2-methyltetrahydrofuran, 2-methyltriazole, 4-methyltriazole, (methylthio) benzene, (methylthio) ethene, [(methylthio) methyl] benzene, 2-methylthiophene, 3-methylthiophene, 3 - (methylthio) -1-propene, methisticin, 2- (4-morpholinothio) benzothiazole, myristicin, 1 , 5-naphthyridine, 1, 6-naphthyridine, nicotheline, octyl phenyl ether, orphenadrine, papaverine, 2- (3-pentenyl) iridine, perazine, phenanthridine, 1,7-phenanthroline, 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, phenyl propyl ether, 4- (3-phenylpropyl) pyridine, 2-phenylpyridine, 3-phenylpyridine, 4-phenylpyridine, 1-phenyl-1H-pyrrole, 1-phenylpyrrolidine, 2-phenylquinoline, phenyl vinyl ether, piprotal, promazine, promethazine, trans-5- (1-propenyl) -1,3-benzodioxole, 5-propyl-l, 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" -tertiofen, tetrabutyl titanate, tetraethoxy-methane, tetraethylene glycol dimethyl ether,?,?,? ' ,? ' -tetraethyl-1, 2-ethanediamine, 1, 2, 3, 4-tetrahydro-6,7-dimethoxy-l, 2-dimethylisoquinoline, (±), 4, 5, 6, 7-tetrahydro-3,6-dimethylbenzofuran , cis-tetrahydro-2, 5-dimethylthiophene, 3,4,5,6-tetrahydro-7-methoxy-2H-azepine, 1,2,3,6-tetrahydro-l-methyl-4-phenylpyridine, tetrahydro-3 -methyl-2H-tipirane, 2,3,4,5-tetrahydro-6-propylpyridine, tetrahydropyran, 5,6,7,8-tetrahydroquinoline, tetrahydrothiophene, N, N, 2,6-tetramethylaniline,?,?,? '?' -tetramethyl-1,4-benzenediamine, ?,?,? ' ,? ' -tetramethyl- [1,1 '-biphenyl] -4,4' -diamine,?,?,? ' ,? ' -tetramethyl-1,4-butanediamine,?,?,? ,? ' -tetramethyl-1, 2-ethanediamine,?,?, ',?' -tetramethyl-1, 6-hexanediamine, fenaldine, tenyldiamine, thiacyclohexane, 1, 2, 5-thiadiazole, thianthrene, thiazole, tiepane, thiethylperazine, thioridazine, 9H-thioxanthene, tipepidine, tributylamine, 1,1-triethoxyethane, triethoxymethane , 1, 1, 1-trietoxypropane, triethylaluminum, triethylamine, triethylarsine, triethylene glycol dimethyl ether, trifenitiorph, trihexylamine, trihexyl borate, triisobutyl aluminate, triisobutylaluminum, triisobutylamine, triisopentylamine, triisopropoxymethane, triisopropyl borate, triisopropyl phosphite, 1,3,5-trimethoxybenzene, trimethoxyboroxin, 1,1,1- trimethoxyethane, trimethoxymethane, trimethyl aluminum, trimethylamine, trimethylarsine, trimethylborane, trimethyl borate, 1, 2,4-trimethylpiperazine, trimethylpyrazine, 2,3,6-trimethylpyridine, 2,4,6-trimethylpyridine, 1, 2, 5 trimethyl-lH-pyrrole, N, N, 2-trimethyl-6-quinolinamine, triphenylarsine, triphenyl phosphite, 2,4,6-triphenyl-1,3,5-triazine, triprolidine, tripropylamine, tripropylborane, borate. tripropyl, tripropyl phosphite, tris (4-dimethylaminophenyl) methane, tris (ethylthio) methane, tris (2-methylphenyl) phosphine, tris (3-methylphenyl) phosphine, tris (4-methylphenyl) phosphine, 2, 4, 6-tris (2-pyridinyl) -1, 3, 5-thiazine, tris (o-tolyl) phosphite, 9-vinyl-9H-carbazol, 2-vinylfuran, l-vinyl-2-methoxybenzene, l-vinyl-3-methoxybenzene, l-vinyl-4-methoxybenzene, 2-vinylpyridine, 3-vinylpyridine, 4-vinylpyridine, 9H-xanthene, dibenzofuran, 3,4-dihydro-2H-benzopyran,. alverine, aluminum 2-butoxide, aluminum isopropoxide, 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'-biquinoline, 1, 3 -bis (l-methyl-4-piperidyl) propane, butyl methyl sulfide, t-butyl methyl sulphide, 4-butyl morpholine, 4-t-butylpyridine, 2-butylthiophene, cusparin, cyclizine, 4- (3-cyclohexen-1-yl) pyridine, cyclohexyldiethyl amine, cyclohexyldimethylamine, silicon-based solvents such as silanes, disilanes, siloxanes and disiloxanes, preferably hexamethyldisiloxane, (CH3) 3SÍOCH2CH2CH3, and (CH3) 2Si (OCHCH2CH3) 2, halogenated silanes, siloxanes, and disiloxanes, preferably fluorinated and anionic liquids such as imidazolium and alkyl imidazolium salts, preferably methylimidazolium and other similar compounds. Additional fluorosolvents or sources thereof comprise tetrafluorosilane, hexafluorodisilane, SinF2n + 2 such as Sii6F34, M2SiF6, wherein M is an alkali metal such as Na2SiF6 and K2SiF6, MSiF6, wherein M is an alkaline earth metal such as MgSiF6, GaF3 , PF5, and MPF6, where M is an alkali metal.

The solvent may comprise a polymer. The polymeric solvent can provide a low vapor pressure at the operating temperature of the cell, preferably the polymer is liquid at the operating temperature of the cell. One such polymer solvent is polypropylene glycol or polypropylene oxide.

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

In an embodiment comprising a liquid solvent, the NaH catalyst is at least one of a component of the reaction mixture and is formed from the reaction mixture. The reaction mixture may further comprise at least one of the group of NaH, Na, NH3, NaNH2, Na2NH, Na3N, H20, NaOH, NaX (X is an anion, preferably a halide), NaB¾, NaAlH4, Ni, Pt black, Pd black, R-Ni, R-Ni doped with a Na species such as at least one of Na, NaOH, and NaH, a HSA support, a rarefactor, a dispersant, a hydrogen source such as H2, and a hydrogen dissociator. Preferably, the support does not form an oxide with components of the reaction mixture such NaOH and the solvent such as an ether, preferably BDO. In this case, the support can 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).

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

In one embodiment, the reaction mixture comprises NaH + solvent + support, wherein (1) the support comprises at least one chosen support of nickel powder of high reduced surface area, La powder, and carbon such as nanotubes, preferably single-wall graphite, graphene, diamond-like carbon (DLC), hydrogenated diamond-like carbon (HDLC), diamond dust, graphite carbon, glassy carbon, and carbon with other metals such as Pd or 'Pt / carbon or impurifiers comprising other elements such as fluorinated carbon, preferably fluorinated graphite or fluorinated diamond; and (2) the solvent comprises an ether such as 1, -dibenzodioxane (BDO), dimethoxyethane (DME), 1,4-dioxane, and biphenylether, N, -dimethylaniline (DMAn), perfluorinated alkane or aryl such as hexafluorobenzene, hexamethylphosphoramide. (HMPA), protic amine and toluene. In other embodiments, at least one of Na, K, H, Li, and LiH replaces NaH. In one embodiment, the reaction mixture comprises species of the group of Na, NaH, NaF, a solvent, preferably a solvent based on fluorinated carbon and an HSA material such as carbon, preferably nanotubes of a single wall.

Suitable reactant mixtures comprise at least one of the group of (1) NaH, hexafluorobenzene, and at least one of single-wall nanotubes, Pr powder, activated carbon, and mesoporous carbon doped with Al, La, and , or Ni powder or the corresponding carbide, (2) NaH or KH, 1,4-dibenzodioxane (BDO), and at least one of La powder, Nd powder, and a carbide of Al, La, Y and Ni, (3) NaH, dioxane and Co or Nd powder, (4) NaH, NaOH, BDO and Teflon powder. The percentages by weight can be in any proportions, preferably they are approximately equivalent. In another embodiment, the reaction mixture comprises selected species of Na, NaH, a solvent, preferably an ether solvent, and an HSA material such as a metal, preferably a rare earth. An appropriate reaction mixture comprises NaH, 1,4-dibenzodioxane (BDO) and La. The percentages by weight may be in any proportions, preferably they are around 10/45/45 weight percent, respectively. In another exemplary energy cell embodiment, the reaction mixture comprises NaH, R-Ni or Ni powder of high surface area and an ether solvent. In certain embodiments of chemical cells, the reaction mixture further comprises a rarefactor for hydride hydride and molecular hydride ions such as an alkali metal halide, preferably a sodium halide, such as at least one of NaF, NaCl, NaBr, and Nal.

In one embodiment, the solvent has a halogen functional group, preferably fluorine. A suitable reaction mixture comprises at least one of hexafluorobenzene and octafluoronaphthalene added to a catalyst such as NaH, and mixed with a support such as activated carbon, a fluoropolymer or R-Ni. In one embodiment, the reaction mixture comprises one or more species from the group of Na, NaH, a solvent, preferably a fluorinated solvent, and an HSA material. The HSA material may comprise at least one of a metal or carbon-coated alloy, such as at least one of Co, Ni, Fe, Mn, and other transition metal powders, preferably nanopowder, which preferably has a to ten layers of carbon and more preferably three layers, according to methods known per se. those experienced in art; carbon coated with metal or alloy, preferably nanopoly, such as a transition metal, preferably at least one carbon coated with Ni, Co and Mn, and a fluoride, preferably a metal fluoride. Preferably, the metal is capable of being coated with a non-reactive layer of fluorine such as steel, nickel, copper or Monel metal. The coated metal can be a powder that has a high surface area. Other suitable metals are the rare earths such as La with a fluoride coating which may comprise LaFx such as LaF3 .. In certain embodiments, the metal fluoride is more stable than MF, where M is the catalyst or a catalyst source. such as Li, Na and K. In a further embodiment, the reaction mixture further comprises a fluoride such as a metal fluoride. The fluoride may comprise the catalyst metal such as NaF, KF and LiF and may further comprise transition metals, noble, intermetallic, rare earth, lanthanides, preferably La or Gd, and actinide metal, Al, Ga, In, Ti, Sn, Pb, metalloids, B, Si, Ge, As, Sb, Te, Y, Zr, Nb, Mo, Te, Ru, R, Pd, Ag, Cd, Hf, Ta,, Re, Os, Go, Pt , Au, Hg, alkali metals, and alkaline earth metals. The fluoride may also comprise a rarefactor as an HSA material. In one embodiment, the metal may comprise an alloy such as La i, and Ni-Y alloy or a carbide, preferably resistant to the formation of an inorganic fluoride.

A suitable fluorinated solvent for regeneration is CF4. A suitable support or HSA material for a fluorinated solvent with NaH catalysts is NaF. In one embodiment, the reaction mixture comprises at least NaH, CF4i and NaF. Other fluorine-based supports or rarefactors comprise M2SiF6, wherein M is an alkali metal such as a2SiF6 and K2SiF6, MSiF6 wherein M is an alkaline earth metal such as MgSiF6, GaF3, PF5, MPF6, wherein M is an alkali metal , MHF2 wherein M is an alkali metal such as NaHF2 and KHF2, K2TaF7, KBF4, K2MnF6 and K2ZrF6 wherein other similar compounds are anticipated, such as those having substitution of another alkaline or alkaline earth metal such as one of Li, Na or K as alkali metal.

In one embodiment, the solvent comprises fluorine and at least one other element, wherein the at least other fluoride-based elements are thermodynamically or kinetically stable to the NaH reaction and are preferably liquid at the operating temperature of the cell which It can be between 200 ° C to 700 ° C. The other element can be Si, Te, Se, or Sb. The solvent can be SixFy, where x and y are integers. In another embodiment, the chemistry of solvents with NaH or any other reactant in the reaction mixture is reversible chemistry, such as a reversible reaction of NaF and H2 to a fluorinated solvent, preferably comprising carbon and NaH. In an embodiment comprising NaH and a fluorinated solvent, H2 is supplied to the reaction of the fluorinated solvent, such that NaH is less reactive than Na to any C-F bond and H2 reduces the amount of Na.

In a modality, at least one of a fluorinated solvent and an HSA material are protected from attack to form NaF. Fluorocarbons are stable to strong bases, and in one embodiment, the source of the NaH catalysts is a strong base. The source can be at least one of Na, NaH, NaNH2, NH3, NaOH, Na20, and a source of hydrogen such as at least one of a hydride and H2 and dissociator. Exemplary reactions to form the NaH catalyst, some regenerative, are given by Equations (158-161), (168), and (177-183), summarized later in this. A cycle of NaOH to form the NaH catalyst is given by Equations (158-161). The reaction given by Equation (158) can limit the amount of Na to react with a fluorinated solvent. A reductant can be added to the reaction mixture that has NaOH to form NaH- and a reductant oxide. The reagent can be recycled by reducing the oxide with hydrogen which can also produce NaOH. The hydrogen can be dissociated by a dissociator. The reductant can be a metal having a corresponding oxide that can be reduced by hydrogen such as Cr, Fe, Sn and Zn. Alternatively, the oxide such as ZnO can be reduced to the metal by heating at a high temperature such as about 1750 ° C. In other embodiments, the fluorinated solvent can be replaced by another type, such as at least one of an ether, preferably one of dibenzodioxin, dibenzo-1,4-dioxane, dioxane and dimethoxyethane, and a hydrocarbon such as at least one of toluene, xylene, benzene, naphthalene, naphthacene, phenanthrene, chrysene, fluoranthene and pyrene. The support can be a metal, preferably at least one of La, Pr, Co, and Nd.

A suitable reaction mixture comprises NaH or a source of NaH, a solvent, preferably a fluorocarbon such as CF4, hexafluorobenzene (HFB) or perfluoroheptane, a support, preferably comprising carbon and a metal, and optionally hydrogen. The carbon may preferably comprise activated carbon (AC), but may also comprise other forms such as vitreous carbon, coke, graphite carbon and carbon with a dissociating metal such as Pt or Pd wherein the weight percent is 0.1 to 5 per cent. cent in weight. The metal may be in the form of at least one of a metal, hydride or carbide powder, such as at least one of the group of an alkali metal, alkaline earth metal, preferably Mg as MgH 2, Al as a metal or carbide such as AI4C3, "a rare earth metal or carbide, preferably La, a metal or alloy, preferably nanopoly, coated with carbon, such as at least one of Co, Ni, Fe, Mn, and other transition metal powders. which preferably have from one to ten layers of carbon and more preferably three layers, and one carbon coated with metal or alloy, preferably nanopowder, such as a transition metal, preferably at least one carbon coated with Ni, Co, and Mn The metal can be intercalated with the carbon.In the case that the intercalated metal is Na and the catalyst is NaH, preferably the intercalation of Na is saturated.The reagents can be in any desired proportions, such as (1) NaH ( 14 weight percent), HFB (14 percent by weight), activated carbon (58 percent by weight), and MgH2 (14 percent by weight); (2) NaH (14 percent by weight), HFB (14 percent by weight), activated carbon (58 percent by weight), and Al (14 percent by weight); (3) NaH (14 percent by weight), HFB (14 percent by weight), activated carbon (58 percent by weight), and AI4C3 (14 percent by weight); (4) NaH (14 percent by weight), HFB (14 percent by weight), activated carbon (58 percent by weight), and nanopod of Co coated with carbon (14 percent by weight); (5) NaH (14 percent by weight), HFB (14 percent by weight), activated carbon (58 percent by weight), and La (14 percent by weight). In other embodiments, activated carbon CA is replaced by mesoporous carbon, and in others, the solvent is increased, preferably by a factor of two to three relative to the other reactants. In other embodiments, another catalyst such as K or Li replaces the NaH catalyst.

In general embodiments, the reaction mixture comprises a component called a protective agent or blocking agent that at least partially suppresses an undesirable reaction of one component of the mixture with another. Preferably, the protective agent or blocking agent is non-reactive with a solvent or a support. Strong bases are non-reactive towards fluorocarbons; while Na does. Thus, in one embodiment, at least one of H2, NaOH, NaNH2 and NH3 can be added to the reaction mixture as a blocking agent to react with any Na formed during the reaction to form hydrino and prevent them from reacting with a support such as a fluorocarbon support. an exemplary reaction mixture comprises NaH, a blocking agent such as at least one of NaOH, NaNH2, NH3, H2, a solvent such as at least one of BDO, capped ether, polypropylene oxide, CF4 and HFB, and a support comprising at least one fluorocarbon such as Teflon powder. Exemplary protective agents are hydride and carbide. The protected reagent can be a metal support. The reaction may comprise NaH, and ether solvent such as BDO, and a metal hydride such as earth metal hydride or a carbide such as at least one of Al, rare earths, and transition metal carbides.

In second general embodiments, the reaction mixture is substantially stable over a long duration towards reaction between components other than hydrine formation. Preferably, the solvent such as a polar solvent is not reactive with the catalyst or a support. For example, an ether solvent is non-reactive towards NaH as a catalyst source, a fluorocarbon support, or a rare earth, hydride or carbide powder at an appropriately low reaction temperature, such as less than 350 ° C. Thus, an exemplary reaction mixture comprises NaH, an ether solvent such as BDO, dioxane or a crown ether,and a rare metal powder carrier such as La powder. Another support comprises an alloy resistant to the reaction to the solvent such as LaNi5. | In a third general embodiment, the reaction mixture comprises reagents that form hydrinos at a high yield as a secondary reaction between components also occur. The reagents can be regenerated to carry out another cycle to form hydrinos. An exemplary reaction mixture comprises NaH, a fluorocarbon solvent such as CF4, and a support such as at least one of Teflon, floured graphite, activated carbon, graphene and mesoporous carbon plus at least one of Al, La, Co, Ni, Mn, Y, and powder of Faith and its carbides. Preferably, the metal and carbide comprise a mixture such as one of Ni, Co, Mn. The metals and carbides may be in any proportion by weight percent. Preferably, the composition and proportions of percent by weight (%) are about 20 to 25% Ni, 60 to 70% Co, and 5 to 15% Mn. In another, the metal and carbide comprises a mixture with other elements such as one of Ni, Co, Mn, Fe, S, and Ca. The metals and carbides and other elements may be in any weight percent proportion. Preferably, the composition and proportions of percent by weight (%) are about 20 ± 5% Ni, 65 + 5% Co, 10 ± 5% Mn, 1 ± 5% Fe, 1% ± 2 S , and 0.5 ± 2% Ca. In other embodiments, the carbon support comprises a high surface area carbon such as activated carbon or mesoporous carbon and at least one metal that forms a less stable fluoride • thermodynamically than NaF such as nickel , iron, iridium, vanadium, lead, molybdenum and tungsten.

Other embodiments comprise reaction mixtures that involve any combination of these three general modalities based on these, any combination of, or any alternative reaction route or strategy.

In one embodiment, the source or sources for providing the catalyst and atomic hydrogen comprise at least one of amides such as LiNH2, imides such as Li2NH, nitrides such as Li3N, and catalyst metal with NH3. The reactions of these species provide both Li atoms and atomic hydrogen. Additionally, K, Cs and Na can replace Li, and the catalyst is atomic, Cs atomic, and molecular NaH. The reaction mixture may further comprise species from the group of Li, LiNH2, Li2NH, Li3N, L1NO3, LiX, NH4X (X is an anion, preferably a halide), NH3, R-Ni, a support of HSA, rarefactor, a dispersant , a source of hydrogen such as H2, and a hydrogen dissociator. b. Inorganic Solvents In another embodiment, the reaction mixture comprises at least one inorganic solvent. The solvent may additionally comprise a molten inorganic compound such as a molten salt. The inorganic solvent can be molten NaOH. In one embodiment, the reaction mixture comprises a catalyst, a source of hydrogen and an inorganic solvent for the catalyst. The catalyst may be at least one of molecules of NaH, Li and K. The solvent may be at least one of a molten or fused or eutectic salt, such as at least one of the molten salts of the group of alkali halides and alkaline halides torrids. The inorganic solvent of the NaH catalyst reaction mixture may comprise a low melting eutectic of a mixture of alkyl halides such as NaCl and KCl. The solvent may be a salt of low melting point, preferably a Na salt, such as at least one of Nal (660 ° C), NaAlCl4 (160 ° C), NaAlF4, and a compound of the same kind as NaMX4, where M is a metal and X is a halide that has a metal halide that is more stable than NaX. The reaction mixture may further comprise a support such as R-Ni.

The inorganic solvent of the Li catalyst reaction mixture can comprise a eutectic of a low melting point mixture of alkali halides such as LiCl and KCl. The molten salt solvent may comprise a fluorine based solvent that is stable to NaH. The melting point of LaF3 is 1493 ° C and the melting point of NaF is 996 ° C. A milled mixture in ball mill in appropriate proportions, optionally with other fluorides, comprises a fluoride salt solvent which is stable to NaH and preferably melts in the range of 600 ° C-700 ° C. In a molten salt embodiment, the reaction mixture comprises NaH + salt mixture such as NaF-KF-LiF (11.5-42.0-46.5) Melting point = 454 ° C or NaH + salt mixture such as LiF-KF ( 52% -48%) Melting point = 492 ° C.

V. Regeneration Systems and Reactions A schematic diagram of a system for the recycling or regeneration of fuel according to the present disclosure is shown in Figure 4. In one embodiment, the side products of the hydrino reaction comprise a metal halide MX, preferably NaX or KX. Then, the fuel recycler 18 (Figure 4) comprises a separator 21 for separating inorganic compounds such as NaX from the support. In one embodiment, the separator or a component thereof comprises a cyclone displacer or separator 22 that effects separation based on density differences of the species. An additional separator or component thereof comprises a magnetic separator 23 in which magnetic particles such as nickel or iron are ejected by a magnet while non-magnetic material such as MX flows through the separator. In another embodiment, the separator or a component thereof comprises a solubilization or suspension system of differential product 24 comprising solvent-layered component 25 that dissolves or suspends at least one component to a greater extent than another to allow separation , and may further comprise a recovery system for compound 26 such as a solvent evaporator 27 and a collector of compound 28. Alternatively, the recovery system comprises a precipitator 29 and a compound and collector dryer 30. In one embodiment, the waste heat from the turbine 14 and water condenser 16 shown in Figure 4 is used to heat at least one of the evaporator 27 and dryer 30 (Figure 4). The heat for any other steps of the recycler 18 (Figure 4) may comprise the heat of waste.

The fuel recycler 18 (Figure 4) further comprises an electrolyser 31 that electrolyzes the recovered MX to metal and halogen gas or another halogenated or halide product. In one embodiment, electrolysis occurs within the powder reactor 36, preferably from a melt such as a eutectic melt. The electrolysis gas and metal product are collected separately in the gas collector. highly volatile 32 and a metal collector 33 which may further comprise a metal still or separator 34 in the case of a mixture of metals, respectively. If the initial reagent is a hydride, the metal is converted to hydride by a hydrization reactor 35 comprising a suitable cell 36 of a pressure less than, greater than or equal to atmospheric, an inlet and outlet 37 for the metal and hydride , an inlet for hydrogen gas 38 and its valve 39, a supply of hydrogen gas 40, a gas outlet 41 and its valve 42, a pump 43, a heater 44, and pressure and temperature meters 45. In one embodiment, the hydrogen supply 40 comprises an aqueous electrolyzer having a gas separator of hydrogen and oxygen. The isolated metal product is at least partially halogenated in a halogenization reactor 46 comprising a cell 47 suitable for pressures less than, greater than and equal to atmospheric, an inlet for the carbon and output for the halogenated product 48, a inlet for fluorine gas 49 and its valve 50, a supply of halogen gas 51, a gas outlet 52 and its valve 53, a pump 54, a heater 55, and pressure and temperature meters 56. Preferably, the reactor also it contains catalysts and other reagents to cause the metal 57 to become the halide of the oxidation state and stoichiometry desired as the product. The at least two of the metal or metal hydride, metal halide, support and other initial reagents are recycled to the kettle 10 after being mixed in a mixer 58 for another power generation cycle.

In exemplary hydrino reactions and regeneration, the reaction mixture comprises the catalyst of NaH, Mg, Mnl2 and support, activated carbon, WC or TiC. In one embodiment, the source of the exothermic reaction is the oxidation reaction of metal hydride by Mnl2 such as 2KH + Mnl2? 2KI + Mn + H2 (86) Mg + Mnl2? Mgl2 + Mn. (87) KI and Mgl2 can be electrolyzed to I2, and Mg of a molten salt. The electrolysis in the molten state can be carried out using a Downs cell or a modified Do ns cell. The Mn can be separated using a mechanical separator and optionally sieves. Unreacted Mg or MgH2 can be separated by melting and by separation of solid and liquid phases. The iodides for electrolysis can be from rinsing the reaction products with an appropriate solvent such as deoxygenated water. The solution can be filtered to remove the support such as activated carbon and optionally the transition metal. The solid can be centrifuged and dried, preferably using the waste heat of the energy system. Alternatively, the halides can be separated by melting them followed by separation of the liquid and solid phases. In another embodiment, the lightest activated carbon can initially be separated from the other reaction products by a method such as cyclone separation. K and Mg are immiscible, and the separated metals such as K can be converted to hydride with H2 gas, preferably from the electrolysis of H2O. Metal iodide can be formed by known reactions with the separated metal or with the metal, without separating from the activated carbon. In one embodiment, the Mn is reacted with HI to form Mnl2 and the H2 which is recycled and reacted with I2 to form HI. In other embodiments, other metals, preferably a transition metal, replace Mn. Another reducer such as Al can replace Mg. Another halide, preferably chloride, can replace the iodide. LiH, H, RbH or CsH can replace NaH.

In exemplary hydrino reactions and regeneration, the reaction mixture comprises the NaH, Mg, AgCl catalyst and support, activated carbon. In one embodiment, the exothermic reaction source is the hydride oxidation reaction of metais by AgCl such as KH + AgCl? KC1. + Ag + 1 / 2H2 '(88) Mg + 2ÁgCl? MgCl2 + 2Ag. (89) KC1 and MgCl2 can be electrolyzed to Cl2, K and Mg of a molten salt. The electrolysis in the molten state can be carried out using a Downs cell or modified Downs cell. The Ag can be separated using a mechanical separator and optionally sieves. The Mg. or unreacted MgH2 can be separated by melting and by separation of the solid and liquid phases. The chlorides for electrolysis can be from rinsing the reaction products with an appropriate solvent such as deoxygenated water. The solution can be filtered to remove the support such as activated carbon and optionally the Ag metal. The solid can be centrifuged and dried, preferably using the waste heat from the energy system. Alternatively, the halides can be separated by melting them followed by the separation of the liquid and solid phases. In another embodiment, the lightest activated carbon can initially be separated from the other reaction products by a method such as cyclone separation. K and Mg are immiscible and the separated metals such as K can be converted to hydride with H2 gas, preferably from the electrolysis of H2O. The metal chloride can be formed by known reactions with the separated metal or with the metal, without being separated from the activated carbon. In one embodiment, Ag is reacted with Cl2 to form AgCl, and the H2 that is recycled and reacted with I2 to form HI. In other embodiments, other metals, preferably a transition metal or In, replaces Ag. Another reductant such as Al can replace Mg. Another halide, preferably chloride, can replace the iodide. LiH, KH, RbH or CsH can replace NaH.

In one embodiment, the reaction mixture is regenerated from hydrino reaction products. In exemplary hydrino reactions and regeneration, the solid fuel reaction mixture comprises KH or NaH, Mg or MgH2 catalyst, and alkaline earth halide such as BaBr2 and support, activated carbon, WC or preferably TiC. In one embodiment, the exothermic reaction source is the oxidation reaction of metal hydride or metals by BaBr2 such as 2KH + Mg + BaBr2? 2KBr + Ba + MgH2 (90) 2 aH + Mg + BaBr2? 2NaBr + Ba + MgH2. (91) The melting points of Ba, magnesium, MgH2, NaBr and KBr are 727 ° C, 650 ° C, 327 ° C, 747 ° C, and 734 ° C, respectively. Thus, MgH2 can be separated from barium and any intermetallic Ba-Mg by maintaining MgH2 with the optional additional H2, preferably by melting MgH2, and separating the liquid from the reaction product mixture. Optionally, it can be thermally decomposed to Mg. Then, the remaining reaction products can be added to an electrolysis melt. The solid support and Ba precipitate to form preferably separable layers. Alternatively, Ba can be separated as liquid by melting. Then, NaBr or KBr can be electrolyzed to form the alkali metal and Br2. The latter is reacted with Ba to form BaBr2. Alternatively, Ba is the anode, and BaBr2 is formed directly in the anode compartment. "The alkali metal can be converted to hydride following electrolysis or formed in the cathode compartment during electrolysis by bubbling H2 into this compartment. Then, gH2 or Mg, NaH or KH, BaBr2 and support are returned to the reaction mixture In other embodiments, another alkaline earth halide replaces BaBr2, preferably BaCl2 In another embodiment, regeneration reactions may occur without electrolysis due to the small energy difference between the reactants and products The reactions given by Equations (90-91) can be reversed by changing the reaction conditions such as temperature or hydrogen pressure.

Alternatively, a molten or volatile species such as K or Na can be selectively removed to drive the reaction back to generate a reagent or a species that can be further reacted and added back to the cell to form the original reaction mixture. . In another embodiment, the volatile species can be continuously refluxed to maintain the reversible reaction between the catalyst or catalyst source such as NaH, KH, Na or and the initial oxidant such as an alkaline earth halide or rare earth halide. In one embodiment, the reflux is obtained using a still such as the still 34 shown in Figure 4. In another embodiment, the reaction conditions such as the temperature or pressure of hydrogen can be changed to reverse the reaction. In this case, the reaction is initially started in the forward direction to form hydrinos and the products of the reaction mixture. Thus, products other than hydrogen of lower energy are converted to the initial reactants. This can be done by changing the reaction conditions and possibly adding or removing at least partially the same or other products or reagents as those used or initially formed. Thus, the forward and regeneration reactions are brought to. out in alternating cycles. Hydrogen can be added to replace that consumed in the formation of hydrinos. In another embodiment, the reaction conditions are maintained, such as a high temperature, where the reversible reaction is optimized in such a way that both of the forward reactions and inverse occur in a manner that obtains the desired hydrine formation speed, preferably maximum.

In exemplary hydrino reactions and regeneration, the solid fuel reaction mixture comprises the NaH, Mg, FeBr2 catalyst and support, activated carbon. In one embodiment, the exothermic reaction source is the oxidation reaction of metal hydride by FeBr2 such as 2NaH + FeBr2? 2NaBr + Fe + ¾ (92) Mg + FeBr2? MgBr2 + Fe. (93) NaBr and gBr2 can be electrolyzed to Br2, Na and Mg of a molten salt. The electrolysis in the molten state can be carried out using a Downs cell or modified Downs cell. The Fe is ferromagnetic and can be separated magnetically using a mechanical separator and optionally sieves. In another modality, the ferromagnetic Ni can replace the Fe. "The unreacted Mg or MgH2 can be separated by fusion and by separation of the solid and liquid phases.The bromides for electrolysis can be rinsing the reaction products with an appropriate solvent such As the deoxygenated water, the solution can be filtered to remove the support such as activated carbon and optionally the transition metal.The solid can be centrifuged and dried, preferably using waste heat from the energy system.Alternatively, the halides can be separated to the melt followed by the separation of the liquid and solid phases In another embodiment, the lightest activated carbon can initially be separated from the other reaction products by a method such as cyclone separation.Na and Mg are immiscible and the metals Separated such as Na can be converted to hydride with H2 gas, preferably electrolyte isis of H20 Metal bromide can be formed by known reactions with the metal separated or with the metal, without separating from the activated carbon. In one embodiment, the Fe is reacted with HBr to form FeBr2 and the H2 which is recycled and reacted with Br2 to form HBr. In other embodiments, other metals, preferably a transition metal, replace the Fe. Another reductant such as Al can replace the Mg.Another halide, preferably the chloride can replace the bromide LiH, KH, RbH or CsH can replace to NaH.

In exemplary hydrino reactions and regeneration, the solid fuel reaction mixture comprises KH or catalyst of NaH, Mg or MgH2, · SnBr2 and support, activated carbon, WC or Tic. In one embodiment, the exothermic reaction source is the oxidation reaction of metal hydride or metals by SnBr2 such as 2KH + SnBr2? 2KBr + Sn + H2 (94) 2 aH + SnBr2? 2NaBr + Sn + H2 (95) Mg + SnBr2? MgBr2 + Sn. (96) The melting points of tin, magnesium, MgH2, NaBr and KBr are 119 ° C, 650 ° C, 327 ° C, 747 ° C, and 734 ° C, respectively. The tin-magnesium alloy will melt at a higher temperature such as 400 ° C by about 5 weight percent Mg as given in its alloy phase diagram. In one embodiment, the metals of tin and magnesium and alloys are separated from the support and halides by melting the metals and alloys and separating the liquid and solid phases. The alloy can be reacted with H2 at a temperature that forms solid MgH2 and tin metal. The solid and liquid phases can be separated to give MgH2 and tin. MgH2 can be thermally decomposed to. Mg and H2. Alternatively, the H2 can be added to the reaction products in itself at a selective temperature to convert any unreacted Mg and any Sn-Mg alloy to solid MgH2 and liquid tin. Tin can be removed selectively. 'Then, the MgH2 can be heated and removed as a liquid. Next, the halides can be removed from the support by such methods (1) by melting and phase separation, (2) cyclone separation based on density differences, where a dense support such as WC is preferred, or (3) sifted based on differences in size. Alternatively, the halides can be dissolved in an appropriate solvent, and the liquid and solid phases separated by methods such as filtration. The liquid can be evaporated and then the halides can be electrolyzed from the melt to Na or K and possibly Mg metals that are immiscible, and each separated. In another embodiment, it is formed by reducing the halide using Na metal which is regenerated by electrolysis of a sodium halide, preferably the same halide as formed in the hydrino reactor. In addition, the halogen gas such as Br2 is collected from the electrolysis melt and reacted with isolated Sn to form SnBr2 which is recycled for another cycle of the hydrino reaction together with NaH or KH, and Mg or MgH2, where the Hydrides are formed by hybridization with H2 gas. In one embodiment, HBr is formed and reacted with Sn to form SnBr2. The HBr can be formed by reaction of Br2 and H2 or during electrolysis by bubbling at the anode which has the advantage of decreasing the electrolysis energy. In another embodiment, another metal replaces Sn, preferably a transition metal, and another halide can replace Br such as I.

In another embodiment, in the initial stage, all the reaction products are reacted with aqueous solution, and the solution is concentrated to precipitate SnBr2 from the solution of MgBr2 and KBr. Other suitable solvents and separation methods can be used to separate the salts. MgBr2 and KBr are then electrolyzed to Mg and K. Alternatively, Mg or MgH2 is first removed using mechanical methods or by selective solvent methods, so that only KBr needs to be electrolyzed. In one embodiment, Sn is removed as a melt from solid MgH2 that can be formed by adding H2 during or after the hydrino reaction. MgH2 or Mg, KBr and support are then added to the electrolysis melt. The support sits in a sedimentary zone due to its large particle size. MgH2 and KBr are part of the melt and are separated based on the density. Mg and K are immiscible and K also forms a separate phase such that Mg and K are collected separately. The anode can be of Sn, such that K, Mg and SnBr2 are the products of electrolysis. The anode can be liquid tin or liquid tin can be bottled at the anode to react with bromine and form SnBr2. In this case, the energy space for regeneration is the space of the compound against the highest elementary space corresponding to elementary products in both electrodes. In a further embodiment, the reagents comprise KH, support and Snl2 or SnBr2. The Sn can be removed as a liquid, and the remaining products such as KX and support can be added to the electrolysis melt, where the support is separated based on the density. In this case, a dense support such as. WC is preferred.

The reagents may comprise an oxygen compound to form an oxide product such as a catalyst oxide or catalyst source such as that of NaH, Li, or K and an oxide of the reductant such as that of Mg, MgH2, Al, Ti , B, Zr, or La. In one embodiment, the reagents are regenerated by reacting the oxide with an acid such as hydrogen halide acid, preferably HC1, to form the corresponding halide such as the chloride. In one embodiment, a kind of oxidized carbon such as carbonate, hydrogen carbonate, a species of carboxylic acid, such as oxalic acid or oxalate can be reduced by a metal or a metal hydride. Preferably, at least one of Li, K, Na, LiH, KH, NaH, Al, Mg and MgH2 reacts with the species comprising carbon and oxygen and forms the corresponding metal oxide or hydroxide and carbon. Each corresponding metal can be regenerated by electrolysis. The electrolysis can be effected using a molten salt such as that of a etic mixture. The product of halogen gas electrolysis such as chlorine gas can be used to form the corresponding acid such as HCl as part of a regeneration cycle. The hydrogen halide acid HX can be formed by reacting the halogen gas with hydrogen gas and optionally by dissolving the hydrogen halide gas in water. Preferably, the hydrogen gas is formed by electrolysis of water. The oxygen may be a reactant of the hydrino reaction mixture or may be reacted to form the oxygen source of the hydrino reaction mixture. The step of reacting the hydride reaction product with acid can comprise rinsing the product with acid to form a solution comprising the metal salts. In one embodiment, the hydrino reaction mixture and the corresponding product mixture comprises a support such as carbon, preferably activated carbon. The metal oxides can be separated from the support by dissolving them in aqueous acid. Thus, the product can be rinsed with acid and can also be filtered to separate the components of the reaction mixture. The water can be removed by evaporation using heat, preferably waste heat from the energy system, and salts such as metal chlorides can be added to the electrolysis mixture to form the metals and halogen gas. In one embodiment, any methane or hydrocarbon product can be reformed to hydrogen and optionally carbon or carbon dioxide. Alternatively, the methane can be separated from the gaseous product mixture and sold as a commercial product. In another embodiment, methane can be formed to other hydrocarbon products by methods known in the art such as Fischer-Tropsch reactions. The formation of methane can be suppressed by adding an interfering gas such as an inert gas and by maintaining unfavorable conditions such as a reduced hydrogen pressure or temperature.

In another embodiment, the metal oxides are electrolyzed directly from a etic mixture. Oxides such as MgO can be reacted with water to form hydroxides such as Mg (OH) 2. In one embodiment, the hydroxide is reduced. The reductant can be an alkali metal or hydride such as Na or NaH. The hydroxide of the product can be electrolyzed directly as a molten salt. Hydrino reaction products such as alkali metal hydroxides can also be used as a commercial product and the corresponding purchased halides. Then, the halides can be electrolyzed to halogen gas and metal. The halogen gas can be used as a commercial industrial gas. The metal can be converted to hydride with hydrogen gas, preferably for electrolysis of water, and supplied to the reactor as part of the hydrino reaction mixture.

The reductant such as an alkali metal can be regenerated from the product comprising a corresponding compound, preferably NaOH or Na20, using methods and systems known to those skilled in the art. One method comprises electrolysis in a mixture such as a eutectic mixture. In a further embodiment, the reducing product may comprise at least some oxide such as a reducing 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 gCl2. The acid treatment can also be an anhydrous reaction. The gases may be flowing at low pressure. The salt can be treated with a product reducer such as an alkaline or alkaline earth metal to form the original reductant. In one embodiment, the second reductant is an alkaline earth metal, preferably Ca, wherein NaCl or MgCl 2 is reduced to Na or Mg metal. The additional product of CaCl3 is recovered and recycled as well. In a . alternative mode, the oxide is reduced with ¾ at high temperature. In exemplary hydrino reactions and regeneration, the reaction mixture comprises the NaH, MgH2, 02 catalyst and support, activated carbon. In one embodiment, the exothermic reaction source is the oxidation reaction of metal hydride by 02 such as MgH2 +02? Mg (0H) 2 (97) MgH2"+ 1.502 + C? MgC03 + H2 (98) • NaH + 3/202 + C? NaHCO3. (99) 2 aH + 02? 2NaOH .. (100) Any MgO product can be converted to the hydroxide by reaction with water MgO + H 20? Mg (OH) 2. (101) Sodium or magnesium carbonate, hydrogen carbonate and other species that comprise carbon and oxygen can be reduced with Na or NaH :.

NaH + Na2C03? 3NaOH + C + 1 / H2 (102) _ NaH + l / 3MgC03? NaOH + 1 / 3C + l / 3Mg (103) Mg (OH) 2 can be reduced to Mg using Na or NaH: 2Na + Mg (0H) 2? .2NaOH + Mg. (104) Then, the NaOH can be electrolyzed to Na metal and NaH and 02 directly from the melt. The Castner process can be used. An appropriate cathode and anode for a basic solution is nickel. The anode can also be carbon, a noble metal such as Pt, a support such as Ti coated with a noble metal such as Pt, or a dimensionally stable anode. In another embodiment, the NaOH is converted to NaCl by reaction with HCl, wherein the Cl 2 of NaCl electrolysis gas can be reacted with ¾ of the water electrolysis to form HCl. The electrolysis of molten NaCl can be carried out using a Do ns cell or modified Downs cell. Alternatively, HCl - can be produced by chloroalkali electrolysis. The aqueous NaCl for this electrolysis can be from rinsing the reaction products with aqueous HCl. The solution can be filtered to remove the support such as activated carbon which can be centrifuged and dried, preferably using waste heat from the energy system.

In one embodiment, the reaction step comprises, (1) rinsing the products with aqueous HCl to form metal chlorides from species such as hydroxides, oxides and carbonates, (2) converting any C02 evolved to, water and C by reducing of H2 using the water gas displacement reaction and the Fischer-Tropsch reaction, where the C is recycled as the support in step 10 and the water can be used in stages 1, 4 or 5, (3) filtering and drying the support such as activated carbon, wherein the drying may include the centrifugation step, (4) electrolyzing water to H2 and 02 to supply steps 8 to 10, (5) optionally forming H2 and HCl from the electrolysis of aqueous NaCl to supply stages 1 and 9, (6) isolate and dry metal chlorides, (7) electrolyze a metal chloride melt to metals and chlorine, (8) form HCl by reaction of Cl2 and H2 to supply stage 1, (9) convert to. hydride any metal to form the corresponding starting reagent, by reaction with hydrogen, and (10) form the initial reaction mixture with the addition of 02 from step 4 or alternatively using 02 isolated from the atmosphere.

In another embodiment, at least one of magnesium oxide and magnesium hydroxide is electrolyzed from a melt to g and 02. The melt can be a NaOH melt, where Na can also be electrolyzed. In one embodiment, carbon oxides such as carbonates and hydrogen carbonates can be decomposed to at least one of CO and C02 that can be added to the reaction mixture as a source of oxygen. Alternatively, carbon oxide species such as CO 2 and CO can be reduced to carbon and water by hydrogen. C02 and CO and can be reduced by the water gas treatment reaction and the Fischer-Tropsch reaction.

In exemplary hydrino reactions and regeneration, the reaction mixture comprises NaH, MgH2, CF4 catalyst and support, activated carbon. In one embodiment, the source of the exothermic reaction is the oxidation reaction of metal hydride by CF4 such as 2MgH2 + CF4? C + 2MgF2 + 2MgH2 + CF4? CH4 + 2MgF2 4NaH + CF4? C + 4NaF + 4 aH + CF4? CH + 4NaF.

The NaF and MgF2 can be electrolyzed to F2, Na and Mg of a molten salt which can additionally comprise HF. Na and Mg are immiscible, and the separated metals can be converted to hydride with H2 gas, preferably from the electrolysis of H2O. The gas of F2 can be reacted with carbon and any CH reaction product to regenerate CF4. Alternatively and preferably, the anode of the electrolysis cell comprises carbon, and the current and electrolysis conditions are maintained such that CF is the electrolysis product of the anode.

In exemplary hydrino reactions and regeneration, the reaction mixture comprises NaH catalyst, MgH2, P20s (P40io), and support, activated carbon. In one embodiment, the source of the exothermic reaction is the oxidation reaction of metal hydride by? 205 such as 5MgH2 + P205? 5 gO + 2P + 5H2 (109) 5NaH + P205? 5NaOH + 2P. '(110) Phosphorus can be converted to P2O5 by combustion in 02 2P + 2.502? P2O5 (111) The MgO product can be converted to the hydroxide by reaction with water MgO + H 20? Mg (OH) 2. (112) Mg (OH) 2 can be reduced to Mg using Na or NaH: 2Na + Mg (0H) 2? 2NaOH + Mg. (113) Then, the NaOH can be electrolyzed to Na metal and NaH and 02 directly from the melt, or it can be converted to NaCl by reaction with HC1, where the Cl2 1 of electrolysis gas of NaCl can be reacted with H2 from the electrolysis of water to form HCl. In some embodiments, metals such as Na and Mg can be converted to the corresponding hydrides by reaction with H2, preferably from the electrolysis of water.

In exemplary hydrino reactions and regeneration, the solid fuel reaction mixture comprises NaH, Mg¾, NaN03 catalyst, and support, activated carbon. In one embodiment, the source of the exothermic reaction is the oxidation reaction of NaN03 metal hydride such as NaN03 + NaH + C? Na2C03 + 1 / 2N2 + 1 / 2H2 (114) NaN03 + 1 / 2H2 + 2NaH? 3NaOH + 1 / 2N2 (115) NaN03 + 3MgH2? 3MgO + NaH + 1 / 2N2 + 5 / 2H2. (116) Sodium or magnesium carbonate, hydrogen carbonate, and other species that comprise carbon- and oxygen can be reduced with Na or NaH: NaH + Na2C03? 3NaOH + C + 1 / H2 (117) NaH + l / 3MgC03? NaOH + 1 / 3C + l / 3Mg. (118) The carbonates can also be decomposed from the aqueous medium to the hydroxides and C02 Na2C03 + H20? 2NaOH + C02. (119) Released C02 can be reacted with water and C by reducing H2 using the gas water displacement reaction and the Fischer-Tropsch reaction C02 + H2? CO + H20 (120) CO +. H2? C + H20. . (121) The MgO product can be converted to the hydroxide by reaction with water MgO + H20? 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 nitrates can be regenerated using methods known to those skilled in the art. In one embodiment, N02 can be regenerated by known industrial methods such as the Haber process followed by the Ostwald process. In one embodiment, the exemplary sequence of steps is: N2 * Specifically, the Haber process can be used to produce H3 from N2 and H2 at elevated temperature and pressure using a catalyst such as some iron-containing oxide. The Ostwald process can be used to oxidize the ammonia to N02, in a catalyst such as a hot platinum catalyst or platinum-rhodium. The heat can be waste heat from the energy system. The N02 can be dissolved in water to form nitric acid which is reacted with NaOH, Na2CC > 3, or NaHCO 3 to form sodium nitrate. Then, the remaining NaOH can be electrolyzed to Na metal and NaH and 02 directly from the melt, can be converted to NaCl by reaction with HC1, where the Cl2 of NaCl electrolysis gas can be reacted with H2 from the electrolysis of water to form HCl. In some (embodiments) metals such as Na and Mg can be converted to the corresponding hydrides by reaction with H2, preferably from the electrolysis of water.In other embodiments, Li and K replace Na.

In exemplary hydrino reactions and regeneration, the reaction mixture comprises the catalyst of NaH, MgH2, SF6, and support, activated carbon. In one embodiment, the source of the exothermic reaction is the oxidation reaction of metal hydride by SF6 such as 4MgH2 + SF6? 3MgF2 + 4H2 + MgS (125) 7NaH +. SF6? 6NaF + 3H2 + NaHS. (126) The NaF and MgF2 and the sulfides can be electrolyzed to Na and Mg of a molten salt which can additionally comprise HF. The fluorine electrolysis gas can react with the sulfides to form SF6 gas that can be removed dynamically. The separation of SF6 from F2 can be by methods known in the art such as cryo-distillation, membrane separation, or chromatography using a medium such as molecular sieves. NaHS melts at 350 ° C and can be part of the melted electrolysis mixture. Any MgS product can be reacted with Na to form NaHS, where the reaction can occur in, if your during electrolysis. S and metals can be products formed during electrolysis. Alternatively, the metals may be in the minority, such that more stable fluorides are formed or F2 may be added to form the fluorides. 3MgH2 + SF6? 3MgF2 + 3H2 + S (127) 6NaH + SF6? 6NaF + 3H2 + S. (128) NaF and MgF2 can be electrolyzed to F2, Na and Mg of a molten salt which can additionally comprise HF. Na and Mg are immiscible, and the separated metals can be converted to hydride with H2 gas, preferably, the compensation is from the electrolysis of H20. The gas of F2 can be reacted with sulfur to regenerate SF6- In exemplary hydrino and regeneration reactions, the reaction mixture comprises NaH catalyst, MgH2 / NF3, and support, activated carbon. In one embodiment, the source of the exothermic reaction is the oxidation reaction of metal hydride by NF3 such as 3MgH2 + 2NF3? 3MgF2 + 3H2 + N2 (129) 6MgH2 + 2NF3? 3MgF2 + Mg3N2 + 6H2 (130) 3 aH + NF3? 3NaF + 1 / 2N2 + 1.5H2. '(131) The NaF and MgF2 can be electrolyzed to F2, Na, and Mg of a molten salt which can additionally comprise HF. The conversion of Mg3N2 to MgF2 can occur in the melt. Na and Mg are immiscible, and the separated metals can be converted to hydride with H2 gas, preferably from the electrolysis of H20. The F2 gas can be reacted with NH3, preferably in a copper packed reactor to form NF3. Ammonia can be created from the Haber process. Alternatively, NF3 can be formed by the electrolysis of NH4F in anhydrous HF.

In exemplary hydrino reactions and regeneration, the solid fuel reaction mixture comprises NaH catalyst, MgH2, Na2S20s and support, activated carbon. In one embodiment, the source of the exothermic reaction is the oxidation reaction of metal hydride by Na2S208 such as 8MgH2 + Na2S208? 2MgS + 2NaOH + 6MgO + 6H2 (132) 7MgH2 + Na2S208 + C? 2MgS + Na2C03 + 5MgO + 7H2 (133) lONaH + Na2S208? 2Na2S + 8NaOH + H2 (134) 9NaH + Na2S208 + c? 2 Na2S + Na2CO3 + 5NaOH + 2H2. (135) Any MgO product can be converted to the hydroxide by reaction with water MgO + H20? Mg (OH) 2. (136) Carbonate of sodium or magnesium, hydrogen carbonate, and other species that comprise carbon and oxygen can be reduced with Na or NaH: NaH + Na2C03? 3NaOH + C + 1 / H2 (137) NaH + l / 3MgC03? NaOH + 1 / 3C + l / 3Mg. (138) MgS can be subjected to combustion in oxygen, hydrolyzed, exchanged with Na to form sodium sulfate, and electrolyzed to Na2S208 2MgS + 10H2O + 2Na0H? Na2S20n + 2Mg (0H) 2 + 9H2. (139) The Na2S can be subjected to combustion in oxygen, hydrolyzed to sodium sulfate, and electrolyzed to form Na2S208 2Na2S + 10H2O? Na2S206- + 2Na0H + 9H2 (140) - Mg (0H) 2 can be reduced to Mg using Na or NaH: 2Na + Mg (OH) 2? 2 aOH + Mg. '(141) Then, the NaOH can be electrolyzed to Na metal and NaH and 02 directly from the melt, or it can be converted to NaCl by reaction with HCl, where the Cl2 of electrolysis gas of NaCl can be reacted with H2 from the electrolysis of water to form HCl.

In exemplary hydrino reactions and regeneration, the solid fuel reaction mixture comprises NaH catalyst, MgH2, S, and support, activated carbon. In one embodiment, the source of the exothermic reaction is the oxidation reaction of metal hydride by S such as MgH2 + S? MgS + H2 (142) 2NaH + .S? Na2S + H2. (143) Magnesium sulphide can be converted to hydroxide by reaction with water MgS + 2H20? Mg (0H) 2 + H2S. (144) The H2S can be decomposed at elevated temperature or used to convert S02 to S. Sodium sulfide can be converted to the hydroxide by combustion and hydrolysis Na2S + 1,502? Na20 + S02 (145) Na20 + H20? 2NaOH Mg (0H) 2 can be reduced to Mg using Na or NaH: 2Na + Mg (0H) 2? 2NaOH + Mg. (146) Then, the NaOH can be electrolyzed to Na metal and NaH and 02 directly from the melt, or it can be converted to NaCl by reaction with HCl, where the Cl2 of NaCl electrolysis gas can be reacted with H2, electrolysis of water to form HCl. S02 can be reduced to high temperature using H2 S02 + 2H2S? 3S + 2H20. (147) In some embodiments, metals such as Na and Mg can be converted to the corresponding hydrides by reaction with H2, preferably from the electrolysis of water. In other embodiments, the S and metal can be regenerated by electrolysis from a melt.

In reactions of. Hydrinogen and exemplary regeneration, the reaction mixture comprises NaH catalyst, MgH2, N20, and support, activated carbon. In one embodiment, the source of the exothermic reaction is the oxidation reaction of metal hydride by N20 such as 4MgH2 + N20? MgO + Mg3N2 + 4H2 (148) NaH + 3N20 + C? NaHCO3 + 3N2 + 1 / 2H2. (149) The MgO product can be "converted to hydroxide by reaction with water MgO + H20? Mg (OH) 2. (150) Magnesium nitride can also be hydrolyzed to magnesium hydroxide: Mg3N2 + 6H20? 3Mg (OH) 2 + 3H2 + N2. (151) Sodium carbonate, hydrogen carbonate and other species that comprise carbon and oxygen can be reduced with Na or NaH: NaH + Na2C03? 3NaOH + C + 1 / H2. (152) Mg (OH) 2 can be reduced to Mg using Na or NaH: 2Na + g (OH) 2? 2NaOH + Mg. '(153) Then, the NaOH can be electrolyzed to metal of -Na and NaH and 02 directly from the melt, or it can be converted to NaCl by reaction with HCl, where the Cl2 of electrolysis gas of NaCl can be reacted with H2 from electrolysis of water to form HCl. The ammonia created from the Haber process is oxidized (Equation (124)) and the temperature is controlled to favor the production of N20 which is separated from the other gases of the steady state reaction product mixture.

In exemplary hydrino reactions and regeneration, the reaction mixture comprises NaH, MgH2, Cl2 catalyst, and support, such as activated carbon, WC or Tic. The reactor may further comprise a high energy light source, preferably ultraviolet light to dissociate Cl2 to initiate the hydrino reaction. In one embodiment, the source of the exothermic reaction is the oxidation reaction of metal hydride by Cl 2 such as 2NaH + Cl2? 2NaCl + H2 (154) Mg¾ + Cl 2? MgCl2 + H2. (155) NaCl and MgCl2 can be electrolyzed to Cl2, Na, and Mg of one, molten salt. The electrolysis of molten NaCl can be done using a Downs cell or a cell. modified Downs cell. The NaCl for this electrolysis can be the rinsing of the reaction products with aqueous solution. The solution can be filtered to remove the support such as activated carbon which can be centrifuged and dried, preferably using waste heat from the energy system. Na and Mg are immiscible, and the separated metals can be converted to hydride with H2 gas, preferably from the electrolysis of H20. An exemplary result is as follows: | 4g of WC + lg of MgH2 + lg of NaH + 0.01 mol of Cl2 initiated with ultraviolet lamp to dissociate Cl2 to Cl, Ein: 162.9 kJ, dE: 16.0 kJ, TSC: 23-42 ° C, Tmax: 85 ° C , the theoretical is 7.10 kJ, the gain is 2.25 times.

Reagents comprising a catalyst or catalyst source such as NaH, K or Li or their hydrides, a reductant such as an alkali metal or hydride, preferably Mg, MgH2 or Al, and an oxidant such as NF3 can be regenerated by electrolysis . Preferably, the metal fluoride products are regenerated to metals and fluorine gas by electrolysis. The electrolyte may comprise a eutectic mixture. The mixture may further comprise HF. The F? it can be regenerated by the electrolysis of NH4F in anhydrous HF. In another embodiment, NH3 is reacted with F2 in a reactor such as a packed copper reactor. The F2 can be generated by electrolysis using a dimensionally stable anode or a carbon anode using conditions that favor the production of F2. The SF6 can be regenerated by reaction of S with F2. Any metal nitride that can be formed in the idrino reaction can be regenerated by at least one- thermal decomposition, H2 reduction, oxidation to the oxide or hydroxide and reaction to the halide followed by electrolysis, and reaction with halogen gas during the fused electrolysis of a metal halide. The NC13 can be formed by reaction of ammonia and chlorine gas or by reaction of ammonia salts such as H4C1 with chlorine gas. The chlorine gas can be from the electrolysis of chlorine salts such as those from the reaction product mixture. H3 can be formed using the Haber process, where the hydrogen can be from electrolysis, preferably from water. In one embodiment, the NC13 is formed in situ in the reactor by the reaction of at least one of NH3 and an ammonium salt such as NH4C1 with Cl2 gas. In one embodiment, BiF5 can be regenerated by reaction of BiF3 with F2 formed from electrolysis of metal fluorides.

In one embodiment, wherein the oxygen or halogen source optionally serves as a reactant for an exothermic activation reaction, an oxide or halide product is preferably regenerated by electrolysis. The electrolyte may comprise a eutectic mixture, such as a mixture of Al203 and Na3AlF6; MgF2, NaF, and HF; Na3AlF6; NaF, - SiF4, and HF; and AlF3, NaF, and HF. The electrolysis of SiF4 to Si and F2 can be from a eutectic mixture of alkaline fluoride. Since Mg and Na have low miscibility, they can be separated into phases of the melts. Since Al and Na have low miscibility, they can be separated into phases of the melts. In another embodiment, the electrolysis products can be separated by distillation. In a further embodiment, Ti203 is regenerated by reaction with C and Cl2 to form CO and TiCU which is further reacted with Mg to form Ti and MgCl2. Mg and Cl2 can be regenerated by electrolysis. In the case that MgO is the product, the Mg can be regenerated by the Pidgeon process. In one embodiment, the MgO is reacted with Si to form Si02 and Mg gas which is condensed. The product of Si02 can be regenerated to Si by reducing H2 at high temperature or by reaction with carbon to form Si and CO and C02. In another embodiment, Si is regenerated by electrolysis using a method such as the electrolysis of solid oxide in molten calcium chloride. In one embodiment, the chlorate or perchlorate such as a chlorate or alkaline perchlorate is regenerated by electrolytic oxidation. The brine can be oxidized electrolytically to chlorate and perchlorate.

To regenerate the reagents, any oxide coating on a metal support that can be formed can be removed by dilute acid following the separation of the reagent or product mixture. In another embodiment, the carbide is generated from the oxide by reaction with carbon with liberation of carbon monoxide or dioxide.

In the case that the reaction mixture comprises a solvent, the solvent can be separated from other reagents or products to be regenerated by removing the solvent using evaporation or by filtration or centrifugation with retention of the solids. In the event that other volatile components such as alkali metals are present, they can be removed selectively by heating to an appropriately elevated temperature such that they are evaporated. For example, a metal such as Na metal is collected by distillation and a support such as carbon remains. The Na can be rehydrated to NaH and returned to the carbon with added solvent to regenerate the reaction mixture. Isolated solids such as R-Ni can be regenerated separately as well. The separated R-Ni can be converted to hydrides again by exposure to hydrogen gas at a pressure in the range of 0.1 to 300 atmospheres.

The solvent can be regenerated in the event that it decomposes during the catalysis reaction to form hydrinos. For example, the decomposition products of DMF can be dimethylamine, carbon monoxide, formic acid, sodium formate and formaldehyde. In one embodiment, dimethyl formamide is produced either with catalyzed reaction of dimethyl amine and carbon monoxide in methanol or the reaction of methyl formate with dimethyl amine. It can also be prepared by reacting dimethylamine with formic acid.

In one embodiment, an exemplary ether solvent can be regenerated from the products of the reaction mixture. Preferably, the reaction mixture and reaction conditions are chosen such that the reaction rate of the ether is minimized in relation to the rate to form hydrins, such that any degradation of ether is negligible in relation to the energy produced from the hydrino reaction. Thus, the ether can be re-added as necessary with the ether degradation product removed. Alternatively, the ether and reaction conditions can be chosen such that the ether reaction product can be isolated and the ether regenerated.

One embodiment comprises at least one of the following: the HSA is a fluoride, the HSA is a metal, and the solvent is fluorinated. A metal fluoride can be a reaction product. The metal and fluorine gas can be regenerated by electrolysis. The electrolyte may comprise the fluoride such as NaF, MgF2, AlF3 or LaF3 and may additionally comprise at least one other species such as HF and other salts that lower the melting point of fluoride, such as those disclosed in U.S. Patent No. 5,427,657 . Excessive HF can dissolve LaF3. The electrodes may be carbon such as "graphite and may also form fluorocarbons as desired degradation products In one embodiment, at least one of the metal or alloy, preferably nanopoly, coated with carbon such as Co, Ni, Fe, coated with carbon, other transition metal powders or alloys, and metal-coated carbon, preferably nanopoly, such as carbon coated with a transition metal or alloy, preferably at least one of Ni, Co, Fe and Mn carbon coated, comprises particles that are magnetic Magnetic particles can be separated from a mixture such as a mixture of a fluoride such as NaF and carbon by using a magnet.The collected particles can be recycled as part of the reaction mixture to form hydrinos.

In one embodiment, the catalyst or catalyst source such as NaH and the fluorinated solvent is regenerated from the products comprising NaF by separation of the products followed by electrolysis. The NaF isolation method can be to rinse the mixture with a polar solvent with a low boiling point followed by one or more filtration and evaporation to give solid NaF. Electrolysis can be electrolysis of molten salt. The molten salt can be a mixture such as a eutectic mixture. Preferably, the mixture comprises NaF and HF as is known in the art. Sodium metal and fluorine gas can be collected from electrolysis. Na can be reacted with H to form NaH. The fluorine gas can be reacted with a hydrocarbon to form a fluorinated hydrocarbon that can serve as the solvent. The HF fluorination product can be returned to the electrolysis mixture. Alternatively, a hydrocarbon and a carbon product such as benzene and graphitic carbon, respectively, can be fluorinated and returned to the reaction mixture. The carbon can be cracked to smaller fluorinated segments, with a lower melting point to serve as the solvent by methods known in the art. The solvent may comprise a mixture. The degree of fluorination can be used as a method to control the reaction rate of hydrogen catalysis. In one embodiment, CF4 is produced by electrolysis of a molten fluoride salt, preferably an alkaline fluoride, using a carbon electrode or by reaction of carbon dioxide with fluorine gas. Any CH4 and hydrocarbon products can also be fluorinated to CF4 and fluorocarbons.

Suitable fluorinated HSA materials and methods for fluorinating carbon to form such HSA materials may be those known in the art such as those disclosed in U.S. Patent Nos. 3,929,920, 3,925,492, 3,925,263 and 4,886,921. Additional methods comprise the preparation of a poly-dicarbon monofluoride as disclosed in U.S. Patent No. 4,139,474, a process for the continuous fluorination of carbon as disclosed in U.S. Patent No. 4,447,663, a process for producing a graphite fluoride which comprises mainly polydicarbon monofluoride represented by the formula (C2F) n as disclosed in U.S. Patent No. 4,423,261, a process for preparing polycarbon monofluoride as disclosed in U.S. Patent No. 3,925,263, a process for the preparation of fluoride of graphite as disclosed in U.S. Patent No. 3,872,032, a process for the preparation of a poly-dicarbon monofluoride as disclosed in U.S. Patent No. 4,243,615, a method for the preparation of graphite fluoride by contact reaction between carbon and fluorine gas as disclosed in U.S. Patent No. 4,438,086, the synthesis of luorograph as disclosed in U.S. Patent No. 3,929,918, the process for the preparation of polycarbon monofluoride as disclosed in U.S. Patent No. 3,925,492, and a mechanism for providing novel synthesis methods to graphite-fluorine chemistry as disclosed by Lagow et al., JCS-Dalton, 1268 (1974), wherein the materials disclosed therein comprise the HSA materials. As a kind of reactor material, Monel metal, nickel, steel or copper can be employed in consideration of fluorine gas corrosion. The carbon materials include amorphous carbons such as carbon black, petroleum coke, petroleum fish coke and mineral coal, and crystalline carbons such as natural graphite, graphene and graphite, artificial, fullerene and nanotubes, preferably single-walled. Preferably Na is not intercalated to the carbon support or forms an acetylide. Such carbon materials can be used in various ways. In general, preferably, the carbon powder materials have an average particle size of not more than 50 microns, but greater are also suitable. In addition to carbon powder materials, other forms are appropriate. The carbon materials can be in the form of blocks, spheres, rods and fibers. The reaction can be carried out in a reactor selected from a fluidized bed type reactor, a rotary kiln type reactor and a turret tower reactor.

In another embodiment, the fluorinated carbon is regenerated using an additive. Carbon can also be fluorinated by inorganic reagents such as CoF3 outside the cell or in situ. The reaction mixture may further comprise a source of inorganic fluorination reagent such as one of Co, CoF, CoF2 and CoF3 which can be added to the reactor and regenerated or can be formed during the operation of the cell of the reaction mixture to form hydrinos and possibly another reagent such as F2 gas with optionally a fluorination catalyst metal such as Pt or Pd. The additive can be NH3 which can form NH4F. At least one carbon and hydrocarbon can react with NH4F to become fluorinated. In one embodiment, the reaction mixture further comprises HNaF2 which can react with carbon to fluorinate it. The fluorocarbon can be formed in itself or externally to the hydrino reactor. The fluorocarbon can serve as a solvent or HSA material.

In an embodiment wherein at least one of the solvent, support or rarefactor comprises fluorine, the products possibly comprise carbon, in such cases that the solvent or support is a fluorinated organic, also as fluorides of the catalyst metal such as NaHF2 and NaF This is in addition to the lower energy hydrogen products such as molecular hydrino gas that can be vented or collected. Using F2, the carbon can be attacked since the CF4 gas that can be used as reactant in another cycle of the reaction to produce energy. The remaining products of NaF and NaHF2 can be electrolyzed to Na and F2. Na can be reacted with hydrogen to form NaH and F2 can be used to attack the carbon product. The NaH, remaining NaF and CF4 can be combined to put into operation another cycle of the energy production reaction to form hydrinos. In other modalities, Li, K, Rb or Cs can replace Na.

SAW. Other Modalities of Liquid and Heterogeneous Fuels In the present disclosure, a "liquid solvent embodiment" comprises any reaction mixture and the corresponding fuel comprises a liquid solvent such as a liquid fuel and a heterogeneous fuel.

In another embodiment comprising a liquid solvent, one of atomic sodium and molecular NaH is provided by a reaction between a metal, ionic or molecular form of Na and at least one other compound or element. The source of Na or NaH may be at least one of Na metal, an inorganic compound comprising Na such as NaOH ,. and other suitable Na compounds such as NaNH2, Na2C03, and Na20, NaX (X is a halide), and NaH (s). The other element can be H, a displacing agent or a reducing agent. The reaction mixture may comprise at least one of (1) a solvent, (2) a source of sodium such as at least one of Na (m), NaH, NaNH2, Na2C03, Na20, NaOH, R-Ni doped with NaOH, NaX (X is a halide), and R-Ni doped with NaX, (3) a hydrogen source such as gas gas and a dissociator and a hydride, (4) a displacing agent such as an alkali metal or alkaline earth, preferably Li, and (5) a reducing agent such as at least one of a metal such as an alkali metal, alkaline earth metal, a lanthanide, a transition metal such as Ti, aluminum, B, an alloy of metal such as AlHg, NaPb, NaAl, LiAl and a metal source alone or in combination with reducing agent such as an alkaline earth halide, transition metal halide, lanthanide halide, and aluminum halide. Preferably, the alkali metal reducer is Na. Other suitable reagents comprise metal hydride such as LiBH 4, NaBH 4, LIAH 4 or NaAlH 4. Preferably, the reducing agent reacts with NaOH to form NaH molecules and a Na product1 such as Na, NaH (s), and Na20. The NaH source can be R-Ni comprising NaOH and a reagent such as a reductant to form the NaH catalyst such as an alkaline or alkaline earth metal or the R-Ni intermetallic Al. Additional exemplary reagents are. an alkaline or alkaline earth metal and an oxidant. such as AlX3, MgX2, LaX3, CeX3 and TiXn, wherein X is a halide, preferably Br or I. Additionally, the reaction mixture may comprise another compound comprising a rarefactor or a dispersant such as at least one of Na2C03, Na3S04, and Na3P04 that can be doped to the dissociator such as R-Ni. The reaction mixture may further comprise a support, wherein the support may be impurified with at least one reagent of the mixture. The support may preferably have a large surface area which favors the production of the NaH catalyst of the reaction mixture. The support may comprise at least one of the group of R-Ni, Al, Sn, Al203 such as gamma, beta or alpha alumina, sodium aluminate (beta-aluminas have other ions present such as Na + and possess the ideal composition Na20- 11A1203), lanthanide oxides such as 203 (preferably M = La, Sm, Dy, Pr, Tb, Gd, and Er), Si, silica, silicates, zeolites, lanthanides, transition metals, metal alloys such as alkaline alloys and alkaline earth with Na, rare earth metals, SiO2-Al203 or Ni SiO2 supported, and other supported metals such as at least one of platinum supported on alumina, palladium or ruthenium. The support can have a high surface area and comprise high surface area materials (HSA) such as R-Ni, zeolites, silicates, aluminates, aluminas, alumina nanoparticles, porous 1203, Pt, Ru or Pd / Al203, carbon, Pt or Pd / C, inorganic compounds such as Na 2 CO 3, silica and zeolite materials, preferably Y zeolite powder, and carbon such as fullerene or nanotubes. In one embodiment, the support such as Al203 (and the Al203 support of the dissociator if present) reacts with the reductant, such as a lanthanide to form a surface-modified support. In a modality, the Al of the surface is exchanged with the lanthanide to form a lanthanide-substituted support. This support can be contaminated with a source of NaH molecules such as NaOH and reacted with a reductant such as a lanthanide. The subsequent reaction of the lanthanide-substituted support with the lanthanide will not change it significantly, and the impurified -NaOH on the surface can be reduced to the NaH catalyst by reaction with the reducing lanthanide.

In an embodiment comprising a liquid solvent, wherein the reaction mixture comprises a source of NaH catalyst, the source of NaH can be an Na alloy and a source of hydrogen. The alloy may comprise at least one of those known in the art such as an alloy of sodium metal and one or more other alkali or alkaline earth metals, transition metals, Al, Sn, Bi, Ag, In, Pb, Hg, Si, Zr, B, Pt, Pd, or other metals and the source of H can be H2 or a hydride.

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

In a liquid-solvent embodiment, the reaction mixture comprises at least one species from the group comprising a solvent, Na or a source of Na, NaH or a source of NaH, a metal hydride or a source of a hydride of metal, a reagent or source of a reagent to form a metal hydride, a hydrogen dissociator and a hydrogen source. The reaction mixture may further comprise a support. Reagent for forming a metal hydride may comprise a lanthanide, preferably La or Gd. In one embodiment, La can react reversibly with NaH to form LaHn (n = 1, 2, 3). In one embodiment, the hydride exchange reaction forms the NaH catalyst. The reversible general reaction can be given by NaH + M Na + MH (156) The reaction given by equation (156) is applied to other MH-type catalysts given in Table 3. The reaction can proceed with the formation of, hydrogen that can be dissociated to form atomic hydrogen that reacts with Na to form the NaH catalyst. The dissociator is preferably at least one of Pt, Pd or Ru powder / AI2O3, Pt / Ti and R-Ni. Preferably, the dissociator support such as Al203 comprises at least one substitution of La on the surface or Al or comprises Pt, Pd or Ru / M203 powder wherein M is a lanthanide. The dissociator can be separated from the rest of the reaction mixture where the separator passes atomic H.

An appropriate liquid-solvent embodiment comprises the reaction mixture of a NaH, La and Pd solvent over Al203 powder, in "where the reaction mixture can be regenerated in one embodiment by removing the solvent, adding H2, separating NaH and hydride of lanthanum by sieving, heating the lanthanum hydride to form La and mixing La and NaH.Alternatively, regeneration involves the steps of separating Na and lanthanium hydride by melting Na and removing the liquid, heating the lanthanium hydride to form La, Hydration of Na to NaH, mix La and NaH and add the solvent.The mixture of La and NaH can be by ball mill.

In a liquid-solvent embodiment, a high surface area material such as R-Ni is doped with NaX (X = F, Cl, Br, I). The contaminated R-Ni is reacted with a reagent that will displace the halide to form at least one of Na and NaH. In one embodiment, the reagent is at least one alkaline or alkaline earth metal, preferably at least one of K, Rb, Cs. In another embodiment, the reagent is an alkaline or alkaline earth hydride, preferably at least one of KH, RbH, CsH, MgH2 and CaH2. The reagent can be either an alkali metal hydride or an alkaline earth metal hydride. The reversible general reaction can be given by NaX + MH NaH + MX (157) A. Reactions of NaOH catalyst to form the NaH catalyst The reaction to form NaOH and Na to Na20 and NaH is NaOH + 2Na? Na20 + NaH (158) The exothermic reaction can promote the formation of NaH (g). Thus, the Na metal can serve as a reductant to form the NaH catalyst (g). Other examples of suitable reductants that have a similar highly exothermic reduction reaction with the source of NaH are alkali metals, alkaline earth metals such as at least one of Mg and Ca, metal hydrides such as LiBH4, NaBH4, LiAlH4 or NaAlH4, B, Al, transition metals such as Ti, lanthanides such as at least one of La, Sm , Dy, Pr, Tb, Gd and Er, preferably La, Tb and Sm. Preferably, the reaction mixture comprises a solvent, a high surface area material (HSA material) having a dopant such as NaOH comprising a source of the NaH catalyst. Preferably, the conversion of the doping agent on the material with a high surface area to the catalyst is obtained. The conversion can occur through a reduction reaction. In addition to Na, other preferred reductants are alkali metals, Ti, a lanthanide or Al. Preferably, the reaction mixture comprises doped NaOH to the HSA material, preferably R-Ni. Where the reducer is Na or Al inter-metallic. The reaction mixture may further comprise a source of H such as a hydride or H2 gas and a dissociator. In certain embodiments, the source of H is R- Ni hydrolyzed.

In a liquid-solvent mode, Na20 formed as a reaction product to generate the NaH catalyst, such as that given by equation 158, is reacted with a hydrogen source to form NaOH which can also serve as a source of the NaH catalyst. In one embodiment, a regenerative NaOH reaction of equation (158) in the presence of atomic hydrogen is Na20 + H? NaOH + Na ?? = -11.6 kj I mol NaOH (159) NaH ?? a +? (1/2) ?? = -10,500 kj I mol ^ 160 ^ y NaH? Na + H (\ / 4) AH = -19,700 kJ mol H. (161) Thus, a small amount of NaOH and Na with a source of atomic hydrogen or atomic hydrogen serves as a catalytic source of the NaH catalyst, which in turn forms a large hydrine yield via multiple cycles of regenerative reactions such as those given by the equations (158-161). In one embodiment, of the reaction given by equation (162), Al (OH) 3 can serve as a source of NaOH and NaH, where with Na and H, the reactions given by equations (158-161) proceed to form hydrins 3Na + Al (OH) 3? NaOH + NaAl02 + NaH + 1 / 2H2. (152) In a liquid-solvent embodiment, the inter-metallic Al serves as the reductant to form the NaH catalyst. The balanced reaction is given by 3NaOH + 2Al? Al203 + 3NaH (163) This exothermic reaction can drive the formation of NaH (g) to drive the very exothermic reaction given by equations (25-30), where the NaH regeneration occurs from Na in the presence of atomic hydrogen.

Two suitable liquid-solvent embodiments comprise the first reaction mixture of Na and R-Ni comprising about 0.5% by weight of NaOH, where Na serves as the reductant and a second reaction mixture of R -Ni comprising approximately 0.5. % by weight of NaOH, where the inter-metallic Al serves as the reducer. The reaction mixture can be regenerated by adding NaOH and NaH which can serve as a source of H and a reductant.

In a liquid-solvent embodiment of the energy reactor, the source of NaH such as NaOH is regenerated by addition of a source of hydrogen, such as at least one of a hydride and hydrogen gas and a dissociator. The hydride and dissociator can be R - Ni hydrolyzed. In another embodiment, the source of NaH such as R-Ni doped with NaOH is regenerated by at least one of re-hydrization, addition of NaH and addition of NaOH, where the addition may be by physical mixing. With the solvent removed first, the mixture can be made mechanically by methods such as by ball milling.

In a liquid-solvent embodiment, the reaction mixture further comprises oxidizing-forming reagents that react with NaOH or Na 2 O to form a very stable oxide and NaH. Such reagents comprise cerium, magnesium, lanthanide, titanium or aluminum or their compounds such as AlX3, gX2 / LaX3, CeX3 and TiXn, wherein X is a halide, preferably Br or I and a reducing compound such as an alkaline or alkaline earth metal . In one embodiment, the source of the ÑaH catalyst comprises R-Ni comprising a sodium compound such as NaOH on its surface. Then, the reaction of NaOH with oxidizing reagents such as A1X3, MgX2, LaX3, CeX3 and TiXn and the alkali metal M forms NaH, MX and Al203, MgO, La203, Ce203 and Ti203, respectively.

In a liquid solvent mode, the reaction mixture comprises R-Ni doped with NaOH and an alkali metal or alkaline earth metal added to form at least one of Na and NaH molecules. The Na can further react with H from a source such as H2 gas or a hydride such as R-Ni to form the NaH catalyst. The subsequent catalysis reaction of NaH forms states of H given by equation (35). The addition of an alkaline or alkaline earth metal M can reduce Na + to Na by the reactions: NaOH + M to MOH + Na (164), 2NaOH + M to M (OH) 2 + 2Na. (165) M can also react with NaOH to "form H also as 2NaOH + M to Na20 + H2 + MO (166) Na20 + M to M20 + 2Na. (167) Next, the NaH catalyst can be formed by the reaction Na + Ha NaH (168) by reacting with H of reactions such as that given by equation (166) also as of R-Ni and any added source of H. Na is an appropriate reductant since it is an additional source of NaH.

Hydrogen can be added to reduce NaOH and form the NaH catalyst: NaOH + Hi to NaH + | H20. (169) The H in R - Ni can reduce NaOH to Na metal and water that can be removed. through, pumping. An organic solvent can be removed first before reduction or a molten inorganic solvent can be used.

In a liquid-solvent embodiment, the reaction mixture comprises one or more compounds that react with a source of NaH to form the NaH catalyst. The source can be NaOH. The compounds may comprise at least one of LiNH2, Li2NH and Li3N. The reaction mixture may further comprise a source of hydrogen such as H2. In some embodiments, the reaction of sodium hydroxide and lithium amide to form NaH and lithium hydroxide is NaOH + LiNH2? LiOH + NaH + 1 / 2N2 + LiH. (170) I The reaction of sodium hydroxide and lithium imide to form NaH and lithium hydroxide is NaOH + Li2NH - Li20 + NaH + 1 / 2N2 + l / 2H2. (171) In addition, the reaction of sodium hydroxide and lithium nitride to form NaH and lithium oxide is: NaOH + Li3N? Li20 + NaH + 1 / 2N2 + Li. (172) B. Reactions of alkaline earth metal hydroxide catalyst to form NaH catalyst In a liquid-solvent embodiment, an H source is supplied to a Na source to form the NaH catalyst. The source of Na can be metal. The source of H can be a hydrogen. The hydrogen may be at least one of alkaline hydroxide, alkaline earth metal, a transition metal hydroxide and Al (OH) 3. In one embodiment, Na reacts with a hydroxide to form the corresponding oxide and the NaH catalyst. In one embodiment, where the hydroxide is Mg (0H) 2, the product is MgO. In one embodiment, where the hydroxide is Ca (C0) 2, the product is CaO. The alkaline earth oxides can be reacted with water to regenerate the hydroxide. The hydroxide can be collected as a precipitate by methods such as filtration and centrifugation.

For example, in one embodiment, the reaction to form the NaH catalyst and regeneration cycle for Mg (OH) 2 are given by the equations: 3Na + Mg (OH) 2? 2NaH + MgO + Na20 (173) MgO + H20? Mg (OH) 2. (174) · In a liquid-solvent embodiment, the reaction to form the NaH catalyst and regeneration cycle for Ca (OH) 2, are given by the reactions: 4Na + Ca? 2NaH + CaO + Na20 (175) CaO + H20? Ca (OH) (176) C. Reactions of Na / N alloy to form the NaH catalyst The alkali metal in solid and liquid states is a metal. In order to generate M or the MH catalyst, M is an alkali metal, the reaction mixture of the liquid or heterogeneous fuel comprises M / N alloy reactants. In one embodiment, the reaction mixture, liquid-fuel reactions, Heterogeneous fuel reactions and regeneration reactions comprise those of the M / N system, where the fuel generates at least one of the catalyst and atomic hydrogen.

In one embodiment, the reaction mixture comprises one or more compounds that react with a source of NaH to form the NaH catalyst. The reaction mixture may comprise at least one of the group of Na, NaH, NaNH2, Na2NH, Na3N, NH3, a dissociator, a hydrogen source such as a H2 gas or a hydride, a support and a rarefactor such as NaX (X is a halide). The dissociator is preferably Pt, Ru or Pd / Al203 powder. The dissociator may comprise Pt or Pd on a support-of high surface area appropriately inert to Na. The dissociator can be Pt or Pd on carbon or Pd / Al203. The last support may comprise a protective surface coating of a material such as NaAl02. The reagents may be present in any percent by weight.

A suitable solvent-liquid embodiment comprises a reaction mixture of a solvent, Na or NaH, NaNH2 and Pd on Al203 powder, wherein the reaction mixture can be regenerated by addition of H2.

In one embodiment, NaNH2 is added to the reaction mixture. NaNH2 generates NaH according to the reversible reactions: Na2 + NaNH2? NaH + Na2NH (177) and 2Na + N NH2? NaH (g) + Na2NH + H2. (178) In the hydrino reaction cycle, Na'-. Na| and NaNH2 react to form the molecule of NaH and Na2NH and NaH forms the hydrino and Na. Thus, the reaction is reversible according to the reactions: ?to,?? + H ,? NaNH, + NaH 179) (180) Na2NH + Na + H? NaNH2 + Na2.

In one embodiment, the NaH of equation (179) is molecular, such that this reaction is another to generate the catalyst.

The reaction of sodium amide and hydrogen to form ammonia and sodium hydride is H2 + NaNH2? NH3 + NaH. (181) In a liquid solvent mode, this reaction is reversible. The reaction can be driven to form NaH by increasing the concentration of ¾. Alternatively, the positive or forward reaction can be driven via the formation of atomic H using a dissociator. The reaction is given by: > 2H + NaNH2? NH3 + NaH. (182) The exothermic reaction is can drive the formation of NaH (g).

In a liquid solvent embodiment, the NaH catalyst is generated from a reaction of NaNH2 and hydrogen, preferably atomic hydrogen as given in the reaction equations (181-182). The proportions of the reagents can be any desired amount. Preferably, the proportions are about stoichiometric to those of the equations (181-182). The reactions to form the catalyst are reversible with the addition of an H source such as H2 gas or a hydride to replace that which reacted to form hydrins, where the reactions of the catalyst are given by equations (25-30) and the sodium amide is formed with the additional NaH catalyst by the reaction of ammonia with Na: NH + Na2? NaNH2 + NaH. (183) In a liquid solvent mode, a HSA material is doped with NaNH2. The doped HSA material is reacted with a reagent that will displace the amide group to form at least one of Na and NaH. In one embodiment, the reagent is an alkaline or alkaline earth metal, preferably Li. In another embodiment, the reagent is an alkaline or alkaline earth hydride, preferably LiH. The reagent can be both an alkali metal hydride. as alkaline earth. A source of H such as H2 gas may be additionally provided in addition to that provided by any other reagent. the reaction mixture, such as a hydride, HSA material and displacement reagent.

In a liquid solvent embodiment, the sodium amide undergoes reaction with lithium to form amide, imide or lithium nitride and Na or NaH catalyst. The reaction of sodium and lithium amide to form lithium imide and NaH is 2Li + NaNH2 - > Li2NH + NaH. (184) The reaction of sodium amide and lithium hydride to form lithium amide and NaH is LiH + NaNH2? LiNH2 + NaH. (185) The reaction of sodium, lithium and hydrogen amide to form lithium amide and NaH is Li + 1 / 2H2 + NaNH2 - LiNH2 + NaH. (186) In a liquid solvent embodiment, the reaction of the mixture forms Na and the reagents further comprises a source of H which reacts with Na to form the NaH catalyst by a reaction such as the following: Li + NaNH2 to LiNH2 + Na (187) V Na + H to NaH (188) IiH + NaNH2 to liNH2 + NaH. (189) In a liquid solvent embodiment, the reagents comprise NaNH2, a reagent for displacing the amide group of NaNH2 such as an alkaline or alkaline earth metal, preferably Li, and may additionally comprise a source of H such as at least one of MH (M = LI, Na,, Rb, Cs, Mg, Ca, Sr and Ba), H2 and a hydrogen dissociator and a hydride.

The reagents of the reaction mixture, such as the solvent M, MH, NaH, NaNH2, HSA material, hydride and the dissociator are in any desired molar ratio. Each of M, MH, NaNH2 and the dissociator are in molar proportions greater than zero and less than 100%, preferably the molar proportions are similar.

Other modalities of liquid solvent systems to generate. The NaH molecular catalyst involves Na and NaBH4 or NH4X (X is an anion such as halide). The molecular HaH catalyst can be generated by the reaction of Na2 and NaBH4: Na 2 - - NaBH, * NaBH 3 + Na + | NaH. (190) NH4X can generate NaNH2 and H2 Na2 + NH4X to NaX + NaNH2 + H2. (191) Then, the NaH catalyst can be generated according to the reaction of equations (177-189). In another embodiment of liquid solvent, the reaction mechanism for the Na / N system to form the hydrinoNaH catalyst is N¾X + Na-Na to NaH + NH3 + NaX. (192) D. Catalysts and additional MH type reactions Another catalytic system of the MH type involves aluminum. The binding energy of AlH is 2.98 eV. The first and second ionization energies of Al are 5,985,768 eV and 18,82855 eV, respectively. Based on these energies, the AlH molecule can serve as a catalyst and source of H, since the binding energy of AlH plus the double ionization (t = 2) from Al to Al2 + is 27.79 eV '(27.2 eV) , which is equivalent to am = 1 in equation (36). The catalytic reactions are given by 27. 79 eV + AIH? ? + 2 + (193) ? + 2e ~ + H? AIH + 27.79 eV, and (194) the overall reaction is H -l21-13.6 eV. (195) In a liquid solvent embodiment, the reaction mixture comprises at least one of AlH molecules and a source of AlH molecules. A source of AlH molecules may comprise Al metal and a source of hydrogen, preferably atomic hydrogen. The source of hydrogen may be a hydride, preferably R-Ni. In another embodiment, the AlH catalyst is generated by the reaction of an Al oxide or hydroxide with a reductant. The reductant comprises at least one of the NaOH reductants previously given. In one embodiment, a source of H is provided to an Al source to form the AlH catalyst. The source of Al can be metal. The source of H can be a hydroxide. The hydroxide may be at least one of an alkaline hydroxide, alkaline earth metal hydroxide, a transition metal hydroxide and Al (OH) 3.

Raney nickel can be prepared by the following two reaction steps: NiA + 2NaOH + 6H20? [NILl * < "* 8? <? · (197) . { +2? A [?? (??) 4] + 3? 2 Na [Al (OH) 4] is easily dissolved in concentrated NaOH. It can be washed in de-oxygenated water. The Ni prepared contains Al (-10% by weight, which can vary) is porous and has a large surface area. It contains large amounts of H, both in the Ni crosslinked and in the form of Ni-A1HX (x = 1, 2, 3).

The R - Ni can be reacted with another element to cause chemical release of AlH molecules, which then undergo catalysis according to the reactions given by the equations (193-195). In one embodiment, the release of AlH is caused by a reduction reaction,. attack or alloy formation. One such other element is an alkaline or alkaline earth metal that reacts with the Ni portion of R-Ni to cause the AlHx component to release AlH molecules which subsequently undergo catalysis. In one embodiment, M can react with Al hydroxides or oxides to form the Al metal which can further react with H to form AlH. The reaction can be initiated by heating and the speed can be controlled by controlling the temperature. The solvent, M (alkaline or alkaline earth metal) and R - Ni are in any desired molar ratio. Each of the solvent, M and R - Ni are in molar proportions greater than zero and less than 100%. Preferably, the molar ratio of M and R-Ni are similar.

In a liquid-solvent mode, the source of AlH comprises R-Ni and other Raney metals or Al alloys known in the art, such as R-NI or an alloy comprising at least one of Ni, Cu, Si, Fe, Ru, Co, Pd, Pt and other elements and compounds. The R-NI or alloy may further comprise promoters such as at least one of Zn, Mo, Fe, and Cr. The R-Ni may be at least one of WR Grace Raney 2400, Raney 2800, Raney 2813, Raney 3201 , Raney 4200 or a modality attacked or doped with Na of these materials. In another embodiment of the liquid solvent of the AlH catalyst system, the catalyst source comprises a Ni / Al alloy, wherein the ratio of Al to Ni is in the range of about 10-90%, preferably about 10-50% and more preferably around 10 -30%. The catalyst source may comprise palladium or platinum and further comprise Al as a Raney metal.

Another catalytic system of the MH type involves 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, HCl can serve as a catalyst and source of H, since the binding energy of HCl plus the triple ionization (t = 3) of Cl to Cl3 + is 80.86 eV (3.27.2 eV), which is equivalent to am = 3 in equation (36). The catalytic reactions are given by: 80. 86 eV + HCl? C / 3 + + 3e + H + f (4) 2 -l21 13. eV (198) Cr + 3e '+ H? HCl + 80.86 eV, and (199) global reaction H -121 · 13.6 eV (200) In a liquid solvent embodiment, the reaction mixture comprises HCl or a source of HCl. A source can be NH4C1 or a solid acid and a chloride, such as an alkaline or alkaline earth chloride. The solid acid may be at least one of MHSO4, MHC03, MH2P0, and MHPO4, wherein M is a cation such as an alkaline or alkaline earth cation. Other such solid acids are known to those skilled in the art. In one embodiment, the reaction mixture comprises a strong acid such as H2SO and an ionic compound such as NaCl. The reaction of the acid with the ionic compound such as NaCl generates HCl to serve as a hydrinogen catalyst and source of H.

In general, MH type hydrogen catalysts to produce hydrinos provided by the breakdown of the M-H bond plus the ionization of t electrons of the M atom each at a continuous energy level, such that the sum of the binding energy and ionization energies of the electrons is approximately m. 27.2 eV where m is a whole number are given in table 3. Each MH catalyst is given in the first column and the corresponding M-H bond energy is given in column 2. The M atom of the MH species given in the first column is ionized for. provide the net reaction enthalpy of m. 27.2 eV with the addition of the binding energy in column 2. The enthalpy of the catalyst is given in the eighth column, where m is given in the ninth column. The electrons involved in the ionization are given with 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 nth electron of the atom or ion is designated by IPn and is given by CRC. This is, for example, Na + 5.13908 eV? Na ++ e "and Na + + 47.2864 eV? Na2 + + e". The first ionization potential, IPi = 5.13908 eV and the second ionization potential, IP2 = 47.2864 eV are given in the second and third columns, respectively. The net reaction enthalpy for the breakdown of the NaH bond and the double ionization of Na is 54.35 eV, as given in the eighth column and m = 2 in equation (36) as given in the ninth column. Additionally, H can react with each of the MH molecules given in Table 3 to form a hydrino having a number of quantum p incremented by one (equation (35)) in relation to the catalytic reaction product of MH alone as it is given by the exemplary equation (23).

Table 3. MH type hydrogen catalysts capable of providing a net reaction enthalpy of approximately m. 27.2 eV.

Catalyst Energy iP. 1P * AN Entalpia m link of M-M A1H 2.98 5.985768 18.82855 27.79 l BiH 2.936 7.2855 16.703 26.92 1 CIH 4.4703 12.96763 23.8136 39.61 80.86 CoH 2.538 7.88101 17.084 27.50 1 OEH 2,728 7.89943 15.93461 26.56 1 InH 2.520 5.78636 18.8703 27.18 1 NaH 1.925 5.139076 47.2864 54.35 RuH 2.311 7.36050 16.76 26.43 1 SbH 2.484 8.60839 16.63 27.72 v SeH 3.239 9.75239 21.19 30.8204 42.9450 107.95 4 SiH 3.040 8.15168 16.34584 27.54 1 SnH 2.736 7.34392 14.6322 30.50260 55.21 2 In other embodiments of the liquid solvent of the MH type catalyst, the reactants comprise sources of 'SbH, SiH, SnH, and InH. In embodiments that provide the catalyst * MH, the sources comprise at least one of M and a source of H2 and MHX, such as at least one of Sb, Si, Sn and In and a source of H2 and SbH3, SiH4, SnH and InHH3.

The liquid solvent reaction mixture may further comprise a source of H and a source of catalyst, wherein the source of at least one of H and catalyst may be a solid acid or NH 4 X wherein X is a halide, preferably Cl for forming the HCl catalyst. "Preferably, the reaction mixture may comprise at least one solvent, H4X, a solid acid, NaX, LiX, KX, NaH, LiH, KH, Na, Li ,. K, a support, a hydrogen and H2 dissociator, wherein 'X is a halide, preferably Cl. The solid acid may be NaHS04, KHS04, LiHS0, NaHCO3, KHC03, LiHC03, Na2HP04, K2HP04, LI2HP0, NaH2P04, KH2P04, and LIH2P0. 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 the case of a MH source comprising an M alloy, such as AlH and Al respectively, the alloy can be converted to hydride with a source of H2 such as H2 gas. The H2 can be supplied to the alloy during the reaction. H2 can be administered to form the alloy of a desired H content, with the H pressure changed during the reaction. In this case, the initial H2 pressure may be approximately zero. The alloy can be activated by the addition of a metal, such as an alkaline or alkaline earth metal. For MH catalysts and MH sources, hydrogen gas can be maintained in the range of about 1 Torr to 100 atm, preferably about 100 Torr at 10 atm, more preferably around 500 Torr at 2 atm. In other embodiments, the hydrogen source is a hydride such as an alkali metal or alkaline earth metal hydride.

I or a transition metal hydride.

Atomic hydrogen at high density can undergo three-body collision reactions to form hydrinos, where an H atom undergoes the transition to form states given by equation (35) when two additional H atoms are ionized. The reactions are given by: (201) 2H * + 2e-? 2H [a "} +27.21 eV, and the overall reaction is (203) In another modality, the reactions are given by: 54.4 ~ 42) I3.6 eV (204) 2H} m + 2e? 2H [aff] +54.4 eV, (205) the global reaction (206) In a liquid solvent mode, the material that provides H atoms with high density is R - Ni. The atomic H can be at least one of the decomposition of H within R-Ni and the dissociation of H2 from a source of H2, such as H2 gas supplied to the cell. The R-Ni can be reacted with an alkaline or alkaline, earth metal M. to improve the production of atomic H layers to cause catalysis. The R-Ni isolated from the solvent mixture can be regenerated by evaporating the metal M followed by the addition of hydrogen to revert the R-Ni to hydride.

Vile. Additional H auto-catalytic reactions Another catalytic reaction involving only H atoms, two hot H2 molecules collide and dissociate, so that three H atoms serve as a catalyst for 3 27.2 eV for the fourth, then the reaction between four hydrogen atoms. , whereby three atoms accept resonant and nonradiantly 81.6 eV of the fourth hydrogen atom, such that 3H serve as the catalyst is given by: i to 81. 6 eV + 3H + / í? 3i L, +3 < f + / H + [42 ~ 12] 13.6 eV (207) 3tf + + 3e-? 3H +81.6 eV, and fast (208) global reaction H? H + [4? -12] · 13.6 eV. (209) 4 The continuous ultraviolet radiation band due to the intermediary H 3 + 1 of the equation (207) is predicted to have a cut of short wavelength at 122.4 eV (10.1 nm) and to extend of longer wavelengths.

In general, the transition from? to to, H p = m + l due to the acceptance of m. 27.2 eV gives a continuous band with a cut of short wavelength in energy given by , = m2-13.6 eV (210) p = m + l corresponding to 91. 2 nm m and extends to wavelengths longer than the corresponding cut.

Another catalytic reaction involving the collision of both H with hot H2 may occur where each of the two H atoms accept 13.6 eV of the third to become ionized to serve as a 27.2 eV catalyst for the third. Then, the reaction between the hydrogen atoms, whereby two atoms accept resonant, and not radiant 27.2 eV of the third hydrogen atom in such a way that 2H serves as the catalyst is given by 1 27. 2 eV + 2H + H? 2H + + le + H + [22-12] · 13.6 eV (211) 2H * + 2e? 2 # +27.2 eV, (212) global reaction to H? H II + [22 -12] · 13.6 eV (213) The continuous ultraviolet radiation band due to the intermediate of to H * 1 + 1 of the equation (211) is predicted to have a cut of short wavelength to 13.6 eV (91.2 nm) and extend to longer wavelengths. The high densities are permissive of another reaction to give the continuous band of 91.2 where an H atom serves as a catalyst by accepting 27.2 eV of a second hydrogen atom. , In the presence of a high field, an ionized electron can undergo transition to a fractional state directly with the binding energy released as a short wavelength continuous band at the binding energy of the final state hydrine atom. The transitions i for H (l / 2) and H (l / 3) are given by H ++ e ~? H + [22-02] 13.6 eV (214) · H ++ e '? H + [32-02] · 13.6 eV. (215) It is predicted that continuous ultraviolet radiation bands have short wavelength cuts at 54.4 eV (22.8 nm) and 122.4 eV (10.1 nm), respectively, and extend at longer wavelengths. Due to the multi-polarity and corresponding selection rules H (1 / ¡4) is a preferred state. It is predicted that continuous ultraviolet radiation has a short wavelength cut at 217.6 eV (5.7 nm) and extends to longer wavelengths. ^ The ionization potential of the H2 molecular hydrino (1 / p) is IPl-Er. { H¡ (\ / p)) - ET (H2 (l¡p)) = -p216.13392 e -p30.118755 eV - (- p231.351 eV -p30.326469 eV) (216) (216) = p215.2171 eV + / > 30.207714 eV The binding energy of the molecular hydrino H¿ (1 / p), ED is given by: ED = -p1Z1.20eV-ET = -p227.20 eV - (- p231351eV-p30326469eV) (217) (217) = p24.151 eV + 30.326469 eV Another aspect of the present disclosure comprises a Ultraviolet radiation light source E. The light source comprises molecular hydrino gas and a component to excite the molecular hydrino gas to the ionization threshold. The de-excitation energy is given by equation (216). The excitation may be with a particle beam, preferably an electron beam. The molecular hydrino gas can be trapped in a matrix, preferably an alkaline or alkaline earth metal halide crystal. The crystal can be bombarded with a beam of electrons at high energy such as approximately 12 k and to provoke the. excitation followed by the emission of de-excitation. In another embodiment, de-excitation also results in the breakdown of the molybdenum linkage. Then the emitted energy is given by the difference in the energies given by equations (216) and (217): E = pa11.0661 eV - p30.118755 ffV. (218) broadcast For p = 4, the radiation is 7.3 nm (169.5 eV) which is in the extreme ultraviolet (EUV). This light could be for extreme ultraviolet lithography to manufacture micro-electronic devices.

In embodiments disclosed herein, at least one of a source of RB + such as Rb or hydride or a source of Cs such as Cs metal or hydride can serve as one; Catalyst - of Rb + or Cs, respectively! The hydride hydride ion can react with an oxidant, such as oxygen or sulfur to form molecular hydrino. Exemplary reactions are:; 2H ~ (l / p) + S? H2 (l / p) + S2- (219 ^ 2H- (Up) +02? H2 (l / p) + 022-. (220) I Thus, in one embodiment of a hydrino chemical reaction, the hydride hydride can be converted to a molecular hydrino when it is the desired product.

VIII. Energy of discharge of hydrogen gas and plasma cell and reactor A hydrogen and plasma gas discharge energy cell and reactor of the present disclosure is shown in Figure 5. The hydrogen and plasma gas discharge energy cell and reactor of Figure 5 includes a gas discharge cell 307 which it comprises a luminescent discharge vacuum vessel filled with hydrogen gas 315 having a chamber 300. A hydrogen source 322 supplies hydrogen to the chamber 300 through the control valve 325 via a hydrogen supply passage 342. A catalyst is contained in the chamber of the cell 300. A source of voltage and current 330 causes the current to pass between a cathode 305 and an anode 320. The current may be reversible. - In one embodiment, the cathode material 305 can be a catalyst source such as Fe, Dy, Be, or Pd. In another embodiment of the hydrogen and plasma gas discharge cell and reactor, the wall of the vessel 313 is conductive and serves as the cathode that replaces the electrode 305 and the anode 320 may be hollow, such as a hollow steel anode stainless. The discharge can vaporize the catalyst source to the catalyst. Molecular hydrogen can be dissociated by the discharge to form hydrogen atoms for generation of hydrines and energy. Further dissociation can be provided by a hydrogen dissociator in the chamber.

Another modality of the cell and reactor of energy discharge of hydrogen gas and plasma in which the catalysis occurs in the gas phase uses a controllable gaseous catalyst. Gaseous hydrogen atoms for conversion to hydrinos are provided by a molecular hydrogen gas discharge. The gas discharge cells 3 07 have a catalyst supply passage 341 for the passage of the catalyst 350 from the catalyst tank 395 into the reaction chamber 3 00. The catalyst tank 395 is heated by a catalyst tank heater 392 having a power source 372 for supplying the gaseous catalyst to the reaction chamber 300. The vapor pressure of the catalyst is controlled by controlling the temperature of the catalyst tank 395, to the adjuster of the heater 392 by means of its power source 372. The reactor further comprises a selective vent valve 301. A chemically opened container i J Resistant, such as a stainless steel, tungsten or ceramic can, placed inside the gas discharge cell can contain the catalyst. The catalyst in the catalytic can can be heated with a canister heater using an associated power source to supply the gaseous catalyst to the reaction chamber. Alternatively, the luminescent gas discharge cell is operated at an elevated temperature, such that the catalyst i in the can is sublimed, boiled or volatilized; to the gas phase. The vapor pressure of the catalyst is controlled by controlling the temperature of the canister or the discharge cell when adjusting the heater with its power source. To prevent the catalyst from condensing in the cell, the temperature is maintained above the temperature, from the catalyst source, the catalyst tank 395 or the catalyst canister. i In one embodiment, catalysis occurs in the gas phase, lithium is the catalyst and a source of atomic lithium such as lithium metal or a lithium compound such as LiNH2 becomes gaseous by maintaining the temperature of the cell in the cell. range of about 300-1000 ° C More preferably, the cell is maintained in the range of about 500-750 ° C. The atomic hydrogen reagent? /? can be maintained at a pressure less than atmospheric, preferably in the range of about I 10 milli Torr to approximately 100 Torr. More 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 range of the operating temperature is preferably in the range of about 300-1000 ° C and more preferably, the pressure is that obtained with the cell in the operating temperature range of about 300-750 ° C. The cell can be controlled at the desired operating temperature by the heating coil such as 380 of Figure 5 which is I energized by the power source 385. The cell may further comprise an internal reaction chamber 300. and an external hydrogen tank 390, such that hydrogen can be supplied to the cell by hydrogen diffusion through the wall 313 which separates the two chambers. The temperature of the wall can be controlled by using a heater to control the speed of diffusion. The diffusion rate can be controlled additionally by controlling the hydrogen pressure in the hydrogen tank.

In another embodiment of a system having a reaction mixture comprising a species from the group Li, iLiN¾, Li 2ÑH, LI 3 N, ?? 3, LiX, H 4X (X is a halide), H 3,? L1BH4, LIAIH4 and H2, at least one of the reagents is regenerated by adding one or more of the reagents and by regenerating plasma. The plasma can be one of the gases such as NH3 and H2. The plasma can be maintained in situ (in the reaction cell) or in an external cell in communication with the reaction cell. In other modalities, k, Cs and Na replace the Li, j where the catalyst is atomic K, atomic Cs and molecular NaH.

To maintain the catalyst pressure at the desired level, the cell having permeation as the source of hydrogen can be sealed. Alternatively, the cell further comprises high temperature valves at each inlet or outlet, such that the valve that comes into contact with the reaction gas mixture is maintained at the desired temperature.

The temperature of the plasma cell can be controlled independently over a wide range. by isolating the cell and by applying complementary heater power with the heater 380. Thus, the vapor pressure of the catalyst can be controlled independently of the plasma energy.

The discharge voltage can be. in the range of approximately 100 to 10,000 volts. The current may be in any desired range at the desired voltage. In addition, the plasma can be pulsed at any desired frequency range, displacement voltage, peak voltage, maximum energy and waveform.

In another embodiment, plasma can occur in a liquid medium such as a catalyst solvent: or reactants of species that are the source of the catalyst. i IX. Fuel cell and battery In modalities of one. fuel cell and a battery 400 shown in Figure 6, hydrino reagents comprising a solid fuel or a heterogeneous catalyst comprise the reagent for corresponding half-cell reactions. During the operation, the catalyst reacts with atomic hydrogen and the energy transfer results in the ionization of the catalyst. This reaction can occur in the anode compartment 402, in such a way that the anode 410 finally accepts the ionized electron stream. At least one of Li, K and NaH can serve as the catalysts to form hydrinos. The reaction step of a non-radiant energy transfer of an integer multiple of 27.2 eV of atomic hydrogen to the catalyst results in ionized catalyst and free electrons. The support such as activated carbon can serve as a conductive electron acceptor in electrical contact with the anode. The final electron acceptor reagents comprise, an oxidant, such as free radicals or a source thereof and a source of a positively charged counter ion which are the components of the cathode-cell reaction mixture that ultimately purge the electrons released from the cell. reaction i of the catalyst to form hydrins. The oxidant or cathode-cell reaction mixture is located in the cathode compartment 401 having the cathode 405. Preferably, the oxidant is at least one of oxygen or an oxygen source, a halogen, preferably F2 or Ci2 or a halogen source, CF4, SF6 and NF3. During operation, the counter-ion such as the catalyst ion can migrate to the anode compartment to the cathode compartment, preferably through a salt bridge 420. Each cell reaction can be supplied by additional reagent or the products can be removed through passages 460 and 461 to sources of reagents or storage tanks for product 430 and 431..

In certain embodiments, the energy, chemical, battery and fuel cell systems disclosed herein that regenerate the reactants and maintain the reaction to form lower energy hydrogen can be closed, except that only the hydrogen has consumed in the Hydrino formation needs to be replaced where the hydrogen fuel consumed can be obtained from the electrolysis of i water. i X. Chemical reactor The present disclosure is also concerned with other reactors for producing hydrogen compounds of the increased binding energy of the present disclosure, such as hydrino molecules and hydride hydride compounds. Additional products of the catalysis are energy and optionally plasma and light depending on the type of cell. Such a reactor is hereinafter referred to as a "hydrogen reactor" or "hydrogen cell". The hydrogen reactor comprises a cell for manufacturing hydrinos. The cell for making hydrines can take the form of a chemical reactor or gas fuel cell, such as a gas discharge cell, a plasma torch cell or microwave energy cell. Exemplary modalities of the cell for making hydrinos can take the form of a liquid fuel cell, a solid fuel cell and a heterogeneous fuel cell. Each of these cells comprises: (i) a source of atomic hydrogen; (ii) at least one catalyst selected from a solid catalyst, a molten catalyst, a liquid catalyst, a gaseous catalyst or mixture thereof to make hydrines and (iii) 1 a container for reacting hydrogen and the catalyst for making hydrinos. As used herein and as contemplated by the present disclosure, the term "hydrogen" unless otherwise specified includes not only proteum (½), but also deuterium (2H) and tritium (3H) J In the case of the use of deuterium as reagent of the hydrino reaction, relatively trace amounts of tritium or helium products of heterogeneous fuels and solid fuels are expected.

In one embodiment the chemical reactor for synthesizing compounds comprising lower energy hydrogen 1 such as hydride hydride compounds, the hydride hydride iron film is synthesized using an iron salt having Fe in a positive oxidation state which can react with H "(1 / p) by displacement of the iron counterion, preferably iron carbide, an iron oxide or a volatile iron salt such as Fel.sub.2 or Fel.sub.3 The catalyst may be K, NaH or LI. H can be of H2 and a dissociator such as R-Ni or Pt / Al203 In another embodiment, the hydride of iron hydride is formed from an iron source, such as an iron halide which decomposes to the iron. i reactor operating temperature, a catalyst such as NaH, Li or K and a hydrogen source such as H2 gas and a dissociator such as R-Ni. The manganese hydride hydride can be formed from a source of manganese such as a metal organ such as Mn (II) 2, 4-pentan dionate which decomposes at the operating temperature. of reactor. A catalyst such as NaH, Li or K and a source of hydrogen such as H2 gas and a dissociator such as R-Ni. In one embodiment, the reactor is maintained in the temperature range of about 252C to 800SC, preferably at the interval from about 4002C to 5002C. ' I I i Since alkali metals are covalent diatomic molecules in gas phase, in one embodiment, the catalyst to form hydrogen compounds of energy from The increased bond is formed from a source by a reaction with at least one other element. The catalyst such as k or Li can be generated by the metal dispersion of K or: Li in an alkaline halide, such as KX or LiX to form KHX LiHX, wherein X is a halide. The catalyst K or Li can be generated by the reaction of K2 or Li2 vaporized with atomic H to form KH and K or LiH and Li, respectively. The hydrogen compounds of increased binding energy can be MHX, in where M is an alkaline, H is a hydride hydride and X1 is a negatively charged ion individually, preferably X is one of a halide and HCO3. "In one embodiment, the reaction mixture to form KHI or KHC1, wherein is hydride 1 hydrino comprises the metal K covered with the KX (X = Cl, I) and a dissociator, preferably nickel metal such as nickel mesh and R-Ni, respectively. The reaction is carried out by keeping the reaction mixture at an elevated temperature, preferably in the range of 400-700 SC with the addition of hydrogen. Preferably, the hydrogen pressure is i maintained at a gauge pressure of approximately 0.35 Kg / cm2 (5 pounds / square inch). Thus, the MX is equiped i on the K, in such a way that the K atoms migrate through the halide lattice and the halide serves to disperse K and I act as a dissociator for K2 which reacts at the interface with H of the dissociator such as nickel mesh or R - Ni to form KHX. ! A reaction mixture suitable for the synthesis of hydride hydride compound ij comprises at least two species from the group of a catalyst, a hydrogen source, an oxidant, a 'reductant and a support, wherein the oxidant is a source of at least one of sulfur, phosphorus and oxygen such as SF6, S, S02, S03, S2O5CL2, F5SOF, M2S208, SxXy, such as S2C12, SC12 ', S2Br2, S2F2, CS2 ,. Sb2S5, SOxXy such as S0Cl2, j S0F2, S02F2, S0Br2, P, P205, P2S5, PxXy such as PF3, PC13, PBr3;, PI3, PF5, PCI5, PBr4F or PCI4F, POxXy such as P0Br3, P0I3, POCl3 or P0F3 , PSxXy such as PSBr3, PSF3, PSC13, a phosphorus-nitrogen compound such as P3N5, (C12PN) 3 or (C12PN) 4, (Br2PN) x (M is an alkali metal, x and y are integers, - X is halogen) , 02,, N20 and Te02. The oxidant may further comprise a source of a I halide, preferably fluorine, such as CF 4, NF 3 or CrF 2. The mixture may also comprise a rarefactor, such as a source of phosphorus and sulfur such as MgS and MHS (M is an alkali metal). A suitable rarefactor is an atom or compound that gives rise to a peak of NMR displaced from field up with ordinary H and a peak of hydride hydride which is field above the peak of ordinary H. Suitable Rarefactors comprise S, P, 0, Se and Te elemental or comprise compounds comprising S, P, 0, Se and Te. A general property of a Suitable rafactor for hydride hydride ions is that it forms chains, cages or rings in elemental form, in elemental doped form or with other elements that trap and stabilize hydride hydride ions. Preferably, the H "(1 / p) can be observed in solid NMR or in solution In another embodiment, either NaH or HCl serves as a catalyst.An appropriate reaction mixture comprises MX and M'HS04 / where M and M 'are alkali metals, preferably Na | y, K, respectively and X is a halogen, preferably Cl.

Reaction mixtures comprise at least one of (1) NaH, MgH2, SF6 and activated carbon (CA) catalyst, (2) NaH, MgH2, S and activated carbon (CA) catalyst, (3) NaH catalyst , MgH2, K2S2Oa, Ag y. activated carbon, (4) KH catalyst, MgH2, K2S208 and activated carbon, (5) MH catalyst (M = Li, Na,, K), Al or MgH2, 02, K2S208 and CA, (6) KH catalyst , Al, CF4 and CA, (7) catalyst of NaH, Al, NF3 and CA, (8) catalyst of KH, MgH2, N20 and CA, (9) catalyst of NaH, MgH2, 02 and (CA) activated carbon;, (10) NaH catalyst, MgH2, CF4 and CA, (11) MH catalyst, MgH2, (M = Li, Na or K) P2O5 (P4Oi0) and CA, (12) MH catalyst, MgH2, MN03, (M = Li, Na or K) and CA, (13) NaH or KH catalyst, Mg, Ca or Sr, a transition metal halide, preferably FeCl2, FeBr2, NiBr2f Mnl2 or a rare earth halide such as EuBr2 and Ca and (14) NaH, Al, CS2 catalyst and activated carbon are appropriate systems for generating energy and also I | to produce lower energy hydrogen compounds. In In other embodiments of the exemplary reaction mixtures given above, the catalytic cation comprises one of Li, Na, K, Rb or Cs and the other species of the reaction mixture are chosen from those of reactions 1 to 14. The reactants may be to be j in any desired proportions. The product of action I of hydrino is at least one of a hydrogen molecule and i a hydride ion that has a proton NMR peak displaced I field above that of ordinary molecular hydrogen or hydrogen hydride, respectively. In one embodiment, the hydrogen product is linked to another element other than hydrogen, where the peak of proton NMR is displaced upstream of that of the ordinary molecule, or compound or compound having the same molecular formula as the product or the Ordinary molecule, species or compound that is not stable at room temperature. i In one embodiment, the energy and hydrogen compounds of increased binding energy are produced by a reaction mixture comprising two or more of the following species: LIN03, NaN03, KN03, LiH, NaH, KH, Li, Na, K, H2, a support such as carbon, for example activated carbon, a metal reducer and metal hydride, for example MgH2. The reagents can be in any proportion! molar Preferably, the reaction mixture comprises 9.3% mole of MH, 8.6% mole of MgH2 / 74% mole of activated carbon and 7.86% 'i in mol of MN03 (M is Li, Na or K), where the mole percent of each species can be varied within a range of plus or minus a factor of 10 of that given for each species. The idrino molecular product and hydride hydride ion having a preferred 1/4 state can be observed using liquid NMR at about 1.22 ppm and -3.85 ppm, respectively. Following extraction of the product mixture with an NMR solvent, preferably deuterated DEM. The product "2003" can serve as a rarefactor for the hydride hydride ion to form a compound such as MHMHCO3.

In another embodiment, the energy and hydrogen compound of increased binding energy are produced by a reaction mixture comprising two or more of the following species: LiH, NaH, KH, Li, Na, K, H2, a metal reducer or metal hydride, preferably MgH2 or powder of Al, preferably nano-powder, a support such as carbon, 1 preferably activated carbon and a fluorine source such as a fluorine gas or a fluoro-carbide, preferably CF or hexafluorobenzene (HFB). The reagents can be in any molar proportion. Preferably, the reaction mixture comprises 9.8% in mol of MN, 9.1% in mol of MgH2 or 9% in mol of Al nano-powder, 79% in mol of activated carbon and 2.4% in mol CF4 or HFB (M is Li, Na or K), where the percent in j mol of each species can be varied within a range of plus or minus a factor of 10 of that given for each species. The hydrinohydride molecular product and hydride hydride ion having a preferred 1/4 state can be observed using liquid NMR at about 1.22 ppm and -3.86 ppm, respectively, following the extraction of the product mixture with a solvent of NMR, preferably DFM 'deuterated or CDC13. .'| In another embodiment, the energy and hydrogen compounds of increased binding energy are produced i by a reaction mixture comprising two or more of the following species: LiH, NaH, KH, Li, Na, K, H2, a metal reducer or metal hydride, preferably MgH2 or Al powder, a support such as carbon, preferably activated carbon and a source of fluorine, preferably SF6;. The reagents can be in any molar proportion. Preferably, the reaction mixture comprises 10 mol% MH, 9.1 mol% MgH2 or 9 mol% Al nano-powder, 78.8% in mol of activated carbon and 24% in mol SF6 or HFB (M is Lij, Na or K), where the mole percent of each species can be varied within a range of plus or minus one factor of 10 of that given for each species. A. Appropriate reaction mixture comprises NaH, MgH2 or Mg, AC and S, in these molar proportions. Hydrinohydrin hydride hydride molecular product having a preferred 1/4 state can be observed using liquid NMR at about j í 1. 22 ppm and -3.86 pm, respectively, following the extraction of the product mixture with an NMR solvent, prably deuterated DFM or CDC13. j j In another embodiment, the energy and hydrogen compounds of increased binding energy are produced by a reaction mixture comprising two or more of the following species: LiH, NaH, KH, Li, Na, K, H2, a metal reducer or metal hydride, prably MgH2 or powder of Al, a support such as carbon, prably activated carbon j, and a source of. at least one of sulfur, phosphorus, and oxygen, prably S or P powder, SF6, CS2, P205, | and MNO3 (M is an alkali metal). The reagents can be in any molar proportion. Prably the reaction mixture comprises 8.1% mol of H, 7.5% mol of MgH2 or Al powder, 65% mol of activated carbon, and 19.5% mol of S (M is Li, Na, or K), where% in mol of each species is I it can vary within a range of plus or minus a factor of 10 from that given for each species. An appropriate reaction mixture comprises NaH, gH2 or Mg, activated carbon, and S powder in these molar proportions. Hydrinoid hydride molecular product and hydride hydride ion having a prred state of 1/4 can be observed using liquid NMR at a about 1.22 ppm and -3.86 ppm, respectively, following the extraction of the product mixture with a solvent of NMR, prably deuterated DFM or CDC13.

In another embodiment, the energy and hydrogen compounds of increased binding energy are produced by a reaction mixture comprising NaHS. The hydrino hydride ion can be isolated from NaHS. In a 'mode, a reaction in solid state occurs within NaHS to form H "(1/4) which can be further reacted with a proton source, such as a solvent, prably H20, to form H2 (l / 4) ).

In one embodiment, the hydride hydride compounds can be purified. The purification method may comprise at least one of extraction and recrystallization using an appropriate solvent. The method may further comprise chromatography and other techniques for separation of inorganic compounds known to those skilled in the art.

In a liquid fuel embodiment, the solvent has a halogen functional group, prably fluorine. A suitable reaction mixture comprises at least one of hexafluorobenzene and octafluoronaphthalene added to a catalyst such as NaH, and mixed with a support such as activated carbon, a fluoropolymer or R-Ni. The reaction mixture may comprise an energetic material that can be used in applications that are known to those skilled in the art. Appropriate applications due to the high energy balance are propellants and piston-motor fuel. In one embodiment, a desired product is at least one of fullerene and nanotubes that are collected.

In one embodiment, the molecular hydride H2 (l / p), prably H2 (l / 4), is a product that is further reduced to form the corresponding hydride ions that can be used in applications such as hydride batteries and surface coatings . The molecular hydrino bond can be broken by a collisional method. The ¾ (l / p) can be dissociated via energy collisions with 'ions or electrons in a plasma or beam. Then, the dissociated hydrino atoms can be reacted to form the desired hydride ions.

In a further embodiment, the hydrine molecule H2 (l / p), prably H2 (l / 4), is a product that is used as a contrast agent in magnetic resonance imaging (MRI). The agent can be inhaled to form the image of the lungs, where it is displaced chemically upwards in relation to the ordinary H allowing it to be distinguishable and thus selective. In another embodiment, at least one of the lowest energy hydrogen compound and the lowest energy hydrogen species such as H "(l / p) is a pharmaceutical agent comprising at least one of the group of antilipidemic drugs., anti-cholesterol drugs, contraceptive agents, anticoagulants, anti-inflammatory agents, immunosuppressive drugs, antiarrhythmic agents, antineoplastic drugs, antihypertensive drugs, epinephrine blocking agents, cardiac inotropic drugs, antidepressant drugs, diuretics, antifungal agents, antibacterial drugs, anxiolytic agents, sedatives, muscle relaxants, anticonvulsants, agents for the treatment of ulcer disease, agents for the treatment of asthma and / or hypersensitivity reactions, antithrombolic agents, agents for the treatment of muscular dystrophy, agents for performing a therapeutic abortion, agents for the treatment of anemia, agents to improve the survival of aloiñjerto, agents for the treatment of metabolism alterations of I purine, agents for the treatment of ischemic heart disease, agents for the treatment of opiate withdrawal, agents that activate the effects of secondary messenger iriositol triphosphate, agents to block spinal reflexes, and antiviral agents in which a drug is included for the treatment of AIDS. In a formulation that occurs naturally, at least one of the lowest energy hydrogen compound and the lowest energy hydrogen species is made to have a desired concentration, such as a concentration higher than that which occurs naturally.

XI. Experimental j A. Batch Calorimetry, Water Flow The balance of force and energy of the mixtures of i j I Catalytic reaction listed on the right side of each infra entry was obtained using cylindrical stainless steel reactors of approximately 130.3 cm3 volume (inner diameter (ID) 3.8 cm (1.5 inches), length 11.4 cm (4.5 inches) and wall thickness of 0.5 cm (0.2 inches)) or a volume of 1988 cubic cm (inner diameter (ID) 9.5 cm (3.75 inches), length of 28 cm (11 inches) and wall thickness of 0.95 cm (0.375 inches)) and a water flow calorimeter comprising a vacuum chamber containing each cell and an external water cooling coil that collected more than 99% of the energy released in the cell to get an error of < ± 1%. The energy recovery was determined by integrating the total output power PT with the passage of time. The power was given by j PT = mCpAT (221) where m is the mass flow velocity, Cp j was the specific heat of the water, and ?? It was the absolute change in temperature between entry and exit. The reaction was initiated by applying precision power to external heaters. Specifically, 100-200 W of power (cell of 130.3 cm3) or 800-1000 W (cell of 1988 cm3) was supplied to the heater. During this period of. heating, the reagents reached a hydrino reaction threshold temperature, where the onset of the reaction was commonly confirmed by a rapid rise in temperature! of the cell. Once the cell temperature reached approximately 400-500 ° C, the input power was set to zero. After 50 minutes, the program directed the power to zero. To increase the heat transfer rate to the coolant, the chamber was re-pressurized with 1000 Tprr.of helium, and the maximum change in water temperature (outlet minus inlet) was approximately 1.2 ° C. The assembly is allowed to reach full equilibrium for a period of 24 hours as confirmed by the observation of full equilibrium in the flow thermistors. ' In each test, the input energy and the output energy were calculated by integration of the corresponding power. The thermal energy in the refrigerant flow at each time increment was calculated using Equation (221) by multiplying the volumetric flow rate of water by the density of the water at 19 ° C (0.998 kg / liter), the specific heat of the water (4181 kJ / kg ° C), the corrected temperature difference, and the time interval. The values were added throughout the experiment to obtain the total energy output. The total energy of the i cell ET must be equal to the energy input Ein and any net energy Enet. Thus, the net energy was given by i Enet = T -Ein. (222) From the energy balance, any excess heat Eex was determined in relation to the theoretical maximum Emt by 1 The calibration test results showed a better heat coupling of 98% of the resistive input to the output refrigerant and heat controls of excess of zero showed that with applied calibration correction, the calorimeter was accurate to an error of less than 1%. The results are given as follows, where Tmax is the maximum cell temperature, Ein is the input energy and dE is the measured output energy in excess of the input energy. All energies are exothermic. Positive values where they are given represent the magnitude of the energy.

Halides, Oxides and Metal Sulphides | 20g AC3-5 + 5g Mg + 8.3g KH + 11.2g Mg3As2, 298.6U, dE: 21.8 kJ, TSC: none, Tmax: 315 ° C, theoretical is endothermic, the gain is infinite. 1 I , | 20 g AC3-5 + 5 g of Mg + 8.3 g of KH + 9.1 g of Ca3P2, Ein: 282.1 kJ, dE: 18.1 kJ, TSC: none, Tmax: 320 ° C is endothermic, the gain is infinite. j | Rowan KH validation 7.47gm + Mg 4.5gm + Tic 18.0 gm + EuBr2 14.04gm, Ein: 321.1 kJ, dE: 40.5 kJ, Tmax ~ 340 ° C, Energy gain -6.5X (1.37 kJ x 4.5 = 6.16 kJ ).

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + TiB2 3. 5gm, Ein: 299 kJ, dE: 10 kJ, Without TSC with Tmax ~ 320 ° C. Energy gain ~ X (X ~ 0 kJ; cell 2.5 cm (1 inch): Energy in excess -5.1 kJ).

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + R Cl 6. 05gm, Ein: 311 kJ, dE: 18 kJ, Without TSC with Tmax ~ 340 ° C, I Energy gain ~ X (X ~ 0 kJ, 2.5 cm (1 inch) cell: Excess energy -6.0 kJ). · J | KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + Li2S 2.3gm, Ein: 323 kJ, dE: 12 kJ, Without TSC with Tmax ~ 340 ° C. Energy gain -X (X-0 kJ, 2.5 cm (1 inch) cell: Excess energy -5.0 kJ). ·! | KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + Mg3N2 5. 05gm, Ein: 323 kJ, dE: 11 kJ, Without TSC with Tmax ~ 330 ° C. Energy gain ~ (X ~ 0 kJ, 2.5 cm (1 inch) cell: Excess energy -5.2 kJ). | 4g AC3-5 + 1 g of Mg + 1.66 g of KH + 3.55g PtBr2, Ein: 95.0 kJ, dE: 15.7 kJ, TSC: 108-327 ° C, Tmax: 346 ° C, the theoretical is 6.66 kJ , the gain is 2.36 times. | 4g AC3-5 + lg of Mg +. lg NaH + 3.55g PtBr2, Ein: 94.0 kJ, dE: 14.3 kJ, TSC: 100-256 ° C, Tmax: 326 ° C, the theoretical is 6.03 kJ, the gain is 2.37 times. ' | 4g WC + lg of MgH2 + lg NaH + 0.01 mol C12 initiated with ultraviolet lamp to dissociate Cl2 to Cl, Ein: 162.9 kJ, dE: 16.0 kJ, TSC: 23-42 ° C, Tmax: 85 ° C, the theoretical is 7.10 kJ, the gain is 2.25 times. · | 4g AC3-5 + lg of Mg + 1.66 g of KH + 2.66g PdBr2, Ein: 113.0 kJ, dE: 11.7kJ, TSC: 133-276 ° C, Tmax: 370 ° C, the theoretical is 6.43 kJ, the gain is 1.82 times. | 4g AC3-5 + lg Mg + lg NaH + 2.66g PdBr2, Ein: 116.0 kJ, dE: 9.4 kJ, TSC: 110-217 ° C, Tmax: 361 ° C, the theoretical is 5.81 kJ, the gain It is 1.63 times. | 4g AC3-5 + lg of Mg + 1.66 g of KH + 3.60 g'Pdl2, Ein: 142.0 kJ, dE: 7.8 kJ, TSC: 177-342 ° C, Tmax: 403 ° C, the theoretical is 5.53 kJ, the gain is 1.41 times.; | 0.41 g of AlN + 1.66 g of KH + lg of Mg powder + 4 g of AC3-5 in a heavy use 2.5 cm (1 inch) cell, the energy gain was 4.9 kJ, but it was not observed no burst of cell temperature. The maximum temperature of the cell was 407 ° C, the theoretical temperature is endothermic.

'KH 8.3 gm + Mg 5.0 p + CAII-300 20.0 gm + CrB2 3.7gm, Ein: 317 kJ, dE: 19 kJ, Without TSC with Tmax ~ 340 ° C, the theoretical energy is endothermic 0.05 kJ, the gain is infinite . | '| | KH 8.3 gm + NEW Mg 5.0 gm + CAII-300 20.0 gm + AgCl_9.36 gm, Ein: 99 kJ, dE: 43 kJ, Small TSC at -250PC with Tmax ~ 3-40 ° C. Energy gain -2.3X (X = 18.88 kJ). ' | KH 8.3 gm + Mg 5.0 + NEW Tic (G06U055) 20., 0 gm + AgCl 7.2 gm, Ein: 315 kJ, dE: 25 kJ, small TSC at ~ 250 ° C with Tmax ~ 340 ° C. Energy gain -1.72X (X = .14.52 kJ).

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + Y203 11.3 gm (Gain ~ 4X with TiC), Ein: 353 kJ, dE: 23 kJ, Without TSC with Tmax ~ 350 ° C. Energy gain ~ 4X (X ~ l .18kJ * 5 = 5.9kJ).

|, KH 4.15 gm + Mg 2.5 gm + CAII-300 lO.Ogm + EuBr3 9.8 gm, Ein: 323 kJ, dE: 27 kJ, Without TSC with Tmax ~ 350 ° C. Energy gain -2.26 X (X = 11.93 kJ). | 4g AC3-5 + lg of Mg + lg of NaH + 2.23 g of Mg3As2, I 133. 0 kJ, dE: 5.8 kJ, TSC: none, Tmax: 371 ° C, the theoretical is endothermic, the gain is infinite. j 4g AC3-5 + lg of Mg + 1.66 g of KH + 2.23 g of Mg3As2, Ein: 139.0 kJ, dE: 6.5 kJ, TSC: none, Tmax: 393 ° C, the theoretical is endothermic, the gain is infinite. "| 4g AC3-5 + lg of Mg + 1.66 g of KH + 1.82 g of Ca3P2, Ein: 133.0 kJ, dE: 5.8 kJ, TSC: none, Tmax: 407i ° C, the theoretical is endothermic, the gain is infinite. í | 4g AC3-5 + lg of Mg + lg of NaH + 3.97g WCl6j; Ein: 99.0 kJ; dE: 21.84 kJ; TSC: 100-342 ° C; Tmax: 375 ° C, the theoretical is 16.7, the gain is 1.3 times. 2.60 g of Csl, 1.66 g of KH, lg g of AC3-4 in a heavy-duty cell of It was finished. The energy gain was He observed no temperature explosion of the cell. The maximum temperature of the cell was 406 ° C, the theoretical temperature is 0, the gain is infinite. 0.42 g of LiCl, 1.66 g of KH, lg of Mg powder and 4 g of AC3-4 was finished. The energy gain was 5.4 kJ, but no burst of cell temperature was observed. The maximum temperature of the cell was 412 ° C, the theoretical one is I of O, the gain is infinite. | 4g AC3-4 + lg of Mg + lg of NaH + 1.21g RbCl, Ein: 136.0 kJ, dE: 5.2 kJ, TSC: none, Tmax: 372 ° C, the theoretical is 0 kJ, the gain- is infinite .

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + CaBr2 10. 0 gm, Ein: 323 kJ, dE: 27 kJ, Without TSC with Tmax ~ 340 ° C. Energy gain -3.0 X (X ~ 1.71kJ * 5 = 8.55 kJ).

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + YF3 7.3 gm, Ein: 320 kJ, dE: 17 kJ, Without TSC with Tmax ~ 340 ° C. Energy gain -4.5 X (X ~ 0.74kJ * 5 = 3.7kJ).

| KH 8.3 gm + Mg 5.0 gm + TiC 20.0 gm + Dry SnBr2 14.0 gm, Ein: 299 kJ, dE: 36 kJ, Small TSC at ~ 130 ° C with Tmax ~ 350 ° C. Energy gain -1.23X (X ~ 5.85kJx5 = 29.25 kJ).

| KH 8.3 gm + Mg 5.0 gm + TiC 20.0 gm + EuBr2 15.6 gm, Ein: 291 kJ, dE: 45 kJ, Small TSC at ~ 50 ° C with Tmax ~ 320 ° C.

Energy gain ~ 32X (X ~ 0.28kJx5 = l .4kJ) and the gain is -6.5X (1.37 kJ x 5 = 6.85 kJ).

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + Dry ZnBr2 11.25 gm, Ein: 288 kJ, dE: 45 kJ, Small TSC at ~ 200 ° C with Tmax ~ 350 ° C. Energy gain -2.1X (X ~ 4.19kJx5 = 20.9kJ).

| NaH 5.0 gm + Mg 5.0 gm + CAII-300 20.0 gm + SF6, Ein: 77.7 kJ, dE: 105 kJ, Tmax ~ 400 ° C. Energy gain -1.43X (X for 0.03 mol SF6-73 kJ).

| NaH 5.0 gm "+ Mg 5.0 gm + CAII-300 20.0 gm + SF6, Ein: 217 kJ, dE: 84 kJ, Tmax ~ 400 ° C Energy gain -1.15X (X for 0.03 mol SF6-73 kJ) .

| KH 8.3 gm + g_ 5.0 gm + CAII-300 20.0 gm + AgCl 7.2 gm, Ein: 357 kJ, dE: 25 > kJ, small TSC at ~250 ° C with Tmax ~ 340 ° C. Energy gain -1.72X (X-14.52 kJ).

| KH 8.3 gm + Mg 5.0 p + CAII-300 20.0 gm + AgCl 7.2 gm, Ein: 487 kJ, dE: 34 kJ, Small TSC at ~ 250 ° C with Tmax ~ 340 ° C. Energy gain -2.34X (X-14.52 kJ). | 20 g AC3-4 + 8.3 g of Ca + 5g NaH + 15.5g Mnl2, Ein: 181.5 kJ, dE: 61.3 kJ, TSC: 159-233 ° C, Tmax: 283 ° C, the theoretical is 29.5 kJ, the gain is 2.08 times. | 4g AC3-4 + 1.66 g of Ca + 1.66 g of KH + 3.09 g Mnl2, Ein: 113.0 kJ, dE: 15.8 kJ, TSC: 228-384 ° C, Tmax: 395 ° C, the theoretical is 6.68 kJ , the gain is 2.37 times. | 4g AC3-4 + lg of Mg + 1.66 g of KH + 0.46g Li2S, Ein: 144.0 kJ, dE: 5.0 kJ, TSC: none, Tmax: 419 ° C, the theoretical is endothermic. | 1.01 g of Mg3N2, 1.66 g of KH, lg of Mg powder and 4 g of AC3-4 in a heavy use cell of 2.5 cm (1 inch), the energy gain was 5.2 kJ, but it was not observed no burst of cell temperature. The maximum temperature of the cell was 401 ° C, the theoretical temperature is 0. " 1.21 g of RbCl, 1.66 g of KH, lg of Mg powder and 4 g of AC3-4, the energy gain was 6.0 kJ, but no burst of cell temperature was observed .. The maximum temperature of the cell was 442 ° C, the theoretical one is 0. 2.24 g of Zn3N2, 1.66 g of KH, lg of Mg powder and 4 g of AC3-4 was finished. The energy gain was 5.5 kJ, but no burst of cell temperature was observed. The maximum temperature of the cell was 410 ° C, the theoretical temperature is 4.41 kJ, the gain is 1.25 times. | 4g AC3-4 + lg Mg + lg NaH + 1.77g PdC12, Ein: 89.0kJ, dE: 10.5kJ, TSC: 83-204 ° C, Tmax: 306 ° C, the theoretical is 6.14 kJ, the Gain is 1.7 times. 0.74 g of CrB2, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-4) in a heavy-duty cell of 2.5 cm (1 inch), the gain of energy was 4.3 kJ, but no burst of cell temperature was observed. The maximum temperature of the cell was 404 ° C, the theoretical temperature is 0. 0.70 g of TiB2, 1.66 g of KH ,. lg of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-4) was finished. The energy gain was 5.1 kJ, but no burst of cell temperature was observed. The maximum temperature of the cell was 431 ° C, the theoretical temperature is 0.

| NaH 5.0 gm + Mg 5.0 gm + CAII-300 20.0 gm + BaBr2 14.85 gm (dry), Ein: 328 kJ, dE: 16 kJ, Without TSC with Tmax ~ 320 ° C. Energy gain 160X (X ~ 0.02kJ * 5 = 0.1 kJ).

| NaH 1.0 gm + Mg 1.0 gm + CAII-300 4..0 gm + BaBr2 2.97 gm (dry), Ein: 140 kJ, dE: 3 kJ, Without TSC with Tmax ~ 360 ° C.

Energy gain -150X (X ~ 0.02kJ).

| NaH 5.0 gm + Mg 5.0 gm + CAII-300 20.0 gm + Mgl2 13.9 gm, Ein: 315 kJ, dE: 16 kJ, Without TSC with Tmax ~ 340 ° C. Energy gain -1.8X (X ~ l .75x5 = 8.75 kJ).

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + MgBr2 9.2 gm, Ein: 334 kJ, dE: 24 kJ, Without TSC with Tmax ~ 340 ° C. Energy gain ~ 2. IX (X ~ 2.23x5 = 11.5 kJ). | 20 g AC3-3 + 8.3 g of KH + 7.2g AgCl, Ein: 286.6 kJ, dE: 29.5 kJ, TSC: 327-391 ° C, Tmax: 394 ° C, the theoretical is 13.57 kJ, the gain is of 2.17 times. | 4g AC3 ^ 3 + lg of MgH2 + 1.66 g of KH + 1.44g AgCl, Ein: 151.0 kJ, dE: 4.8 kJ, TSC: none, Tmax: 397 ° C, the theoretical is 2.53 kJ, the gain is 1.89 times | 4g AC3-3 + lg of Mg + lg of NaH + 1.48 g of Ca3N2, Ein: 140.0 kJ, dE: 4.9 kJ, TSC: none, Tmax: 392 ° C, the theoretical is 2.01 kJ, the gain is 2.21 times | 4g AC3-3 + lg of Mg + lg of NaH + 1.86g InC12, Ein: 125.0 kJ, dE: 7.9 kJ, TSC: 163-259 ° C, Tmax: 374 ° C, the theoretical is 4.22 kJ, the gain is 1.87 times. '| 4g AC3-3 + lg of Mg + 1.66 g of KH + 1.86g InC12, Ein: 105.0 kJ, dE: 7.5. kJ, 'TSC: 186-30.2 ° C, Tmax: 370 ° C, the theoretical is 4.7 kJ, the gain is 1.5.9 times. | 4g AC3-3 + lg of Mg + 1.66 g of KH + 2.5g Dyl2, Ein: 135.0 kJ, dE: 6.1 kJ, TSC: none, Tmax: 403 ° C, the theory is 1.89 kJ, the gain It is 3.22 times. 3.92 g of EuBr3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-3) in a heavy-duty cell of 2.5 cm (1 inch), the gain of energy was 10.5 kJ, but no burst of cell temperature was observed. The maximum temperature of the cell was 429 ° C, the theoretical temperature is 3.4 kJ, the gain is 3 times. | 4.56 g of AsI3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-3), the energy gain was 13.5 kJ, and the burst temperature of the cell it was 166 ° C (237 - 403 ° C). The maximum temperature of the cell was 425 ° C, the theoretical temperature is 8.65 kJ, the gain is 1.56 times. | 4g AC3-3 + lg of Mg + lg of NaH + 2.09g EuF3, Ein: 185.1 kJ, dE: '8.0 kJ, TSC: none, Tmax: 463 ° C, the theoretical is 1.69 kJ, the gain is 4.73 times | 4g AC3-3 + lg of Mg + 1.66 g of KH + 1.27g AgF; Ein: 127.0 kJ; dE: 6.04 kJ; TSC: 84-190 ° C; Tmax: 369 ° C, the theoretical is 3.58 kJ, the gain is 1.69 times. 4g AC3-3 + lg Mg + lg NaH + 3.92g EuBr3; Ein: 162.5 kJ; dE: 7.54 kJ; TSC: not observed; Tmax: 471 ° C, the theoretical is 3.41 kJ, the gain is 2.21 times. | 2.09 g of EuF3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-3) in a heavy use cell of 2.5 cm (1 inch), the gain of energy was 5.5 kJ, but no burst of cell temperature was observed. The maximum temperature of the cell was 417 ° C, the theoretical temperature is 1.71 kJ, the gain is 3.25 times. 3.29 g of YBr3, 1.66 g of KH, lg of Mg powder and 4 g of CA-III 300 activated carbon powder (AC3-3), the energy gain was 7.0 kJ, but no burst of cell temperature. The maximum temperature of the cell was 441 ° C, the theoretical temperature is 4.16 kJ, the gain is 1.68 times.

| NaH 5.0 gm + Mg 5.0 gm + CAII-300 20.0 gm + Bal2 19.5 gm, Ein: 334 kJ, dE: 13 kJ, Without TSC with Tmax ~ 350 ° C. Energy gain -2.95 X (X-0.88 kJ x5 = 4.4 kJ).

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + BaC12 10.4 gm, Ein: 331 kJ, dE: 18 kJ, Without TSC with Tmax ~ 320 ° C. Power gain -6.9X (X ~ 0.52x5 = 2.6 kJ).

| KH 8.3 gm + Mg 5.0 gm + Tic 20.0 gm + LaF3 9.8 gm, Ein: - 338 kJ, dE: 7 kJ, Without TSC with Tmax ~ 320 ° C. Energy gain -1.9X (X ~ 3.65 kJ).

| NaH 5.0 gm + Mg 5.0 gm + CAII-300 20.0 gm + BaBr2 14.85 gm (dry), Ein: 280 kJ, dE: 10 kJ, Without TSC with Tmax ~ 320 ° C. Energy gain -100 X (X ~ 0.01 = 0.02x5 kJ).

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + BaBr2 14.85 gm (dry), Ein: 267 kJ, dE: 8 kJ, Without TSC with Tmax ~ 360 ° C. Energy gain -2.5 X (X-3.2 kJ).

| NaH 5.0 gm + Mg 5.0 gm + TiC 20.0 gm + ZnS 4.85 gm, Ein: 319 kJ, dE: 12 kJ, Without TSC with Tmax ~ 340 ° C. Energy gain ~ 1.5 X (X-8.0 kJ).

| KH 8.3 gm + Mg 5.0 gm + Tic 20.0 gm + AgCl 7.2 gm (Dried at 070109), Ein: 219 kJ, dE: .26 kJ, Small TSC at ~ 250 ° C with Tmax ~ 340 ° C. Energy gain -1.8X (X-14.52 kJ).

| KH 8.3 gm + Mg 5.0 gm + Tic 20.0 gm + Y203 11.3 gm, Ein: 339 kJ, dE: 24 kJ, small TSC at ~ 300 ° C with Tmax ~ 350 ° C. Energy gain -4.0 X (X ~ 5.9kJ with NaH). | 4g AC3-3 + lg of Mg + lg of NaH + 1.95g YC13, Ein: 137.0 kJ, dE: 7.1 kJ, TSC: none, Tmax: 384 ° C, the theoretical is 3.3 kJ, the gain is 2.15. times. 4.70 g of YI3, 1.66 g of KH, 'lg of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-1) in a heavy-duty cell of 2.5 cm (1 inch), the Energy gain was 6.9 kJ, but no burst of cell temperature was observed. The maximum temperature of the cell was 426 ° C, the theoretical temperature is 3.37 kJ, the gain is 2.0'4 times. 1.51 g of Sn02, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-1), the energy gain was 9.4 kJ, but no burst of cell temperature. The maximum temperature of the cell was 460 ° C, the theoretical temperature is 7.06 kJ, the gain is 1.33 times. 4.56 g of Asl3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-1), the energy gain was 11.5 kJ, and the burst temperature of the cell 'was 144 ° C (221-365 ° C). The maximum temperature of the cell was 463 ° C, the theoretical temperature is 8.65 kJ, the gain is 1.33 times. | 3.09 g of Mnl2, 1.66 g of KH, lg of Mg powder and 4 g of STiC-1 (Tic of Sigma Aldrich), the energy gain was 9.6 kJ, and the burst temperature of the cell was 137 ° C (38 - 175 ° C). The maximum temperature of the cell was 396 ° C, the theoretical temperature is 3.73 kJ, the gain is 2.57 times. 3.99 g of SeBr4, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-1), the energy gain was 20.9 kJ, and the burst temperature of the cell was 224 ° C (47 - 271 ° C). The maximum temperature of the cell was 383 ° C, the theoretical temperature is 16.93 kJ, the gain is 1.23 times. | 20 g AC3-3 + 5 g of Mg '+ 8.3 g of KH + 11.65 g Ag, Ein: 238.6 kJ, dE: 31.7 kJ, TSC: 230-316 ° C, Tmax: 317 ° C, the theoretical is 12.3 kJ, the gain is 2.57 times. | 4g AC3-3 + lg of Mg + 1.66 g of KH + 0.91g CoS, Ein: 145.1 kJ, dE: 8.7 kJ, TSC: none, Tmax: 420 ° C, the theoretical is 2.63 kj, the gain is 3.3 times 4g. AC3-3 + lg de. Mg + 1.66 g of KH + 1.84 g of MgBr2; Ein: 134.1 kJ; dE: 5.75 kJ; TSC: not observed; Tmax: 400 ° C, the theoretical is 2.23 kJ, the gain is 2.58 times. | 5.02 g of Sbl3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-1), the energy gain was 12.2 kJ, and the burst temperature of the , cell was 154 ° C (141 - 295 ° C). The maximum temperature of the cell was 379 ° C, the theoretical temperature is 9.71 kJ, the gain is 1.26 times "KH 8.3 gm + Mg 5.0 gm + TiC 20.0 gm + AgCl 7.2 gm, Ein: 304 kJ, dE: 30 kJ, small TSC at ~ 275 ° C with Tmax ~ 340 ° C. Energy gain -2.1X (X-14.52 kJ).

| KH 1.66 gm + Mg 1.0 gm + TiC 5.0 gm + BaBr2 2.97 gm Loaded BaBr2-KH-Mg-TiC, Ein: 130 kJ, dE: 2 kJ, Without TSC with Tmax ~ 360 ° C, the theoretical is 0.64 kJ , the gain is 3 times.

| KH 8.3 gm + Mg 5.0 gm + TiC 20.0 gm + CuS 4.8 gm, Ein: 318 kJ, dE: 30 kJ, Small TSC at ~ 250 ° C with Tmax ~ 360 ° C. Energy gain ~ 2. IX (X-14.4 kJ).

| KH 8.3 p + Mg 5.0 p + TiC 20.0 gm + MnS 4.35 gm, Ein: 326 kJ, dE: 14 kJ, Without TSC with Tmax ~ 350 ° C. Energy gain ~ 2.2X (X-6.3 kJ).

| KH 8.3 p + Mg 5.0 p + TiC 20.0 gm + GdF3 10.7 gm, Ein: 339 kJ, dE: 7 kJ, Without TSC with Tmax ~ 360 ° C. Energy gain ~ 2.54X. (X ~ 2.75 kJ). | 20 g AC3-2 + 5 g Mg + 8.3 g KH + 7.2 g AgCl, Ein: 327.1 kJ, dE: 40.4 kJ, TSC: 288-318 ° C, Tmax: 326 ° C, the theoretical is 14.52 , the gain is 2.78 times. | 20 g AC3-2 + 5 g Mg + 8.3 g KH + 7.2 g CuBr, Ein: 205.1 kJ, dE: 22.5 kJ, TSC: 216-268 ° C, Tmax: 280 ° C, the theoretical is 13.46 , the gain is 1.67 times. | 4g AC3-2 + lg of Mg + lg of NaH + 1.46g YF3, Ein: 157.0 kJ, dE: 4.3 kJ, TSC: none, Tmax: 405 ° C, the theoretical is 0.77, the gain is 5.65 times . | 4g AC3-2 + lg of Mg + 1.66 g of KH + 1.46g YF3, Ein: 137.0 kJ, dE: 5.6 kJ, TSC: none, Tmax: 398 ° C, the theoretical is 0.74, the gain is 7.54 times. | 11.3 g of Y203, 5 g of NaH, 5 g of Mg powder and 20 g of activated carbon powder CA-III 300 (AC3-2) in a 5 cm (2 inch) heavy-duty cell, the gain of energy was 24.5 kJ, but no burst of cell temperature was observed. The maximum temperature of the cell was 386 ° C, the theoretical temperature is 5.9, the gain is 4.2 times. | 4g AC3-2 + lg Mg + lg NaH + 3.91g Bal2, Ein: 135.0 kJ, dE: 5.3 kJ, TSC: none, Tmax: 378 ° C, the theoretical is 0.1 kJ, the gain is 51 times. | 4g AC3-2 + lg of Mg + 1.66 g of KH + 3.91g Bal2, Ein: 123.1 kJ, dE: 3.3 kJ, TSC: none, Tmax: 390 ° C, the theoretical is 0.88 kJ, the gain is 3.8 times | 4g AC3-2 + lg of Mg + 1.66 g of KH + 2.08g BaCl2, Ein: 141.0 kJ, dE: 5.5 kJ, TSC: none, Tmax: 403 ° c; the theoretical is 0.52 kJ, the gain is 10.5 times. | 4g AC3-2 + lg of Mg + 1.66 g of KH + 3.42g Srl2; Ein: 128.2 kJ; dE: 4.35 kJ; TSC: not observed; Tmax: 383 ° C, the theoretical is 1.62 kJ, the gain is 3.3 times. 4.04 g of Sb2S5, 1.66 g of KH, lg of g powder and 4 g of activated carbon powder CA-III 300 (AC3-2) was terminated. The energy gain was 18.0 kJ, and the burst temperature of the cell was 25L ° C (224 -475 ° C). The maximum temperature of the cell was 481 ° C, the theoretical temperature is 12.7 kJ, the gain is 1.4 times. | 4g AC3-2 + lg of Mg + lg of NaH + 0.97g ZnS, Ein: 132.1 kJ, dE: 7.5kJ, TSC: none, Tmax: 370 ° C, the theoretical 'is 1.4 kJ, the gain is 5.33 times | 4g AC3-2 + lg of Mg + lg of NaH + 3.12g EuBr2, Ein: 135. 0 kJ, dE: 5.0 kJ, TSC: 114-182 ° C, Tmax: 371 ° C, the theoretical is endothermic +0.35 kJ, the gain is infinite. | 4g AC3-2 + lg of Mg + 1.66 g of KH + 3.12g EuBr2, Ein: 122.0 kJ, dE: 9.4kJ, TSC: 73-135 ° C, Tmax: '385 ° C, the theoretical is 0.28 kJ , the gain is 34 times. 4g CA3-2 + lg Mg + 1.66 g KH + 3.67g PbBr2; Ein: 126.0 kJ; dE: 6.98 kJ; TSC: 270-408 ° C; Tmax: 421 ° C, the theoretical is 5.17 kJ, the gain is 1.35 times. 4g CA3-2 + lg of Mg + lg of NaH + 1.27g AgF; Ein: 125.0 kJ; dE: 7.21 kJ; TSC: 74-175 ° C; Tmax: 372 ° C, the theoretical is 3.58 kJ, the gain is 2 times. 1.80 g of GdBr3 (0.01 mol of GdBr3 is 3.97 g, but there was not enough GdBr3), 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-1), the Energy gain was 2.8 kJ, but no burst of cell temperature was observed. The maximum temperature of the cell was 431 ° C, the theoretical temperature is 1.84 kJ, the gain is 1.52 times. | 0.97 g of ZnS, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-1), the energy gain was 4.0 kJ, but no burst of cell temperature. The maximum temperature of the cell was 444 ° C, the theoretical temperature is 1.61 kJ, the gain is 2.49 times. · 3.92 g of BI3 (in PP bottle), 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-1), the energy gain was 13.2 kJ, and the change in the temperature gradient of the cell was 87 ° C (152-239 ° C). The maximum temperature of the cell was 465 ° C, the theoretical temperature is 9.7 kJ, the gain is 1.36 times. | 4g AC3-2 + lg of Mg + lg of NaH + 3.2g HfC14, Ein: 131.0 kJ, dE: 10.5 kJ, TSC: 277-439 ° C, Tmax: 440 ° C, the theoretical is 8.1 kJ, the Gain is 1.29 times. | 4g AC3-2 + lg of Mg + 1.66 g of KH + 3.2g HfCl4, Ein: 125.0 kJ, dE: 11.5 kJ, TSC: 254-357 ° C, Tmax: 405 ° C, the theoretical is 9.06 kJ, the gain is 1.27 times. 4g CA3-2. + Lg, Mg + 1.66 g KH + 2.97g BaBr2; Ein: 132.1 kJ; dE: 4.65 kJ; TSC .: not observed; Tmax: 361 ° C, the theoretical is 0.64 kJ, the gain is 7.24 times. | 4g CA3-2 + lg of Mg + 1:66 g of KH "+ 2.35g Agí; Ein: 142.9 kJ; dE: 7.32 kJ; TSC: not observed; Tmax: 420 ° C, the theoretical is 2.46 kJ, the gain is 2.98 times. 4.12 g of PI3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-1) was finished. The energy gain was 13.8 kJ, and the burst temperature of the cell was 189 ° C (184-373 ° C). The maximum temperature of the cell was 438 ° C, the theoretical temperature is 11.1 kJ; the gain is 1.24 times. 1.57 g of SnF2, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-1), the energy gain was 7.9 kJ, and the change in the slope of Cell temperature was 72 ° C (149-221 ° C). The maximum temperature of the cell was 407 ° C, the theoretical temperature is 5.28 kJ, the gain is 1.5 times. 1.96 g of LaF3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-1), the energy gain was 4.2 kJ, but no burst of cell temperature. The maximum temperature of the cell was 442 ° C, the theoretical temperature is 0.68 kJ, the gain is 6.16 times. . | 4g CAIII-300 + lg of Mg + lg of NaH + 2.78 g of Mgl2, Ein: 129.0 kJ, "dE: 6.6 kJ, TSC: none, Tmax: 371 ° C, the theoretical is 1.75 kJ, the gain is 3.8 times. | 4g CAIII-300 + lg of Mg + 1.66 g of KH + 2.48g SrBr2, Ein: 137.0 kJ, dE: 6.1 kJ, TSC: none, Tmax: 402 ° C, the theoretical is 1.35 kJ, the gain is 4.54 times 4g CA3-2 + lg Mg + 1.66 g KH + 2.0 g CaBr2; Ein: 147.0 kJ; dE: 6.33 kJ; TSC: not observed; Tmax: 445 ° C, the theoretical is 1.71 kJ, the gain is 3.7 times. 4g CA3-2 + lg of Mg + lg of NaH + 2.97g BaBr2; Ein: 140. 1 kJ; dE: 8.01 kJ; TSC: not observed; Tmax: 405 ° C, the theoretical is 0.02 kJ, the gain is 483 times. 0.90 g of CrF2, 1.66 g of KH, ig of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-1) was terminated. The energy gain was 4.7 kJ, but no burst of cell temperature was observed. The maximum temperature of the cell was 415 ° C, the theoretical temperature is 3.46 kJ, the gain is 1.36 times.

| KH 8.3 gm + Mg 5.0 gm + TiC 20.0 gm + InCl 7.5 gm, Ein: 275 kJ, dE: 26 kJ, Without TSC with Tmax ~ 340 ° C. Energy gain -2.2 X (X-11.45 kJ).

| KH 8.3 gm + Mg 5.0 gm + TiC 20.0 gm + Inl 12.1 gm, Ein: 320 kJ, dE: 12 kJ, Without TSC with Tmax ~ 340 ° C. Energy gain -1.25 X (X-9.6 kJ).

| KH 8.3 gm + Mg 5.0 gm + TiC 20.0 gm + InBr 9.75 gm, Ein: 323 kJ, dE: 17 kJ, Without TSC with Tmax ~ 340 ° C. Energy gain -1.7X (X-10 kJ).

| KH 8.3 p + Mg 5.0 + TiC 20.0 gm + Mnl2 15.45 gm VALIDATION experiment by Dr. Peter Jansson, Ein: 292 kJ, dE: 45 kJ, small TSC at ~ 30 ° C with Tmax ~ 340 ° C. Energy gain -2.43X (X-18.5 kJ).

| KH 8.3 gm + Mg 5.0 gm + TiC 20.0 gm + FeBr2 10.8 gm (FeBr2 from STREM Chemicals) VALIDATION experiment by Dr. Peter Jansson, Ein: 308 kJ, dE: 46 kJ, TSC at ~ 220 ° C with Tmax ~ 330 ° C. Energy gain -1.84X (X ~ 25 kJ).

| KH_8.3 gm + Mg_ 5.0 gm + TiC 20.0 gm + Col2_15.65 gm, Ein: 243 kJ, dE: 55 kJ, Small TSC at ~ 170 ° C with Tmax ~ 330 ° C, the theoretical is 26.35 kJ, the gain is 2.08 times.

"KH 8.3 gm + Mg 5.0 gm + TiC 20.0 gm + NiBr2 ll.Ogm, Ein: 270 kJ, dE: 45 kj, TSC at ~ 220 ° C with Tmax ~ 340 ° C, the theoretical is 23 kJ, the gain is 1.95 times.

| KH 8.3 gm + Mg 5. 0 gm + TiC 20.0 gm + FeBr2 10.8 gm (FeBr2 from STREM Chemicals), Ein: 291 kJ, dE: 38 kJ, TSC at ~ 200 ° C with Tmax ~ 330 ° C, the theoretical is 25 kJ, the gain is of 1.52 times.

| KH 8.3 gm +, Mg 5.0 gm + CAII-300 20.0 gm + ZnBr2_11.25 gm, Ein: 302 kJ, dE: 42 kJ, Small TSC at ~ 200 ° C with Tmax ~ 375 ° C. Energy gain ~ 2X (X-20.9 kJ).

| KH 8.30 gm + Mg 5.0 gm + TiC 20.0 gm + GdBr3 19. 85 gm, Ein: 308 kJ, dE: 26 kJ, TSC at ~250 ° C with Tmax ~ 340 ° C. Energy gain -1.3X (X-20.3 kJ).

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + MnS 4.35 gm, Ein: 349 kJ, dE: 24 kJ, TSC at ~ 260 ° C with Tmax ~ 350 ° C. Energy gain ~ 3.6 X (X-6.6 kJ). | 4g CAIII-300 + lg of Mg + lg of NaH + .3.79g LaBr3, Ein: 143.0 kJ, dE: 4.8 kJ, TSC: none, Tmax: 392 ° C, the theoretical is 2.46 kJ, the gain is 1.96 times | 4g CAIII-300 + lg of Mg + 1.66 g of KH + 3.80 g CeBr3, Ein: 145.0 kJ, dE: 7.6 kJ, TSC: none, Tmax: 413 ° C, the theoretical is 3.84 kJ, the gain is 1.97 times 4g CAIII-300 + lg Mg + 1.66 g KH + 1.44g AgCl; Ein: 136.2 kJ; dE: 7.14 kJ; TSC: not observed; Tmax: 420 ° C, the theoretical is 2.90 kJ, the gain is 2.46 times. | 4g CAIII-300 + lg of Mg + 1.66 g of KH + 1.60 g Cu2S, Ein: 137.0 kJ, dE: 5.5 kJ, TSC: none, Tmax: 405 ° C, the theoretical is 2.67 kJ, the gain is 2.06 times. 2.54 g of Tel4 (0.01 mol Tel4 is 6.35 g, but not enough Tel4), 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (AC3-1), the gain of energy was 8.3 kJ, and the burst temperature of the cell was 113 ° C (202 - 315 ° C). The maximum temperature of the cell was 395 ° C, the theoretical temperature is 5.61 kJ, the gain is 1. 48 times 2.51 g of BBr3, 1.66 g of KH, lg of Mg powder and 4 g of · activated carbon powder CA-III.300 (AC3-1), the energy gain was 12.4 kJ. The change of the temperature slope of the. cell was 52 ° C (77 - 129 ° C) (and the burst temperature of the cell was 88 ° C (245 - 333 ° C) .The maximum temperature of the cell was 438 ° C, the theoretical of 9.28 kJ, the gain is 1.34 times. | 4g CAIII-300 + lg Mg + 1.0 g NaH + 3.59g TaCl-5, Ein: 102.0 kJ, dE: 16.9 kJ, TSC: 80-293 ° C, Tmax: 366 ° C, the theoretical is 11.89 kJ , the gain is 1.42 times. 2.72 g of CdBr2, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 6.6 kJ, and the burst temperature of the cell was 56 ° C (253 - 309 ° C). The maximum temperature of the cell was 414 ° C, the theoretical temperature is 4.31 kJ, the gain is 1.53 times. . 2.73 g of MoC15, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 20.1 kJ, and the bursting temperature of the cell was 240 ° C (67 - 307 ° C). The maximum temperature of the cell was 511 ° C, the theoretical temperature is 15.04 kJ, the gain is 1.34 times. 2.75 g of InBr2, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 7.3 kJ, but no burst of cell temperature. The maximum temperature of the cell was 481 ° C, the theoretical temperature is 4.46 kJ, the gain is 1.64 times. 1.88 g of bF5, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 15.5 kJ, but no burst of cell temperature. The maximum temperature of the cell was 448 ° C, the theoretical temperature is 11.36 kJ, the gain is 1.36 times. 2.33 g of ZrC14, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 12.9 kJ, and the bursting temperature of the cell was 156 ° C (311 - 467 ° C). The maximum temperature of the cell was 472 ° C, -the theoretical temperature is 8.82 kJ, the gain is 1.46 times. 3.66 g of Cdl2, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 6.7 kJ, and the change in Cell temperature slope was .74 ° C (125 - 199 ° C). The maximum temperature of the cell was 417 ° C, the theoretical temperature is 4.12 kJ, the gain is 1.62 times. 4g CAIII-300 + lg Mg + 1.66 g KH + 2.64g GdCl3; Ein: 127.0 kJ; dE: 4.82 kJ; TSC: not observed; Tmax: 395 ° C, the theoretical is 3.54 kJ, the gain is 1.36 times.

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + InCl 7.5 gm, Ein: 305 kJ, dE: 32 kJ, Small TSC at ~ 150 ° C with Tmax ~ 350 ° C. Energy gain ~ 2.8X (X-11.5 kJ).

| KH 8.3 gm + Mg 5.0 gm + WC 20.0 gm + Col2 .15.65 gm, Ein: 306 kJ, dE: 41 kJ, - Small TSC at ~ 20 ° C with Tmax ~ 350 ° C. Energy gain -1.55 X (X-26.4 kJ).

| NaH 5.0 gm + Mg 5.0 gm + WC 20.0 gm + GdBr3 19.85 gm, Ein: 309 kJ, dE: 28 kJ, Small TSC at ~ 250 ° C with Tmax ~ 340 ° C. Energy gain ~ 1.8X (X-15.6 kJ). . '- | KH_4.98 gm + Mg_ 3.0 gm + CAII-300_12.0 gm + InBr_5.85 gm 3X system, Ein: 297 kJ, dE: 13 kJ, small TSC at ~ 200 ° C with Tmax ~ 33O ° C. Energy gain -1.3X (X ~ 10 kJ). | 4g CAIII-300 + lg of Mg + Ig of NaH + 2.26g Y203, Ein: 133.1 kJ, dE: 5.2 kJ, TSC: none, Tmax: 384 ° C, the theoretical is of i.18 kJ, the gain is 4.44 times 4.11 g of ZrBr4, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 11.2 kJ, and the bursting temperature of the cell was 154 ° C (280-434 ° C). The maximum temperature of the cell was 444 ° C, the theoretical temperature is 9.31 kJ, the gain is 1.2 times. 5.99 g of ?? 4, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 11.3 kJ, and the bursting temperature of the cell was 200 ° C (214 - 414 ° C). The maximum temperature of the cell was 454 ° C, the theoretical temperature is 9.4 kJ, the gain is 1.2 times. 2.70 g of bCl5, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 16.4 kJ,, and the temperature of burst of the cell was 213 ° C (137 - 350 ° C). The maximum temperature of the cell was 395 ° C, the theoretical temperature is 13.40 kJ, the gain is 1.22 times. 2.02 g of MoCl3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 12.1 kJ, but no burst of cell temperature. The maximum temperature of the cell was 536 ° C, the theoretical temperature is 8.48 kJ, the gain is 1.43 times. 3.13 g of Nil2, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 8.0 kJ, and the bursting temperature of the cell was 33 ° C (335-368 ° C). The maximum temperature of the cell was 438 ° C, the theoretical temperature is 5.89 kJ, the gain is 1.36 times. 3.87 g of As2Se3, '1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 12.3 kJ, and the temperature of Burst of the cell was 241 ° C (195 - 436 ° C). The maximum temperature of the cell was 446 ° C, the theoretical temperature is 8.4 kJ, the gain is 1.46 times. 2.74 g of Y2S3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 5.2 kJ, but no burst of cell temperature. The maximum temperature of the cell was 444 ° C, the theoretical temperature is 0.41 kJ, the gain is 12.64 times. | 4g CAIII-300 + lg of Mg + 1.66 g of KH + 3.79g LaBr3, Ein: 147.1 kJ, dE: 7.1 kJ, TSC: none, Tmax: 443 ° C, the theoretical is 3.39 kJ, the gain is 2 times 4g CAIII-300 + lg Mg + 1.66 g KH + 2.15g MnBr2; Ein: 124.0 kJ; dE: 5.55 kJ; TSC: 360-405 ° C; Tmax: 411 ° C, the theoretical is 3.63 kJ, the gain is 1.53 times. 2.60 g of Bi (OH) 3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (drying at 30.0 ° C), the energy gain was 14.8 kJ, and the burst temperature of the cell was 173 ° C (202-375 ° C). The maximum temperature of the cell was 452 ° C, the theoretical temperature is 12.23 kJ, the gain is 1.2 times.

| KH 8.3 gm + Mg 5.0 gm + Tick 20.0 gm + Snl2 18.5 gm Strem, Ein: 244 kJ, dE: 53 kJ, TSC at ~ 150 ° C with Tmax ~ 330 ° C, the theoretical is 28.1 kJ, the gain It is 1.9 times.

| KH 8.3 gm + Mg 5.0 gm + TiC 20.0 gm + FeBr2 10.8 gm, Ein: 335 kJ, dE: 43 kJ, TSC at ~ 250 ° C with Tmax ~ 375 ° C, the theoretical is 22 kJ, the gain is of 1.95 times.

| KH 8.3 gm + Mg 5r0 gm + WC 20.0 gm + FeBr2 10.8 gm, Ein: 335 kJ, dE: 32 kJ, TSC at ~ 230 ° C with Tmax ~ 360 ° C, the theoretical is 22 kJ, the gain is of 1.45 times.

| KH 8.3 gm + Mg 5.0 gm + TiC 20.0 gm + Mnl2 15.45 gm Strem, Ein: 269 kJ, dE: 49 kJ, Small TSC at ~ 50 ° C with Tmax ~ 350 ° C. Energy gain -3.4X (X ~ 14.8kJ). 4g CAIII-300 + 1.66 g of Ca + lg of NaH + 3.09g Mnl2; Ein: 112.0 kJ; dE: 9.98 kJ; TSC: 178-374 ° C; Tmax: 383 ° C, the theoretical is 5.90 kJ, the gain is 1.69 times. | 0.96 g of CuS, "1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 5.5 kJ, but it was not observed No explosion of temperature of the cell.The maximum temperature of the cell was 409 ° C, the theoretical temperature is 2.93 kJ, the gain is 1.88 times. | 0.87 g of MnS, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 4.7 kJ, but no burst of cell temperature. The maximum temperature of the cell was -412 ° C, the theoretical is 1.32 kJ, the gain is 3.57 times.

| KH 8.3 p + Mg 5.0 p + TiC 20.0 gm + Mnl2 15.45 gm, Ein: 269 kJ, dE: 49 kJ, Small TSC at ~ 50 ° C with Tmax ~ 350 ° C, the theoretical is 18.65 kJ, the gain It is 2.6 times.

| NaH 5.0 gm + Mg 5.0 p + .TiC 20.0 gm + NiBr2 11.0 gm, Ein: 245 kJ, dE: 43 kJ, TSC at ~ 200 ° C with Tmax ~ 310 ° C, the theoretical is 26 kJ, the gain It is 1.6 times.

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + MnCl2 6.3 gm, Ein: 333 kJ, dE: 34 kJ, TSC at ~ 250 ° C with Tmax ~ 340 ° C, the theoretical is 17.6 kJ, the gain is 2 times. 2r42 g of Inl, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 4.4 kJ, but no burst of cell temperature. The maximum temperature of the cell was 438 ° C, the theoretical temperature is 1.92 kJ, the gain is 2.3 times. 1.72 g of InF3, 1.66 g of H, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 9.2 kJ, but no burst of temperature of. the cell. The maximum temperature of the cell was 446 ° C, the theoretical temperature is 5 kJ, the gain is 1.85 times. | 4g CAIII-300 + lg Mg + lg NaH + 1.98g As203, Ein: 110.5kJ, dE: 17.1kJ, TSC: 325-452 ° C, Tmax: 471 ° C, the theoretical is 11.48 kJ, the gain is 1.49 times. | 4g CAIII-300 + lg of Mg + lg of NaH + 4.66g BÍ203, Ein: 152.0 kJ, dE: 17.7 kJ, TSC: 185-403 ° C, Tmax: 481 ° C, the theoretical is 13.8 kJ, the Gain is 1.28 times. 4g CAIII-300 + lg Mg + lg NaH + 2.02g MoC13; Ein: 118.0 kJ; dE: 11.10 kJ; TSC: 342-496 ° C; Tmax: 496 ° C, the theoretical is 7.76, the gain is 1.43 times. 2.83 g of PbF4, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 13.9 kJ, and the bursting temperature of the cell. it was 245 ° C (217 - 462 ° C). The maximum temperature of the cell was 464 C, the theoretical temperature is 13.38 kJ, the gain is 1.32 times. 2.78 g of PbC12, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 C), the energy gain was 6.8 kJ, but no burst was observed of cell temperature. The maximum temperature of the cell was 488 ° C, the theoretical temperature is 5.22 kJ, the gain is 1.3 times. | 4g CAIII-300 + 1.66 g of KH + 2.19g NiBr2, Ein: 136.0 kJ, dE: 7.5 kJ, TSC: 275-350 ° C, Tmax: 385 ° C, the theoretical is 4.6 kJ, the gain is 1.6 times 4g CAIII-300 + lg of Mg + lg of NaH + 2.74g, MoC15, Ein: 96.0 kJ, dE: 19.0 kJ, TSC: 86-334C, Tmax: 373 ° C, the theoretical is 14.06 kJ, the gain is 1.35 times. 4g CAIII-300 + 1.66 g of Ca + lg of NaH + 2.19g NiBr2; Ein: 127.1 kJ; dE: 10.69 kJ; TSC: 300-420 ° C; Tmax: 10.69 ° C, the theoretical is 7.67 kJ, the gain is 1.39 times. 5.90 g of Bil3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 10.9 kJ, and the change in slope of cell temperature was 70 ° C. (217 - 287 ° C). The maximum temperature of the cell was 458 ° C, the theoretical temperature is 8.87 kJ, the gain is 1.23 times. 1.79 g of SbF3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 C), the energy gain was 11.7 kJ, and the burst temperature of the cell was 169 ° C (138 - 307 ° C). The maximum temperature of the cell was 454 ° C, the theoretical temperature is 9.21 kJ, the gain is 1.27 times. | 4g CAIII-300 + 1.66 g of Ca + lg of NaH + 3.09g Mnl2, Ein: 111.0 kJ, dE: 12.6 kJ, TSC: 178-340 ° C, Tmax: 373 ° C, the theoretical is 5.9 kJ, the gain is 2.13 times. 4g CAIII-300 + 1.66 g of Ca + lg of NaH + 1.34g CuCl2; Ein: 135.2 kJ; dE: 12.26 kJ; TSC: 250-390 ° C; Tmax: 437 ° C, the theoretical is 8.55 kJ, the gain is 1.43 times. 1.50 g of InCl, 1.66 g of KH, lg of Mg powder and 4 g 'of activated carbon powder CA-III 300 (dried at 300 C), the energy gain was 5.1 kJ, but no burst of cell temperature: The maximum temperature of the cell was 410 ° C, the theoretical temperature is 2.29 kJ, the gain is 2.22 times. 2.21 g of lnCl3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 C), the energy gain was 10.9 kJ and the burst temperature of the cell was 191 ° C (235-426 ° C). The maximum temperature of the cell was 431 ° C, the theoretical temperature is 7.11 kJ, the gain is 1.5 times. 1.95 g of InBr, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 6.0 kJ, but no burst of cell temperature. The maximum temperature of the cell was 435 ° C, the theoretical temperature is 2 kJ, the gain is 3 times. | 3.55 g of InBr3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 9.1 kJ, and the bursting temperature of the cell was 152 ° C '(156 - 308 ° C). The maximum temperature of the cell was 386 ° C, the theoretical temperature is 6.92 kJ, the gain is 1.3 times. | 4g CAIII-300 + 1.66 g of KH + 3.79g Snl2, Ein: 169.1 kJ, dE: 6.0 kJ, TSC: 200-289 ° C, Tmax: 431 ° C, the theoretical is 4.03 kJ, the gain is 1.49 times.

| KH 8.3 gm + Mg 5.0 gm + WC 20.0 gm + MnBr2 10.75 gm, Ein: 309 kJ, dE: 35 kJ, Without TSC with Tmax ~ 335 ° C. Energy gain ~ 1.9X (X-18.1 kJ).

| KH 8.3 p + Mg 5.0 p + CAII-300 20.0 gm + MnBr2 10. 75 gm, Ein: 280 kJ, dE: 41 kJ, TSC at ~ 28 ° C with Tmax ~ 35 ° C. Energy gain ~ 2.2 X (X-18.1 kJ).

| KH 1.66 gm + Mg 1.0 gm + TiC .0 gm + TiF3 1.05 gm 5X Cell # 1086 with CAII-300, Ein: 143 kJ, dE: 6 kJ, Without TSC with Tmax ~ 280 ° C, the theoretical is 2.5 kJ, the gain is 2.4 times.

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + FeF2 4.7 gm, Ein: 280 kJ, dE: 40 kJ, TSC at ~ 260 ° C with Tmax ~ 340 ° C, the theoretical is 20.65 kJ, the gain is 1.93 times.

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0-gm + CuF2 5.1 gm, Ein: 203 kJ, dE: 57 kJ, TSC at -125C with Tmax ~ 28 ° C, the theoretical is 29 kJ, the gain It is 1.96 times.

| KH 83.0 gm + Mg 50.0 gm + WC 200.0 gm + Snl2 185 gm URS, Ein: 1310 kJ, dE: 428 kJ, TSC at ~ 140 ° C with Tmax ~ 350 ° C, the theoretical is 200 kJ, the gain It is 2.14 times. | 061009KAWFCl # 1102 NaH 1.0 gm + Mg 1.0 gm + WC 4.0 gm + GdBr3_3.97gm, Ein: 148 kJ, dE: 7 kJ, Small TSC at ~ 300 ° C with Tmax ~ 420 ° C. Energy gain ~ 3.5 X (X-2 kJ).

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + FeO 3.6 gm, Ein: 355 kJ, dE: 24 kJ, Small TSC at ~ 260 ° C with Tmax ~ 360 ° C. Energy gain -1.45 X (X-16.6 kJ).

| KH 83.0 gm + Mg 50.0 gm + WC 200.0 gm + Snl2 185 gm ROWAN, Ein: 1379 kJ, dE: 416 kJ, TSC - ~ 14 ° C with Tmax ~ 350 ° C, -the theoretical is 200 kJ, the gain is 2 times.

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + Col2 15. 65 gm, Ein: 361 kJ, dE: 69 kJ, TSC at ~ 200 ° C with Tmax ~ 410 ° C, the theoretical is 26.35 kJ, the gain is 2.6 times.

| KH 8.3 gm + 5.0 gm + CAII 300 20.0 gm + FeS 4.4 gm, Ein: 312 kJ, dE: 22 kJ, Without TSC with Tmax ~ 350 ° C. Energy gain -1.7 X (X-12.3 kJ).

| KH 8.3 gm + WC 40.0 gm + Snl2 18.5 gm, Ein: 315 kJ, dE: 27 kJ, Small TSC at ~ 140 ° C with Tmax ~ 340 ° C. Energy gain -1.35 X (X-20 kJ).

| NaH 5.0 gm + Mg 5.0 gm + .WC 20.0 gm + Mnl2 15.45 gm, Ein: 108 kJ, dE: 30 kJ, TSC at ~ 70 ° C with Tmax ~ 170 ° C, the theoretical is 14.8 kJ, the gain is of 2 times.

| NaH 5.0 gm + Mg 5.0 gm + WC 20.0 gm + NiBr2 11.0 gm, Ein: 248 kJ, dE: 34 kJ, TSC at ~ 170 ° C with Tmax ~ 300 ° C. Energy gain -1.7 X (X ~ 20 kJ), the theoretical is -26.25 kJ, the gain is 1.3 times.

| KH 8.3 gm + Mg 5.0 gm + WC 20.0 gm + NiBr2 11.0 gm, Ein: 291 kJ, dE: 30 kJ, Small TSC at ~ 250 ° C with Tmax ~ 340 ° C. Energy gain -1.5 X (X-20 kJ), the theoretical is 26.25 kJ, the gain is 1.14 times.

| NaH 5.0 gm + Mg 5.0 gm + WC 20.0 gm + NiBr2 11.0 gm Repetition of Cell # 1105, Ein: 242 kJ, dE: 33 kJ, TSC at ~ 70 ° C with Tmax ~ 280 ° C. Energy gain -1.65 X (X-20 kJ).

| NaH 5.0 gm + Mg 5.0 gm + CAII-300 20.0 gm + InC13 11..1 gm, Ein: 189 kJ, 'dE: 48 kJ, small TSC at ~80 ° C with Tmax ~ 260 ° C. Energy gain -1.5X (X-31 kJ).

'KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + Mnl2 15.45 gm, Ein: 248 kJ, dE: 46 kJ, Small TSC at ~ 200 ° C with Tmax ~ 325 ° C. Power gain -3 X (X-14.8 kJ). 2.96 g of FeBr3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 12.5 kJ, and the bursting temperature of the cell was 77 ° C (72-149 ° C). The maximum temperature of the cell was 418 ° C, the theoretical temperature is 8.35 kJ, the gain is 1.5 times | 0.72 g of FeO, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 6.7 kJ, but no burst of cell temperature. The maximum temperature of the cell -was 448 ° C, the theoretical temperature is 3.3 kJ, the gain is 2 times. 1.26 g of MnCl2, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 8.6 kJ, but no burst of cell temperature. -The maximum temperature of the cell was 437 ° C, the theoretical temperature is 3.52 kJ, the gain is 2.45 times. 1.13 g of FeF3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 12.6 kJ, but no burst of cell temperature. The maximum temperature of the cell was 618 ° C, the theoretical temperature is 6.44 kJ, the energy gain is 1.96 times. | 4g CAIII-300 + lg of Mg + lg of NaH + 3.97g GdBr3, Ein: 143.1 kJ, dE: 5.4 kJ, TSC: none, Tmax: 403 ° C, the theoretical is 1.99 kJ, the gain is 2.73 times . 4g CAIII-300 + lg Mg + lg NaH + 1.57g SnF2; Ein: 139.0 kJ; dE: 7.24 kJ; TSC: not observed; Tmax: 413 ° C, the theoretical is 5.28 kJ, the gain is 1.37 times. | 4g CAIII-300 + lg Mg + lg NaH + 4.04g Sb2S5, Ein: 125.0 kJ, dE: 19.3 kJ, TSC: 421-651C, Tmax: 651C, the theoretical is 12.37 kJ, the gain is 1.56 times. 1.36 g of ZnC12, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 6.6 kJ, but no burst of cell temperature. The maximum temperature of the cell was 402 ° C, the theoretical temperature is 4.34 kJ, the gain is 1.52 times. 1.03 g of ZnF2, 1.66 g of KH, lg. of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 6.5 kJ, but no burst of cell temperature was observed. The maximum temperature of the cell was 427 ° C, the theoretical temperature is 3.76 kJ, the gain is 1.73 times. 4g CAIII-300 + lg Mg + lg NaH + 2.22g InCl3, dE Experimental: -12.6 kJ Considered reaction: InCl3 (c) + 3NaH (c) + 1.5Mg (c) = 3NaCl (c) + In (c) + 1.5MgH2 (c) Q = -640.45 kJ / theoretical chemical reaction energy: -6.4 kJ, excess heat: -6.2 kJ, 2.0X excess heat. | 1.08 g of VF3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 9.5 kJ, but no burst of cell temperature. The maximum temperature of the cell was 447 ° C, the theoretical temperature is 4.9 kJ, the gain is 1.94 times. '8.3 g of KH + 5.0 g of Mg + 20.0 g activated carbon (11-300) + 5.4 g VF3, Ein: 286 kJ, dE: 58 kJ, the theoretical is 24.5 kJ, the gain is 2.3 times. 4g CAIII-300 + lg of Mg + lg of NaH + 1.72g InF3, Ein: 134.0 kJ, dE: 8.1 kJ, TSC: none, Tmax: 391C, the theoretical is 5 kJ, the gain is 1.62 times. | 4g CAIII-300 + lg of Mg + 1.66 g of KH + 1.02g CuF2, dE Experimental: -9.4 kJ Reaction considered: CuF2 (c) + Mg (c) = MgF2 (c) + Cu (c) Q = - 581.5 kJ / theoretical chemical reaction energy: -5.82 kJ, excess heat: -3.59 kJ, 1.6X excess heat. | 4g CAIII-300 + lg Mg + lg NaH + 2.83g PbF4, dE Experimental: -17.6 kJ Reaction considered: PbF4 (c) + 2Mg (c) + 4NaH (c) = 2MgH2 (c) + 4NaF (c ) + Pb (c) Q = -1290.0 kJ / theoretical chemical reaction energy: -12.9 kJ, -Overall value: -4.7 kJ 1.4X excess heat.

| KH 1.66 gm + Mg 1.0 gm + Tick 4.0 gm + Snl4 6.26gm, Ein: 97 kJ, dE: 17 kJ, TSC at ~ 150 ° C with Tmax ~ 370 ° C, the theoretical is 10.1 kJ, the gain is 1.7 times | 4g CAIII-300 + lg of Mg + 1.66 g of KH + 3.7g TiBr4, dE Experimental: -16.1 kJ Reaction considered: TiBr4 (c) + 4KH (c) + 2Mg (c) + C (s) = 4KBr (c) + TiC (c) + 2MgH2 (c) Q = -1062.3 kJ / theoretical chemical reaction energy: -10.7 kJ, excess heat: -5.4 kJ 1.5X excess heat.

BI3 | 4g CAIII-300 + lg of Mg + lg of NaH + 2.4g BI3, Ein: 128.1 kJ, dE: 7.9 kj, TSC: 180-263C, Tmax: 365 ° C, the theoretical is 5.55 kJ, the gain is 1.4 times MnBr2 | 4g CAIII-300 + lg of Mg + 1.66 g of KH + 2.15g MnBr2, dE Experimental: -7.0 kJ Reaction considered: MnBr2 (c) + 2KH (c) + Mg (c) = 2KBr (c) + Mn ( c) + gH2 (c) Q = - 362.6 kJ / theoretical chemical reaction energy: -3.63 kJ, excess heat: -3.4 kJ 1.9X excess heat.

| KH 8.3 gm + Mg 5.0 p + CAII-300 20.0 gm + MnBr2 10. 75 gm, Ein: 280 kJ, dE: 41 kJ, TSC at ~ 280 ° C with Tmax ~ 350 ° C. Energy gain ~ 2.2 X (X-18.1 kJ).

FeF2 | 4g CAIII-300 + lg of Mg + 1.66 g of KH + 0.94g FeF2, dE Experimental: -9.8 kj Reaction considered: FeF2 (c) + Mg (c) = MgF2 (c) + Fe (c) Q = -412.9 kJ / theoretical chemical reaction energy: -4.13 kJ, excess heat: -5.67 kJ, 2.4X excess heat.

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + FeF2 4.7 gm, Ein: 280 kJ, dE: 40 kJ, TSC at ~ 260 ° C with Tmax ~ 340 ° C, the theoretical is 20.65 kJ, the Gain is 1.94 times.

TIFF3 | H 1.66 gm + Mg 1.0 gm + TiC 4.0 gm + TiF3 1.05 gm (5X Cell # 1086 with CAII-300), Ein: 143 kJ, dE: 6 kJ, Without TSC with Tmax ~ 280 ° C, the theoretical is 2.5, the gain is 2.4 times.

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + TiF3 5.25 gm, Ein: 268 kJ, dE: 7 kJ, Without TSC with Tmax ~ 280 ° C. Without energy gain (X-21.7 kJ).

CuF2 | KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + CuF2 5.1 gm, Ein: 203 kJ, dE: 57 kJ, TSC at -125C with Tmax ~ 280 ° C, the theoretical is 29.1 kJ, the gain is 2 times nl2 | NaH .4.0 gm + Mg 4.0 gm + CAII-300 16.0 gm + Mnl2 12.36 gm (scaled up 4x up), Ein: 253 kJ, dE: 30 kJ, Without TSC with Tmax ~ 300 ° C, the theoretical is 11.8 kJ, the gain is 2.5 times.

The heat measurement with 3.09 g of Mnl2, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 8.8 kJ, and the burst temperature of the cell was 92 ° C (172-264 ° C). The maximum temperature of the cell was 410 ° C, the theoretical temperature is 2.96 kJ, the gain is 3 times. | 4g CAIII-300 + lg Mg + lg NaH + 3.09g Mnl2, Ein: 126.1 kJ, dE: 8.0 kJ, TSC: 157-241 ° C, Tmax: 385 ° C, the theoretical is 2.96 kJ, the Gain is 2.69 times.

ZnBr2 2.25 g of ZnBr2, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 10.3 kJ, and the bursting temperature of the cell was 82 ° C (253 - 335 ° C). The maximum temperature of the cell was 456 ° C, the theoretical temperature is 3.56 kJ, the gain is 2.9 times.

| NaH 5.0 gm + Mg 5.0 gm + CAII-300 20.0 gm + ZnBr2 11. 25 gm, Ein: 291 kJ, dE: 26 kJ, Without TSC with Tmax ~ 330 ° C, the theoretical is 17.8 kJ, the gain is 1.46 times.

COC12 1.3 g of CoC12, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 10.4 kJ, and the change of the temperature gradient of the cell was 105 ° C (316 - 421 ° C). The maximum temperature of the cell was 450PC, theoretical is -of 5.2 kJ, the gain is 2 times. . | 1.3 g of CoCl2, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 9.6 kJ, and the bursting temperature of the cell was 181 ° C (295 - 476 ° C). The maximum temperature of the cell was 478 ° C, the theoretical temperature is 5.2 kJ, the gain is 1.89 times.

SnBr2 2.8 g of SnBr2, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder 'CA-III 300 (dried at 300 ° C), the energy gain was 14.2 kJ, and the temperature of burst was 148 ° C (148 - 296 ° C). The maximum temperature of the cell was 376 ° C, the theoretical temperature is 3.75 kJ, the gain is 3.78 times. | 4g CAIII-300 + lg of Mg + lg of NaH + 2.79g SnBr2, Ein: 116.0 kJ, dE: 7.7 kJ, TSC: 135-236 ° C, Tmax: 370 ° C, the theoretical is 3.75 kJ, the gain is 2 times.

| KH 8.3 gm + 'Mg powder 5.0 gm + CAII 300 20.0 -gm + SnBr2 11.4 gm, Ein: 211 kJ, dE: 41 kJ, TSC at ~ 17 ° C with Tmax ~ 30 ° C; the theoretical is 15.5 kJ, the gain is 2.6 times.

| KH 8.3 gm + Mg 5.0 gm + TiC 20.0 gm + SnBr2 14.0 gm, Ein: 229 kJ, dE: 46 kJ, TSC at ~ 150 ° C with Tmax ~ 310 ° C and Gain -2.4X (X-19 kJ) , the theoretical is 18.8 kJ, the gain is 2.4 times.

| KH 1.66 gm + Mg 1.0 gm + WC 4.0 gm + SnBr2 2.8 gm, Ein: 101 kJ, dE: 10 kJ, TSC at ~ 150 ° C with Tmax ~ 350 ° C, the theoretical is 3.75 kJ, the gain is 2.66 times | 4g CAIII-300 + 1.66 g of KH + 2.79g SnBr2, Ein: 132.0 kJ, dE: 9.6 kJ, TSC: 168-263, Tmax: 381 ° C, the theoretical is 4.29 kJ, the gain is 2.25 times.

Lg of Mg + 1.66 g of KH + 2.79g SnBr2; Ein: 123.0 kJ; dE: 7.82 kJ; TSC: 125-22 ° C; Tmax: 386 ° C, the theoretical is 5.85 kJ, the gain is 1.33 times.

Snl2 | KH 6.64gm + Mg powder 4.0 gm + TiC 18.0 gm + Snl2 14.8 gm, Ein: 232 kJ, dE: 47 kJ, TSC at ~ 150 ° C with Tmax ~ 280 ° C. Gain, energy ~ 3.6X (X-12.8 kJ), the theoretical is 12.6 kJ, the gain is 3.7 times. | 3.7 g of Snl2, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 11.9 kJ, but no explosion was observed Of temperature. The maximum temperature of the cell was 455 ° C, the theoretical temperature is 3.2 kJ, the gain is 3.7 times.

| KH 1.6 gm + Mg Powder 1.0 gm + Tic 4.0 gm + SnI2 3. 7 gm, Ein: 162 kJ, dE: 13 kJ; TSC at 100 ° C with Tmax ~ 490 ° C; the theoretical is 3.2 kJ, the gain is 4 times.

- | KH 8.3 gm + Mg Powder 5.0 gm + CAII 300 20.0 gm + Snl2 18.5 gm, Ein: 221 kJ, dE: 47 kJ, TSC at ~ 170 ° C with Tmax ~ 300 ° C, the theoretical is 15.9 kJ , the gain is 3 times. 4g CAIII-300 + lg of Mg + lg of NaH + 3.73g Snl2; Ein: 121.9 kJ; dE: 7.56 kJ; TSC: observed nq; Tmax: 391 ° C, the theoretical is 3.2 kJ, the gain is 2-36 times. 1.66 g of KH + 3.79g Snl2, Ein: 114.0 kJ, dE: 8.8 kJ, TSC: 161-259C, Tmax: 359 ° C, the theoretical is 4 kJ, the gain is 2.17 times.

SnCl2 | NaH 5.0 gm + g 5.0 gm + CAII-300 20.0 gm + SnC12 9.6 gm, Ein: 181 kJ ,. dE: 30 kJ, TSC at ~ 140 ° C with Tmax ~ 280 ° C, the theoretical is 19 kJ, the gain is 1.57 times.

NiBr2 4g CAIII-300 + lg of Mg + lg of NaH + 2.19g NiBr2; Ein: 126.0 kJ; dE: 12.01 kJ; TSC: 290-370 ° C; Tmax: 417 ° C, the theoretical is 4 kJ, the gain is 3 times.

| NaH 1.0 gm + MgH2 powder 1.0 gm + TiC 4.0 gm) Mixture + NiBr2_2.2 gm, Ein: 121 kJ, dE: 11 kJ, temperature slope jump at 260 ° C with Tmax ~ 390 ° C, the theoretical is 4 kJ, the gain is 2.75 times. 4g CAIII-300 + lg Al + lg of NaH + 2.19g NiBr2; Ein: 122.0 kJ; dE: 7.78 kJ; TSC: not observed; Tmax: 392 ° C, the theoretical is 4 kJ, the gain is 1.95 times. 4g CAIII-300 + lg Mg + 0.33g LiH + 2.19g NiBr2; Ein: .128.0 kJ; dE: 10.72 kJ; TSC: 270-436 ° C; Tmax: '440 ° C, the theoretical is 4 kJ, the gain is 2.68 times 4g CAIII-300 + lg Mg + 1.66 g KH + 2.19g NiBr2; Ein: 126.0 kJ; dE: 10.45 kJ; TSC: 285-423 ° C; Tmax: 423 ° C, the theoretical is 4 kJ, the gain is 2.6 times. | 4g CAIII-300 + lg of gH2 + lg of NaH + 2.19g NiBr2; Ein: 138.1 kJ; dE: 8.12 kJ; TSC: not observed; Tmax: 425 ° C, the theoretical is 4 kJ, the gain is 2 times.

| NaH 5.0 gm + Mg powder 5.0 gm + Activated carbon CAII 300 20.0 gm) Mixture + NiBr2 11.0 gm (Theoretical 23.6 kJ),, Ein: 224 kJ, dE: 53 kJ, slope of temperature at 16 ° C with Tmax ~ 280 ° C, the theoretical is 20 kJ, the gain is 2.65 times.

| NaH 1.0 gm + Mg 1.0 gm + WC 4.0 gm + NiBr2 2.2gm, Ein: 197 kJ, dE: 11 kJ, Small TSC at ~ 200 ° C with Tmax ~ 500 ° C; the theoretical is 4 kJ, the gain is 2.75 times.

| NaH 50.0 gm + Mg 50.0 gm + CAII-300 200.0 gm + NiBr2 109.5 gm, Ein: 1990 kJ, dE: 577 kJ, TSC at ~ 14 ° C with Tmax ~ 980 ° C, the theoretical is 199 kJ, the gain is 2.9 times.

| Without Mg control: 4g CAIII-300 + lg of NaH + 2.19g NiBr2; Ein: 134.0 kJ; dE: 5.37 kJ; TSC: not observed, - Tmax: 375 ° C, the theoretical is 3.98 kJ, the gain is 1.35 · times.

Control: lg of Mg + lg of NaH + 2.19g NiBr2; Ein: 129.0 kJ; dE: 5.13 kJ; TSC: 195-310 ° C; Tmax: 416 ° C, the theoretical is 5.25 kJ.

Control: Ig NaH + 2.19g NiBr2; Ein: 138.2 kJ; dE: -0.18 kJ; TSC: not observed, - Tmax: 377 ° C, the theoretical is 3.98 kJ.

CuC12 4g CAIII-300 + lg Mg + lg NaH + 1.34g CuCl2, Ein: 119.0 kJ, dE: 10.5 kJ, TSC: 250-381C, Tmax: 393 ° C, the theoretical is 4.9 kJ, the gain is 2.15 times. | 4g CAIII-300 + lg of Al + lg of NaH + 1.34g CuC12, Ein: 126.0 kJ, dE: 7.4 kJ, TSC: 229-354 ° C, Tmax: 418 ° C, the theoretical is 4.9 kJ, the Gain is 1.5 times. | 4g CAIII-300 + lg of MgH2 + lg of NaH + 1.34g CuC12, Ein: 144.0 kJ, dE: 8.3 kJ, TSC: 229-314 ° C, Tmax: 409 ° C, the theoretical is 4.9 kJ, the Gain is 1.69 times.

|.NaH 5.0 gm + Mg powder 5.0 gm + Activated carbon CAII 300 20.0 gm) Mixture + CuC12 10.75gm (the theoretical is 45 kJ), Ein: 268 kJ, dE: 80 kJ, temperature slope jump to 21 ° C with Tmax ~ 360 ° C, the theoretical is 39 kJ, the gain is 2 times. 1.4 g of CuCl2, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-lli 300 (dried at 300 ° C) in a heavy-duty cell of 2.5 cm (1 inch), the Energy gain was 14.6 kJ, and the burst temperature was 190 ° C (188 - 378 ° C). The maximum temperature of the cell was 437 ° C, the theoretical temperature is 4.9 kJ, the gain is 3 times.

| KH 8.3 gm + Mg Powder 5.0 gm + CAII-300 20.0 gm + CuCl2 6.7 gm, Ein: 255 kJ, dE: 55 kJ, TSC at ~ 200 ° C with Tmax ~ 320 ° C, the theoretical is 24.5 kJ , the gain is 2.24 times CuCl 4g CAIII-300 + lg of Mg + lg of NaH + lg CuCl; Ein: 128. 1 kJ; dE: 4.94 kJ; TSC: not observed; Tmax: 395 ° C, the theoretical is 2.18 kJ, the gain is 2.26 times.

Col2 4g CAIII-300 + lg of Mg + lg of NaH + 3.13g Col2, Ein: 141.1 kJ, dE: 9.7 kJ, TSC: none, Tmax: 411 ° C Reaction considered: 2NaH (c) + Col2 (c) + Mg (c) = 2Nal (c) + Co (c) + MgH2 (c ) Q = -449.8 kJ / theoretical chemical reaction energy: -4.50 kJ, excess heat: -5.18 kJ, the gain is 1.9 times. 3.13 g of Col2, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 10.7 kJ, and the bursting temperature of the cell was 117 ° C (248-365 ° C). The maximum temperature of the cell was 438 ° C, the theoretical temperature is 5.27 kJ, the gain is 2.03 times.

Znl2 4g CAIII-300 + lg of Mg + lg of NaH + 3.19g Znl2,. Ein: 157.1 kJ, dE: 5.8 kJ, TSC: none, Tmax: 330 ° C Reaction considered: 2NaH (c) + Znl2 (c) + Mg (c) = 2Nal (c) + Zn (c) + MgH2 (c ) Q = -330.47 kJ / theoretical chemical reaction energy: - 3.30 kJ, Heat in excess: -2.50 kJ, the gain is 1.75 · times. 3.19 g of Znl2, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 5.9 kJ, and the change in The temperature gradient of the cell was 79 ° C (180 - 259 ° C). The maximum temperature of the cell was 423 ° C, the theoretical temperature is 4.29 kJ, the gain is 1.38 times.

NiF2 | 4g CAIII-300 + lg Mg + lg NaH + 0.97g NiF2, Ein: 135.0 kJ, dE: 7.9 kJ, TSC: 253-335 ° C, Tmax: 385 ° C Reaction considered: 2NaH (c) + NiF2 (cj + Mg (c) = 2NaF (c) + Ni (c) + - MgH2 (c) Q = -464.4 kJ / theoretical chemical reaction energy: - 4.64 kJ, excess heat: -3.24 kJ, the gain is 1.7 times. | 0.97 g of NiF2, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 8.7 kJ, and the change in Slope of cell temperature was 63 ° C (256 - 319 ° C). The maximum temperature of the cell was 410 ° C, the theoretical temperature is 5.25 kJ, the gain is 1.66 times.

CoBr2 4g CAIII-300 + lg Mg + lg NaH + 2.19g CoBr2, Ein: 140.0 kJ, dE: 7.6 kJ, TSC: none, Tmax: 461 ° C Reaction considered: 2NaH (c). + CoBr2 (c) + Mg (c) = 2NaBr (c) + Co (c) + MgH2 (c) Q = -464 kJ / theoretical chemical reaction energy: -4.64 kJ, excess heat: -2.9 kJ, the gain is 1.64 times. 2.19 g of CoBr2, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300. (dried at 300 ° C), the energy gain was 10.4 kJ, and the burst temperature of the cell was 110 ° C (306 - 416 ° C). Temperature . maximum of the cell was 450 ° C, the theoretical is 5.27 kJ, the gain is 1.97 times. 2.19 g of CoBr2, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 10.2 kJ, but no burst of cell temperature. The maximum temperature of the cell was 446 ° C, the theoretical temperature is 5.27 kJ, the gain is 1.94 times.

FeC12 | 4g CAIII-300 + lg Mg + lg NaH + 1.27g FeC12, Ein: 155.0 kJ, dE: 10.5 kJ, TSC: none, Tmax: 450 ° C, the theoretical is 3.68 kJ, the gain is 2.85 times. | 4g CAIII-300 + lg Al + lg of NaH + 1.27g FeC12, Ein: 141.7 kJ, dE: 7.0 kJ, TSC: none, Tmax: 440 ° C, the theoretical is 3.68 kJ, the gain is 1.9 times . 1.3 g of FeC12, - 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C) in a heavy-duty cell of 2.5 cm (1 inch), the energy gain was 11.5 kJ, and the burst temperature was 142 ° C (287 - 429 ° C). The maximum temperature of the cell was 448 ° C, the theoretical temperature is 4.1 kJ, the gain is 2.8 times.

| NaH_5.0 gm + Powder Mg_ 5.0 gm + Activated carbon CAII 300_20.0 gm) Mix + FeC12_6.35gm, Ein: 296 kJ, dE: 37 kJ, slope of temperature at 220 ° C with Tmax ~ 330 ° C , the theoretical is 18.4 kJ, the gain is 2 times.

FeC13 2.7 g of FeCl3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 21.3 kJ, and the bursting temperature of the cell was 205 ° C (147 - 352 ° C). The maximum temperature of the cell was 445 ° C, the theoretical temperature is 10.8 kJ, the gain is 1.97 times.

| NaH 1.0 gm + Mg Powder - 1.0 gm + Tic 4.0 gm + FeC13 1.6 gm, Ein: 88 kJ, dE: 14 kJ; TSC at 80 ° C with Tmax ~ 350 ° C, the theoretical is 6.65 kJ, the gain s of 2.1 times.

| KH 8.3 gm + MgH2 powder 5.0 gm + CAII 300 20.0 gm + FeCB 8.1 gm, Ein: 253 kJ, dE: 52 kJ /; Without TSC with Tmax ~ 300 ° C, the theoretical is 33 kJ, the gain is 1.56 times.

| KH 8.3 gm + Mg 5.0 gm + CAII-300 20.0 gm + FeC12 6.5 gm, Ein: 299 kJ, dE: 44 kJ, Without TSC with Tmax ~ 350 ° C, the theoretical is 18.9 kJ, the gain is 2.3 times.

FeBr2 4g CAIII-300 + lg Mg + 1.66 g KH + 2.16g FeBr2; Ein: 144.0 kJ; dE: 9.90 kJ; TSC: not observed; Tmax: 455 ° C, the theoretical is 3.6 kJ, the gain is 2.75 times. 4g CAIII-300 + lg of MgH2 + lg of NaH + 2.16g FeBr2; Ein: 142.0 kJ; dE: 8.81 kJ; TSC: not observed; Tmax: 428 ° C, the theoretical is 3.6 kJ, the gain is 2.44 times. | 4g CAIII-300 + lg of MgH2 + 0.33g LiH + 2.16g FeBr2; Ein: 164.0 kJ; dE: 8.68 kJ; TSC: not observed; Tmax: 450 ° C, the theoretical is 3.6 kJ, the gain is 2.4 times. 4g CAIII-300 + lg of MgH2 + 1.66 g of KH + 2.16g FeBr2; Ein: 159.8 kJ; dE: 9.07 kJ; TSC: not observed; Tmax: 459 ° C, the theoretical is 3.6 kJ, the gain is 2.5 times. | 4g CAIII-300 + lg Mg + lg NaH + 2.96g FeBr2, dE Experimental: -6.7 kJ Reaction considered: 2NaH (c) + FeBr2 (c) + g ('c) = 2NaBr (c) + Fe ( c) + MgH2 (c) Q = -435.1 kJ / theoretical chemical reaction energy: -4.35 kJ, excess heat: -2.35 kJ, 1.54X excess heat.

NIC12 | 4g CAIII-300 + lg of Mg + lg of NaH + 1.30g NIC12, Ein: 112.0 kJ, dE: 9.7 kJ, TSC: 230-368 ° C, Tmax: 376 ° C, the theoretical is 4 kJ, the Gain is 2.4 times. 1.3 g of NIC12, 0.33 g of LiH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C) in a heavy-duty cell of 2.5 cm (1 inch), the Energy gain was 9.2 kJ, and the change of the. Temperature slope was 100 ° C (205 - 305 ° C). The maximum temperature of the cell was 432 ° C, the theoretical temperature is 4 kJ, the gain is 2.3 times. 1.3 g of NIC12, 0.33 g of LiH, lg of Al powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C) in a heavy duty 2.5 cm (1 inch) cell, the Energy gain was 8.0 kJ, and the change in temperature slope was 85 ° C (206 - 291 ° C). The maximum temperature of the cell was 447 ° C, the theoretical temperature is 4 kJ, the gain is 2 times.

CuBr 4g CAIII-300 + lg Mg + lg NaH + 1.44g CuBr; Ein: 125.0 kJ; dE: 4.67 kJ; TSC: not observed; Tmax: 382 ° C, the theoretical is 2 kJ, the gain is 2.33 times. | 4g CAIII-300 + lg of 'Mg + 1.66 g of KH + 1.44g CuBr, of Experimental: -7.6 kJ Reaction. considered: CuBr (c) + KH (c) + 0.5Mg (c) = KBr (c) + Cu (c) + 0.5 MgH2 (c) Q = -269.2 kJ / theoretical chemical reaction energy: -2.70 kJ, Heat in excess: -4.90 kJ 2.8X excess heat.

CuBr2 4g CAIII-300 + lg Mg + lg NaH + 2.23g CuBr2; Ein: 118.1 kJ; dE: 8.04 kJ; TSC: 108-180 ° C; Tmax: 369 ° C, the theoretical is 4.68 kJ, the gain is 1.7 · times.

SnF4 2.0 g of SnF4, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 18.4 kJ, but no explosion was observed Of temperature. The maximum temperature of the cell was 576 ° C, the theoretical temperature is 9.3 kJ, the gain is 1.98 times A1I3 4.1 g of A1I3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 10.1 kJ, but no burst was observed Of temperature. The maximum temperature of the cell was 412 ° C, the theoretical temperature is 6.68 kJ, the gain is 1.51 times.

| KH 8.3 gm '+ Mg 5.0 gm + CAII-300 20.0 gm + A1I3 20.5 gm, Ein: 318 kJ, dE: 48 kJ, the theoretical is 33.4 kJ, the gain is 1.4 times.

SIC14 | 1.7 g of SIC14, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 12.6 kJ, and the bursting temperature it was 68 ° C (366 - 434 ° C). The maximum temperature of the cell was 473 ° C, the theoretical temperature is 7.32 kJ, the gain is 1.72 times. | 4g CAIII-300 + lg of Mg + lg of NaH + 0.01 mol SIC14 (1.15 ce); Ein: 114.0 kJ; dE: 14.19 kJ; TSC: 260-410 ° C; Tmax: 423 ° C, the theoretical is 7.3-2 kJ, the gain is 1.94 times.

AlBr3 2.7 g of AlBr3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 7.5 kJ, but no explosion was observed Of temperature. The maximum temperature of the cell was 412 ° C, the theoretical temperature is 4.46 kJ, the gain is 1.68 times.

FeCl3 2.7 g of FeCl3, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 21.3 kJ, and the bursting temperature of the cell was 205 ° C (147 - 352 ° C) The maximum temperature of the cell was 445 ° C, the theoretical temperature is 10.8 kJ, the gain is 1.97 times.

SeBr4 4g CAIII-300 + lg Mg + lg NaH + 3.99g SeBr4; Ein: 112.0 kJ; dE: 23.40 kJ; TSC: 132-448 ° C; max: 448 ° C, the theoretical is 15.7 kJ, the gain 'is 1.5 times.

SnBr4 4g CAIII-300 + lg Mg + lg NaH + 4.38g SnBr4; Ein: 98.0 kJ; dE: 12.44 kJ; TSC: 120-270 ° C; Tmax: 359 ° C, the theoretical is 8.4 kJ, the gain is 1.48 times.

| KH 8.3 gm + Mg Powder 5.0 gm + CAII 300 20.0 gm + SnBr4 22.0 gm, Ein: 163 kJ, dE: 78 kJ; TSC at 60 ° C with Tmax ~ 290 ° C, the theoretical is 42 kJ, the gain is 1.86 times.

SiBr4 | 3.5 g of SiBr4, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C), the energy gain was 11.9 kJ, and the bursting temperature it was 99 ° C (304 - 403 ° C). The maximum temperature of the cell was 449 ° C, the theoretical temperature is 7.62 kJ, the gain is 1.56 times.

TeBr4 | 4g CAIII-300 + lg Mg + lg NaH + 4.47g TeBr4, Ein: 99.0 kJ, dE: 18.4 kJ, TSC: 186-411C, Tmax: 418 ° C, the theoretical is 11.3 kJ, the gain is of 1.63 times. | 4g CAIII-300 + lg of Al + lg of < NaH + 4.47g TeBr4, Ein: 101.0 kJ, dE: 14.7 kJ, TSC: 144-305 ° C, Tmax: 374 ° C, the theoretical is 11.4 kJ, the gain is 1.29 times. | 4.5 g of TeBr4, 1.66 g of KH, lg of MgH2 powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C) in a heavy duty 2.5 cm (1 inch) cell, the Energy gain was 19.1 kJ, and the burst temperature was 218 ° C (172 - 3909C). The maximum temperature of the cell was 410 ° C, the theoretical temperature is 12.65 kJ, the gain is 1.5 times. 4.5 g of TeBr4, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C) in a heavy duty 2.5 cm (1 inch) cell, the Energy gain was 23.5 kJ, and the burst temperature was 247 ° C (184 - 431 ° C). The maximum temperature of the cell was 436 ° C, the theoretical temperature is 12.4 kJ, the gain is 1.89 times.

| KH 6.64 gm + Mg Powder 4.0 gm + Activated Carbon CAII 300 16gm) + TeBr4 18 gm (Theoretical kJ) (80% climbing upwards 5X), Ein: 213 kJ, dE: 77 kJ, slope of temperature slope at 140 ° C with Tmax ~ 320 ° C, the theoretical is 48.4 kJ, the gain is 1.59 times TeC14 4g CAIII-300 + lg of Mg + lg of NaH + 2.7g TeCl4; Ein: 99.0 kJ; dE: 16.76 kJ; TSC: 114-300 ° C; Tmax: 385 ° C, the theoretical is 13 kJ, the gain is 1.29 times. 2.7 g of TeC14, 0.33 g of LiH, ig of MgH2 powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C) in a heavy-duty cell of 2.5 cm (1 inch), Energy gain was 20.4 kJ, and the burst temperature was 140 ° C (138 - 278 ° C). The maximum temperature of the cell was 399 ° C, the theoretical temperature is 12.1 kJ, the gain is 1.69 times. 2.7 g of TeC14, 0.33 g of LiH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C) in a heavy duty 2.5 cm (1 inch) cell, the Energy gain was 17.2 kJ, and the burst temperature was 240 ° C (137 - 377 ° C). The maximum temperature of the cell was 398 ° C, the theoretical temperature is 12.8 kJ, the gain is 1.34 times. 2.7 g of TeC14, 1.66 g of KH, lg of powder of MgH2 and 4 g of powder of activated carbon CA-III 300 (dried at 300 ° C) in a heavy-duty cell of 2.5 cm (1 inch), the Energy gain was 15.6 kJ, and the burst temperature was 216 ° C (139 - 355 ° C). The maximum temperature of the cell was 358 ° C, the theoretical temperature is 12.1 kJ, the gain is 1.29 times. 2.7 g of TeC14, 1.66 g of KH, lg of Al powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C) in a heavy duty 2.5 cm (1 inch) cell, the Energy gain was 19.4 kJ, and the burst temperature was 202 ° C (89 - 291 ° C). The maximum temperature of the cell was 543 ° C, the theoretical temperature is 10.9 kJ, the gain is 1.78 times. 2.7 g of TeCl4, 0.33 g of LiH, lg of Al powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C) in a heavy-duty cell of 2.5 cm (1 inch), the Energy gain was 19.0 kJ, and the burst temperature was 288 ° C (155 - 443 ° C). The maximum temperature of the cell was 443 ° C, the theoretical temperature is 10.9 kJ, the gain is 1.74 times. 2.7 g of TeC14, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C) in a heavy-duty cell of 2.5 cm (1 inch), the Energy gain was 17.7 kJ, and the burst temperature was 208 ° C (84 - 292 ° C). The maximum temperature of the cell was 396 ° C, the theoretical temperature is 13 kJ, the gain is 1.36 times. 2.7 g of TeC14, 1.66 g of KH, lg of Al powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C) in a heavy duty 2.5 cm (1 inch) cell, the Energy gain was 18.7 kJ, and the burst temperature was 224 ° C (112 - 336 ° C). The maximum temperature of > the cell was 398 ° C, the theoretical one is 12 kJ, the gain is 1.56 times.

SeCl4 4g CAIII-300 + lg of Mg + lg of NaH + 2.21g SeC14; Ein: 93.0 kJ; dE: 22.14 kJ; TSC: 141-435 ° C; Tmax: 435 ° C, the theoretical is 15 kJ, the gain is 1.48 times. | 4g CAIII-300 + lg of Mg + 1.66 g of KH + 2.20 g SeC14, dE Experimental: -25.2 kJ Reaction considered: SeCl4 (c) + 4KH (c) + 3Mg (c) = 4KCl (, c) + MgSe (c) + 2MgH2 (c) Q = -1750.4 kJ / theoretical chemical reaction energy: -17.5 kJ, excess heat: -7.7 kJ, 1.44X excess heat.

CF4 | NaH 50 gm + At 50 gm + Activated carbon CAII300 200 gm + CF4 0.3 mol; 3.1 Kg / cm2 (45 pounds / square inches gauge), reservoir cell volume: 2221.8CC, Ein: 2190 kJ, dE: 482 kJ, temperature jump at 200 ° C with Tmax ~ 760 ° C, the theoretical one is 345 kJ, the gain is 1.4 times.

| NaH 50.0 gm + Mg Powder 50 gm + Activated Carbon CAII-30'0 200 gm + CF4_ 5.3 - 0.7 Kg / cm2 (75-9.9 pounds / square inches gauge) after Evacuation. The volume of the deposit is 1800 ° CC and for this pressure drop, n = 0.356 mol and the theoretical energy is -392 kJ, Ein: 1810 kJ, dE: 765 kJ, slope of temperature slope at 170 ° C with Tmax ~ 1000 ° C and the gain is 765/392 = 1.95 X.

| NaH l.Ogm + (Mg powder 1.0 gm + Activated carbon CAII 300 4gm) Ball mill + CF4 0.0123 mol and theoretical energy -13.6 kJ), Ein: 143 kJ, dE: 25 kJ, slope of temperature slope at 250 ° C with Tmax ~ 500 ° C and Energy Gain -1.8 X.

| NaH l.Ogm + (Mg powder 1.0 gm + Activated carbon CAII-300 4gm 4gm) Ball mill + CF4 -0.01 mol Theoretical energy -10.2 kJ, Ein: 121 kJ, dE: 18 kJ, slope of temperature slope at 260 ° C with Tmax ~ 500 ° C and Energy Gain -1.7 X.

| NaH l.Ogm + (Mg powder 1.0 gm + activated carbon CAII-300 4gm 4gm) Ball mill + CF4 0.006 · mol and theoretical energy -7.2 kJ), Ein: 133 kJ, dE: 15 kJ, slope jump of temperature at 300 ° C with Tmax ~ 440 ° C and Energy gain -2.0 X. 4g CAIII-300 + lg of MgH2 + 3.55g Rb + 0.0082 mol CF4 + 0.0063 mol H2; Ein: 76.0 kJ; dE: 20.72 kJ; TSC: 30-200 ° C; Tmax: 348 ° C, the theoretical is 10 kJ, the gain is 2 times.

SF6 NaH 50 gm + MgH2_50 gm + Activated carbon CAII300 200 gm + SF6 0.29 mol; 3 Kg / cm2 (43 pounds / square inches gauge), reservoir cell volume: 2221.8CC, Ein: 1760 kJ, dE: 920 kJ, temperature slope jump to ~ 140 ° C with Tmax -1100 ° C, the theoretical is 638 kJ, the gain is 1.44 times. 4g CAIII-300 + lg of MgH2 + lg of NaH + 0.0094 mol SF6; Ein: 96.7 kJ; dE: 33.14 kJ; TSC: 110-455 ° C; Tmax: 455 ° C, the theoretical is 20.65 kJ, the excess is 12.5 kJ, the gain is 1.6 times.

| NaH 1.0 gm + Al 1.0 gm powder + CAII 300 activated carbon 4gm) Ball mill + SF6 0:01 mol and theoretical energy -20 kJ), Ein: 95 kJ, dE: 30 kJ, change of temperature slope to ~ 100 ° C with Tmax -400 ° C, the theoretical, is 20.4 kJ-, the excess is 9.6 kJ, the gain is 1.47 times.

| NaH 1.0 gm + Powder of MgH2 1.0 gm + Activated carbon CAII 300 4gm) Ball mill + SF6 0.01 mol and Theoretical energy -22 kJ), Ein: 85 kJ, dE: 28 kJ, change of temperature slope to ~ 110 ° C with Tmax ~ 410 ° C, the theoretical is 22 kJ, the excess is 6 kJ, the gain is 1.27 times.

| NaH 1.0 gm + nano powder of Al 1.0 gm + Activated carbon CAII 300 4gm) Ball mill + SF6 0.005 mol, Ein: 107 kJ, dE: 21 kJ, change of temperature slope to -160 ° C with Tmax ~ 380 ° C, the theoretical is 10.2 kJ, the gain is 2 times | NaH 1.0 gm + Mg powder 1.0 gm + Activated carbon CAII 300 4gm) Ball mill + SF6 0.005 mol, Ein: 104 kJ, dE: 18 kJ, change temperature slope to ~ 150 ° C with Tmax ~ 370 ° C, the theoretical is 12.5 kJ, the excess is 5.5 kJ, the gain is 1.44 times.

| NaH 1.0 gm + Powder MgH2 1.0 gm + Activated carbon CAII 300 4gm) Ball mill + SF6 0.0025 mol and Theoretical energy -5.5 kJ), Ein: 100 kJ, dE: 10 kJ, change of temperature slope to ~ 160 ° C with Tmax ~ 335 ° C, the theoretical is 5.5 kJ, the gain is 1.8 times. 4g CAIII-300 + 0.5g B + lg NaH + 0.0047 mol SF6; Ein: 112.0 kJ; dE: 15.14 kJ; TSC: 210-350 ° C; Tmax: 409 ° C, the theoretical is 10.12 kJ, the excess is 5 kJ, the gain is 1.49 times. | 4g CAIII-300 + lg of MgH2 + 1.66 g of KH + 0.00929 mol SF6 (the temperature of the cell rose up to 29 ° C in the filling with SF6); Ein: 66.0 kJ; dE: 26.11 kJ; TSC: 37-375 ° C; Tmax: 375 ° C, the theoretical is 20.4 kJ, the gain is 1.28 times. | 4g CAIII-300 + lg Mg + 0.33g LiH + 0.00929 mol SF6 (the temperature of the cell was raised to 260C when filling with SF6); Ein: 128.0 kJ; dE: 32.45 kJ; TSC: 275-540 ° C; Tmax: 550 ° C, the theoretical is 23.2 kJ, the gain is 1.4 times. | 4g CAIII-300 + lg S + lg of NaH + 0.0106 mol SF6 (in line), Ein: 86.0 kJ, dE: 18.1 kJ, TSC: 51-313 ° C, Tmax: 354 ° C, the theoretical is 11.2 kJ, the gain is 1.6.

| NaH 5.0 gm + MgH2 5.0 gm + Activated carbon CAII 300 20.0 gm) Ball mill + SF6 - 2.8 Kg / cm2 (40 pounds / square inch gauge); 0.026 mol ONLINE (Theoretical energy -57 kJ) cell of 5 cm (2 inches), Ein: 224 kJ, dE: 86 kJ, temperature jump to 150 ° C with Tmax ~ 350 ° C, the theoretical is 57 kJ , the gain is 1.5 times. .

Te02 4g CAIII-300 + lg of MgH2 + lg of NaH + 1.6g Te02; Ein: 325.1 kJ; dE: 18.46 kJ; TSC: 210-440 ° C; Tmax: 44 ° C, the theoretical is 9.67 kJ, the excess is 8.8 kJ., The gain is 1.9 times. 4g CAIII-300 + 2g MgH2 + 2g NaH + 3.2g Te02, Ein: 103'.0 kJ, dE: 31.6 kJ, TSC :. 185-491 ° C, Tmax: 498 ° C, the theoretical is 17.28 kJ, the gain is 1.83 times. 1.6 g of Te02, 0.33 g of LiH, lg of Al powder and 4 g of activated carbon dust CA-III 300 (dried at 300 ° C) in a heavy duty 2.5 cm (1 inch) cell, the energy gain was 18.1 kJ, but no temperature burst was observed. The maximum temperature of the cell was 637 ° C, theoretical 8.66 kJ, the gain is 2.1 times. 1.6 g of Te02, 1.66 g of KH, lg of gH2 powder and 4 g of CA-.III 300 activated carbon powder (dried at 300 ° C) in a 2.5 cm (1 inch) heavy-duty cell, the energy gain was 22.0 kJ, and the burst temperature was 233 ° C (316 - 549 ° C). The maximum temperature of the cell was 554 ° C, theoretical 8.64 kJ, the gain is 2.55 times. 1.6 g of Te02, 1.66 g of KH, lg of Mg powder and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C) in a heavy-duty cell of 2.5 cm (1 inch), the Energy gain was 20.3 kJ, and the burst temperature was 274 ° C (268 - 542 ° C). The maximum temperature of the cell was 549 ° C, the theoretical temperature is 10.9 kJ, the gain is 1.86.

| NaH 5.0 gm + Powder of MgH2 5.0 gm + Charcoal activated CAII 300 20 gm) Ball mill + Te02 8.0gm, Ein: 253 kJ, dE: 77 kJ, jumped of temperature slope at 20 ° C with Tmax ~ 400 ° C, the theoretical is 48.35 kJ, the gain is 1.6 times. | NaH 1. O gm + MgH2 powder 1.0 gm + Activated carbon CAII 300 4.0 gm) Ball mill + Te02 1.6gm, Ein: 110 kJ, dE: 16 kJ, temperature slope jump at 190 ° C with Tmax ~ 400 ° C, the theoretical is 9.67 kJ, the gain is 1.65 times.

| KH 1.66 gm + MgH2 powder 1.0 gm + Activated carbon CAII 300 4.0 gm) Ball mill + Te02 1.6gm, Ein: 119 kJ, dE: 19 kJ, temperature slope jump at 340 ° C with Tmax ~ 570 ° C, the theoretical one is 9.67 kJ, the gain is 2 times | 4g CAIII-300 + lg of NaH + 1.6g Te02, Ein: 116.0 kJ, dE: 11.0 kJ, TSC: 207-352 ° C, Tmax: 381 ° C, the theoretical is of 6. 6 kJ, the gain is 1.67 times.

| KH 1.66 gm + MgH2 Powder 1.0 gm + TiC 4.0 gm + Te02 1.6gm, Ein: 133 kJ, dE: 15 kJ, temperature slope jump to 280 ° C with Tmax ~ 460 ° C, the theoretical is 8.64 kJ, the gain is 1,745 times. | 4g CAIII-300 + lg of Mg + lg of NaH + 1.60 g Te02, dE Experimental: -17.0 kJ Reaction considered: Te02 (c) + 3Mg ('c) + 2NaH (c) = 2MgO (c) + Na2Te ( c) + MgH2 (c) Q = - 1192.7 kJ / theoretical chemical reaction energy: -11.9 kJ, excess heat: -5.1 kJ. 1.43X excess heat.

P2Q5 1.66 g of KH, 2 g of P205 and lg of MgH2 and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C) in a heavy-duty cell of 2.5 cm (1 inch), the gain of energy was 21.2 kJ, and the burst temperature was 242 ° C (299 - 541 ° C). The maximum temperature of the cell was 549 ° C, the theoretical temperature is 10.8 kJ, the excess is 10.35 kJ, the gain is 1.96 times 032609GC4: 031909RC F4 / 1.66 g of KH + 2 g P205 + 1 g of MgH2 + 4 g CA III-300 in DMF-d7 (as received), strong -3.86 ppm peak. | 4g CAIII-300 + lg of MgH2 + 1.66 g of KH + 2g P205, Ein: 138.0 kJ, dE: 21.6 kJ, TSG320-616 ° C, Tmax: 616 ° C, the theoretical is of 11.5 kJ, the excess is of 10.1 kJ, the gain is 1.9 times.

| KH 8.3 gm + Powder of MgH2 5.0 gm + Activated carbon CAII 3? 0 20 gm) Ball mill + P205 lO.Ogm, Ein: 272 kJ, dE: 98 kJ, jump at 250 ° C with Tmax ~ 450 ° C , the theoretical is 54 kJ, the gain is 1.81 times.

| KH 1.66 gm + MgH2 powder 1.0 gm + Activated carbon CAII 300 4gm) Ball mill + P205 2.0 gm, Ein: 130 kJ, dE: 21 kJ, jump at 300 ° C with Tmax ~ 550 ° C, the theoretical is of 10.8 kJ, the gain is 1.94 times.

| KH 1.66 gm + Powder of MgH2 1.0 gm + Tic 4.0 gm + P205 2.0 gm, Ein: 129 kJ, dE: 21 kJ, slope of temperature slope at 270 ° C with Tmax ~ 600 ° C the theoretical is 10.8 kJ, the gain is 1.95 times.

NaMn04 4g CAIII-300 + lg Si + lg of NaH + 3.5g NaMn04; Ein: 123.0 kJ; dE: 26.25 kJ; TSC: 45-33 ° C; Tmax: 465 ° C, the theoretical is 17.6 kJ, the excess is 8.7 kJ, the gain is 1.5 times. 4g CAIII-300 + lg of Al + lg of NaH + 3.5g NaMn04; Ein: 120.0 kJ; dE: 32.41 kJ; TSC: 44-373 ° C; Tmax: 433 ° C, the theoretical is 20.5 kJ, the excess is 7.7 kJ, the gain is 1.58 times. 4g CAIII-300 + lg Mg + lg NaH + 3.5g NaMn04; Ein: 66.0 kJ; dE: 32.27 kJ; TSC: 74-43 ° C; Tmax: 430 ° C, the theoretical is 17.4 kJ, the excess is 14.9 kJ, the gain is 1.85 times. | 4g CAIII-300 + lg Mg + lg NaH + 3.5g NaMn04, Ein: 72.0 kJ, dE: 34.1 kJ, TSC: 49-362 ° C, Tmax: 364 ° C, the theoretical is 17.4 kJ, the excess is 16.7 kJ, the gain is 2.

| KH 8.3 gm + Mg powder 5.0 gm + Activated carbon CAII 300 20 gm) Ball mill + NaMn04 17.5gm, Ein: 130 kJ, dE: 160 kJ, slope of temperature at 70 ° C with Tmax ~ 350 ° C, the theoretical is 87 kJ, the gain is 1.84 times | KH 8.3 gm + Al powder 5.0 gm + Activated carbon CAII 300 20 gm) Ball mill + NaMn04 17.5gm, Ein: 134 kJ, dE: 171 kJ, temperature slope jump at 50 ° C with Tmax ~ 350 ° C, the theoretical is 102.5 kJ, the gain is 1.66 times.

| NaH 1.0 gm + Mg Powder 1.0 gm + Activated Carbon CAII 300 4.0 gm) Ball Mill + NaMn04 3.5gm (Theoretical -17.4 kJ), Ein: 54 kJ, dE: 32 kJ, temperature slope jump to 60 ° C with Tmax ~ 450 ° C, the theoretical is 17.4 kJ, the gain is 1.8 times.

| KH 1.66 gm + Mg powder 1.0 gm + Tick 4.0 gm + NaMn04 3.5gm, Ein: 65 kJ, dE: 30 kJ, temperature slope jump to 70 ° C with Tmax ~ 410 ° C, the theoretical is 17.4 kJ, the gain is 1.7 times.

Nitrate 2 g of NaH, 3 g of NaN03 and the mixture of lg of Ti powder and 4 g of activated C powder (dried at 300 ° C) in a 2.5 cm (1 inch) cell, the energy gain was 33.2 kJ, and the burst temperature was 418 ° C (110 - 528 ° C). The maximum temperature of the cell was 530 ° C, the theoretical temperature is 24.8 kJ, the excess is 8.4 kJ, the gain is 1.3 times. | 3 g of NaH, 3 g of NaN03 and the mixture of lg of nanopoly of Al and 4 g of activated C powder (dried at 300 ° C) in a cell of 2.5 cm (1 inch), the gain of energy was 42.3 kJ, and the burst temperature was 384 ° C (150 -534 ° C). The maximum temperature of the cell was 540 ° C, the theoretical temperature is 33.3 kJ, the excess is 9 kJ, the gain is 1.27 times 2.1 g of NaH, 3 g of NaN03 and the mixture of lg of MgH2 and 4 g of activated C powder (dried at 300 ° C) in a 2.5 cm (1 inch) cell, the energy gain was 43.4 kJ , and the burst temperature was 382 ° C (67 - 449 ° C). The maximum temperature of the cell was 451 ° C, the theoretical temperature is 28.6 kJ, the excess is 14.8 kJ, the gain is 1.52 times. | 0.33 g of LiH, 1.7 g of LÍN03 and the mixture of lg of MgH2 and 4 g of activated C powder (dried at 300 ° C) in a heavy-duty cell of 2.5 cm (1 inch), the energy gain it was 40.1 kJ, and the burst temperature was 337 ° C (92 -429 ° C). The maximum temperature of the cell was 431 ° C, the theoretical temperature is 21.6 kJ, the excess is 18.5 kJ, the gain is 1.86 times. | 0.33 g of LiH, 1.7 g of LiN03 and the mixture of lg of Ti and 4 g of activated C powder (dried at 300 ° C) in cell 2. 5 cm (1 inch), the energy gain was 36.5 kJ, and the burst temperature was 319 ° C (83-402 ° C). The maximum temperature of the cell was 450 ° C, the theoretical temperature is 18.4 kJ, the excess is 18 kJ, the gain is 2 times. | 4g CAIII-300 + lg of MgH2 + lg of NaH + 2.42g LINE 03; Ein: 75.0 kJ; dE: 39.01 kJ; TSC: 57-492 ° C; Tmax: 492 ° C, the theoretical is 28.5 kJ, the excess is 10.5 kJ, the gain is. of 1.37 times 4g CAIII-300 + lg of Al + lg of NaH + 2.42g LÍN03; Ein: 81.2 kJ; dE: 41.8 kJ; TSC: 73-528 ° C; Tmax: 528 ° C, the theoretical is 34.6 kJ, the excess is 7.3 kJ, the gain is 1.21 times.

C1Q4 | 4g CAIII-300 + lg of MgH2 + 2g of NaCl04 + lg of NaH; Ein: 86.0 kJ; dE: 38.88 kJ; TSC: 130-551 ° C; Tmax: 551 ° C, the theoretical is 30.7 kJ, the excess is 8.2 kJ, the gain is 1.27 times. 4g CAIII-300 + lg of Al + lg of NaH + 4.29g NaCl04; Ein: 88.0 kJ; dE: 58.24 kJ; TSC: 119-615 ° C; Tmax: 615 ° C, the theoretical is 47.1 kJ, the excess is 11.14 kJ, the gain is .2.23 times. 4g CAIII-300 + lg of MgH2 + lg of NaH + 4.29g NaCl04; Ein: 98.0 kJ; dE: 56.26 kJ; TSC: 113-571 ° C; Tmax: 571 ° C, the theoretical is 36.2 kJ, the excess is 20.1 kJ, the gain is 1.55 times.

K2S2Q8 | 4g CAIII-300 + lg of MgH2 + 1.66 g of KH + 2.7g K2S208, Ein: 121.0 kJ, dE: 27.4 kJ, TSC: 178-462 ° C, Tmax: 468 ° C, the theoretical is 19.6 kJ, the excess is 7.8 kJ, the gain is 1.40 times.

SQ2 | 4g CAIII-300 + lg MgH2 + lg NaH + 0.0146 mol S02, Ein: 58.0 kJ, dE: 20.7 kJ, TSC: 42-287 ° C, Tmax: 309 ° C, the theoretical is 15 kJ, the excess is 5.7 kJ, the gain is 1.38 times.

S | 4g CAIII-300 + lg of MgH2 + lg of NaH + 3.2g S, Ein: 67.0 kJ, dE: 22.7 kJ, TSC: 49-356 ° C, Tmax: 366 ° C, the theoretical is 17.9 kJ, the excess is 4.8 kJ, the gain is 1.27 times. | 1.3 g of S powder, 1.66 g of KH, lg of powder If and 4 g of activated carbon powder CA-III 300 (dried at 300 ° C) in a heavy-duty cell of '2.5 cm (1 inch), the energy gain was 13.7 kJ, and the burst temperature was of 129 ° C (66 - 195 ° C). The maximum temperature of the cell was 415 ° C, the theoretical temperature is 7.5 kJ, the excess is 1.82 times. | 3.2 g of S powder, 0.33 g of LiH, lg of Al powder and 4 g of activated carbon powder CA-IV 300 (dried at 300 ° C) in a heavy duty 2.5 cm (1 inch) cell , the energy gain was 27.1 kJ, and the burst temperature was 301 ° C (163 - 464 ° C). The maximum temperature of the cell was 484 ° C, the theoretical temperature is 20.9 kJ, the excess is 6.2 kJ, the gain is 1.3 times. | 3.2 g of S powder, 0.33 g of LiH, lg of Si powder and 4 g of activated carbon powder CA-IV 300 (dried at 300 ° C) in a heavy duty 2.5 cm (1 inch) cell , the energy gain was 17.7 kJ, and the burst temperature was 233 ° C (212 - 445 ° C). The maximum temperature of the cell was 451 ° C, the theoretical temperature is 13.7 kJ, the excess is 4 kJ, the gain is 1.3 times. | 4g CAIII-300 + lg of Si + 1.66 g of KH + 1.3g of S, Ein: 81.0 kJ, dE: 10.8 kJ, TSC: 52-196 ° C, Tmax: 326 ° C, the theoretical is 7.4 kJ , the gain is 1.45 times.

SnF4 4g CAIII-300 + lg Mg + lg NaH + 1.95g SnF4; Ein: 130.2 kJ; dE: 13.89 kJ; TSC: 375-520 ° C Tmax: 525 ° C, the theoretical is 9.3 kJ, the gain is 1.5 times. 4g CAIII-300 + lg Mg + lg NaH + 1.95g SnF4; Ein: 130.2 kJ; dE: 13.89 kJ; TSC: 375-520 ° C; Tmax: 525 ° C, the theoretical is 9.3 kJ, the gain is 1.5 times.

Se02 | 4g CAIII-300 + 2 g of MgH2 + 2g of NaH + 2.2g Se02, Ein: 82.0 kJ, dE: 29.5 kJ, TSC: 99-388 ° C, Tmax: 393 ° C, the theoretical is 20.5 kJ, the gain is 1.4 times.

CS2 | NaH 1.0 gm + (Al 1.0 gm powder + CAII 300 4gm activated carbon) Ball mill + CS2 1.2 ml in PP bottle, Ein: 72 kJ, dE: 18 kJ, temperature slope jump to ~ 80 ° C with Tmax ~ 320 ° C, the theoretical is 11.4 kJ, the gain is 1.58 times.

| NaH 1.0 gm + Powder of MgH2 1.0 gm + Activated carbon CAII 300 4gm) Ball mill + CS2 1.2 ml in PP bottle, Ein: 82 kJ, dE: 18 kJ, temperature slope jump to ~ 80 ° C with Tmax ~ 330 ° C, the theoretical one is 12.6 kJ, the gain is 1.4 times.

CQ2 4g CAIII-300 + lg of MgH2 + lg of NaH + 0.00953 mol C02 (the cell temperature was raised to 45 ° C at filling with C02); Ein: 188.4. kJ; dE: 10.37 kJ; TSC: 80-120 ° C; Tmax: 508 ° C, the theoretical is 6.3 kJ, the gain is 1.65 times.

PF5 4g CAIII-300 + lg of Al + lg of NaH + 0.010 mol PF5; Ein: 127.0 kJ; dE: 15.65 kJ; TSC: 210-371 ° C; Tmax: 371 ° C, the theoretical is 10 kJ, the excess is 6.45 kJ, the gain is 1.57 times. | 4g CAIII-300 + lg of Al + lg of NaH + 0.01 mol PF5, Ein: 101.0 kJ, dE: 15.7 kJ, TSC: 178-370 ° C, Tmax: 391 ° C, the theoretical is 10 kJ, the Gain is 1.57 times.

NF3 | NaH l.Ogm + (Mg powder 1.0 gm + Activated carbon CAII-300 4gm) Ball mill + NF3 0.011 mol and theoretical energy kJ), Ein: 136 kJ, dE: 28 kJ, temperature slope jump to 70 ° C with Tmax ~ 470 ° C, the theoretical is 19.6 kJ, the gain is 1.4 times.

PCI5 4g CAIII-300 + lg of MgH2 + 2.08g of PC15 + lg of NaH; Ein: 90.0 kJ; dE: 20.29 kJ; TSC: 180-379 ° C; Tmax: 391 ° C < the theoretical one is 13.92 kJ, the gain is 1.45 times.

P2S5 4g CAIII-300 + lg of MgH2 + lg of NaH + 2.22g P2S5; Ein: 105.0 kJ; dE: 13.79 kJ; TSC: 150-363 ° C; Tmax: 398 ° C, the theoretical is 10.5 kJ, the excess is 3.3 kJ, the gain is 1.3 times.

| NaH 1.0 gm + Al powder 1.0 gm + Activated carbon CAII 300 4gm) Ball mill + P2S5 2.22 gm), Ein: 110 kJ, dE: 14 kJ, slope of temperature slope at ~ 170 ° C with Tmax ~ 425 ° C, the theoretical is 10.1 kJ, the gain is 1.39 times.

Oxide | 4g activated carbon + lg MgH2 + 1.66 g 'of KH + 1.35g K02, Ein: 86.0 kJ, dE: 21.0 kJ, TSC: 157-408 ° C, Tmax: 416 ° C, the theoretical is 15.4 kJ , the gain is 1.36 times. n04 4g CAIII-300 + lg of Mg + lg of NaH + 3.5g Mn02; Ein: 108.0 kJ; FROM: 22.11 kJ; TSC: 170-498 ° C; Tmax: 498 ° C, the theoretical is 18.4 kJ, the excess is 3.7 kJ, the gain is 1.2 times.

N2Q | 4g Pt / C + lg of Mg + lg of NaH + 0.0198 'mol N20, Ein: 72.0 kJ, dE: 22.2 kJ, TSC: 73-346 ° C, Tmax: 361 ° C, the theoretical is 16.2 kJ, the gain is 1.37 times.

HFB | NaH 1. Ogm + (nano aluminum powder lgm + Activated carbon (AC) 5gm) Ball mill + HFB 1 mi, Ein: 108 kJ, dE 35 kJ, temperature jump from 450 ° C to 90 ° C.

| NaH l.Ogm + (5gm + Activated carbon 5gm) Ball mill + hexafluorobenzene 1 ml, Ein: 109 kJ, dE: 38 kJ, temperature jump from 400 ° C to 90 ° C. , (4g of activated carbon (AC) + lg of MgH2) Ball mill + lml of HFB + lg of NaH, Ein: 150.0 kJ, dE: 45.1 kJ, • TSC: -50-240, Tmax ~ 250 ° C .

Mixture (4g of activated carbon + lg of MgH2) + lml of HFB + lg of NaH, Ein: 150.0 kJ, dE: 35.0 kJ, TSC: 54-255 ° C, 45- 241 ° C, 48-199 ° C; Tmax: 258 ° C, 247 ° C, 206 ° C (three cells in tandem). 1.66 g of KH, 1 ml of hexadecafluoroheptane (HDFH), and the mixture of 4 g of activated C powder and lg of MgH2 in a 2.5 cm (1 inch) cell, dE: 34.3 kJ, and the outbreak was 419 ° C (145 - 564 ° C), Tmax ~ 575 ° C.

B. NMR in Solution Representative reaction mixtures for forming hydrino comprise (i) at least one catalyst such as one chosen from LiH, KH, and NaH, (ii) at least one oxidant such as one selected from NiBr2, Mnl2, AgCl, EuBr2, SF6 , S, CF4, NF3, LiN03, M2S20a with Ag, and P205, (iii) at least one reducing agent such as one chosen from Mg powder or MgH2, Al powder, or aluminum nano-powder (Al NP), Sr and Ca, and (iv) at least one support such as a chosen activated carbon and Tic. 50 mg of the reaction product of the reaction mixtures were added to 1.5 ml of deuterated N, N-dimethylformamide-d7 (DCON (CD3) 2, DMF-d7, (99.5% Cambridge Isotope Laboratories, Inc.) in a flask that was sealed with a glass TEFLON ™ valve, agitated and allowed to dissolve for a period of 12 hours in a glove compartment under an argon atmosphere.The solution in the absence of any solid 'was transferred to an NMR tube (5 mm OD, 23 cm length, Wilmad) by a gas tight connection, followed by sealing to the tube flare.The NMR spectra were recorded with a 500 MHz Bruker NMR spectrometer that was blocked with deuterium. Chemical shifts were referred to the frequency of solvent such as DMF-d7 at 8.03 ppm relative to tmethylsilane (TMS).

The hydride hydride ion H ~ (l / 4) was predicted to be observed at approximately -3.86 ppm and it was predicted that the hydrino molecular H2 (l / 4) was observed at 1.25 ppm relative to TMS. The position of the presence of these peaks with the displacement and intensity for a specific reaction mixture are given in TABLE 4.

TABLE 4. NMR in 1H solution followed by solvent extraction of DMF-d7 from the product of the heterogeneous hydrino catalyst system comprising reactants (I) catalysts such as LiH, KH, or NaH, (ii) reducing agent such as Al , To NP, Mg or MgH2, and (iii) oxidant such as CF4, N20, NF3, 2S20a, FeS04, 02, LiN03, P205, SF6, S, CS2, NiBr2, Te02, NaMN04, SnF4 and Snl4 mixed with (iv) ) a support such as activated carbon or Pt / C.

Reagents Position and Position and intensity peak intensity of H2 peak of H- (1/4) (1/4) 1. 66 g of KH, lg of Al, 4 g 1.22 ppm less 3.85 ppm of activated carbon, and 0.01 strong strong of CF4 1 g of NaH, lg of Al, 4 g of 1.23 ppm activated carbon, and 0.01 strong moles of CF4 1 g of NaH, 1 g of MgH2, 4 g 1.22 ppm of activated carbon, and 0.01 strong moles of CF4 1 g of NaH, lg of MgH2, 4 g 1.22 ppm of activated carbon and 0,004 strong mol CF4 1 g of NaH, lg of Mg, 4 g of 1.21 ppm activated carbon. and 52 medium millimeters of CF4 1 g of NaH, lg of Al, 4 g of 1.21 ppm • activated carbon and 52 strong millimeters of CF4 1 g of NaH, 1 g of MgH2, 4 g of 1.27 ppm less 3.86 of Pt / C and 0.01 mol of CF4 medium mean ppm 1 g of NaH, lg of Al, 4 g of 1.21 ppm Pt / C and 0.002 mol of strong CF4 0. 5 g of NaH, 0.5 g of Mg, 2 1.22 ppm g activated carbon and 52 strong Millimoles of CF4 0. 5 g of NaH, 0.5 g of Al, 2 1.21 ppm g activated carbon and 0.002 strong moles of CF4 1. 66 g of KH, 1 g of MgH2, 4 1.22 ppm, much less 3.85 g of activated carbon, 0.01 strong ppm, half a mole of N20 1 g of NaH, lg of Al, 4 g of 1.21 ppm activated carbon, 0.002 moles strong of N20 1 g of NaH, lg of Al, 4 g of 1.21 ppm activated carbon, 0.004 moles strong of N20 1 g of NaH, 1 g of MgH2, 4 g 1.21 ppm activated carbon, 0.002 strong moles of N20 1 g of NaH, 1 g of MgH2, 4 g 1.22 ppm activated carbon, 0.004 medium moles of N20 1 g of NaH, 1 < g of MgH2, 4 g 1.24 ppm activated carbon and 0.01 strong mol N20 1 g of NaH, 1 g of MgH2, 4 g 1.24 ppm less 3. 84 of activated carbon and 0.018 strong ppm of strong moles of N20 0. 33 g LiH, lg of Al, 4 g of 1.22 ppm less 3. 85 Al and 0.004 mol of N20 medium strong ppm 1 g of. NaH, 1 g of MgH2, 4 g 1.24 ppm very of Pd / C (l%) and 0.01 mol of strength N20 1 g of NaH, 4 g of carbon 1.21 ppm very activated and 0.004 mol of strong N20 1 g of NaH, 1 g of MgH2, 5 g of 1.23 ppm of Er203, 4 g of Ac and 0.01 strong mol of N20 1 g of NaH, lg of Al, 5 g of 1.24 ppm Er203, 4 g of Ac and 0.01 mol strong of N20 1 g NaH, 1 g Mg, 4 g 1.23 ppm of Ac and 0.00-4 mol of strong N20 0. 5 g of NaH, 0.5 g of MgH2, 1.22 ppm 4 g of activated and strong carbon 0. 004 mol of N20 0. 33 g of LiH, lg of Al, 4 g 1.26 ppm less 3.85 of activated carbon, 0.21 g of medium ppm K2S208 and 0.01 mol of 02 strong 0. 33 g of LiH, lg of Al, 4 g 1.27 ppm less 3.85 of activated carbon and 0.01 medium ppm of strong mol of 02 0. 33 g of LÍH, 1 g of MgH2, 1.27 ppm less 3 .85 4 g activated carbon, 0.21 medium ppm very g of K2S208 and 0.01 mol of 02 strong 1 g of NaH, 1 g of MgH2, 4 g of 1.24 ppm activated carbon, 0.15 g strong of FeS04 and 0.01 mol of 02 1. 66 g. Of KH, 1 g of Mg, 4 g 1.21 ppm of activated carbon and 0.004 strong mol of 02 1 g of NaH, lg Si, 4 g of 1.21 ppm Activated carbon and 0.01 mol strong of 02 1 g of NaH, 10 g of Pt / Ti, 1 1.22 ppm very g of MgH2 4 g of strong carbon activated, 0.01 mol of NH3 and 0. 01 mol of 02 0. 5 g of NaH, 0.5 g of Al, 4 1.22 ppm less 3.85 g of activated carbon and 0.002 medium ppm strong of NF3 0. 5 NaH, 0.5 g MgH2, 4 1.21 ppm very g of activated carbon and 0.004 strong mol of NF3 lg of NaH, lg of Al, 4 g of 1.21 ppm activated carbon and 0.002 mol strong of NF3 0. 5 g of NaH, 0.5 g of gH2, minus 3 .85 4 g of activated carbon and ppm average 0.004 mol of NF3 0. 5 of NaH, 0.5 g of MgH2, 4 1.22 ppm g of activated carbon and 0.002 strong mol of NF3 1. 66 g of KH, 2.5 g of 1.22 ppm less 3 .85 LiN03, 4 g of strong activated strong ppm coal and 1 g of MgH2 lg of NaH, 3 g of Na 03, 4 g less 3 .84 of activated carbon and 1 g of average ppm MgH2 lg of NaH, 2.5 g of L03, 4 minus 3.84 g of activated carbon "and 1 g ppm of MgH2 1. 66 g of KH, 2.5 g of LÍN03 1.22 ppm very and 1 g of strong MgH2 1. 66 g of KH, 2 g of P205, 4 1.28 ppm very less 3.86 g of activated carbon and 1 g strong strong ppm of MgH2 0. 33 g of LiH, 2 g of P205, minus 3 .85 4 g of activated carbon and 1 g ppm of MgH2 lg of NaH, 2 g of P205, 4 g less 3.85 of activated carbon and 1 g of average ppm MgH2 lg of NaH, 2 g of P205, 4 g '1.20 ppm less 3.85 of activated carbon and lg of strong average ppm To the 1. 66 g of KH, 1 g of MgC12, 1 .23 · ppm very less 3.85 4 g of activated carbon, 4.5 strong ppm medium g K02 and 0.1 g of CoC12 1 g of NaH, 1 g of gH2, 4"g minus 3.84 of activated carbon and 0. 0094 ppm very mol SF6 strong lg of NaH, 0.5 g of B, 4 g less 3.85 of activated carbon and 0. 0047 ppm strong mol of SF6 lg of NaH, 1 g of Mg, 4 g of minus 3.86 activated carbon and 0.01 mol of strong ppm of SF6 lg of NaH, lg of Al, 4 g of 1 .20 ppm less 3.86 activated carbon and 0.005 mol strong weak ppm of SF6 1. 66 g of KH, lg of Si, g minus 3.86 of activated carbon and 0. 0092 ppm very mol of strong SF6 1. 66 g of KH, lg of Al, 4 g less 3.86 of activated carbon and 0. 0092 ppm very 1.66 g of KH, 1 g of MgH2, 4 minus 3.86 g of activated carbon and ppm very 0.0092 mol of strong SF6 0. 33 g LiH, 1 g of MgH2, 4 g less 3.82 of activated carbon and 0.009 ppm very mol of strong SF6 0. 33 g LiH, 1 g Mg, 4 g less 3.84 activated carbon and 0.009 ppm half mole of SF6 0. 33 g LiH, lg of La, 4 g of minus 3.75 · activated carbon and 0.0094 mol ppm SF6 board • 1.66 g of KH, 1 g of MgH2, 4 1.21 ppm less 3.86 g of activated carbon and strong 'weak ppm 0. 0093 mol of SF6 lg of NaH, 5 g of La, 4 g of 1.21 ppm less 3.86 activated carbon and 0.0047 mol medium weak ppm of SF6 minus 2.83 1 g of NaH, 1 g of MgH2, 4 g of highly activated carbon and 3.2 g of strong S 1 g of NaH, 1 g of MgH2, 4 g less 2.83 of activated carbon and 3.2 g of strong ppm and of S (outside) board 0. 33 g of LiH, lg of Si, 4 g less 3.81 of activated carbon and 1.3 g ppm of strong S 0. 33 g of LiH, lg of Al, 4 g less 3.81 of activated carbon and 1.3 g of very strong S 1. 66 g of KH, lg of Al, 4 g less 3.47 of activated carbon and 1.3 g of very strong S 1. 66 g of KH, lg of Al, 4 g less 3.86 of activated carbon and 1.3 g of very strong S 1. 66 g of KH, lg of Si, 4 g less 3.55 of activated carbon and 1.3 g of very strong S 1. 66 g of KH, lg of Si, 4 g less 3.85 of activated carbon and 1.3 g of strong ppm of S 1. 66 g of KH, 1 g of MgH2, 4 1.24 ppm less 3.85 g of activated carbon and 2.7 g of strong ppm of strong K2S208 1 g of NaH, lg of Al, 4 g of minus 3.85 activated carbon and 1.2 ml of ppm very strong CS2 1 g of NaH, 1 g of MgH2, 4 g of 1.21 ppm less 3.86 of activated carbon and 0.0146 half ppm of half a mol of S02 1 g of NaH, 1 g of MgH2, 4 g of activated carbon and 2.2 g 1.23 ppm of strong NiBr2 1 g of NaH, 1 g of g, 4 g 1.25 ppm activated carbon and 2.2 g medium of NiBr2 1 g of NaH, 4 g of .coal 1.24 ppm very activated and 2.2 g of strong NiBr2 1. 66 g of KH, 4 g of carbon 1.22 ppm very activated and 2.2 g of strong NiBr2 1 g of NaH, 1.66 g of Ca, 4 1.24 ppm very g of activated carbon and 2: 2 g strong of NiBr2 1 g of NaH, 3.67 g of Sr, 4 1.24 ppm very g of activated carbon and 3.1 g strong of Mnl2 83 g of KH, 50 g of Mg, 200 1.24 ppm g of Tic and 154.5 g of strong Mnl2 1 g of NaH, 1.66 g of Ca, 4 1.23 ppm very g of activated carbon and 3.1 g strong 1 g of NaH, 4 g of carbon 1.21 ppm less 3.85 activated and 1.6 g of Te02 strong strong ppm 2 g of NaH, '2 g of gH2, 4 g 1.21 ppm of activated carbon and 3.2 g medium of Te02 1. 66 g of KH, 1 g of MgH2, 4 1.21 ppm g activated carbon and 1.6 g strong of Te02 0. 33 g of LiH, 1 g of MgH2, 1.22 ppm 4 g ¾e activated carbon and 1.6 medium g of Te02 1 g of NaH, 1 g of Mg, 4 g 1.21 ppm activated carbon and 3.5 g medium of NaMn04 8. 3 g of KH, 5 g of Mg, 20 g 1.21 ppm of activated carbon and 17.5 g strong of NaMn0 1. 66 g of KH, 1 g of Mg, 4 g 1.23 ppm of activated carbon and 2.0 g medium of SnF4 1. 66 g of KH, 1 g of Mg, 4 g 1.21 ppm activated carbon and 6.3 g medium of Snl4 1. 66 g of KH, 4 g of carbon 1.24 ppm very activated and 3.79 g of strong Snl2 lg of NaH, 1 g of Mg, 4 g of 1.22 ppm activated carbon and 1.57 g of strong SnF2 83 g of KH, 50 g of Mg, 200 1.23 ppm g of WC and 185 g of Snl2 medium 1 g of NaH, 1.66 g of Ca, 4 1.22 ppm very g of activated carbon and 1.34 strong g CuCl2 1 g of NaH, 1 g of Mg, 4 g 1.21 ppm of activated carbon and 0.96 g strong 1 of CuS 8. 3 g of KH + 5 g of Mg + 20 1.22 ppm g of CA 11-300 + 14.85 g of strength BaBr2 '5 g of NaH + 5 g of Mg + 20 1.22 ppm g of CA 11-300 + 14.85 g of medium BaBr2 20 g of activated carbon 3-3 1.22 ppm + 8.3 g of KH + 7.2 g of medium AgCl 3. 09 g of Mnl2 + 1.66 g of 1.25 ppm

Claims

CLAIMS 1. A source of energy characterized because it comprises: a reaction cell for the catalysis of atomic hydrogen to form a species of hydrogen having a total energy that is more negative and more stable to that of the uncatalyzed hydrogen species and compositions of matter comprising the species of hydrogen; a reaction vessel; a vacuum pump; a source of atomic hydrogen from a source in communication with the reaction vessel; a source of a hydrogen catalyst in communication with the reaction vessel, the source of at least one of the atomic hydrogen source and the hydrogen catalyst source comprises a reaction mixture of at least one reagent comprising the element or elements that form at least one of the atomic hydrogen and the hydrogen and at least one other element, whereby at least one of the atomic hydrogen and hydrogen catalyst is formed from the source, at least one other reagent to cause catalysis by effecting at least one function of activating and propagating the catalysis; Y a heater for the vessel that initiates the formation of at least one of atomic hydrogen and the hydrogen catalyst in the reaction vessel, and initiates the reaction to cause catalysis, whereby the catalysis of atomic hydrogen releases energy in an amount greater than about 300.kJ per mole of hydrogen during the catalysis of the hydrogen atom. 2. The energy source according to claim 1, characterized in that the reaction for causing the catalysis reaction comprises a reaction chosen from: (i) exothermic reactions that provide the activation energy for the catalysis reaction; (ii) coupled reactions that provide at least one of a source of catalyst or atomic hydrogen to support the catalysis reaction; (iii) free radical reactions that serve as an electron acceptor of the catalyst during the catalysis reaction; (iv) oxidation-reduction reactions that serve as an electron acceptor of the catalyst during the catalysis reaction; (v) exchange reactions that facilitate the action of the catalyst to become ionized as it accepts atomic hydrogen energy to form the hydrogen species, and (vi) Catalysis reactions aided by the rater, support or matrix. 3. The power source according to claim 1, characterized in that the reaction mixture comprises an electrically conductive support for enabling the catalysis reaction. 4. The energy source according to claim 1, characterized in that the reaction mixture comprises a solid, liquid or heterogeneous catalysis reaction mixture. 5. The energy source according to claim 2, characterized in that the reaction mixture comprises an oxidation-reduction reaction to cause the catalysis reaction comprising: (i) at least one catalyst chosen from Li, LiH, K, KH, Nati, Rb, RbH, Cs, and CsH; (ii) H2 gas, a source of H2 gas, or a hydride; (iii) at least one oxidant chosen from metal compounds comprising halides, phosphides, borides, oxides, hydroxide, silicides, nitrides, arsenides, selenides, teluluses, antimonides, carbides, sulfides, hydrides, carbonate, hydrogen carbonate, sulfates , hydrogen sulphates, phosphates, hydrogen phosphates, dihydrogen phosphates, nitrates, nitrites, permanganates, chlorates, perchlorates, chlorites, perclorites, hypochlorites,. bromates, perbromatos, bromitos, perbromitos, iodatos, periodatos, ioditos, perioditos, chromates, dichromates, teluratos, selenates, arsenates, silicates, borates, oxides of cobalt, oxides of tellurium and oxyanions of halogens, P, B, Si, N, As, S, Te, Sb, C, S, P, Mn, Cr, Co, and, Te; a transition metal, Sn, Ga, In, lead, germanium, alkali metal and alkaline earth metal compound; GeF2, GeCl2, GeBr2, Gel2, GeO, GeP, GeS, Gel4, and GeCl, fluorocarbon, CF4, CICF3, chlorocarbon, CC14, 02, MN03, MC10, M02, NF3, N20, NO, N02, a boron compound nitrogen such as B3N3H6, a sulfur compound such as SF6, S, SO2, S03, S205C12, F5SOF, M2S208, SxXy such as S2C12, SC12, S2Br2 or S2F2, CS2, SOxXy, SOCI2, SOF2, S02F2, SOBr2 ,. ??? '? , C1F5, XXX'Y0Z, C102F, C102F2, CIOF3, CIO3F, CIO2F3, boron-nitrogen compound, B3N3H6, Se, Te, Bi, As, Sb, Bi, TeXx, TeF4, TeF6, TeOx, Te02, Te03, SeXx , SeF6, SeOx, Se02 or Se03, a tellurium oxide, halide, tellurium compound, Te02, Te03, Te (OH) 6, TeBr2, TeCl2, TeBr4, TeCl4, TeF, Tel4, TeF6, CoTe, or NiTe, a composed of selenium, selenium oxide, selenium halide, selenium sulphide, Se02, Se03, Se2Br2, Se2Cl2, SeBr4, SeCl4, SeF4, SeF6, SeOBr2, SeOCl2, SeOF2, Se02F2, SeS2, Se2S6, Se4S4 or Se6S2 , P, P205, P2S5, PxXy, PF3, PCI3, PBr3, PI3, PF5, PCI5, PBrF, PC14F, POxXy, POBr3, P0I3, POCl3 or POF3, PSxXy, (M is an alkali metal, x, y and z are numbers integers, X and X 'are halogen) PSBr3, PSF3, PSCI3, a phosphorus-nitrogen compound, P3N5, (C12PN) 3, (C12PN), (Br2PN) x an arsenic compound, an arsenic oxide, arsenic halide, arsenic halide, arsenic selenide, arsenic telulide, AlAs, AS2I4, As2Se, AS4S4, AsBr3, AsCl3, AsF3, Asl3, As203, As2Se 3, As2S3, As2Te3, ASCI5, AsF5, As205, As2Ses, As2S5, an antimony compound, an antimony oxide, an antimony halide, an antimony sulfide, an antimony sulfate, an antimony selenide, an antimony arsenide , SbAs, SbBr3, SbCl3, SbF3, Sbl3, Sb203, SbOCl, Sb2Se3, Sb2 (S04) 3, Sb2S3, Sb2Te3, Sb204, SbCl5f SbF5, SbCl2F3, Sb205, Sb2S5, a bismuth compound, a bismuth oxide, a halide of bismuth, a bismuth sulfide, a bismuth selenide, BiAs04, BiBr3, BiCl3, BiF3, BiF5, Bi (0H) 3, Bil3, Bi203, BiOBr, BiOCl, BiOl, Bi2Se3 (Bi2S3, Bi2Te3, Bi204, SiCl4, SiBr4 , a transition metal halide, CrCl3, ZnF2, ZnBr2, ZnL2, MnCl2, MnBr2, nl2, CoBr2, CoI2, CoCl2, NiCl2, NiBr2, NiF2, FeF2, FeCl2, FeBr2, FeCl3 (TiF3, CuBr, CuBr2, VF3, CuCl2, a metal halide, SnF2, SnCl2, SnBr2, Snl2, SnF4, SnCl4, SnBr4, Snl4, InF, InCl, InBr, Inl, AgCl, Agl, AlF3 (AlBr3, All3, YF3, CdCl2, CdBr2, Cdl2, InCl3, ZrCl4, NbF5, TaCl5, M0Cl3, M0Cl5, NbCl5, AsCl3, TiBr4, SeCl2; SeCl4, InF3, InCl3, PbF4, Tel4, WC16, OsCl3, GaCl3, PtCl3, ReCl3, RhCl3, RuCl3, metal oxide, a metal hydroxide, Y203, FeO, Fe203 or NbO, NiO, Ni203 > SnO, Sn02, Ag20, AgO, Ga20, As203 Se02, Te02, In (0H) 3, Sn (0H) 2, In (0H) 3, Ga (0H) 3, Bi (0H) 3, C02, As2Se3, SF6 , S, SbF3, CF4, NF3, a metal permanganate, KMn04, NaMn04, P2Os, a metal nitrate, LÍNO3, NaN03, K 03, a boron halide, BBr3, BI3, a halide of group 13, a halide of indium, InBr2, InCl2, Inl3, a silver halide, AgCl, Agi, a lead halide, a cadmium halide, a zirconium halide, a transition metal oxide, a transition metal sulfide, or a halide of transition metal (Se, Ti, V, Cr, Mn, Fe, Co, Ni, Cu or Zn with F, Cl, Br or I), a halide of the second or third transition series, YF3, an oxide of the second or third transition series, sulfur of the second or third transition series, Y2S3, a halide of Y, Zr, b, Mo, Te, Ag, Cd, Hf, Ta, W, Os, such as NbX3, NbX5 or TaX5, Li2S, ZnS, FeS, NiS, MnS, Cu2S, CuS, SnS, an alkaline earth halide, BaBr2, BaCl2, Bal2, SrBr2, Srl2, CaBr2, Cal2, MgBr2 or Mgl2, a rare earth halide, EuBr 3, LaF3, LaBr3, CeBr3, GdF3, GdBr3, a rare earth halide with the metal in state II, Cel2, EuF2, EuCl, EuBr2, Eul2, Dyl2, Ndl2, Sml2, Ybl2 and Tml2, a metal boride, a Europium boride, a boride of MB2, CrB2, TiB2, MgB2, ZrB2, GdB2, an alkali halide, LiCl, RbCl, or Csl, a metal phosphide, such as Ca3P2, a noble metal halide, a noble metal oxide , a noble metal sulfide, PtCl2, PtBr2, Ptl2, PtCl4, PdCl2, PbBr2, Pbl2, a rare earth sulfide, CeS, a La halide, a Gd halide, a metal and an anion, Na2Te04, Na2Te03, Co (CN) 2, CoSb, CoAs, Co2P, CoO, CoSe, CoTe, NiSb, NiAs, NiSe, Ni2Si, MgSe, a rare earth telulide, .EuTe, a rare earth selenide, EuSe, a rare earth nitride, Eu, a metal nitride, AlN, GdN, Mg3N2, a compound containing at least two chosen oxygen atoms and different halogen atoms, F20, CI2O, C102, C1206; Cl207i C1F, CIF3, CIOF3, C1F5 C102F, C102F3, CIO3.F, BrF3, BrF5, I205, IBr, IC1, IC13, SI, IF3, IF5, IF7, a metal halide of second or third transition series, OsF6, PtF6 or IrFg, a compound that can form a metal after reduction, a metal hydride, a rare earth hydride, an alkaline earth hydride, or alkali hydride; (iv) at least one metal, alkaline, alkaline earth, transitional reducer, of the second and third transition series and rare earth metals, Al, Mg, MgH2, Si, La,?, · Zr , and powders of Ti, and H2, and (v) at least one electrically conductive support chosen from activated carbon, 1% Pt. o Pd on carbon (Pt / C, Pd / C), a carbide, Tic and WC. 6. The energy source according to claim 2, characterized in that "the reaction mixture comprises an oxidation-reduction reaction to cause the catalysis reaction comprises: (i) at least one catalyst or catalyst source comprising a metal or a hydride of the elements of Group I; (ii) at least one hydrogen source comprising H2 gas or a H2 gas source, or a hydride; (iii) at least one oxidant comprising an atom or ion or a compound comprising at least one of the elements of Groups 13, 14, 15, 16 and 17 chosen from F, Cl, Br, I, B, C, N, 0, Al, Si, P, S, Se and Te; (iv) at least one reducer, which comprises an element or hydride chosen from Mg, MgH2, Al, Si, B, Zr and a rare earth metal; Y (v) at least one electrically conductive support selected from carbon, activated carbon, graphene, carbon impregnated with a metal, Pt / C, Pd / C, a carbide, TiC and WC. 7. The energy source according to claim 2, characterized in that the reaction mixture comprising an oxidation-reduction reaction to cause the catalysis reaction comprises: (i) at least one catalyst or catalyst source comprising a metal or a hydride of the elements of Group I; (ii) at least one source of hydrogen comprising H 2 gas or a source of H 2 gas, or a hydride; (iii) at least one oxidant comprising a halide, oxide or sulfide compound of the selected elements of the Groups ??, HA, 3d, 4d, 5d, 6d, 7d, 8d, 9d, 10d, lid, 12d , and lanthanides; (iv) at least one reducing agent comprising an element or hydride selected from Mg, MgH2, 'Al, Si, B, Zr, and a rare earth metal; Y (v) at least one electrically conductive support selected from carbon, activated carbon, graphene, carbon impregnated with a metal such as Pt or Pd / C, a carbide, Tic and WC. 8. The source of energy . according to claim 2, characterized in that the exchange reaction to cause the catalysis reaction comprises an anion exchange between at least two of the oxidant, reductant and catalyst, wherein the anion is chosen from halide, hydride, oxide, sulfide, nitride, boride, carbide, silicide, arsenide, selenide, telulide, phosphide, nitrate, hydrogen sulfide, carbonate, sulfate, hydrogen sulfate, phosphate, hydrogen phosphate, dihydrogen phosphate, perchlorate, chromate, dichromate, cobalt oxide and oxyanions. 9. The power source according to claim 8, characterized in that the exchange reaction to cause the catalysis is thermally reversible to regenerate the initial exchange reagents. 10. The energy source according to claim 9, characterized in that the thermally regenerative reagents comprise: (i) at least one catalyst or catalyst source chosen from NaH and KH; (ii) a hydrogen source chosen from NaH, KH, and MgH2; (iii) at least one oxidant chosen from: (a) an alkaline earth metal halide selected from BaBr2, BaCl2, Bal2, CaBr2, MgBr2 and Mgl2; (b) a rare earth halide chosen from EuBr2, EuBr3 < EuF3, Dyl2, LaF3 and GdF3; (c) a metal halide of the second or third transition series chosen from YF3; (d) a metal boride chosen from CrB2 and TiB2; (e) an alkaline halide chosen from LiCl, RbCl and Csl; (f) a metal sulfide chosen from LiS, ZnS and Y2S3; (h) a metal oxide chosen from Y203, and (i) a metal phosphide selected from Ca3P2; (iv) at least one reducer chosen from Mg and MgH2; Y (v) at least one chosen support of activated carbon, TiC and WC. 11. The power source according to claim 2, characterized in that the catalysis reaction aided by the rarefactor, support or matrix to cause the catalysis reaction comprises at least one of a chemical environment for the catalysis reaction, acts to transfer electrons to facilitate the function of the H catalyst, it undergoes a reversible phase or other physical change or change in its electronic state, and binds to the hydrogen species product to increase at least one of the extent or speed of the catalysis reaction. 12. The power source according to claim 11, characterized in that the catalysis reaction assisted by the rarefactor, support or matrix can be thermally inverted to regenerate the initial exchange reagents. 13. The energy source according to claim 12, characterized in that the catalysis reaction assisted by the rarefactor, support or matrix comprises: (i) at least one catalyst or a catalyst source chosen from NaH and KH; (ii) a hydrogen source chosen from NaH, KH and Mg¾; (iii) at least one oxidant chosen from (a) a metal arsenide chosen from Mg3As2; Y (b) a selected metal nitride of Mg3N2 and AlN; (iv) at least one reducer chosen from Mg and MgH2; Y (v) at least one chosen support of activated carbon, Tic and WC. 14. The energy source according to claim 1, characterized in that the reaction mixture for causing the catalysis reaction comprises a catalyst comprising an alkali metal being regenerated from the products by separating one or more of the components and regenerating the alkali metal by electrolysis. 15. A hydride reactor characterized in that it comprises: a reaction cell for the catalysis of atomic hydrogen to form a hydrogen species having a total energy that is more negative and stable than that of the uncatalyzed hydrogen species and compositions of matter comprising the hydrogen species; a reaction vessel; an empty pump - a source of atomic hydrogen from a source in communication with the reaction vessel; a source of a hydrogen catalyst in communication with the reaction vessel, the source of at least one of the atomic hydrogen source and source of hydrogen catalyst comprising a reaction mixture of at least one reagent comprising the element or elements that form at least one of atomic hydrogen and hydrogen catalyst and at least one other element, whereby at least one of the atomic hydrogen and hydrogen catalyst is formed from the source, at least one other reagent to cause the catalysis by effecting at least one activation and propagation function of the catalysis; Y a heater for the vessel that initiates the formation of at least one of the atomic hydrogen and the hydrogen catalyst in the reaction vessel, and initiates the reaction to cause catalysis, by which catalysis of atomic hydrogen releases energy into a greater than about 300 kJ / mol of hydrogen during the catalysis of the hydrogen atom. 16. The hydride reactor according to claim 15, characterized in that the reaction mixture for the synthesis of the compounds comprises at least two selected species of the following kind of components (i) - (v): (i) a catalyst, (ii) a source of hydrogen, (iii) an oxidant, (iv) a reductant and (v) a support. 17. The hydride reactor according to claim 16, characterized in that the oxidant is chosen from sulfur, phosphorus, oxygen, SF6, S, SO2", SO3, S2O5CI2, F5SOF, M2S208, SxX and S2C12, SC12, S2Br2, S2F2, CS2, Sb2S5 / SOxXy / SOCI2, SOF2, SO2F2, SOBr2, -P, P205, P2S5, PxXy, PF3, PCI3, PBr3, PI3, PF5, PCI5, PBr4F, PC1F, POxXy, · POBr3, POI3, POCl3, POF3, PSxXy / PSBr3, PSF3, PSCI3, a phosphorus-nitrogen compound, P3N5, (C12PN) 3 or (C12PN) 4, (Br2PN) x (M is an alkali metal, x and y are integers, X is halogen), 02, N20, Y Te02, a halide, CF4, NF3, CrF2, a source of phosphorus, a source of sulfur, MgS, MHS (M is an alkali metal). 18 The hydride reactor according to claim 17, characterized in that the reaction mixture further comprises a rarefactor for the catalyzed hydrogen chosen from S, P, 0, Se elementals and Te, and compounds comprising S, P, 0, Se and Tea. 19. The power source according to claim 1, characterized in that the catalyst is able to accept atomic hydrogen energy in units of whole 27 2 of about 27. 2 eV + 0 5 eV and - ^ - eV ± 0. 5 eV. twenty . The power source according to claim 1, characterized in that the catalyst comprises an atom or M ion, where the ionization of t electrons of the atom or M ion each at a continuous energy level is such that the sum of ionization energies of the t 27 2 electrons is approximately one of m »27. 2 eV and m * - eF, where m is a whole number. twenty-one . The power source according to claim 1, characterized in that the catalyst consists of a diatomic molecule MH, wherein the breakdown of the MH bond plus the ionization of t electrons of the M atom each at a continuous energy level is such that the sum of the bonding energy and ionization energy of the t 27. 2 electrons is approximately one of m »27. 2 eV and m * - ^ - eV, where m is an integer. 22 The energy source according to claim 1, characterized in that the catalyst comprises atoms, ions and / or molecules chosen from molecules of AlH, BiH, C1H, CoH, GeH, InH, NaH, RuH, SbH, SeH, SiH, SnH , C2, N2, 02, C02, N02 and NO3, and atoms or ions of 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 +, Xe \ Ar2 + and H +, and Ne + and H +. 23. The power source according to claim 1, characterized in that it is put into operation continuously as the production and regeneration of energy are maintained in synchrony using electrolysis or thermal regeneration reactions. 24. The power source according to claim 1, characterized in that it also comprises an energy converter. 25. The power source according to claim 24, characterized in that the converter comprises a steam generator in communication with the reaction vessel, a steam turbine in communication with the steam generator, and an electric generator in communication with the turbine of steam. SUMMARY OF THE INVENTION A hydride reactor and power source is provided comprising a reaction cell for the catalysis of atomic hydrogen to form hydrins, a source of atomic hydrogen, a source of hydrogen catalyst comprising a solid, liquid or heterogeneous catalytic reaction mixture. . The catalysis reaction is activated or initiated and propagated by one or more other chemical reactions. These reactions maintained on an electrically conductive support can be of various kinds, such as (i) exothermic reactions that provide the activation energy for the hydrine catalysis reaction, (ii) coupled reactions that provide at least one of a source of catalyst or atomic hydrogen to support the reaction of hydride catalysis, (iii) free radical reactions that serve as an electron acceptor of the catalyst during the hydrine catalysis reaction, (iv) oxidation-reduction reactions that, in a mode, they serve as an electron acceptor of the catalyst during the hydrine catalysis reaction, (v) exchange reactions such as anion exchange that facilitate the action of the catalyst to become ionized as it accepts atomic hydrogen energy to form hydrinos, and ( vi) a hydrino reaction aided by a rarefactor, support or matrix that can provide at least one of a gave chemical environment for the hydrino reaction, act to transfer electrons to facilitate the function of the H catalyst, undergo a reversible phase change or other physical change or change in its. electronic state and binds to a lower energy hydrogen product to increase at least one of the hydrine extension or reaction rate. Power plants and chemical plants can be put into operation continuously using electrolysis or thermal regeneration reactions maintained in synchrony with at least one of energy production and chemical production of lower energy hydrogen.