KR20100017342A - Hydrogen-catalyst reactor - Google Patents

Abstract

A power source and hydride reactor is provided comprising a reaction cell for the catalysis of atomic hydrogen to form novel hydrogen species and compositions of matter comprising new forms of hydrogen, a source of atomic hydrogen, a source of a hydrogen catalyst comprising a reaction mixture of at least one reactant comprising the element or elements that form the catalyst and at least one other element, whereby the catalyst is formed from the source and 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.

Description

Hydrogen-Catalyst Reactor

Cross Reference to Related Application

The applicant claims the following advantages and what is disclosed in this application is incorporated herein by reference in its entirety:

(1) Application No. 60 / 913,556 filed on April 24, 2007; (2) Application No. 60 / 952,305 filed on July 27, 2007; (3) Application No. 60 / 954,426 filed on August 7, 2007; (4) Application No. 60 / 935,373 filed on August 9, 2007; (5) Application No. 60 / 955,465 filed on August 13, 2007; (6) Application No. 60 / 956,821 filed on August 20, 2007; (7) Application No. 60 / 957,540 filed on August 23, 2007; (8) Application No. 60 / 972,342 filed on September 14, 2007; (9) Application No. 60 / 974,191 filed on September 21, 2007; (10) Application No. 60 / 975,330 filed on September 26, 2007; (11) Application No. 60 / 976,004 filed on September 28, 2007; (12) Application No. 60 / 978,435 filed on October 9, 2007; (13) Application No. 60 / 987,552 filed on November 13, 2007; (14) Application No. 60 / 987,946 filed on November 14, 2007; (15) Application No. 60 / 989,677 filed on November 21, 2007; (16) Application No. 60 / 991,434 filed on November 30, 2007; (17) Application No. 60 / 991,974 filed on December 3, 2007; (18) Application No. 60 / 992,601 filed on December 5, 2007; (19) Application No. 61 / 012,717 filed on December 10, 2007; (20) Application No. 61 / 014,860 filed on December 19, 2007; (21) Application No. 61 / 016,790 filed on December 26, 2007; (22) Application No. 61 / 020,023 filed on January 9, 2008; (23) Application No. 61 / 021,205 filed on January 15, 2008; (24) Application No. 61 / 021,808 filed on January 17, 2008; (25) Application No. 61 / 022,112 filed on January 18, 2008; (26) Application No. 61 / 022,949 filed on January 23, 2008; (27) Application No. 61 / 023,297 filed on January 24, 2008; (28) Application No. 61 / 023,687 filed on January 25, 2008; (29) Application No. 61 / 024,730 filed on January 30, 2008; (30) Application No. 61 / 025,520 filed on February 1, 2008; (31) Application No. 61 / 028,605 filed on February 14, 2008; (32) Application No. 61 / 030,468 filed on February 21, 2008; (33) Application No. 61 / 064,453 filed on March 6, 2008; (34) Application No. 61 / xxx, xxx filed on March 21, 2008, and (35) Application No. 61 / xxx, xxx filed on April 17, 2008.

Technology of the invention

1. Field of the Invention

(p≤137이 정수임)이 수소 여기 상태를 위한 리드베리 방정식에서 잘 알려진 변수인 n=정수를 대체한다. He+, Ar+ 및 K는 촉매로서 기능할 것으로 예측되는데, 왜냐하면 이들의 화학 또는 물리적 공정의 엔탈피 변화가 수소 원자의 포텐셜 에너지인 27.2 eV의 정수배와 같아서, 촉매 조건(catalyst criterion)을 충족시키기 때문이다. 에너지 준위에 관한 닫힌 형태(closed-form) 방정식에 근거한 특정 예측들을 시험하였다. 예를 들면, 두 개의 H(1/p)은 반응하여, 촉매화되지 않은 수소 원자를 포함하는 H2의 P2배의 진동 및 회전 에너지를 갖는 H2(1/p)을 형성할 수 있다. 대기압 전자빔 여기 아르곤-수소 플라즈마로부터 145-300 nm 영역에서 회전선들이 관찰되었다. 수소의 42배의 전례가 없는 에너지 간격(spacing)이 핵간 거리가 H2의 1/4임을 입증하였고, 임을 확인하였다.* Papers incorporated herein by reference, R. Mills, J. He, Z. Chang, W. Good, Y. Lu, B. Dhandapani, "Catalysis of Atomic Hydrogen to Novel Hydrogen Species H- (1/4) ) and H2 (1/4) as a New Power Source ", Int. J. Hydrogen Energy, Vol. 32, no. 12, (2007), pp. As disclosed in 2573-2584, the data obtained from a wide range of irradiation techniques suggest that hydrogen can be present in a low energy state that was once thought possible. Predicted reactions include the transfer of resonant, non-radioactive energy from stable hydrogen atoms to catalysts that can accept energy. The product is H (1 / p) in the Rydberg fractional state of hydrogen atoms, where

(p ≦ 137 is an integer) replaces n = integer, a well known variable in the Lidbury equation for hydrogen excited states. He +, Ar + and K are expected to function as catalysts because their enthalpy change in their chemical or physical processes is equal to an integral multiple of 27.2 eV, the potential energy of the hydrogen atom, to meet the catalyst criterion. Specific predictions based on closed-form equations for energy levels were tested. For example, two H (1 / p) can react to form H2 (1 / p) with vibration and rotational energy P2 times that of H2 containing uncatalyzed hydrogen atoms. Rotational lines were observed in the 145-300 nm region from the atmospheric electron beam excitation argon-hydrogen plasma. An unprecedented energy spacing of 42 times that of hydrogen proved that the internuclear distance was 1/4 of H2.

The product of the predicted alkali catalyst K is H- (1 / p), which can form KH * X, a novel alkali halide (X) hydride compound, and H2 (1/4), which can be trapped in the crystals. . The 1 H MAS NMR spectrum of the new compound KH * Cl relative to external tetramethylsilane (TMS) showed a large and clear upfield resonance at -4.4 ppm, corresponding to an absolute resonance shift of -35.9 ppm. This is consistent with the theoretical prediction of H- (1 / p) with p = 4. The predicted frequencies of ortho and para-H2 (1/4) were at 1943 cm-1 and 2012 cm-1 in the high resolution FTIR spectrum of KH * I with a -4.6 ppm NMR peak assigned to H- (1/4). Was observed. The 1943/2012 cm-1-strength ratio was consistent with the characteristic 3: 1 ortho: para-peak-intensity ratio, and the 69 cm-1 ortho-para splitting was consistent with that predicted. KH * Cl with H- (1/4) by NMR was commonly present in 12.5 KeV electron beams that excited similar emission of gap H2 (1/4), as observed in argon-hydrogen plasma. As sources of K catalyst and atomic hydrogen, KNO3 and Raney nickel, respectively, were used to produce the corresponding exothermic reactions. The energy balance was ΔH = 17,925 kcal / mole KNO3, about 300 times that expected for the KNO3 chemical reaction, which is known to be the most intense due to the combustion between hydrogen and atmospheric oxygen, and -57.8 kcal / mole H2, which is the theoretical maximum enthalpy. 60 times greater than -3585 kcal / mole H2. The reduction of KNO3 to water, potassium metal and NH3, calculated from the heat of production, only released -14.2 kcal / mole H2, which could not explain the observed heat or hydrogen combustion. However, the results are consistent with the formation of H- (1/4) and H2 (1/4) with a production enthalpy of at least 100 times the combustion.

In embodiments, the present invention includes reactors and power sources that form low energy hydrogen species and compounds. The invention further comprises a catalyst reaction mixture providing the catalyst and atomic hydrogen. Preferred atomic catalysts are lithium, potassium, and cesium atoms. Preferred molecular catalyst is NaH.

Hydrino

The binding energy given by

(1)

(One)

Hydrogen atoms having (p is an integer greater than 1, preferably 2 to 137) are disclosed in the following documents:

R. L. Mills, "The Grand Unified Theory of Classical Quantum Mechanics", October 2007 Edition, (posted at http://www.blacklightpower.com/theory/book.shtml); R. Mills, The Grand Unified Theory of Classical Quantum Mechanics, May 2006 Edition, BlackLight Power, Inc., provided by BlackLight Power, Inc., 493 Old Trenton Road, Cranbury, NJ, 08512 (posted at www.blacklightpower.com). , Cranbury, New Jersey, ("'06 Mills GUT"); R. Mills, The Grand Unified Theory of Classical Quantum Mechanics, January 2004 Edition, BlackLight Power, Inc., Cranbury, New Jersey, provided by BlackLight Power, Inc., 493 Old Trenton Road, Cranbury, NJ, 08512. 04 Mills GUT "); R. Mills, The Grand Unified Theory of Classical Quantum Mechanics, September 2003 Edition, BlackLight Power, Inc., Cranbury, NewJersey, provided by BlackLight Power, Inc., 493 Old Trenton Road, Cranbury, NJ, 08512. 03 Mills GUT "); R. Mills, The Grand Unified Theory of Classical Quantum Mechanics, September 2002 Edition, BlackLight Power, Inc., Cranbury, New Jersey, provided by BlackLight Power, Inc., 493 Old Trenton Road, Cranbury, NJ, 08512. 02 Mills GUT "); R. Mills, The Grand Unified Theory of Classical Quantum Mechanics, September 2001 Edition, BlackLight Power, Inc., Cranbury, NewJersey, Distributed by Amazon, provided by BlackLight Power, Inc., 493 Old Trenton Road, Cranbury, NJ, 08512. .com ("'01 Mills GUT"); R. Mills, The Grand Unified Theory of Classical Quantum Mechanics, January 2000 Edition, BlackLight Power, Inc., Cranbury, NewJersey, Distributed by Amazon, provided by BlackLight Power, Inc., 493 Old Trenton Road, Cranbury, NJ, 08512. .com ("'00 Mills GUT"); R. L. Mills, "Physical Solutions of the Nature of the Atom, Photon, and Their Interactions to Form Excited and Predicted Hydrino States," Physics Essay, inpress; R. L. Mills, "Exact Classical Quantum Mechanical Solution for Atomic Helium which Predicts Conjugate Parameters from a Unique Solution for the First Time," Physics Essays, inpress; R. L. Mills, P. Ray, B. Dhandapani, "Excessive Balmer Line Broadening of Water-Vapor Capacitively-Coupled RF Discharge Plasmas," International Journal of Hydrogen Energy, Vol. 33, (2008), 802 815; R. L. Mills, J. He, M. Nansteel, B. Dhandapani, "Catalysis of Atomic Hydrogen to New Hydrides as a New Power Source,"; R. L. Mills, H. Zea, J. He, B. Dhandapani, "Water Bath Calorimetry on a Catalytic Reaction of Atomic Hydrogen,"; J. Phillips, C. K. Chen, R. L. Mills, "Evidence of Catalytic Production of Hot Hydrogen in RF-Generated Hydrogen / Argon Plasmas,"; R. L. Mills, J. He, Y. Lu, M. Nansteel, Z. Chang, B. Dhandapani, "Comprehensive Identification and Potential Applications of New States of Hydrogen," Int. J. Hydrogen Energy, Vol. 32 (14), (2007), 29883009; RL Mills, J. He, Z. Chang, W. Good, Y. Lu, B. Dhandapani, "Catalysis of Atomic Hydrogen to Novel Hydrogen Species H- (1/4) and H2 (1/4) as a New Power Source, "Int. J. Hydrogen Energy, Vol. 32 (13), (2007), pp. 25732584; R. L. Mills, "Maxwell's Equations and QED: Which is Fact and Which is Fiction," Physics Essays, Vol. 19, (2006), 225 262; R. L. Mills, P. Ray, B. Dhandapani, Evidence of an energy transfer reaction between atomic hydrogen and argon II or helium II as the source of excessively hot H atoms in radio-frequency plasmas, J. Plasma Physics, Vol. 72, No. 4, (2006), 469 484; R. L. Mills, "Exact Classical Quantum Mechanical Solutions for One-through Twenty-Electron Atoms," Physics Essays, Vol. 18, (2005), 321361; R. L. Mills, P. C. Ray, R. M. Mayo, M. Nansteel, B. Dhandapani, J. Phillips, "Spectroscopic Study of Unique Line Broadening and Inversion in Low Pressure Microwave Generated Water Plasmas," J. Plasma Physics, Vol. 71, No 6, (2005), 877 888; R. L. Mills, "The Fallacy of Feynman's Argument on the Stability of the Hydrogen Atom According to Quantum Mechanics," Ann. Fund. Louis de Broglie, Vol. 30, no. 2, (2005), pp. 129151; R. L. Mills, B. Dhandapani, J. He, "Highly Stable Amorphous Silicon Hydride from a Helium Plasma Reaction," Materials Chemistry and Physics, 94/23, (2005), 298307; R. L. Mills, J. He, Z, Chang, W. Good, Y. Lu, B. Dhandapani, "Catalysis of Atomic Hydrogen to Novel Hydrides as a New Power Source," Prepr. Pap.Am. Chem. Soc. Conf., Div. Fuel Chem., Vol. 50, no. 2, (2005); RL Mills, J. Sankar, A. Voigt, J. He, P. Ray, B. Dhandapani, "Role of Atomic Hydrogen Density and Energy in Low Power CVD Synthesis of Diamond Films," Thin Solid Films, 478, (2005) 7790; R. L. Mills, "The Nature of the Chemical Bond Revisited and an Alternative Maxwellian Approach," Physics Essays, Vol. 17, (2004), 342389; R. L. Mills, P. Ray, "Stationary Inverted Lyman Population and a Very Stable Novel Hydride Formed by a Catalytic Reaction of Atomic Hydrogen and Certain Catalysts," J. Opt. Mat., 27, (2004), 181 186; W. Good, P. Jansson, M. Nansteel, J. He, A. Voigt, "Spectroscopic and NMR Identification of Novel Hydride Ions in Fractional Quantum Energy States Formed by an Exothermic Reaction of Atomic Hydrogen with Certain Catalysts," European Physical Journal Applied Physics, 28, (2004), 83104; J. Phillips, R. L. Mills, X. Chen, "Water Bath Calorimetric Study of Excess Heat in 'Resonance Transfer' Plasmas," J. Appl. Phys., Vol. 96, No. 6, (2004) 30953102; RL Mills, Y. Lu, M. Nansteel, J. He, A. Voigt, W. Good, B. Dhandapani, "Energetic Catalyst-Hydrogen Plasma Reaction as a Potential New Energy Source," Division of Fuel Chemistry, Session: Advances in Hydrogen Energy, Prepr. Pap.Am. Chem. Soc. Conf., Vol. 49, no. 2, (2004); R. L. Mills, J. Sankar, A. Voigt, J. He, B. Dhandapani, "Synthesis of HDLC Films from Solid Carbon," J. Materials Science, J. Mater. Sci. 39 (2004) 33093318; RL Mills, Y. Lu, M. Nansteel, J. He, A. Voigt, B. Dhandapani, "Energetic Catalyst-Hydrogen Plasma Reaction as a Potential New Energy Source," Division of Fuel Chemistry, Session: Chemistry of Solid, Liquid , and Gaseous Fuels, Prepr. Pap.Am. Chem. Soc. Conf., Vol. 49, no. 1, (2004); R. L. Mills, "Classical Quantum Mechanics," Physics Essays, Vol. 16, (2003), 433498; R. L. Mills, P. Ray, M. Nansteel, J. He, X. Chen, A. Voigt, B. Dhandapani, "Characterization of an Energetic Catalyst-Hydrogen Plasma Reaction as a Potential New Energy Source," Am. Chem. Soc. Div. Fuel Chem. Prepr., Vol. 48, No. 2, (2003); RL Mills, J. Sankar, A. Voigt, J. He, B. Dhandapani, "Spectroscopic Characterization of the Atomic Hydrogen Energies and Densities and Carbon Species During Helium-Hydrogen-Methane Plasma CVD Synthesis of Diamond Films," Chemistry of Materials, Vol. 15, (2003), pp. 13131321; R. L. Mills, P. Ray, "Extreme Ultraviolet Spectroscopy of Helium-Hydrogen Plasma," J. Phys. D, Applied Physics, Vol. 36, (2003), pp. 15351542; R. L. Mills, X. Chen, P. Ray, J. He, B. Dhandapani, "Plasma Power Source Based on a Catalytic Reaction of Atomic Hydrogen Measured by Water Bath Calorimetry," Thermochimica Acta, Vol. 406/12, (2003), pp. 3553; R. L. Mills, B. Dhandapani, J. He, "Highly Stable Amorphous Silicon Hydride," Solar Energy Materials & Solar Cells, Vol. 80, no. 1, (2003), pp. 120; R. L. Mills, P. Ray, R. M. Mayo, "The Potential for a Hydrogen Water-Plasma Laser," Applied Physics Letters, Vol. 82, No. 11, (2003), pp. 16791681; R. L. Mills, P. Ray, "Stationary Inverted Lyman Population Formed from Incandescently Heated Hydrogen Gas with Certain Catalysts," J. Phys. D, Applied Physics, Vol. 36, (2003), pp. 15041509; R. L. Mills, P. Ray, B. Dhandapani, J. He, "Comparison of Excessive Balmer α Line Broadening of Inductively and Capacitively Coupled RF, Microwave, and Glow Discharge Hydrogen Plasmas with Certain Catalysts," IEEE Transactions on Plasma Science, Vol. 31, No. (2003), pp. 338355; R. L. Mills, P. Ray, R. M. Mayo, "CW HI Laser Based on a Stationary Inverted Lyman Population Formed from Incandescently Heated Hydrogen Gas with Certain Group I Catalysts," IEEE Transactions on Plasma Science, Vol. 31, No. 2, (2003), pp. 236247; R. L. Mills, P. Ray, J. Dong, M. Nansteel, B. Dhandapani, J. He, "Spectral Emission of Fractional-Principal-Quantum-Energy-Level Atomic and Molecular Hydrogen," Vibrational Spectroscopy, Vol. 31, No. 2, (2003), pp. 195213; H. Conrads, R. L. Mills, Th. Wrubel, "Emission in the Deep Vacuum Ultraviolet from a Plasma Formed by Incandescently Heating Hydrogen Gas with Trace Amounts of Potassium Carbonate," Plasma Sources Science and Technology, Vol. 12, (2003), pp. 389395; R. L. Mills, J. He, P. Ray, B. Dhandapani, X. Chen, "Synthesis and Characterization of a Highly Stable Amorphous Silicon Hydride as the Product of a Catalytic Helium-Hydrogen Plasma Reaction," Int. J. Hydrogen Energy, Vol. 28, No. 12, (2003), pp. 14011424; R. L. Mills, P. Ray, "A Comprehensive Study of Spectra of the Bound-Free Hyperfine Levels of Novel Hydride Ion H- (1/2), Hydrogen, Nitrogen, and Air," Int. J. Hydrogen Energy, Vol. 28, No. 8, (2003), pp. 825871; R. L. Mills, M. Nansteel, and P. Ray, "Excessively Bright Hydrogen-Strontium Plasma Light Source Due to Energy Resonance of Strontium with Hydrogen," J. Plasma Physics, Vol. 69, (2003), pp. 131158; R. L. Mills, "Highly Stable Novel Inorganic Hydrides," J. New Materials for Electrochemical Systems, Vol. 6, (2003), pp. 4554; R. L. Mills, P. Ray, "Substantial Changes in the Characteristics of a Microwave Plasma Due to Combining Argon and Hydrogen," New Journal of Physics, www.njp.org, Vol. 4, (2002), pp. 22.122.17; R. M. Mayo, R. L. Mills, M. Nansteel, "Direct Plasmadynamic Conversion of Plasma Thermal Power to Electricity," IEEE Transactions on Plasma Science, October, (2002), Vol. 30, no. 5, pp. 20662073; R. L. Mills, M. Nansteel, P. Ray, "Bright Hydrogen-Light Source due to a Resonant Energy Transfer with Strontium and Argon Ions," New Journal of Physics, Vol. 4, (2002), pp. 70.170.28; R. M. Mayo, R. L. Mills, M. Nansteel, "On the Potential of Direct and MHD Conversion of Power from a Novel Plasma Source to Electricity for Microdistributed Power Applications," IEEE Transactions on Plasma Science, August, (2002), Vol. 30, no. 4, pp. 15681578; R. M. Mayo, R. L. Mills, "Direct Plasmadynamic Conversion of Plasma Thermal Power to Electricity for Microdistributed Power Applications," 40th Annual Power Sources Conference, Cherry Hill, NJ, June 1013, (2002), pp. 14; R. L. Mills, E. Dayalan, P. Ray, B. Dhandapani, J. He, "Highly Stable Novel Inorganic Hydrides from Aqueous Electrolysis and Plasma Electrolysis," Electrochimica Acta, Vol. 47, No. 24, (2002), pp. 39093926; R. L. Mills, P. Ray, B. Dhandapani, R. M. Mayo, J. He, "Comparison of Excessive Balmer α Line Broadening of Glow Discharge and Microwave Hydrogen Plasmas with Certain Catalysts," J. of Applied Physics, Vol. 92, No. 12, (2002), pp. 70087022; R. L. Mills, P. Ray, B. Dhandapani, M. Nansteel, X. Chen, J. He, "New Power Source from Fractional Quantum Energy Levels of Atomic Hydrogen that Surpasses Internal Combustion," J. Mol. Struct., Vol. 643, No. 13, (2002), pp. 4354; R. L. Mills, J. Dong, W. Good, P. Ray, J. He, B. Dhandapani, "Measurement of Energy Balances of Noble Gas-Hydrogen Discharge Plasmas Using Calvet Calorimetry," Int. J. Hydrogen Energy, Vol. 27, No. 9, (2002), pp. 967978; R. L. Mills, P. Ray, "Spectroscopic Identification of a Novel Catalytic Reaction of Rubidium Ion with Atomic Hydrogen and the Hydride Ion Product," Int. J. Hydrogen Energy, Vol. 27, No. 9, (2002), pp. 927935; R. L. Mills, A. Voigt, P. Ray, M. Nansteel, B. Dhandapani, "Measurement of Hydrogen Balmer Line Broadening and Thermal Power Balances of Noble Gas-Hydrogen Discharge Plasmas," Int. J. Hydrogen Energy, Vol. 27, No. 6, (2002), pp. 671685; R. L. Mills, N. Greenig, S. Hicks, "Optically Measured Power Balances of Glow Discharges of Mixtures of Argon, Hydrogen, and Potassium, Rubidium, Cesium, or Strontium Vapor," Int. J. Hydrogen Energy, Vol. 27, No. 6, (2002), pp. 651670; R. L. Mills, "The Grand Unified Theory of Classical Quantum Mechanics," Int. J. Hydrogen Energy, Vol. 27, No. 5, (2002), pp. 565590; R. L. Mills, P. Ray, "Vibrational Spectral Emission of Fractional-Principal-Quantum-Energy-Level Hydrogen Molecular Ion," Int. J. Hydrogen Energy, Vol. 27, No. 5, (2002), pp. 533564; R. L. Mills and M. Nansteel, P. Ray, "Argon-Hydrogen-Strontium Discharge Light Source," IEEE Transactions on Plasma Science, Vol. 30, no. 2, (2002), pp. 639653; R. L. Mills, P. Ray, "Spectral Emission of Fractional Quantum Energy Levels of Atomic Hydrogen from a Helium-Hydrogen Plasma and the Implications for Dark Matter," Int. J. Hydrogen Energy, (2002), Vol. 27, No. 3, pp. 301322; R. L. Mills, P. Ray, "Spectroscopic Identification of a Novel Catalytic Reaction of Potassium and Atomic Hydrogen and the Hydride Ion Product," Int. J. Hydrogen Energy, Vol. 27, No. 2, (2002), pp. 183192; RL Mills, E. Dayalan, "Novel Alkali and Alkaline Earth Hydrides for High Voltage and High Energy Density Batteries," Proceedings of the 17th Annual Battery Conference on Applications and Advances, California State University, Long Beach, CA, (January 1518, 2002 ), pp. 16; R. L. Mills, W. Good, A. Voigt, Jinquan Dong, "Minimum Heat of Formation of Potassium Iodo Hydride," Int. J. Hydrogen Energy, Vol. 26, No. 11, (2001), pp. 11991208; R. L. Mills, "The Nature of Free Electrons in Superfluid Heliuma Test of Quantum Mechanics and a Basis to Review its Foundations and Make a Comparison to Classical Theory," Int. J. Hydrogen Energy, Vol. 26, No. 10, (2001), pp. 10591096; R. L. Mills, "Spectroscopic Identification of a Novel Catalytic Reaction of Atomic Hydrogen and the Hydride Ion Product," Int. J. Hydrogen Energy, Vol. 26, No. 10, (2001), pp. 10411058; R. L. Mills, B. Dhandapani, M. Nansteel, J. He, A. Voigt, "Identification of Compounds Containing Novel Hydride Ions by Nuclear Magnetic Resonance Spectroscopy," Int. J. Hydrogen Energy, Vol. 26, No. 9, (2001), pp. 965979; R. L. Mills, T. Onuma, and Y. Lu, "Formation of a Hydrogen Plasma from an Incandescently Heated Hydrogen-Catalyst Gas Mixture with an Anomalous Afterglow Duration," Int. J. Hydrogen Energy, Vol. 26, No. 7, July, (2001), pp. 749762; R. L. Mills, "Observation of Extreme Ultraviolet Emission from Hydrogen-KI Plasmas Produced by a Hollow Cathode Discharge," Int. J. Hydrogen Energy, Vol. 26, No. 6, (2001), pp. 579592; R. L. Mills, B. Dhandapani, M. Nansteel, J. He, T. Shannon, A. Echezuria, “Synthesis and Characterization of Novel Hydride Compounds,” Int. J. of Hydrogen Energy, Vol. 26, No. 4, (2001), pp. 339367; R. L. Mills, "Temporal Behavior of Light-Emission in the Visible Spectral Range from a Ti-K2CO3-H-Cell," Int. J. Hydrogen Energy, Vol. 26, No. 4, (2001), pp. 327332; R. L. Mills, M. Nansteel, and Y. Lu, "Observation of Extreme Ultraviolet Hydrogen Emission from Incandescently Heated Hydrogen Gas with Strontium that Produced an Anomalous Optically Measured Power Balance," Int. J. Hydrogen Energy, Vol. 26, No. 4, (2001), pp. 309326; R. L. Mills, "BlackLight Power Technology A New Clean Hydrogen Energy Source with the Potential for Direct Conversion to Electricity," Proceedings of the National Hydrogen Association, 12th Annual U.S. Hydrogen Meeting and Exposition, Hydrogen: The Common Thread, The Washington Hilton and Towers, Washington DC, (March 68, 2001), pp. 671697; R. L. Mills, "The Grand Unified Theory of Classical Quantum Mechanics," Global Foundation, Inc. Orbis Scientiae entitled The Role of Attractive and Repulsive Gravitational Forces in Cosmic Acceleration of Particles The Origin of the Cosmic Gamma Ray Bursts, (29th Conference on High Energy Physics and Cosmology Since 1964). Behram N. Kursunoglu, Chairman, December 1417, 2000, Lago Mar Resort, Fort Lauderdale, FL, Kluwer Academic / Plenum Publishers, New York, pp. 243258; R. L. Mills, B. Dhandapani, N. Greenig, J. He, "Synthesis and Characterization of Potassium Iodo Hydride," Int. J. of Hydrogen Energy, Vol. 25, Issue 12, December, (2000), pp. 11851203; R. L. Mills, "The Hydrogen Atom Revisited," Int. J. of Hydrogen Energy, Vol. 25, Issue 12, December, (2000), pp. 11711183; R. L. Mills, "BlackLight Power Technology A New Clean Energy Source with the Potential for Direct Conversion to Electricity," Global Foundation International Conferenceon "Global Warming and Energy Policy," BehramN. Kursunoglu, Chairman, Fort Lauderdale, FL, November 2628, 2000, Kluwer Academic / Plenum Publishers, New York, pp. 187202; R. L. Mills, J. Dong, Y. Lu, "Observation of Extreme Ultraviolet Hydrogen Emission from Incandescently Heated Hydrogen Gas with Certain Catalysts," Int. J. Hydrogen Energy, Vol. 25, (2000), pp. 919943; R. L. Mills, "Novel Inorganic Hydride," Int. J. of Hydrogen Energy, Vol. 25, (2000), pp. 669683; R. L. Mills, "Novel Hydrogen Compounds from a Potassium Carbonate Electrolytic Cell," Fusion Technol., Vol. 37, No "Fractional Quantum Energy Levels of Hydrogen," Fusion Technology, Vol. 28, No. 4, November, (1995), pp. 16971719; R. L. Mills, W. Good, R. Shaubach, "Dihydrino Molecule Identification," Fusion Technol., Vol. 25, (1994), 103; R. L. Mills and S. Kneizys, Fusion Technol. Vol. 20, (1991), 65; And PCT application numbers previously published. WO 90/13126; WO 92/10838; WO 94/29873; WO 96/42085; WO 99/05735; WO 99/26078; WO 99/34322; WO 99/35698; WO 00/07931; WO 00/07932; WO 01/095944; WO 01/18948; WO 01/21300; WO 01/22472; WO 01/70627; WO 02/087291; WO 02/088020; WO 02/16956; WO 03/093173; WO 03/066516; WO 04/092058; WO 05/041368; WO 05/067678; WO 2005/116630; WO 2007/051078; And WO 2007/053486; And US Pat. Nos. 6,024,935 and 7,188,033. All of these disclosures are incorporated herein by reference ("Mills prior art").

(여기서, aH는 일반적인 수소 원자의 반지름이고 p는 정수임)인 하이드리노에 대한 표시는

이다. 반지름 aH를 갖는 수소 원자는 이하에서 "일반적인 수소 원자" 또는 "정상적인 수소 원자"라고 지칭한다. 일반적인 수소 원자는 결합 에너지가 13.6 eV인 것을 특징으로 한다. The binding energy of an atom, ion or molecule, also known as ionization energy, is the energy required to remove one electron from an atom, ion or molecule. The hydrogen atom having the binding energy given in the formula (1) is hereinafter referred to as hydrino atom or hydrino. Radius

The indication for hydrino, where aH is the radius of a common hydrogen atom and p is an integer,

to be. Hydrogen atoms having a radius aH are hereinafter referred to as "general hydrogen atoms" or "normal hydrogen atoms". Typical hydrogen atoms are characterized by a binding energy of 13.6 eV.

Hydrino is a common hydrogen atom

m · 27.2 eV (2)

It is formed by reacting with a catalyst having a net reaction enthalpy of where m is an integer. This catalyst was referred to as a source of energy holes or energy holes in Mills' previously filed patent application. The rate of catalysis is believed to increase as the net reaction enthalpy approaches m · 27.2 eV. It has been found that catalysts with a net reaction enthalpy within ± 10%, preferably ± 5% of m · 27.2 eV, are suitable for most applications.

This catalysis releases energy from the hydrogen atoms as the size of the hydrogen atoms, rn = naH, is moderately reduced. For example, catalysis of H (n = 1) to H (n = 1/2) releases 40.8 eV and the hydrogen radius is reduced from aH to 1/2 aH. In the catalyst system, t electrons are ionized from one atom and provided at each continuum energy level such that the sum of the ionization energies of the t electrons is approximately m · 27.2 eV (m is an integer).

One such catalyst system comprises lithium metal. The primary and secondary ionization energies of lithium are 5.39172 eV and 75.64018 eV, respectively [1]. And the divalent ionization (t = 2) reaction in which Li is Li2 + has a net reaction enthalpy of 81.0319 eV, which is the same as m = 3 in formula (2).

(3)

(3)

(4)

And the overall reaction is:

(5)

(5)

In another embodiment, the catalyst system comprises cesium. The primary and secondary ionization energies of cesium are 3.89390 eV and 23.15745 eV, respectively. And, the divalent ionization (t = 2) reaction where Cs becomes Cs2 + has a net reaction enthalpy of 27.05135 eV, which is equivalent to m = 1 in equation (2).

(6)

(6)

(7)

(7)

And the overall reaction is:

(8)

(8)

Another catalyst system includes potassium metal. The primary, secondary and tertiary ionization energies of potassium are 4.34066 eV, 31.63 eV, and 45.806 eV [1]. And, the trivalent ionization (t = 3) reaction in which K is K3 + has a net reaction enthalpy of 81.7767 eV, which is the same as m = 3 in Equation (2).

(9)

(9)

(10)

10

And the overall reaction is as follows:

(11)

(11)

As with the power source, the energy released during catalysis is much greater than the energy absorbed by the catalyst. The release energy is large compared to conventional chemical reactions. For example, when hydrogen and oxygen gas are burned to form water,

(12)

(12)

Known water formation enthalpy is ΔHf = -286 kJ / mole or 1.48 eV per hydrogen atom. On the other hand, each catalyzed (n = 1) common hydrogen atom emits a net enthalpy of 40.8 eV. Moreover, additional catalytic transfer can occur:

등. 일단 촉매작용이 시작되면, 하이드리노는 추가로 불균형(disproportionation)이라 불리는 과정에서 자가촉매작용을 한다. 상기 메커니즘은 무기 이온 촉매작용의 메커니즘과 유사하다. 하지만, 하이드리노 촉매작용은 엔탈피가 m·27.2 eV에 더 잘 매치되므로 무기 이온 촉매작용에 비해 반응 속도가 빠르다.

Etc. Once catalysis begins, the hydrinos self-catalyze in a process called disproportionation. The mechanism is similar to that of inorganic ion catalysis. However, the hydrino catalysis is faster than the inorganic ion catalysis because the enthalpy matches m · 27.2 eV better.

Additional Catalytic Product of the Invention

(여기서, n은 1/p이고, p는 1보다 큰 정수임)의 결합 에너지를 갖는 수소 원자와 반응함으로써 형성될 수 있다. 상기 하이드리노 수소화물 이온은 H-(n=1/p) 또는 H-(1/p)로 표현된다. Hydrino hydride ions of the invention have an electron source of hydrino, ie, about

It can be formed by reacting with a hydrogen atom having a binding energy of (where n is 1 / p and p is an integer greater than 1). The hydrino hydride ions are represented by H- (n = 1 / p) or H- (1 / p).

(13)

(13)

(14)

(14)

Hydrino hydride ions are distinguished from common hydride ions containing a common hydrogen nucleus and two electrons having a binding energy of about 0.8 eV. The latter is referred to hereinafter as "common hydride ions" or "normal hydride ions". Hydrino hydride ions include a hydrogen nucleus including proteum, deuterium or tritium, and two indistinguishable electrons in the binding energy according to formula (15).

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

(15)

(15)

에 의해 주어진 감소된 전자 질량이고, 여기서, mp는 양자의 질량이고, aH는 수소 원자의 반지름이며, a0는 보어(Bohr) 반지름이고, e는 기본 전하이다. 상기 반지름들은 하기에 의해 주어진다. Where p is an integer greater than 1, s = 1/2, π is pi, h is Planck's constant bar, μ0 is vacuum permeability, me is mass of electrons, μe is

Is the reduced electron mass given by, where mp is the mass of protons, aH is the radius of the hydrogen atom, a0 is the Bohr radius, and e is the basic charge. The radii are given by

(16)

(16)

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

According to the invention, having a binding energy according to formula (15-16), which is larger than the bond of a typical hydride ion (about 0.8 eV) when p = 2 to 23, and smaller than when p = 24 (H−) Hydrino hydride ions (H-) are provided. In the case of p = 2 to p = 24 in the formula (15-16), the binding energy of the hydride ions is 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. Also provided are compositions comprising the novel hydride ions.

Hydrino ions are distinguished from common hydrogen ions comprising a common hydrogen nucleus and two electrons having a binding energy of about 0.8 eV. The latter is referred to hereinafter as "general hydrogen ions" or "normal hydrogen ions". Hydrino hydride ions include two indistinguishable electrons in a hydrogen nucleus including proteum, deuterium, or tritium and binding energy according to formula (15-16).

New compounds are provided that include one or more hydrino hydrate ions and one or more other elements. Such compounds are referred to as hydrino hydride compounds.

Common hydrogen species include the following binding energies: (A) hydride ions, 0.754 eV (“common hydride ions”); (b) hydrogen atom (“common hydrogen atom”), 13.6 eV; (c) diatomic hydrogen molecules, 15.3 eV (“general hydrogen molecules”); (d) hydrogen molecular ions, 16.3 eV (“common hydrogen molecular ions”); And (e) H + 3, 22.6 eV (“common trihydrogen.” In this specification, “normal” and “ordinary” are synonymous with respect to the hydrogen form. to be.

(여기서, p는 정수로서, 바람직하게는 2 내지 137의 정수임)의 결합 에너지, 바람직하게는 ±10%, 보다 바람직하게는 ±5% 내의 결합 에너지를 갖는 수소 원자; (b) 약 According to another embodiment of the invention, (a) about

A hydrogen atom having a binding energy of preferably ± 10%, more preferably ± 5%, where p is an integer, preferably an integer from 2 to 137; (b) about

(여기서, P는 정수로서, 바람직하게는 2 내지 137의 정수임)의 결합 에너지, 바람직하게는 ±10%, 보다 바람직하게는 ±5% 내의 결합 에너지를 갖는 트리하이드리노(trihydrino) 분자 이온, H+3(1/p); (e) 약

(여기서, P는 정수로서, 바람직하게는 2 내지 137의 정수임)의 결합 에너지, 바람직하게는 ±10%, 보다 바람직하게는 ±5% 내의 결합 에너지를 갖는 디하이드리노(diihydrino) 분자 이온; (f) 약

(여기서, P는 정수로서, 바람직하게는 2 내지 137의 정수임)의 결합 에너지, 바람직하게는 ±10%, 보다 바람직하게는 ±5% 내의 결합 에너지를 갖는 디하이드리노(diihydrino) 분자 이온과 같은 적어도 하나 의 결합 에너지가 증가된 수소종을 포함하는 화합물이 제공된다. Hydride ions (H−) having a binding energy of (where p is an integer, preferably an integer from 2 to 24), preferably ± 10%, more preferably ± 5%; (c) H + 4 (1 / p); (d) approximately

Trihydrino molecular ion, H, having a binding energy of preferably ± 10%, more preferably ± 5%, where P is an integer, preferably an integer from 2 to 137. +3 (1 / p); (e) about

Dihydrino molecular ions having a binding energy of preferably ± 10%, more preferably ± 5%, where P is an integer, preferably an integer from 2 to 137; (f) about

(Where P is an integer, preferably an integer from 2 to 137), such as dihydrino molecular ions having a binding energy within the range of ± 10%, more preferably ± 5%. Compounds are provided that include hydrogen species with increased at least one binding energy.

According to another preferred embodiment of the present invention, (a)

(17)

(17)

 (Where p is an integer, h is Planck's constant bar, me is the mass of electrons, c is the luminous flux in vacuum, μ is the mass of the reduced nucleus, and k is a pre-calculated harmonic force constant) Dihydrino molecular ions having a total energy of [2]), preferably within ± 10%, more preferably within ± 5%, and (b)

(18)

(18)

At least one binding energy, such as dihydrino molecular ions, having a total energy of preferably within ± 10%, more preferably within ± 5%, of p is an integer and a0 is a bore radius Compounds comprising increased hydrogen species are provided.

According to one embodiment of the invention, wherein the compound comprises hydrogen species with increased binding energy in which the compound is negatively charged, the compound adds one or more cations such as protons, general H + 2, and general H + 3. It includes.

(여기서, m은 1보다 큰 정수로서, 바람직하게는 400보다 작은 정수임)의 순 반응 엔탈피를 갖는 촉매와 반응시켜, 약

(여기서, p는 정수로서, 바람직하게는 2 내지 137의 정수임)의 결합 에너지를 갖는 결합 에너지가 증가된 수소 원자를 생성하는 단계를 포함한다.A method is provided for preparing a compound comprising at least one or more hydride ions with increased binding energy. Such compounds are hereinafter referred to as "hydrino hydride compounds". The method is about hydrogen atoms

Reacting with a catalyst having a net reaction enthalpy of (where m is an integer greater than 1, preferably an integer less than 400),

Generating a hydrogen atom with an increased binding energy, where p is an integer, preferably an integer from 2 to 137.

An additional product of the catalysis is energy. Hydrogen atoms with increased binding energy can react with electron sources to produce hydride ions with increased binding energy. The hydride ions with increased binding energy may react with one or more cations to produce a compound comprising hydride ions with increased binding energy of at least one.

A composition of matter comprising a new form of hydrogen formed by the catalysis of new hydrogen species and atomic hydrogen is disclosed in "Mills prior art." Hydrogen compositions of the novel materials include:

(a) at least one neutral, positive, or negative hydrogen species having a binding energy as follows (“hydrogen species with increased binding energy”);

(i) a binding energy greater than that of the corresponding common hydrogen species, or

(ii) the binding energy of a typical hydrogen species is less or negative than the thermal energy of ambient conditions (standard temperature and pressure, STP), so that the corresponding common hydrogen species is less than the bond energy of any unstable or unobservable hydrogen species. Greater binding energy; And

(b) at least one other element. The compounds of the present invention are hereinafter referred to as "hydrogen compounds with increased binding energy".

Here, "another element" means an element other than hydrogen species with increased binding energy. Thus, the other element may be a general hydrogen species or any element other than hydrogen. In one group of compounds, other species and hydrogen species with increased binding energy are neutral. In other groups of compounds, hydrogen species with increased binding energy and other elements are charged in order for the other elements to provide a balancing charge to form neutral compounds. The former group of compounds is characterized by molecular and coordination bonds; The latter group is characterized by ionic bonds.

In addition, novel compounds and molecular ions are provided, including:

(a) at least one neutral, positive, or negative hydrogen species having the following total energy (hereinafter "hydrogen species with increased binding energy")

(i) a binding energy greater than the total energy of the corresponding common hydrogen species, or

(ii) since the total energy of a typical hydrogen species is less or negative than the thermal energy of ambient conditions (standard temperature and pressure, STP), the corresponding common hydrogen species is less than the total energy of any hydrogen species that is unstable or unobservable. Greater total energy; And

(b) at least one other element.

The total energy of the hydrogen species is the sum of the energies for removing all electrons from the hydrogen species. Hydrogen species according to the invention have a total energy greater than the total energy of the corresponding general hydrogen species. While some embodiments of hydrogen species with increased total energy may have a first electron bond energy that is less than the first electron bond energy of the corresponding generic hydrogen species, the hydrogen species with increased total energy in accordance with the present invention are also "bonded". Hydrogen species with increased energy ". For example, when p = 24, the hydride ions of formula (15-16) have a first binding energy less than the first binding energy of a typical hydride ion, whereas when p = 24, the formula ( The total energy of the hydride ions of 15-16) is much greater than the total energy of the corresponding general hydride ions.

In addition, novel compounds and molecular ions are provided, including:

(a) a plurality of neutral, positive, or negative hydrogen species having a binding energy as follows (“hydrogen species with increased binding energy”);

(i) a binding energy greater than that of the corresponding common hydrogen species, or

(ii) because the binding energy of a typical hydrogen species is less or negative than the thermal energy of the ambient conditions, the binding energy of the corresponding generic hydrogen species is greater than the binding energy of any hydrogen species that is unstable or unobserved; And

(b) optional one other element. The compounds of the present invention are hereinafter referred to as "hydrogen compounds with increased binding energy".

Hydrogen species with increased binding energy include at least one hydrino atom with at least one electron, hydrino atom, at least one compound comprising a hydrogen species with increased binding energy, and at least one other atom, molecule, or binding energy. Can be formed by reacting with ions other than increased hydrogen species.

Also provided are novel compounds and molecular ions comprising:

(a) a plurality of neutral, positive, or negative hydrogen species having a total energy of the following (“hydrogen species with increased binding energy”):

(i) the total energy greater than the total energy of ordinary molecular hydrogen, or

(ii) the total energy of the corresponding generic hydrogen species is greater than the total energy of any hydrogen species that is unstable or unobservable because the total energy of the typical hydrogen species is less or negative than the thermal energy of the ambient conditions; And

(b) optional one other element. The compounds of the present invention are hereinafter referred to as "hydrogen compounds with increased binding energy".

In one embodiment, (a) a binding energy according to formula (15-16), which is greater than the binding energy of a typical hydrogen ion (about 0.8 eV) for p = 2 to 23 and less than for p = 24 Hydride ions having (“hydride ions with increased binding energy” or “hydrino hydride ions”); (b) a hydrogen atom with a binding energy greater than the binding energy of a typical hydrogen atom (about 13.6 eV) ("hydrogen atom with increased binding energy" or "hydrino"); (c) hydrogen molecules having a first binding energy greater than about 15.3 eV (“hydrogen molecules with increased binding energy” or “dihydrino”); And (d) an increase in at least one binding energy selected from the group consisting of molecular hydrogen ions having a binding energy greater than about 16.3 eV ("molecular hydrogen ions with increased binding energy" or "dihydrino molecular ions") Provided are compounds comprising hydrogen species.

Characterization and identification of species with increased binding energy

Based on resonant energy transfer mechanisms (rt-plasma) between hydrogen atoms and specific catalysts, new chemically generated or auxiliary plasma sources have been developed that could be new power sources. Products are more stable hydride and molecular hydrogen species such as H- (1/4) and H2 (1/4). The source operates by heating a hydrogen dissociator and a catalyst with an incandescent lamp to provide a hydrogen atom and a gas catalyst, respectively, and the catalyst reacts with the hydrogen atoms to produce a plasma. Mills et al. [3-10] show low temperatures (e.g., 103 K) from hydrogen atoms and specific atomization elements or certain gas ions ionizing singly or multiplely at integer multiples of 27.2 eV, the potential energy of the hydrogen atoms; It was surprising that strong extreme ultraviolet (EUV) was observed at very low field strengths. Numerous independent experimental observations confirm that rt-plasma results from the reaction of new hydrogen atoms to produce hydrogen in quantum fractional state as a chemical intermediate at lower energy than a typical “bottom” (n = 1) state. . Power is released [3, 9, 11-13] and the final reaction product is a novel hydride compound [3, 14-16] or low energy molecular hydrogen [17]. Data supporting this include EUV spectroscopy [3-10, 13, 17-22, 25, 27-28], characteristic release from catalyst and hydride ion products [3, 5, 7, 21-22, 27-28] , Low energy hydrogen emission [12-13, 18-20], chemically formed plasma [3-10, 21-22, 27-28], significant (> 100 eV) ballmer α broadening [3-5, 7, 9-10, 12, 18-19, 21, 23-28], density reversal of H line [3, 21, 27-29], elevated electron temperature [19, 23-25], anomalous plasma afterglow ( afterglow) duration [3, 8], power generation [3, 9, 11-13], and analysis of novel compounds [3, 14-16].

The theory provided previously [6, 18-20, 30] is based on Maxwell's equations for solving the structure of electrons. The familiar Lidbury equation (Eq. (19)) arises for the hydrogen excited state where n> 1 in Eq. (20).

(19)

(19)

(20)

20

(p는 정수임) (21)A further result is that the hydrogen atom is capable of catalyzing reactions with certain atoms, excimers, and ions that provide a reaction with a net enthalpy of an integer multiple of the hydrogen atom's potential energy, ie m · 27.2 eV, where m is an integer. Can be. The reaction involves a non-radioactive energy transfer that forms a hydrogen atom called hydrino, which is lower in energy than the unreacted hydrogen atoms corresponding to fractional proton counts. That is, in the case of hydrogen excited state,

(p is an integer) (21)

It replaces the well known variable n = integer in this Lidbury equation. Although the hydrogen state with n = 1 and the hydrogen state with n = 1 / integer are non-radioactive, non-radioactive energy transfer allows for transitions between two non-radioactive states, n = 1 to n = 1/2. Thus, the catalyst has a positive net reaction enthalpy of m · 27.2 eV (ie, it resonantly accepts non-radioactive energy transfer from the hydrogen atom and releases energy to the surroundings, which affects the electron transition to the fractional quantum energy level). to provide. As a result of this non-radioactive energy transfer, the hydrogen atoms become unstable and release additional energy until reaching a low energy non-radioactive state with the main energy level given by equations (19) and (21). Processes that occur without photons and require collisions, such as hydrogen molecule bond formation, are common [31]. In addition, some commercially available phosphors are based on resonant non-radioactive energy transfer, including multipole coupling.

Two H (1 / p) can react to form H2 (1 / p). Hydrogen molecular ions and molecular charge and current density actions, bond distances, and energy have conventionally been solved with surprising accuracy [30, 33]. Using Laplacian in ellipsoidal coordinates with a non-radiative constraint, each field of the prolate spheroid molecular orbital has a central field of + pe. The total energy of the hydrogen molecule is:

                                                                   (22)

Where p is an integer, h is Planck's constant bar, me is the mass of electrons, C is the luminous flux in vacuum, μ is the mass of the reduced nucleus, and k has only the fundamental constant [30, 33]. Is a precalculated harmonic constant in a closed form equation, a0 is the bore radius). The vibrational and rotational energy of the fractional-Leadbury-state molecular hydrogen H2 (1 / p) is P2 times H2. Thus, for the transition from v = 0 to v = 1 of the hydrogen-form molecule H2 (1 / p), the vibrational energy Evib is

Evib = P20.515902 eV (23)

(Here, the experimental vibrational energy EH2 (υ = 0 → υ = 1) when H2 transitions from υ = 0 to υ = 1 is shown in Beutler [34] and Herzberg [35]. Given by The rotational energy, Erot [30, 33], when the hydrogen-form molecule H2 (1 / p) transitions from J to J + 1

(24)

(24)

Where I is the moment of inertia and the experimental rotational energy when H2 transitions from J = 0 to J = 1 is given by Atkins [36]. The p2 dependence of rotational energy is derived from the inverse p dependency of internuclear distance and the impact on the corresponding I. The estimated internuclear distance 2c 'of H2 (1 / p) is:

(25)

(25)

Rotational energy makes it possible to measure I and internuclear distances very accurately using well-established theory [37].

Ar + can function as a catalyst because the ionization energy is about 27.2 eV. The catalytic reaction from Ar + to Ar2 + forms H (1/2), which additionally functions as a catalyst and reactant to form H (1/4) [19-20, 30]. Therefore, H (1/4) is expected to be observed depending on the flow, because the formation of H2 (1/4) requires accumulation of intermediates. The mechanism was tested by experiment with flowing plasma gas. For high pressure argon-hydrogen plasmas excited by 12.5 keV electron beam, neutral molecular emission was expected. For H2 (1/4), a line of rotation was expected and found in the 150-250 nm region. The spectral lines were compared with those predicted by Eqs. (23-24) corresponding to 1/4 the internuclear distance of H2 given by Eq. (25). For p = 4 in equation (23-24), the predicted energy for the υ = 1 → υ = 0 oscillation-rotation series of H2 (1/4) is:

(26)

(26)

Since He + ionizes at 54.417 eV, which is 2 · 2.27 eV, it also satisfies the catalytic condition that the enthalpy change in the chemical or physical process must be equal to an integer multiple of 27.2 eV. H (1/3), the product of the catalytic reaction of He +, can further act as a catalyst to form H (1/4) and H (1/2) [19-20, 30], which is a different state Can cause a transition to H (1 / p). A novel emission line with an energy of q · 13.6 eV (where q = 1,2,3,4,6,7,8 or 11) was recorded during the microwave discharge with 2% hydrogen of helium Previously observed by (EUV) spectroscopy [18-20]. The lines corresponded to H (1 / p), which is the fractional Lidbury state of hydrogen atoms given by equations (19) and (21).

Rotation lines were observed in the 145-300 nm region from argon-hydrogen plasma excited with atmospheric electron beams. The 42 times energy interval of this unprecedented hydrogen confirms the internuclear distance to 1/4 times H2, confirming that it is H2 (1/4) (Equation (23-26)). H2 (1 / p) gas was separated by liquefaction of helium-hydrogen plasma gas using a liquid nitrogen cryotrap capable of high-vacuum (10-6 Torr) and identified by mass spectroscopy (MS) It became. The condensable gas had higher ionization energy than H2 by MS [17]. The H2 (1/4) gas obtained from the chemical decomposition of the hydride containing the corresponding hydride ion H- (1/4) as well as from the liquefaction of the catalysis-plasma gas was confirmed by 1 H NMR, H2 being identified at 4.63. Compared to 2.18 ppm upfield was identified as a shifted single peak. Vibration-rotated emission from an electron beam holding an argon-hydrogen plasma and from Fourier transform ultraviolet (FTIR) spectroscopy of solid samples containing H- (1/4) with interstitial H2 (1/4). The study further identified H2 (1/4).

Reservoir calorimetry was used to determine whether a measurable power occurred in the rt-plasma due to the reaction forming the state given by equations (19) and (21). Specifically, He / H 2 (10%) (500 mTorr), Ar / H 2 (10%) (500 mTorr) and H 2 O (g) (500 and 200) generated using an Evanson microwave cavity. mTorr) plasma generated 5% higher heat than non-rt-plasma such as He, Kr, Kr / H2 (10%) under the same conditions of gas flow, pressure and microwave operating conditions. The excess power density of the rt-plasma was about 10 W · cm −3. In addition to the unique vacuum ultraviolet (VUV), these early studies of rt-plasma increased the rapid linewidth of hydrogen ballmer series [3-5, 7, 9-10, 12, 18-19, 21, 23-28] and water plasma In the case of, it was demonstrated that other unique features exist, including density reversal of hydrogen excited states. Current and past results are consistent with the existence of an unknown exothermic chemical reaction occurring in rt-plasma.

Since the ionization energy from Sr + to Sr3 + has a net reaction enthalpy of 2 · 27.2 eV, Sr + can function as a catalyst either alone or in combination with an Ar + catalyst. It has been reported previously that rt-plasma was formed with a low field (1 V / cm) at low temperatures (eg 103 K) from hydrogen atoms generated in tungsten filaments and strontium evaporated by heating. [4-5,7,9-10]. Increased with the addition of argon, strong VUV emissions were observed, but not when sodium, magnesium or barium replaced strontium or hydrogen, argon or strontium alone was added. Without typical Lidbury series Ar I and Ar II lines, a characteristic emission was observed from the continuum state of Ar2 + at 45.6 nm, confirming that 27.2 eV of resonant non-radioactive energy was transferred from the hydrogen atom to Ar +. Predicted Sr3 + emission lines were also observed from strontium-hydrogen plasmas supporting the rt-plasma mechanism [5, 7]. A time-dependent linewidth increase of H Balmer α rays corresponding to very fast H (25 eV) was observed. Excess power of 20 mW · cm − was measured calorimetrically on the rt-plasma formed when Ar + was added to Sr + as the addition catalyst.

와 비교하였다. 동일한 광출력을 얻기 위하여, 수소-나트륨, 수소-마그네슘, 및 수소-바륨 혼합물은 수소-스트론튬 혼합물의 전력의 각각 4000, 7000, 및 6500 배를 요구하였고, 아르곤의 첨가시 약 2배 만큼 상기 비율이 증가하였다. 수소-스트론튬 혼합물의 경우, 수소 단독 및 나트륨-수소 혼합물의 경우가 250 V, 수소-마그네슘 및 수소-바륨 혼합물의 경우가 약 140-150 V와 비교하여 볼 때, 약 2 V의 매우 낮은 전압에서 글로 방전(glow discharge) 플라즈마를 형성하였다 [4-5, 7]. 이러한 전압은 너무 낮아서 적용 장(field)이 높은 가속화 이온을 포함하는 통상적인 메커니즘에는 적용할 수 없다. 낮은 전압의 EUV 및 가시광선 공급원이 유용하다[10]. Significant linewidth enhancements of the Balmer α-rays corresponding to average hydrogen atom temperatures of 14, 24 eV, and 23-45 eV were observed for strontium and argon-strontium rt-plasma, strontium-hydrogen, helium-hydrogen, argon-hydrogen, Discharges of strontium-helium-hydrogen, and strontium-argon-hydrogen for pure hydrogen, xenon-hydrogen, and magnesium-hydrogen, respectively

Compared with. In order to achieve the same light output, the hydrogen-sodium, hydrogen-magnesium, and hydrogen-barium mixtures required 4000, 7000, and 6500 times the power of the hydrogen-strontium mixture, respectively, and the ratio was approximately twice that with the addition of argon. Increased. For the hydrogen-strontium mixture, at a very low voltage of about 2 V, the hydrogen alone and sodium-hydrogen mixtures are 250 V, and the hydrogen-magnesium and hydrogen-barium mixtures are about 140-150 V A glow discharge plasma was formed [4-5, 7]. These voltages are so low that they are not applicable to conventional mechanisms involving high acceleration ions in the field of application. Low voltage EUV and visible light sources are useful [10].

의 반지름까지 m 수준이하로 떨어진다. K가 K3+로 되면서 수소 원자의 포텐셜 에너지의 3배, 즉 3·27.2 eV만큼의 순 엔탈피를 갖는 반응을 제공하기 때문에, K는 촉매로 기능하여 촉매작용을 겪는 각 일반적인 수소 원자들이 총 204 eV를 방출하게 할 수 있다[3]. 그리고 나서, K는 생성물인 H(1/4)과 반응하여 낮은 상태의 H(1/7)을 형성하거나, 불균형이라 불리는 공정에서 하이드리노만을 포함하는 다음과 같은 추가적인 촉매 전이가 일어날 수 있다:

등. 포텐셜 에너지의 다극 확대(multipole expansion)에 대응하는 하이드리노의 이온화 에너지 및 준안정 공진 상태(metastable resonant state)가 이전에 주어진 바와 같이[19-20, 30], m·27.2 eV (수식 (10 및 (21))이기 때문에, 촉매작용이 시작되면 하이드리노는 추가로 더 낮은 상태로의 전이를 자가촉매한다. 이 메커니즘은 무기 이온 촉매작용의 메커니즘과 유사하다. 제1 하이드리노 원자로부터 제2 하이드리노 원자로 m·27.2 eV의 에너지가 전달되면 제1 원자의 중심장이 m 배만큼 증가하고 전자가 반지름

에서 반지름

로 m 수준 아래로 떨어진다. 촉매 생성물 H(1/p)는 또한 전자와 반응하여 다음의 결합 에너지 EB를 갖는 신규 수소화물 이온 H-(1/p)을 형성할 수 있다[3, 14, 16, 21, 30] In general, the transfer of m · 27.2 eV of energy from a hydrogen atom to a catalyst increases the central field interaction of H atoms by m times, and the electrons from the hydrogen atom radius aH

Drops below m level to. Since K becomes K3 + and provides a reaction with a net enthalpy of three times the potential energy of the hydrogen atom, i.e. 3,27.2 eV, K acts as a catalyst and each of the common hydrogen atoms undergoing catalysis total 204 eV. Can be released [3]. K can then react with the product H (1/4) to form a low level H (1/7), or in the process called unbalance, additional catalytic transitions involving only hydrinos can occur:

Etc. The ionization energy and metastable resonant state of hydrinos corresponding to multipole expansion of potential energy are given previously [19-20, 30], m.27.2 eV (Equation (10 and (21)), the hydrinos further autocatalyze the transition to a lower state once the catalysis begins, a mechanism similar to that of the inorganic ion catalysis. When the energy of the Reno reactor m · 27.2 eV is transferred, the center field of the first atom is increased by m times and the electron radius is

Radius

As m falls down the level. The catalyst product H (1 / p) can also react with the electrons to form new hydride ions H- (1 / p) with the following binding energy EB [3, 14, 16, 21, 30].

(27)

(27)

(여기서, mp는 양자의 질량이고, aH는 수소 원자의 반지름이며, a0는 보어 반지름이고, e는 기본 전하임)에서 주어진 감소된 전자 질량임). 이온 반지름은

이다. 수식 (27)로부터, 계산된 수소화물 이온의 이온화 에너지는 0.75418 eV이고, 리케(Lykke)[38]에 의한 실험값은 6082.99±0.15 cm-1(0.75418 eV)이다. (Where p is an integer greater than 1, S = 1/2, h is Planck's constant bigo, μ0 is vacuum permeability, me is electron mass, and μe is

(Where mp is the mass of protons, aH is the radius of the hydrogen atom, a0 is the bore radius, and e is the fundamental charge). Ion radius is

to be. From equation (27), the calculated ionization energy of hydride ions is 0.75418 eV, and the experimental value by Lykke [38] is 6082.99 ± 0.15 cm-1 (0.75418 eV).

Substantial evidence of an active catalytic reaction, including the resonance energy transfer between K and a hydrogen atom forming a highly stable novel hydride ion H- (1 / p) called hydrino hydride with predicted fractional donor number p = 4 Have been previously reported [3]. Characteristic emission was observed from K3 +, confirming the transfer of resonant non-radioactive energy of 3 · 27.2 eV from the hydrogen atom to K. From equation (27), the binding energy EB of H- (1/4) is as follows:

 EB = 11.232 eV (λvac = 1103.8 Å) (28)

The product hydride ion H- (1/4) was spectroscopically observed at 110 nm corresponding to the predicted binding energy of 11.2 eV [3, 21].

는 H-(1/1)의 시프트 및 낮은 전자 에너지 상태로 인한 공헌도의 합으로 주어진다:The upfield-shift NMR peak is direct evidence that there is a low energy state of hydrogen, which has a reduced radius compared to normal hydride ions, and an increase in both diamagnetic shielding. Total theoretical shift for H- (1 / p)

Is given as the sum of the contributions due to the shift of H- (1/1) and the low electron energy state:

(29)

(29)

Where p = integer> 1. The corresponding alkali hydrides and alkali hydrino hydrides (including H- (1 / p)) were identified by 1 H MAS NMR and compared with theoretical values. The agreement between the predicted and observed peaks indicates the accuracy of the test.

The 1 H MAS NMR spectrum of the new compound KH * Cl relative to external tetramethylsilane (TMS) showed a large and clear upfield resonance at -4.4 ppm corresponding to an absolute resonance shift of -35.9 ppm, which is the theoretical prediction of P = 4. Consistent with [3,14-16]. The result is a strong hydrogen Lyman-releasing rt-plasma, fixed inverted Lyman density, afterglow duration, highly active hydrogen atoms, characteristic alkali-ion release due to catalysis, predicted New spectral lines, and previous observations from measurements of power beyond conventional chemistry [3], have been confirmed, which corroborates the catalysis of atomic hydrogen to form more stable hydride ions named H- (1 / p). Was consistent with the prediction. Since comparing the theoretical and experimental shifts of KH * Cl is direct evidence of low-energy hydrogen with strong exotherm inherent during formation, further analysis by infrared (FTIR) spectroscopy to eliminate any known explanation [39] Was repeated.

Basic analysis [14, 16] confirmed that these compounds contained alkali metals, halogens and hydrogen, and no known hydride compounds with upfield-shift hydride NMR peaks in this composition were found in the literature. Typical alkali hydrides mixed with alkali hydrides alone or exhibit a down-field shift peak [3, 14-16]. In the literature, what can be used as an alternative to H- (1 / p) as a possible source of upfield NMR peaks is limited to U centered H. The strong, characteristic infrared rotational band at 503 cm −1 resulting from the substitution of Cl— with H— in KCl allowed the removal of H centered U as a source of upfield-shift NMR peaks [39].

As further elucidation, an X-ray photoelectron spectrum (XPS) of hydrino hydride KH * I was performed to determine whether the binding energy of the predicted H- (1/4) given by equation (28) was observed. FTIR analysis of the crystals with H- (1/4) before and after storage in argon for 90 days was performed to provide an interstitial H2 (1/4) with the predicted rotational energy given by equation (24). ). Identifying a single rotational peak in an energy state with ortho-para splitting due to the free rotation of very small hydrogen molecules would be solid proof of existence because there are no other potential challenges [39].

Rotational emissions of H2 (1/4) were observed in the determination of KH * I with peaks corresponding to H- (1/4), and oscillation-rotational emissions of H2 (1/4) were H2 (1/4) Observed from a 12.5 keV-electron beam retaining argon plasma with 1% hydrogen due to the collision excitation of H2 (1/4), or H2 formed from H- (1/4) trapped in a lattice of KH * Cl (1/4) or H2 (1/4) formed in situ from K catalysis of H through electron bombardment can produce a gaseous detectable emission (<10-5 Torr) [39] Below pressure, irradiation was carried out by a windowless EUV spectrometer on the electron beam excitation of the crystal using a 12.5 keV electron gun. The rotational energy of H 2 (1/4) was also confirmed by the above technique. Consistent results from extensive irradiation techniques provide clear evidence that hydrogen can exist in low energy states in the form of H- (1/4) and H2 (1/4), which were previously thought possible. In one embodiment, the products of Li catalysis and NaH catalysis are H- (1/4) and H2 (1/4), and in the case of NaH, additionally H- (1/3) and H2 (1/3). . The present invention provides for their identification and characteristic emission from EUV spectroscopy, catalyst and hydride ion products, low energy hydrogen emission, chemically formed plasma, unique Balmer α linewidth, H-density inversion, elevated electron temperature, anomalous plasma afterglow (afterglow) Duration, power generation, and analysis of new compounds provide corresponding active exothermic reactions. Preferred identification techniques of species H- (1 / p) and H2 (1 / p) include NMR of H- (1 / p) and H2 (1 / p), FTIR of H2 (1 / p) trapped in crystals, XPS of H- (1 / p), TOF-SIMS of H- (1 / p), electron beam excitation emission spectroscopy of H2 (1 / p), electron beam emission spectroscopy of H2 (1 / p) trapped in the crystal lattice, And TOF-SIMS identification of novel compounds comprising H- (1 / p). Preferred techniques for robust catalysis and power balance are line broadening, plasma formation, and calorimetry. Preferably, H- (1 / p) and H2 (1 / p) are H- (1/4) and H2 (1/4), respectively.

Brief description of the drawings

1A is a schematic diagram of an energy reactor and a power plant according to the present invention.

2A is a schematic diagram of an energy reactor and power generation device for recycling or recycling fuel in accordance with the present invention.

3A is a schematic diagram of a power reactor according to the present invention.

4A is a schematic diagram of a discharge power and a plasma cell and a reactor according to the present invention.

1 is an experimental instrument comprising a filament gas cell forming lithium-argon-hydrogen and lithium-hydrogen rt-plasma.

FIG. 2 is a schematic diagram of a reaction cell and a cut plane of water flow calorimetry used to measure the energy balance of NaH catalyzed reactions forming hydrinos. The configuration is as follows: 1-entry / exit thermistor; 2-high temperature valve; 3-ceramic fiber heaters; 4-copper water-cooled coils; 5-reactor; 6-insulator; 7-cell thermocouple, and 8-water chamber.

3 is a schematic diagram of a water flow calorimeter used to measure the energy balance of a NaH catalyzed reaction to form hydrinos.

4 shows LiH * Br, LiH * comprising (i) R—Ni, Li, LiNH 2, and LiBr or LiI or (ii) NaCl or NaBr such as Pt / Ti dissociating agent, Na, NaH, and reactants. Schematic of a stainless steel gas cell synthesizing I, NaH * Cl and NaH * Br. The configuration is as follows: 101-stainless steel cell; Internal cavity of the 117-cell; 118-high vacuum conflat flange; 119-mating blank coneflat flange; 102-stainless steel tube vacuum line and gas supply line; 103- kiln or top insulator lid, heater cover wrapped with 104- high temperature insulator; 108-Pt / Ti dissociating agent; 109-reactant; 110-high vacuum turbopump; 112-pressure gauge; 111-vacuum pump valve; 113-valve; 114-valve; 115-regulator, and 116-hydrogen tank

FIG. 5 shows 656.3 nm Ballmer α linewidth recorded with high resolution visual spectroscopy at the initial release of (A) lithium-argon-hydrogen rt-plasma and (B) at 70 hours of operation. Significant broadening of lithium and only H-rays was observed for times corresponding to average hydrogen atom temperatures of> 40 eV and fractional densities of at least 90%.

FIG. 6 shows 656.3 nm Ballmer α linewidth recorded with a high resolution (± 0.006 nm) visual spectrometer at (A) initial release of lithium-hydrogen-plasma and (B) at 70 hours of operation. Lithium wire and only H broadening were observed over time, but decreased compared to the case with the argon-hydrogen group (95/5%).

7 shows the DSC (100-750 ° C.) results of NaH at a scan rate of 0.1 degrees / minute. A wide exothermic peak was observed at 350-420 ° C. corresponding to 47 KJ / mole, consistent with sodium hydride decomposition in this temperature range with a corresponding enthalpy of 57 KJ / mole. A large exotherm was observed under conditions forming a NaH catalyst in the region of 640 to 825 ° C., which is the largest exothermic reaction for H, the combustion enthalpy of hydrogen, i.e. at least -354 KJ / mole H2 greater than -241.8 KJ / mole H2. Is equivalent to.

8 shows the results of DSC (100-750 ° C.) of MgH 2 at a scan rate of 0.1 degrees / minute. Two sharp endothermic peaks were observed. The first peak centered at 351.75 ° C., corresponding to 68.81 KJ / mole MgH 2, corresponds to the decomposition energy of 74.4 KJ / mole MgH 2. The second peak at 647.66 ° C., corresponding to 6.65 KJ / mole MgH 2, is consistent with the known melting point of Mg (m), 650 ° C. and fusion enthalpy 8.48 KJ / mole MgH 2. Thus, the predicted behavior was observed in the case of degradation of the control, noncatalytic hydride.

Figure 9 shows the temperature versus time for a calibration run with a vacuum test cell and a resistive heater.

FIG. 10 shows power versus time for a calibration run with a vacuum test cell and resistive heating. The numerical integration of the input and output power curves represents an output energy of 292.2 KJ and an input energy of 303.1 KJ, which corresponds to the output cooling of a 96.4% flow of resistive input.

FIG. 11 shows the cell temperature with time upon hydrino reaction with a cell containing reagent material, 1 g Li, 0.5 g LiNH 2, 10 g LiBr, and 15 g Pd / Al 2 O 3. The reaction released less than 120 seconds to release energy of 19.1 KJ, resulting in a system-response-corrected peak power exceeding 160 W.

FIG. 12 shows the cooling power over time for hydrino reaction with a cell containing a reagent comprising catalyst material, 1 g Li, 0.5 g LiNH 2, 10 g LiBr, and 15 g Pd / Al 2 O 3. The numerical integration of the input and output power curves with the applied calibration correction produced an output energy of 227.2 kJ and an input energy of 208.1 kJ, corresponding to excess energy of 19.1 kJ.

FIG. 13 shows the temperature of cells containing R-Ni, a 15 g R-Ni / Al alloy powder, and a reagent comprising 3.28 g of Na as starting material and the cell over time in the R-Ni controlled power test.

FIG. 14 shows the cooling power over time in a control power test and a cell containing a reagent comprising R-Ni, 15 g R-Ni / Al alloy powder, and 3.28 g Na as starting material. The energy balance was obtained by calibration-correction numerical integration of the input and output power curves producing an output energy of 384 kJ and an input energy of 385 kJ.

FIG. 15 shows the temperature of a cell containing a catalyst material, a reagent containing 15 g NaOH-doped R-Ni 2800, and 3.28 g Na, and the cell over time in the hydrino reaction. The reaction released less than 90 seconds and released 36 KJ of energy resulting in a system-response-corrected peak power of greater than 0.5 W.

FIG. 16 shows cooling with time upon hydrino reaction with a cell containing a reagent material, a reagent comprising 15 g NaOH-doped R-Ni 2800, and 3.28 g Na. The numerical integration of the input and output power curves with the applied calibration correction produced 185.1 kJ output energy and 149.1 kJ input energy corresponding to excess energy of 36 kJ.

FIG. 17 shows the temperature of the cell with time upon reaction with a cell containing a reagent comprising a catalyst material, 15 g NaOH-doped R-Ni 2400. The cell temperature jumped rapidly from 60 ° C. to 205 ° C. in 60 seconds, and the reaction released 11.7 KJ of energy in a short time resulting in a system-response-corrected peak power of greater than 0.25 W.

FIG. 18 shows the cooling power over time in a hydrino reaction with a cell containing a reagent comprising a catalyst material, 15 g NaOH-doped R-Ni 2400. The numerical integration of the input and output power curves with calibration correction produced 184.0 kJ input energy, corresponding to an output energy of 195.7 kJ and an excess energy of 11.7 kJ.

19 shows the positive TOF-SIMS spectrum (m / e = 0-100) of LiBr.

20 shows a positive TOF-SIMS spectrum (m / e = 0-100) of LiH * Br crystals.

21 shows the negative TOF-SIMS spectrum (m / e = 0-100) of LiBr.

FIG. 22 shows the negative TOF-SIMS spectrum (m / e = 0-100) of the LiH * Br crystals. Major hydride, LiHBr-, and Li2H2Br- peaks were uniquely observed.

Figure 23 shows a positive TOF-SIMS spectrum (m / e = 0-200) of LiI.

24 shows a positive TOF-SIMS spectrum (m / e = 0-200) of LiH * I crystals. LiH +, Li2H2I +, Li4H2I +, and Li6H2I + were observed only in the cation spectrum of LiH * I crystals.

25 shows the negative TOF-SIMS spectrum (m / e = 0-180) of LiI.

26 shows the negative TOF-SIMS spectrum (m / e = 0-180) of LiH * I crystals. The main hydrates LiHI-, and Li2H2I-, and NaHI- peaks were uniquely observed.

27 shows the negative TOF-SIMS spectrum (m / e = 20-30) of NaH * -coated Pt / Ti with generation of 15 kJ of excess heat. Hydrino hydride compound NaHx- was observed.

28 shows a positive TOF-SIMS spectrum (m / e = 0-100) of R-Ni reacted at 50 ° C. for 48 hours or more. The main ion on the surface was Na +, consistent with the NaOH doping of the surface. In addition, other main element ions of R—Ni 2400 such as Al +, Ni +, Cr +, and Fe + were observed.

Fig. 29 shows the negative TOF-SIMS spectrum (m / e = 0-180) of R-Ni reacted at 50 ° C for 48 hours or more. Sodium hydrino hydrides and other unique ions corresponding to the sodium hydride hydride NaHx- combined with NaOH, NaO, OH and O- as well as the major hydrides NaH- and NaH3NaOH- which are bonded to the ions and NaOH Observed.

30A-B show 1H MAS NMR spectra relative to external TMS.

(A) LiH * Br represents a broad -2.5 ppm upfield-shift peak and a peak at 1.13 ppm corresponding to H- (1/4) and H2 (1/4), respectively,

(B) LiH * I shows a broad -2.09 pppm upfield-shift peak corresponding to H- (1/4) and peaks at 1.06 ppm and 4.38 ppm corresponding to H2 (1/4) and H2, respectively.

31A-B show 1H MAS NMR spectra relative to external TMS.

(A) KH * Cl exhibits a very sharp -4.46 ppm upfield-shift peak, essentially corresponding to the environment of free ions,

(B) KH * I exhibits a -2.31 ppm upfield-shift peak similar to that of LiH * Br and LiH * I. Both spectra also had a 1.13 ppm peak corresponding to H2 (1/4).

FIG. 32A-B shows H content selectivity of LiH * X for molecular species based on the nonpolarity of halides and the corresponding non-reactivity to H- (1/4), 1H relative to external TMS. MAS NMR spectrum is shown. (A) LiH * F containing unpolarized fluorine has a peak at 4.31 ppm corresponding to H2 and a peak at 1.16 ppm corresponding to H2 (1/4) (no H- (1/4) ion peak) (H) LiH * Cl containing unpolarized chlorine has a peak at 4.28 ppm corresponding to H2 and a peak at 1.2 ppm corresponding to H2 (1/4) (H- (1/4) ion peak) Is absent).

FIG. 33 is an external TMS comparison showing -3.58 ppm upfield-shift peaks corresponding to H- (1/4), H2 (1/4), and H2, peaks at 1.13 ppm, and peaks at 4.3 ppm, respectively. The 1 H MAS NMR spectrum of NaH * Br is shown.

34A-B show the effect of hydrogenation on the relative strengths of H2, H2 (1/4), and H- (1/4). Hydrogenation increased the H- (1/4) peak and decreased H2 (1/4), while increasing H2. (A) NaH * Cl synthesized by hydrogenation is -4 ppm upfield-shift peak corresponding to H- (1/4), 1.1 ppm peak corresponding to H2 (1/4), and predominantly corresponding to H2 NaH * Cl synthesized without hydrogenation shows a 4 ppm peak, and the -4 ppm upfield-shift peak corresponding to H- (1/4), the main 1.0 ppm peak corresponding to H2 (1/4) , And a small 4.1 ppm peak corresponding to H2.

FIG. 35 shows the 1 H MAS NMR spectrum of the external TMS of NaH * Cl resulting from the reaction of NaCl and the solid acid KHSO 4, the only source of hydrogen, wherein NaH * Cl exhibits an H- (1/4) peak and H at −3.97 ppm. Upfield-shift peak at -3.15 ppm corresponding to-(1/3) is shown. Peaks corresponding to H 2 (1/4) and H 2 (1/3) appear at 1.15 ppm and 1.7 ppm, respectively. The positive fractional hydrogen state was present and there was no H2 peak at 4.3 ppm because NaH * Cl was synthesized using solid acid as the H source without the addition of hydrogen gas and dissociator. (SB = side band).

36A-B show XPS irradiation spectra (Eb = 0 eV to 1200 eV). (A) LiBr. (B) LiH * Br.

37 shows 0-85 eV binding energy regions of high resolution XPS spectra of LiH * Br and control LiBr (dashed). The XPS spectra of LiH * Br differ from LiBr in that they have additional peaks at 9.5 eV and 12.3 eV that do not correspond to the peaks of known or other major elements. The peaks coincide with H- (1/4) in two different chemical environments.

38A-B show XPS irradiation spectra (Eb = 0 eV to 1200 eV). (A) NaBr. (B) NaH * Br.

39 shows 0-40 eV binding energy regions of high resolution XPS spectra of NaH * Br and control NaBr (dashed). The XPS spectrum of NaH * Br differs from NaBr in that it has additional peaks at 9.5 eV and 12.3 eV that do not correspond to the peaks of known or other major elements. The peaks coincide with H- (1/4) in two different chemical environments.

40A-B show XPS irradiation spectra (Eb = 0 eV to 1200 eV). (A) Pt / Ti. (B) NaH * -coated Pt / Ti with generation of 15 kJ excess heat.

41A-B show high resolution XPS spectra (Eb = 0 eV to 100 eV). (A) Pt / Ti. (B) NaH * -coated Pt / Ti with generation of 15 kJ excess heat. Pt4f7 / 2, Pt4f5 / 2, and O2s peaks on NaH * -coated Pt / Ti were observed at 70.7 eV, 74 eV, and 23 eV, respectively, and the only outermost band was observed for Pt / Ti. It became. Na2p and Na2s peaks were observed at 31 eV and 64 eV on NaH * -coated Pt / Ti, and the outermost band was only observed for Pt / Ti.

42A-B show high resolution XPS spectra (Eb = 0 eV to 50 eV). (A) Pt / Ti. (B) NaH * -coated Pt / Ti with generation of 15 kJ excess heat. The XPS spectrum of NaH * -coated Pt / Ti differs from Pt / Ti in that it has additional peaks at 6 eV, 10.8 eV and 12.8 eV, which do not correspond to known or other major element peaks. The 10.8 eV and 12.8 eV peaks coincide with H- (1/4) in two different chemical environments, and the 6 eV peak coincides with and corresponds to H- (1/3). Thus, fractional hydrogen states, 1/3 and 1/4, were present as predicted by equation (27).

43 shows XPS irradiation spectra (Eb = 0 eV to 120 eV) of NaH * -coated Si with major element peaks identified.

FIG. 44 shows XPS irradiation spectra (Eb = 0 eV to 120 eV) of NaH * -coated Si with peaks at 6 eV, 10.8 eV and 12.8 eV that do not correspond to known or other major element peaks. The 10.8 eV and 12.8 eV peaks coincide with H- (1/4) in two different chemical environments, and the 6 eV peak coincides with and corresponds to H- (1/3). Thus, fractional hydrogen states, 1/3 and 1/4, were consistent with the results of NaH * -coated Pt / Ti shown in FIG. 42B as predicted by Equation (27).

45A-B show high resolution (0.5 cm −1) FTIR spectra (490-4000 cm −1). (A) LiBr. (B) LiH * Br with an NMR peak corresponding to H- (1/4) heated to> 600 ° C. under dynamic vaccum maintained at −2.5 ppm NMR peak. Amide peaks at 3314, 3259, 2079 (wide), 1567, and 1541 cm −1 and imide peaks at 3172 (wide), 1953, and 1578 cm −1 were removed; Thus, they were not a source of sustained -2.5 ppm NMR peaks. -2.5 ppm in the 1 H MAS NMR spectrum corresponded to H- (1/4). Furthermore, the FTIR peak at 1989 cm −1 could not correspond to any known compound, but was consistent with the predicted frequency of para H 2 (1/4).

46 shows 150-350 nm spectra of electron beam excited CsCl containing H 2 (1/4). A series of flatly laid lines were observed in the 220-300 nm region, consistent with the spacing and intensity profiles of the P branches of H2 (1/4).

FIG. 47 shows spectra of 100-550 nm of an electron beam excited silicon wafer coated with NaH * Cl containing H 2 (1/4). A series of flatly laid lines were observed in the 220-300 nm region, consistent with the spacing and intensity profiles of the P branches of H2 (1/4).

Detailed Description of the Preferred Embodiments

Hydrogen catalytic reactor

A hydrogen catalytic reactor 50 for generating energy and low energy hydrogen species in accordance with the present invention is shown in FIG. 1A, an energy reaction mixture 54, a heat exchanger 60, and a steam generator 62 and a turbine 70. A vessel 52 containing a power converter, such as; In one embodiment, the catalysis includes reacting hydrogen atoms from source 56 with catalyst 58 to form a low energy hydrogen “hydrino” and generate power. Heat exchanger 60 absorbs heat released by catalysis when the reaction mixture consisting of hydrogen and catalyst reacts to form low energy hydrogen. The heat exchanger exchanges heat with the steam generator 62 which absorbs heat from the exchanger 60 to produce steam. The energy reactor 50 further includes a turbine which receives steam from the steam generator 62 and then supplies mechanical power to the power generator 80 that converts steam energy into electrical energy. Energy is delivered to the rod 90 for generating work or for decomposition.

In one embodiment, the energy reaction mixture 54 includes an energy releasing material 56 such as a solid fuel supplied through a supply passage 42. The reaction mixture comprises a source of hydrogen isotope atoms or a source of molecular hydrogen isotopes and a source of catalyst 58 which resonantly removes approximately m · 27.2 eV to form a low energy hydrogen atom, where m is An integer, preferably an integer less than 400, wherein the reaction with hydrogen in the low energy state occurs by contacting hydrogen with a catalyst. The catalyst can be in molten, liquid, gas or solid state. Catalysis releases energy in a form such as heat and forms at least one of low energy hydrogen isotope atoms, molecules, hydride ions, and low energy hydrogen compounds. Thus, the power cell also includes a low energy hydrogen chemical reactor.

The hydrogen source can be hydrogen gas, dissociation of water including thermal dissociation, electrolysis of water, hydrogen obtained from hydrides, or hydrogen obtained from metal-hydrogen solutions. In another embodiment, the hydrogen molecules in the energy releasing material 56 dissociate into hydrogen atoms by the hydrogen molecular dissociation catalyst of the mixture 54. The dissociation catalyst can absorb hydrogen, deuterium, tritium atoms and / or molecules, for example elements, compounds, alloys, or precious metals such as palladium and platinum, refractory metals such as molybdenum and tungsten, nickel , Transition metals such as titanium, internal transition metals such as niobium and zirconium, and other materials mentioned in the Mills literature. Preferably, the dissociating agent has a high surface area, such as noble metals such as Pt, Pd, Ru, Ir, Re or Rh or Al 2 O 3, Ni on SiO 2, or a combination thereof.

In one embodiment, the catalyst is provided by ionizing t electrons up to a continuum energy level where the sum of ionization energies of t electrons from atoms or ions is approximately m · 27.2 eV, where t and m are each integers. . The catalyst can also be provided by transferring t electrons between participating ions. The transfer of t electrons from one ion to another provides the net enthalpy of the reaction, whereby the t ionization energy of the ion giving electron minus the ionization energy of the t electron of the receiving ion is m · 27.2 eV (Where t and m are each an integer). In another preferred embodiment, the catalyst comprises MH, such as NaH with M atoms bonded to hydrogen, provided m · 27.2 eV as the sum of the M-H binding energy and the ionization energy of t electrons.

In a preferred embodiment, the catalyst source comprises catalyst material 58 fed through the catalyst feed path 41 and generally provides a net enthalpy of approximately ± 1 eV. The catalyst is the atom described in the specification and in Mills prior art (see, eg, Table 4 of PCT / US90 / 01998 and 25-46, pages 80-108 of PCT / US94 / 02219), incorporated herein by reference, Ions, molecules, and hydrinos. In an embodiment, the catalyst is a molecule of AlH, BiH, ClH, CoH, GeH, InH, NaH, RuH, SbH, SeH, SiH, SnH, C2, N2, O2, CO2, NO2 and NO3 and Li, Be, K, Ca, Ti, V, Cr, Mn, Fe, Co, Ni, Cu, Zn, As, Se, Kr, Rb, Sr, Nb, Mo, Pd, Sn, Te, Cs, Ce, Pr, Sm, Atoms and ions of Gd, Dy, Pb, Pt, Kr, 2K +, He +, Na +, Rb +, Sr +, Fe3 +, Mo2 +, Mo4 +, In3 +, He +, Ar +, Xe +, Ar2 + and H +, and Ne + and H + It may include at least one species.

Hydrogen Catalytic Reactor and Electric Force System

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

 One embodiment of a hydrogen catalytic energy and low energy hydrogen species generation reactor 5 for recycling or regenerating fuel according to the invention is shown in FIG. 2A, which is a solid fuel mixture 11, a hydrogen source 12, a steam pipe and A boiler containing a steam generator 13, a power converter such as a turbine, a water condenser 16, a water-supplement source 17, a solid fuel recycler 18, and a hydrogen-dihydrino gas separator 19. 10). In step 1, the solid fuel comprising the catalyst and the hydrogen source reacts to form hydrino and low energy hydrogen products. In step 2, the spent fuel is reprocessed and resupplied to the boiler 10 to maintain thermal power generation. Heat generated in the boiler 10 forms steam in the pipe and steam generator 13 and is transferred to the turbine 14 to generate electricity by running a generator this time. In step 3, water is condensed by the water cooler 16. Water loss is caused by the water source 17 to complete the cycle and maintain thermo-electric force conversion. In step 4, low energy hydrogen products, such as hydrino hydride compounds and dihydrino gas, can be removed, and unreacted hydrogen is returned to the fuel recycler 18 or hydrogen source 12 and added back to the spent fuel. To replenish recycled fuel. The gas product and unreacted hydrogen can be separated by a hydrogen-dihydrino gas separator 19. Any product, the hydrino hydride compound, can be separated and removed using the solid-fuel recycler 18. The process can be carried out inside or outside the boiler where the solid fuel is returned. Thus, the system may further include at least one gas and mass transfer device that moves the reactants and products to achieve spent fuel removal, regeneration, and re-feed. Hydrogen to supplement the hydrogen used to form the hydrinos is added from the source 12 during fuel regeneration, which may include recycled unconsumed hydrogen. The recycled fuel maintains thermal power production, causing the power generator to produce electricity.

In a preferred embodiment, the reaction mixture can produce a reactant of an atomic or molecular catalyst and further react with hydrogen atoms to form hydrinos, wherein the product species formed by the production of catalyst and atomic hydrogen is at least hydrogen It can be regenerated by the step of reacting with. In one embodiment, the reactor comprises a moving bed reactor, which may further comprise a fluidization reactor section in which the reactants are continuously fed and by-products are removed and regenerated and returned to the reactor. In one embodiment, low energy hydrogen products, such as hydrino hydride compounds or dihydrino molecules, are recovered as the reactants are regenerated. Furthermore, hydrino hydride ions can be converted to dihydrino molecules during formation of other compounds or during the regeneration of the reactants.

The power system may further comprise catalytic condenser means for maintaining the catalyst vapor pressure by means of temperature control means for regulating the surface temperature to a lower temperature than the reaction cell. The surface temperature is maintained at the desired value to provide the desired vapor pressure of the catalyst. In one embodiment, the catalyst condenser means is a tube grid in the cell. In one embodiment of the heat exchanger, the flow rate of the heat exchange medium may be adjusted at a rate that keeps the condenser at a desired temperature lower than the main heat exchanger. In one embodiment, the working medium is water and the flow rate is higher in the cooler than in the water wall, in order to bring the condenser to a lower and preferred temperature. Each flow of working medium can be recombined to be delivered for conversion to space and thermal processes or steam.

The energy invention is further described in the Mills preceding document incorporated by reference into the specification. Cells of the present invention include those previously described and further include the catalysts, reaction mixtures, methods, and systems disclosed herein. Electrolytic cell energy reactor, plasma electrolysis reactor, gas discharge energy reactor, barrier electrode reactor, RF plasma reactor, pressurized gas energy reactor, gas discharge energy reactor, microwave cell energy reactor, and glow discharge cell and microwave and / or Combinations of RF plasma reactors include: hydrogen sources; One of a solid, molten, liquid and gas source of the catalyst; A vessel containing hydrogen and a catalyst, wherein the reaction to form low energy hydrogen is brought about by contacting the hydrogen with the catalyst or by reaction of the MH catalyst. For power conversion, each cell type is adapted to mechanically or thermally convert thermal energy or plasma as described in the Mills prior art, as well as transducers known to those skilled in the art such as thermal engines, steam or gas turbine systems, stirling engines or thermal ion or thermal power converters. It can be connected with any transducer that converts to electric force.

Additional plasma converters include magnetic mirror magnetic fluid power converters, plasmadynamic power converters, gyrotrons, photon bunching microwave power converters, charge drift power or Photoelectric converters.

In one embodiment, the cell comprises at least one cylinder of an internal combustion engine as set forth in Mills prior art.

Hydrogen Gas Cells and Solid Fuel Reactors

According to one embodiment of the invention, the hydrino and reactor for generating power may take the form of a hydrogen gas cell. The gas cell hydrogen reactor of the present invention is shown in FIG. 3A. The reactant hydrinos are provided by catalysis with a catalyst. Catalysis may occur in the gas phase or in the solid or liquid state.

 The reactor of FIG. 3A includes a reaction vessel 207 having a chamber 200 which may include pressure rather than vacuum or atmospheric pressure. The hydrogen source 201 connected with the chamber 200 delivers hydrogen to the chamber via the hydrogen supply path 242. The regulator 222 is positioned to regulate the pressure and flow of hydrogen entering the vessel through the hydrogen supply path 242. Pressure sensor 223 monitors the pressure in the vessel. Vacuum pump 256 is used to remove air from the chamber through vacuum tube 257.

In one embodiment, the catalysis takes place in the gas phase. The catalyst is gasified by keeping the cell temperature at a high temperature, which in turn determines the air pressure of the catalyst. Atomic and / or molecular hydrogen reactants are also maintained at the desired pressure, which can be in any range of force. In one embodiment, the pressure is lower than air pressure, preferably in the range of about 10 mTorr to about 100 mTorr. In another embodiment, the pressure is determined by maintaining a mixture of a catalyst source, such as a metal source, and a corresponding hydride, such as a metal hydride, in a cell maintained at a desired operating temperature.

Catalyst source 250 for generating hydrino atoms can be placed in catalyst reservoir 295 and a gas catalyst can be formed by heating. The reaction vessel 207 has a catalyst feed path 241 for the passage of the gas catalyst from the catalyst reservoir 295 to the reaction chamber 200. Alternatively, the catalyst may be disposed in a chemical resistant open container such as a boat inside the container.

The hydrogen source can be hydrogen gas and molecular hydrogen. Hydrogen can be dissociated into hydrogen atoms by molecular hydrogen dissociation catalysts. The dissociation catalyst or dissociating agent includes, for example, Raney nickel (R-Ni), a valuable metal or precious metal, a valuable metal or precious metal on a support. The oil value or precious metal may be Pt, Pd, Ru, Ir, and Rh, and the support may be at least one of Ti, Nb, Al 2 O 3, SiO 2, and a combination thereof. Additional dissociating agents such as hydrogen spillover catalysts, nickel fiber mats, Pd sheets, Ti sponges, Ti or Ni sponges or Pt or Pd, TiH, Pt black, and Pd black, molybdenum and tungsten electroplated on the mat Pt or Pd on carbon, which may include refractory metals, transition metals such as nickel and titanium, and other such materials mentioned in the previous Mills literature. In a preferred embodiment, the hydrogen dissociates on Pt or Pd. The Pt or Pd may be coated on a support material such as titanium or Al 2 O 3. In another embodiment, the dissociating agent is a refractory metal such as tungsten or molybdenum, the dissociating material being raised by means of temperature control means 230 which can take the form of a heating coil as shown in the cross-sectional view of FIG. 3A. Can be maintained at a temperature. The heating coil is powered by a power supply 225. Preferably, the dissociation material is maintained at the operating temperature of the cell. The dissociating agent may be further operated at a temperature above the cell temperature to dissociate more effectively, and the elevated temperature may prevent the catalyst from condensing on the dissociating agent. Hydrogen crackers may also be provided by hot filaments such as 280 powered by feeder 285.

In one embodiment, hydrogen dissociation occurs such that the dissociated hydrogen atoms come into contact with the gaseous catalyst to produce hydrino atoms. The catalytic vapor pressure is maintained at the desired pressure by adjusting the temperature of the catalyst reservoir 295 with the catalyst reservoir heater 298 powered from the power supply 272. Once the catalyst is contained in the boat inside the reactor, the catalyst vapor pressure is maintained at the desired value by controlling the temperature of the catalyst boat by regulating the boat's power supply. The cell temperature may be adjusted at the desired operating temperature by the heating coil 230 powered by the power supply 225. The cell (called permeate cell) further includes an internal reaction chamber 200 and an external hydrogen reservoir 290 so that hydrogen can be supplied to the cell by hydrogen diffusion through the walls 291 separating the two chambers. have. The temperature of the wall can be controlled with a heater to control the rate of diffusion. The diffusion rate can be further controlled by adjusting the hydrogen pressure in the hydrogen reservoir.

In order to maintain the catalyst pressure at the desired level, a cell with permeation, such as a hydrogen source, can be sealed. Alternatively, the cell further includes a high temperature valve at each inlet or outlet such that the valve in contact with the reaction gas mixture is maintained at the desired temperature. The cell may further comprise a getter or trap 225 for selectively collecting low energy hydrogen species and / or hydrogen compounds with increased binding energy, and an optional valve for releasing the dihydrino gas product. 206 may further include.

The catalyst may comprise at least one or more of a group of lithium atoms, potassium atoms or cesium atoms, NaH molecules and hydrino atoms, wherein the catalysis comprises a disproportion reaction. The lithium catalyst becomes a gas by keeping the cell temperature in the range of 500-1000 ° C. Preferably the cell is maintained in the range of 500-750 ° C. The cell pressure may be maintained at less than atmospheric pressure, preferably in the range of about 10 mTorr to about 100 Torr. Most preferably, at least one of the catalyst and hydrogen pressure is desired for a mixture of catalytic metals and corresponding hydrides, such as lithium and lithium hydrides, potassium and potassium hydrides, sodium and sodium hydrides, and cesium and cesium hydrides. Determined by keeping in a cell maintained at the operating temperature. The gas phase catalyst may include lithium atoms from metal or lithium metal sources. Preferably, the lithium catalyst is maintained at a pressure determined by a mixture of lithium metal and lithium hydride in the operating temperature range of 500-1000 ° C., most preferably at a pressure having a cell in the operating temperature range of 500-750 ° C. . In another embodiment, K, Cs, and Na replace Li, wherein the catalyst is a K atom, a Cs atom, and a NaH molecule.

One embodiment of a gas cell reactor that includes a catalyst reservoir or boat, gaseous Na, NaH catalyst, or gaseous catalysts such as Li, K, and Cs vapors, overheats in the cell relative to the vapor in the reservoir or boat that is the source of cell steam. maintained in super-heated conditions. In one embodiment, the superheated steam reduces the condensation of the catalyst on the dissociating agent of at least one of the hydrogen dissociating agent or the metal and metal hydride molecules disclosed in the infra. In one embodiment that includes Li as catalyst from a reservoir or boat, the reservoir or boat is maintained at a temperature at which Li evaporates. H2 is maintained at a pressure lower than the pressure at which LiH forms a sharp mole fraction at the reservoir temperature. The pressure and temperature to achieve this condition can be determined from a data straight line such as Mueller et al. As shown in FIG. 6.1 [40] of H2 pressure versus LiH mole fraction at a given isotherm. In one embodiment, the cell reaction chamber containing the dissociating agent is operated at high temperatures at which Li does not condense on the wall or dissociating agent. H2 may flow from the reservoir into the cell to increase the catalyst delivery rate. The flow out of the cell after flowing from the catalyst reservoir to the cell is a means of removing the hydrino product to prevent the hydrino from inhibiting the reaction. In another embodiment, K, Cs and Na replace Li, wherein the catalyst is a K atom, a Cs atom and a NaH molecule.

Hydrogen is supplied to the reaction from a hydrogen source. Preferably, hydrogen is supplied by the permeable membrane from the hydrogen reservoir. The pressure of the hydrogen reservoir may be in the range of 10 Torr to 10,000 Torr, preferably 100 Torr to 1000 Torr, most preferably approximately atmospheric pressure. The cell may be operated at a temperature of about 100 ° C. to 3000 ° C., preferably at a temperature of about 100 ° C. to 1500 ° C., and most preferably about 500 ° C. to 800 ° C.

The hydrogen source may be from the decomposition of the added hydride. The cell design of supplying H2 by the permeable membrane includes internal metal hydrides located in sealed containers where H atoms are permeated at high temperatures. The container may comprise Pd, Ni, Ti or Nb. In one embodiment, the hydride is located in a sealed tube, such as an Nb tube containing hydride, and both ends are sealed with a sealing device, such as a swage lock. In the sealed case, the hydride can be an alkaline or alkaline earth hydride. Alternatively, in the case of the internal-hydride-reagent case, the hydrides are saline hydrides, titanium hydrides, vanadium, niobium and tantalum hydrides, zirconium and hafnium hydrides, rare earth hydrides, yttrium and scandium Hydrides, transition metal hydrides, intermetalic hydrides and at least one of the groups of alloys presented by WM Mueller et al. [40].

In one embodiment, based on each hydride decomposition temperature, the hydride and operating temperature ± 200 ° C. are at least one of the following list:

Rare earth hydrides having an operating temperature of 800 ° C .; Lanthanum hydride having an operating temperature of 700 ° C .; Gadolinium hydride with an operating temperature of 750 ° C .; Neodymium hydride with an operating temperature of 750 ° C .; Yttrium hydride with an operating temperature of 800 ° C .; Scandium hydride having an operating temperature of 800 ° C .; Ytterbium hydride with an operating temperature of 850-900 ° C .; Titanium hydride having an operating temperature of about 450 ° C .; Cerium hydride having an operating temperature of about 950 ° C .; Praseodymium hydride having an operating temperature of about 700 ° C .; Zirconium-titanium (50% / 50%) hydride having an operating temperature of about 600 ° C .; Alkali metal / alkali metal hydride mixtures such as Rb / RbH or K / KH having an operating temperature of about 450 ° C .; And alkaline earth metal / alkaline earth metal hydride mixtures such as Ba / BaH 2 having an operating temperature of about 900-1000 ° C .;

The gaseous metal contains diatomic covalent molecules. It is an object of the present invention to provide atomic catalysts such as Li as well as K and Cs. Thus, the reactor may further comprise a dissociating agent of at least one of metal molecules ("MM") and metal hydride molecules ("MH"). Preferably, the catalyst source, H2 source, and dissociating agents of MM, MH and HH, where M is an atomic catalyst, are matched to operate at the desired cell conditions, for example, of temperature and reactant concentration. In one embodiment, when a H2 hydride source is used, its decomposition temperature is within the range of temperatures that produce the vapor pressure of the desired catalyst. When the hydrogen source is permeated from the hydrogen reservoir to the reaction chamber, the preferred catalyst sources for continuous operation are Sr and Li, since their respective vapor pressures are within the desired range of 0.01 to 100 Torr at the temperature at which permeation occurs. In another embodiment of the permeate cell, the cell is operated at a high temperature that permits permeation and then down to a temperature at which the cell temperature maintains the vapor pressure of the volatile catalyst at the desired pressure.

In one embodiment of the gas cell, the dissociating agent comprises means for producing catalyst and H from the source. Pt on Ti or Pd, surface catalysts such as iridium or rhodium alone or on substrates such as Ti, also function as dissociating agents of molecules in which the catalyst and atomic hydrogen are combined. Preferably, the dissociating agent has a high surface area such as Pt / Al 2 O 3 orPd / Al 2 O 3.

The H2 source can also absorb H2 gas. In this case, the pressure is observed and adjusted. This is possible with catalysts and catalyst sources such as K or Cs metals and LiNH2, respectively, since they volatilize at low temperatures allowing the use of high temperature valves. LiNH2 also lowers the required operating temperature of the Li cell and allows long-duration operations by injecting the filament through the inside of the casing of the filament cell where the corrosion is low and the filament acts as a hydrogen dissociating agent.

A further embodiment of a gas cell hydrogen reactor with NaH as catalyst comprises a filament with Na in the reservoir and a dissociating agent in the reactor cell. H2 can flow into the main chamber through the reservoir. The power is regulated by adjusting the gas flow rate, H2 pressure and Na vapor pressure. The latter can be adjusted by adjusting the reservoir temperature. In another embodiment, the hydrino reaction is initiated by heating with an external heater and H atoms are supplied by the dissociating agent.

The invention also relates to other reactors for producing hydrogen compounds with increased binding energy of the invention such as dihydrino molecules and hydrino hydride compounds. Additional products of catalysis are plasma, light and power. The reactor is hereinafter referred to as "hydrogen reactor" or "hydrogen cell". The hydrogen reactor includes a cell for making hydrinos. The cells for making hydrinos may take the form of, for example, gas cells, gas discharge cells, plasma torch cells or microwave power cells. Such exemplary cells are disclosed in Mills prior art and incorporated by reference. Each such cell comprises a hydrogen atom source; At least one of a solid, molten or gaseous catalyst for making hydrinos; And a vessel for reacting hydrogen and catalyst for making hydrinos. As used and discussed in this specification, the term "hydrogen" includes proteum (1H) as well as deuterium (2H) and tritium (3H) unless otherwise specified.

Hydrogen Gas Discharge Power and Plasma Cells and Reactors

The hydrogen gas discharge power and plasma cell and reactor of the present invention are shown in FIG. 4A. The hydrogen gas discharge power and plasma cell and reactor of FIG. 4A include a gas discharge cell 307 including a glow discharge vacuum vessel 355 filled with hydrogen gas having a chamber 300. Hydrogen source 322 supplies hydrogen to chamber 300 via control valve 325 by hydrogen supply path 342. The catalyst is contained in the cell chamber 300. Voltage and current source 330 allows current to pass between anode 305 and cathode 320. The current can be reversible.

In one embodiment, the material of anode 305 may be a catalyst source such as Fe, Dy, Be, or Pd. In another embodiment of hydrogen gas discharge power and plasma cells and reactors, the walls of the vessel 313 are conductive and serve as anodes that replace the electrodes 305, and the cathode 320 is centered like a stainless steel hollow cathode. May be pierced. The discharge can evaporate the catalyst source to the catalyst. Hydrogen molecules can be dissociated by discharge to form hydrogen atoms for generating hydrinos and energy. Further dissociation may occur by hydrogen dissociation agent in the chamber.

Another embodiment of hydrogen gas discharge power and plasma cells and reactors where the catalyst occurs in the gas phase utilizes an adjustable gas catalyst. Gas hydrogen atoms for conversion to hydrinos are provided by the discharge of hydrogen molecular gas. The gas discharge cell 307 has a catalyst feed path 341 for the passage of the gas catalyst 350 from the catalyst reservoir 395 to the reaction chamber 300. The catalyst reservoir 395 is heated by a catalyst reservoir heater 392 having a power source 372 for supplying a gaseous catalyst to the reaction chamber 300. The catalyst vapor pressure is controlled by adjusting the heater 392 by the power supply 372 to adjust the temperature of the catalyst reservoir 395. The reactor also further includes an optional venting valve 301. Chemically resistant open containers, such as stainless steel, tungsten or ceramic boats, which are located inside the gas discharge cell, may contain a catalyst. The catalyst in the catalyst boat may be heated by a boat heater using an associated power supply to provide a gas catalyst to the reaction chamber. Alternatively, the glow gas discharge cell is operated at an elevated temperature such that the catalyst in the boat sublimes, boils or evaporates to become gaseous. To prevent the catalyst from condensing in the cell, the temperature is maintained above the temperature of the catalyst source, catalyst reservoir 395 or catalyst boat.

In a preferred embodiment, the catalysis takes place in the gas phase, lithium is the catalyst, and a lithium atom source such as lithium metal or a lithium compound such as LiNH 2 is gasified by maintaining the cell temperature in the range of about 300-1000 ° C. More preferably, the cell is maintained in the range of about 500-750 ° C. Atomic and / or molecular hydrogen reactants are maintained at pressures below atmospheric pressure, preferably in the range of about 10 mTorr to about 100 Torr. Most preferably, the pressure is determined by maintaining a mixture of lithium metal and lithium hydride in a cell maintained at the desired operating temperature. The operating temperature range is preferably in the range of 300-1000 ° C. and most preferably the pressure is achieved with a cell at an operating temperature of about 300-750 ° C. The cell can be adjusted to a desired operating temperature by a heating coil such as 380 of FIG. 4A powered by power supply 385. The cell may further include an internal reaction chamber 300 and an external hydrogen reservoir 390 so that hydrogen can be supplied to the cell by diffusing hydrogen through the wall 313 separating the two chambers. The temperature of the wall can be controlled with a heater to control the rate of diffusion. The diffusion rate can be further controlled by adjusting the hydrogen pressure in the hydrogen reservoir.

One embodiment of the plasma cell of the present invention regenerates reactants such as Li and LiNH 2. In one embodiment, the reaction given by equations (32) and (37) occurs to produce hydrino reactants, Li and H, with significant excess energy released due to hydrino production. The product is then hydrogenated by a hydrogen source. When LiH is formed, one reaction to produce a low energy hydrogen catalyzed reactant is shown in equation (66). This may be accomplished with a reactant located in the reaction region in the plasma cell, such as in the anode region in the hydrogen plasma cell. The reaction may be LiH + e--> Li and H- (30), after which a reaction of Li2NH + H-> Li + LiNH2 (31) occurs to a certain extent and the steady-state of Li + LiNH2 ) Can maintain the level. The pressure, electron density, and energy can be adjusted to achieve a maximum or desired degree of reaction to produce the hydrino reactant Li + LiNH 2.

In one embodiment, the mixture is stirred or mixed during the plasma reaction. In a further embodiment of the plasma regeneration system and method of the present invention, the cell comprises a heated flat-bottom stainless steel plasma chamber. LiH and Li 2 NH include molten Li mixtures. Since stainless steel is not magnetic, the liquid mixture can be agitated with a stainless steel coated stir bar driven by a stir motor installed in a flat-bottom plasma reactor. The Li-metal mixture can serve as an anode. Reduction of LiH to Li and further reaction of H- + Li2NH to Li and LiNH2 can be monitored by XRD and FTIR of the product. In another embodiment of a system having a reaction mixture comprising species of the group Li, LiNH2, Li2NH, Li3N, LiNO3, LiX, NH4X (Xisahalide), NH3, and H2, the addition of one or more reagents and the plasma regeneration Thereby regenerating at least one of the reactants. Plasma was NH3andH2. It may be any one of such gases. The plasma may be maintained in place (in the reaction cell) or in an outer cell in communication with the reaction cell. In another embodiment, K, Cs, and Na replace Li, where the catalyst is a K atom, a Cs atom, and a NaH molecule.

In order to maintain the catalyst pressure at the desired level, a cell with permeation, such as a hydrogen source, can be sealed. Alternatively, a high temperature valve is further included at each entry or exit to maintain the valve in contact with the reaction gas mixture at a desired temperature.

The plasma cell temperature can be adjusted independently and broadly by isolating the cell and supplying supplemental heater power to the heater 380. Thus, the catalytic vapor pressure can be adjusted independently of the plasma power.

The discharge voltage is in the range of about 100 to 10,000 volts. The current can be in any desired range at the desired volts. Further, the plasma may be pulsed as disclosed in Mills prior art, such as PCT / US04 / 10608 (named “Pulsed Plasma Power Cell and Novel Spectral Lines”), incorporated herein by reference.

Boron nitride may include feed-through of the plasma cell because the material is stable to Li vapor. Crystalline or transparent alumina is another stable feed through material of the present invention.

Solid Fuel and Hydrogen Catalytic Reactors

The gaseous metal contains diatomic covalent molecules. It is an object of the present invention to provide atomic and molecular catalysts NaH such as Li as well as K and Cs. Thus, in one embodiment of a solid-fuel, the reactant comprises a source of a composite which reversibly forms and decomposes or reacts with the alloy, complex or metal catalyst M to provide a gas catalyst such as Li. In yet another embodiment, at least one of the catalyst source and the hydrogen atom source further comprises at least one reactant that reacts to form at least one of the catalyst and atomic hydrogen. In one embodiment, the source comprises at least one of an amide such as LiNH2, an imide such as Li2NH, a nitride such as Li3N, and at least one of a catalytic metal with NH3. These and other examples are given in infra., Where additionally K, Cs, and Na can replace Li and the catalyst is a K atom, a Cs atom and a NaH molecule.

The present invention relates to an energy reactor comprising a reaction vessel constructed and arranged to contain a pressure lower than, equal to, or higher than atmospheric pressure, a source of hydrogen atoms for chemically producing hydrogen atoms in communication with the vessel, lithium in communication with the vessel. And a source of catalyst comprising at least one of atoms, cesium atoms, potassium atoms, and NaH molecules, and may further comprise a getter, such as a source of ionic compounds for binding or reacting with low energy hydrides. Sources of catalyst and reactant hydrogen atoms can include solid fuels that are continuously or batch-regenerated inside or outside the cell, where physical processes or chemical reactions are performed to cause H catalysis and hydrinos to form. The catalyst and H are produced from the source. Thus, embodiments of the hydrino reactant of the present invention include solid fuels, and preferred embodiments include solid fuels that can be recycled. Solid fuels can be used in a variety of applications, including space and process heating, electricity generation, power applications, propellants, and other application ranges well known to those skilled in the art.

Gas cells or plasma cells of the present invention as shown in FIGS. 3A and 4A include means for forming catalyst and H from a source. In a solid-fuel embodiment, the cell further comprises a reactant to provide catalyst and H when initiating a chemical or physical process. The process is initiated by means such as heating or plasma reaction. Preferably, the need for external power to maintain hydrino production is low or little compared to the large power of the H catalytic reaction to produce hydrinos. The reactants can be regenerated with net release energy for reaction and regeneration.

In another embodiment, the reactor shown in FIG. 3A includes a solid fuel reactor, where the reaction mixture comprises a catalyst source and a hydrogen source. The reaction mixture can be regenerated by feeding the stream of reactants and by removing the product from the corresponding product mixture. In one embodiment, reaction vessel 207 has a chamber 200 that may contain a vacuum or a pressure equal to or greater than atmospheric pressure. At least one source of reagent is in communication with the chamber, such as gaseous reagent 221, and delivers the reagent to the chamber via at least one or more reagent supply paths 242. The controller 222 is arranged to regulate the pressure of the reagent and the flow of the reagent into the vessel through the reagent supply path 242. Vacuum pump 256 is used to empty the chamber through vacuum line 257. Alternatively, line 257 represents at least one outlet, such as a product pathway line, which removes material from the reactor. The reactor further includes a heat source such as a heater 230 for raising the reactants to the desired temperature to initiate solid fuel chemistry and hydrino-forming catalytic reactions. In one embodiment, the temperature is in the range of about 50-1000 ° C., preferably in the range of about 100-600 ° C., and at least for reactants comprising a Li / N-alloy system, the desired temperature is 100-500 ° C. Range.

The cell may further comprise a hydrogen gas source and a dissociating agent to form hydrogen atoms of the hydrogen gas. The vessel may further include a hydrogen source 221 in communication with the vessel for producing at least one of an atomic catalyst source, such as a lithium atom, and a hydrogen atom source. The hydrogen source may be hydrogen gas. H2 gas may be supplied from hydrogen reservoir 290 by hydrogen line 242 or by permeation. In an exemplary regeneration reaction, the source of lithium atoms and atomic hydrogen can be regenerated by hydrogenation according to formula (66-71). The first step of an alternative regeneration reaction can be given by equation (69).

In one embodiment, cell size and material is such that a high operating temperature is recorded. The cell may be suitably fabricated in accordance with the power outlet to achieve the desired operating temperature. High temperature materials for cell fabrication are high temperature stainless steels such as niobium and Hastorloy. The H2 source may be an internal metal hydride that does not react with LiNH2 but releases only H at very high temperatures. In addition, when hydrides react with LiNH 2, they can be separated from reagents such as Li and LiNH 2 by placing them in an open or closed vessel in the cell. The cell design of supplying H2 by permeation includes internal metal hydrides disposed within a sealed vessel through which hydrogen atoms permeate at high temperatures.

The reactor may further comprise means for separating the components of the product mixture, such as a sieve which mechanically separates due to differences in physical properties such as size. The reactor may further comprise means for separating one or more components based on phase change or reaction difference. In one embodiment, the phase change comprises melting with a heater, and the liquid is separated from the solid by means known in the art, such as gravity filtration, filtration with pressurized gas, and centrifugation. The reaction may include decomposition such as hydride decomposition, and the separation may be performed by melting the corresponding metals, respectively, and then separating them or mechanically separating the hydrides. The latter can be achieved by sifting. In one embodiment, the phase change or reaction may produce the desired reactant or intermediate. In an embodiment, the regeneration comprising any desired separation step may occur inside or outside the reactor.

Chemical reactor

The chemical reactor of the present invention further comprises a source of an inorganic compound, such as MX, where M is an alkali metal and X is a halide. In addition to hydrides, inorganic compounds include alkaline earth salts such as alkalis or hydroxides, oxides, carbonates, sulfates, phosphates, borates, and silicates (other suitable inorganic compounds are described herein by DR Lide, CRCH and book). of Chemistry and Physics, 86th Edition, CRC Press, Taylor & Francis, Boca Raton, (2005-6), pp. 4-45 to 4-97). Inorganic compounds can additionally act as getters in producing power or inhibiting other products by preventing product accumulation and the resulting back reaction. Preferred Li chemical-type power cells include Li, LiNH 2, LiBr or LiI and R—Ni in hydrogen cells operating at about 760 Torr H 2 and about 700 + ° C. Preferred NaH chemical-type power cells include Na, NaX (X is a halide, preferably Br or I) and R-Ni in a hydrogen cell operating at about 760 Torr H2 and about 700+ ° C. The cell may further comprise at least any one of. Preferred K chemical-type power cells include K, KI, and Ni screens or R-Ni dissociating agents in hydrogen cells operating at about 760 Torr H2 and about 700+ ° C. In one embodiment, the H2 pressure range is about 1 Torr to 105 Torr. Preferably the hydrogen is maintained in the range of about 760-1000 Torr. LiHX such as LiHBr and LiHI are generally synthesized at a temperature range of about 450-550 ° C., but can be operated at lower temperatures (˜350 ° C.) with LiH present. NaHX such as NaHBr and NaHI are generally synthesized in the temperature range of about 450-550 ° C. KHX, such as KHI, is synthesized in the temperature range of about 450-550 ° C. In embodiments of the NaHX and KHX reactors, NaH and K are fed from a source such as a catalyst reservoir, where the cell temperature is maintained at a higher level than the catalyst reservoir. Preferably, the cell is maintained at a temperature range of about 300-500 ° C. and the reservoir is maintained at a temperature range of about 50-200 ° C. or less.

Another embodiment of a hydrogen reactor with NaH as a catalyst is a plasma torch for the generation of hydrogen compounds with increased binding energy such as power and NaHX (where H is hydrogen with increased binding energy and X is halide). It includes. At least one of NaF, NaCl, NaBr, NaI can be sprayed into a plasma gas, such as H2 or a noble gas / hydrogen mixture such as He / H2 or Ar / H2.

General solid fuel chemistry

The reaction mixture of the present invention comprises a catalyst or catalyst source and a hydrogen atom or atomic hydrogen (H) source, wherein at least one of the catalyst and the hydrogen atom is by chemical reaction between one or more reaction mixture species or two or more reaction mixture species Is released. Preferably, the reaction is reversible. Preferably, the released energy is greater than the enthalpy of the reaction of the formation of the catalyst and reactant hydrogen, and when the reactants of the reaction mixture are recycled and recycled, preferably, the greater of the product H state given by formula (1) Formation energy releases net energy over the cycle of reaction and regeneration. The species may be one or more of elements, alloys or compounds such as molecules or organic compounds, each of which may be one or more of the reactants or products in the reactor. In one embodiment, the species may form an alloy or compound such as a molecule or an organic compound with at least one of hydrogen and a catalyst. The one or more reaction mixture species form one or more reaction product species such that the release energy of H or free catalyst is relatively lower than without the formation of the reaction product species. In an embodiment in which the reactant provides a catalyst and atomic hydrogen to form a state having an energy level given by Formula (1), the reactant comprises at least one of a solid, a liquid (including molten state) and a gaseous reactant . The reaction for forming the catalyst and atomic hydrogen to form a state having an energy level given by formula (1) takes place in one or more of the solid, liquid (including molten state) and gas phases. Exemplary solid-fuel reactions presented herein are not meant to be limiting in any way, as other reactions involving additional reagents are also within the scope of the present invention.

In one embodiment, said reaction product species is an alloy or compound of at least one of said catalyst and hydrogen or a source thereof. In one embodiment, the reaction mixture species is catalytic hydride and the reaction product species is a catalyst alloy or compound having a relatively low hydrogen content. The energy to release H from the hydride of the catalyst can be lowered by the formation of an alloy or a second compound with one or more other species such as an element or a first compound. In one embodiment, the catalyst is one of Li, K, Cs and NaH molecules, the hydride is one of LiH, KH, CsH and NaH, and the one or more other elements are M (catalyst), Al, B, Si, C, N, Sn, Te, P, S, Ni, Ta, Pt and Pd. The first and second compounds are H 2, H 2 O, NH 3, NH 4 X (X is a counterion such as a halide, and other anions are described in DR Lide, CRC Handbook of Chemistry and Physics, 86th Edition, CRC Press, Taylor & Francis, Boca Raton, (2005-6), pp.4-45 to 4-97, which is incorporated herein by reference), MX, MNO3, MAlH4, M3AlH6, MBH4, M3N, M2NH and MNH2 Where M is an alkali metal, which may be a catalyst. In another embodiment, hydrides comprising at least one element other than the catalytic element release H by reversible decomposition.

One or more reaction mixture species may form one or more reaction product species such that the free catalyst release energy is relatively lower than in the absence of reaction product species formation. Reactive species such as alloys or compounds may release the free catalyst by reversible reaction or decomposition. The free catalyst may also be formed by reversible reaction of the catalyst source using one or more other species such as an element or a first compound to form a species such as an alloy or a second compound. The element or alloy may include one or more of M (catalyst atom), H, Al, B, Si, C, N, Sn, Te, P, S, Ni, Ta, Pt and Pd. The first and second compounds may be one of the group of H 2, NH 3 and NH 4 X, where M is an alkali metal, which may be a catalyst. The catalyst may be one of Li, K and Cs atoms, and NaH molecules. The catalyst source can be M-M such as LiLi, KK, CsCs and NaNa. The H source may be MH such as LiH, KH, CsH or NaH.

The Li catalyst can be alloyed or reacted to form a compound having one or more other elements or compounds to lower the energy barrier to Li release from LiH, or from LiH and LiLi molecules. In addition, the alloy or compound may release H or Li by decomposition or reaction with additional reactive species. The alloy or compound may be one or more of the group of LiAlH4, Li3AlH6, LiBH4, Li3N, Li2NH, LiNH2, LiX and LiNO3. The alloy or compound may be one or more of Li / Ni, Li / Ta, Li / Pd, Li / Te, Li / C, Li / Si, and Li / Sn, wherein Li and any other element of the alloy or compound Li and H can be optimally released depending on the equivalent ratio of the liver, which then reacts during the catalytic reaction to form hydrogen in a relatively low energy state. In other embodiments, K, Cs and Na replace Li, wherein the catalyst is a K atom, a Cs atom and a NaH molecule.

In one embodiment, the alloy or compound has the formula MxEy, where M is a catalyst such as Li, K or Cs or Na, E is another element, and x and y represent equivalent ratios. M and Ey may be in any desired molar ratio. In one embodiment, x is in the range from 1 to 50, y is in the range from 1 to 50, preferably x is in the range from 1 to 10, and y is in the range from 1 to 10.

In another embodiment, the alloy or compound has the formula MxEyEz, wherein M is a catalyst such as Li, K or Cs or Na, Ey is the first other element, Ez is the second other element, x, y And z represents an equivalent ratio. M, Ey and Ez may be any desired molar ratios. In one embodiment, x is in the range from 1 to 50, y is in the range from 1 to 50, z is in the range from 1 to 50, preferably x is in the range from 1 to 10, y is in the range from 1 to 10, and z is Range from 1 to 10. In a preferred embodiment, Ey and Ez are selected from the group of H, N, C, Si and Sn. The alloy or compound may be one or more of LixCySiz, LixSnySiz, LixNySiz, LixSnyCz, LixNySnz, LixCyNz, LixCyHz, LixSnyHz, LixNyHz and LixSiyHz. In other embodiments, K, Cs and Na replace Li, wherein the catalyst is a K atom, a Cs atom and a NaH molecule.

In another embodiment, the alloy or compound has the formula MxEwEyEz, wherein M is a catalyst such as Li, K or Cs or Na, Ew is the first other element, Ey is the second other element, and Ez is the first 3 different elements, and x, w, y and z represent an equivalent ratio. M, Ew, Ey and Ez may be any desired molar ratios. In one embodiment, x is in the range from 1 to 50, w is in the range from 1 to 50, y is in the range from 1 to 50, z is in the range from 1 to 50, preferably x is in the range from 1 to 10, and w is In the range 1-10, y is in the range 1-10, and z is in the range 1-10. In a preferred embodiment, Ew, Ey and Ez are selected from the group of H, N, C, Si and Sn. The alloy or compound may be one or more of LixHwCySiz, LixHwSnySiz, LixHwNySiz, LixHwSnyCz, LixHwNySnz and LixHwCyNz. In other embodiments, K, Cs and Na replace Li, wherein the catalyst is a K atom, a Cs atom and a NaH molecule. Species such as MxEwEyEz are illustrative and not meant to be limiting, as other species containing additional elements are also within the scope of the present invention.

In one embodiment, the reaction contains a source of hydrogen atoms and a source of Li catalyst. The reaction contains one or more species from the group of hydrogen dissociating agent, H2, hydrogen atom source, Li, LiH, LiNO3, LiNH2, Li2NH, Li3N, LiX, NH3, LiBH4, LiAlH4, Li3AlH6, NH3 and NH4X, wherein X Is the counterion as shown in halides and CRCs [41]. The weight percent of the reactants may be in any desired molar range. The reactants can be mixed well using a ball mill.

In one embodiment, the reaction mixture comprises a catalyst source and an H source. In one embodiment, the reaction mixture further comprises a reactant that performs the reaction to form a Li catalyst and atomic hydrogen. The reactant may comprise one or more of the group of H2, hydrino catalyst, MNH2, M2NH, M3N, NH3, LiX, NH4X (X is a counter ion such as halide), MNO3, MAlH4, M3AlH6 and MBH4 M is an alkali metal which may be a catalyst. The reaction mixture is Li, LiH, LiNO3, LiNO, LiNO2, Li3N, Li2NH, LiNH2, LiX, NH3, LiBH4, LiAlH4, Li3AlH6, LiOH, Li2S, LiHS, LiFeSi, Li2CO3, LiHCO3, Li2SO4, LiHSO4, Li3PO4, Li2H LiH2PO4, Li2MoO4, LiNbO3, Li2B4O7 (Lithium Tetraborate), LiBO2, Li2WO4, LiAlCl4, LiGaCl4, Li2CrO4, Li2Cr2O7, Li2TiO3, LiZrO3, LiAlO, LiCoO2, Li2O2, Li2O2, Li2O2, Li2O2, Li2O2 , LiIO3, LiFeO2, LiIO4, LiClO4, LiScOn, LiTiOn, LiVOn, LiCrOn, LiCr2On, LiMn2On, LiFeOn, LiCoOn, LiNiOn, LiNi2On, LiCuOn and LiZnOn, where n is 1, 2, 3 or 4) ), Strong oxidized anions, oxidants, molecular oxidants such as V2O3, I2O5, MnO2, Re2O7, CrO3, RuO2, AgO, PdO, PdO2, PtO, PtO2 and NH4X (where X is nitrate or other CRCs [41] Suitable anion), and a reagent selected from the group of reducing agents. In each case, the mixture further comprises hydrogen or a hydrogen source. In other embodiments, other dissociating agents may or may not be used, wherein hydrogen atoms and optionally catalyst atoms are chemically produced by the reaction of the mixture species. In further embodiments, the reactant catalyst may be added to the reaction mixture.

The reaction mixture may also further comprise an acid such as H 2 SO 3, H 2 SO 4, H 2 CO 3, HNO 2, HNO 3, HClO 4, H 3 PO 3 and H 3 PO 4 or an acid source such as anhydrous acid. The latter may include one or more of the group of SO2, SO3, CO2, NO2, N2O3, N2O5, Cl207, PO2, P2O3 and P2O5.

In one embodiment, the reaction mixture further comprises a reactant catalyst to produce a reactant that acts as a low-energy-hydrogen catalyst or low-energy-hydrogen catalyst source and a hydrogen atom or a hydrogen atom source. Suitable reactant catalysts include one or more of acid, base, halide ions, metal ions, and free radical source groups. The reactant catalyst may comprise a weak-base-catalyst such as Li2SO4, a weak-acid catalyst such as a solid acid such as LiHSO4, a metal ion source such as TiCl3 or AlCl3 providing Ti3 + and Al3 + ions, respectively, a free radical source such as CoX2, where X is Cl and The same halide, where Co 2+ may react with O 2 to form O 2 radicals), metals such as Ni, Fe and Co, X— ion sources (X is halide) such as LiX— From Cl- or F-, free radical initiator / propagating source such as peroxides, azo-group compounds and UV light.

In one embodiment, the reaction mixture for low-energy hydrogen is adapted to ionize the hydrogen source, catalyst source, and catalyst to resonantly receive energy from the hydrogen atoms to form hydrinos having the energy given by equation (1). At least one hydrino getter and electron getter from the catalyst according to the present invention. Hydrino getters can combine with low-energy hydrogen to prevent reverse reactions with ordinary hydrogen. In one embodiment, the reaction mixture comprises a hydrino getter such as LiX or Li2X, where X is a halide or other anion such as an anion from CRC [41]. The electron getter may perform one or more functions to receive electrons from the catalyst and to stabilize the catalyst-ion intermediates such as Li 2+ intermediates such that the catalytic reaction occurs at a high rate. The getter may be an inorganic compound comprising one or more cations and one anion. The cation may be Li +. The anions are halides or other anions given to CRC [41] such as F-, Cl-, Br-, I-, NO3-, NO2-, SO42-, HSO4-, CoO2-, IO3-, IO4-, TiO3-, It may be one of the group containing CrO4-, FeO2-, PO43-, HPO42-, H2PO4-, VO3-, ClO4- and Cr2O72-, and the other anions in the reactants. The hydride binder and / or stabilizer may be one or more of the group of LiX (X is a halide), and other compounds comprising the reactants.

In embodiments of the reaction mixtures such as Li, LiNH 2 and X, wherein X is the hydride bond compound, X is at least one of LiHBr, LiHI, hydrino hydride compound and low-energy hydrogen compound. In one embodiment, the catalytic reaction mixture is regenerated by hydrogen addition from a hydrogen source.

In one embodiment, the hydrino product can be combined to form a stable hydrino hydride compound. The hydride binder may be LiX, where X is a halide or other anion. The hydride binder can react with hydrides having an NMR upfield shift that is greater than the upfield shift of TMS. The binder may be an alkali halide and the hydride bond product may be an alkali hydride with an NMR higher field transition that is greater than the upper field transition of TMS. The hydride may have a binding energy determined by XPS of 11 to 12 eV. In one embodiment, the product of the catalysis is a hydrogen molecule H 2 (1/4) having a binding energy of about 250 eV trapped in the solid NMR peak and crystalline ion lattice at about 1 ppm relative to TMS. In one embodiment, product H2 (1/4) is trapped in the crystalline lattice of the ionic compound of the reactor such that infrared absorption selectivity is such that the molecule becomes IR active and an FTIR peak is observed at about 1990 cm-1.

Additional Li atom sources of the invention include additional Li alloys such as Li and one or more alkali metals, alkaline earth metals, transition metals, rare earth metals, precious metals, tin, aluminum, other Group III and IV metals, actinides, and lanthanides. Contains alloys containing elements. Some typical alloys are LiBi, LiAg, LiIn, LiMg, LiAl, LiMgSi, LiFeSi, LiZr, LiAlCu, LiAlZr, LiAlMg, LiB, LiCa, LiZn, LiBSi, LiNa, LiCu, LiPt, LiCaNa, LiAlCuMgZr, LiPb, LiPb, LiCb At least one member of the group of LiSn and LiNi. In other embodiments, K, Cs and Na replace Li, wherein the catalyst is a K atom, a Cs atom and a NaH molecule.

In another embodiment, the anion may form a hydrogen-type bond with the Li atom of the covalently bonded Li-Li molecule. This hydrogen-type bond can weaken the Li-Li bond to the point where it is under vacuum energy (which liberates the atom) so that the Li atom can act as a catalyst atom to form hydrinos. In other embodiments, K, Cs and Na replace Li, with the catalyst being a K atom, a Cs atom and a NaH molecule.

In one embodiment, the function of the hydrogen dissociating agent is provided by a chemical reaction. H atoms are produced by reaction of two or more reaction mixture species or by decomposition of one or more species. In one embodiment, Li-Li reacts with LiNH 2 to form Li atoms, H atoms and Li 2 NH. Li atoms may also be formed by decomposition or reaction of LiNO 3. In other embodiments, K, Cs and Na replace Li, with the catalyst being a K atom, a Cs atom and a NaH molecule.

In a further embodiment, in addition to the catalyst or catalyst source for forming low-energy hydrogen, the reaction mixture comprises a heterogeneous catalyst to provide M and H atoms by decomposing MM and MH such as LiLi and LiH. Heterogeneous catalysts may be selected from the group consisting of transition elements, precious metals, rare earths and other metals and atoms such as W, Ta, Ni, Pt, Pd, Ti, Al, Fe, Ag, Cr, Cu, Zn, Co and Sn. It may include.

In an embodiment of the Li carbon alloy, the reaction mixture comprises an excess of Li above the Li-carbon intercalation limit. Excess may range from 1% to 1000%, preferably 1% to 10%. The carbon may further comprise a hydrogen spillover catalyst having a hydrogen dissociating agent such as Pd or Pt on the activated carbon. In further embodiments, the cell temperature is higher than the temperature at which Li is fully intercalated into carbon. The cell temperature may range from about 100 to 2000 ° C, preferably from 200 to 800 ° C, most preferably from about 300 to 700 ° C. In other embodiments, K, Cs and Na replace Li, with the catalyst being a K atom, a Cs atom and a NaH molecule.

In an embodiment of the Li silicon alloy, the cell temperature is in a range such that the silicon alloy further comprising H releases a hydrogen atom. The range may be in the range of about 50 to 1500 ° C., preferably about 100 to 800 ° C., and most preferably about 100 to 500 ° C. The hydrogen pressure may range from about 0.01 to 105 Torr, preferably from about 10 to 5000 Torr, most preferably from about 0.1 to 760 Torr. In other embodiments, K, Cs and Na replace Li, with the catalyst being a K atom, a Cs atom and a NaH molecule.

The reaction mixtures, alloys and compounds may comprise catalysts such as Li or catalyst sources such as catalytic hydrides with other element (s) or compound (s) or other element (s) or source of compound (s) such as the number of other element (s). It can be formed by mixing with a digest. The catalytic hydride can be LiH, KH, CsH or NaH. The reagents can be mixed by ball milling. In addition, the catalyst alloy may be formed from an alloy source comprising the catalyst and one or more other elements or compounds.

In one embodiment, the reaction mechanism for the Li / N system to form hydrino reactants of Li and H atoms is as follows.

LiNH2 + Li-Li → Li + H + Li2NH (32)

In embodiments of other Li-alloy systems, the reaction mechanism is similar to that of Li / N systems, with other alloy element (s) replacing N. An exemplary reaction mechanism for carrying out the reaction for forming the hydrino reactant, Li and H atoms, involving a reaction mixture comprising Li and S, Sn, Si and C, is as follows.

SH + Li-Li → Li + H + LiS (33)

SnH + Li-Li → Li + H + LiSn (34)

SiH + Li-Li → Li + H + LiSi, and (35)

CH + Li-Li → Li + H + LiC (36)

Preferred embodiments of a LiS alloy-catalyst system include Li with Li 2 S and Li with LiHS. In other embodiments, K, Cs and Na replace Li, with the catalyst being a K atom, a Cs atom and a NaH molecule.

Primary Li / N Alloy Reaction

In the solid and liquid states lithium is a metal and the gas contains covalent Li 2 molecules. To produce lithium atoms, the reaction mixture of solid fuels includes Li / N alloy reactants. The reaction mixture may comprise one or more from the group of Li, LiH, LiNH 2, Li 2 NH, Li 3 N, NH 3, dissociating agent, hydrogen source such as H 2 gas or hydride, support and getter such as LiX (X is halide). The dissociating agent is preferably Pt or Pd on a high surface area support which is inert to Li. It may comprise Pt or Pd on carbon or Pd / Al 2 O 3. The latter support may comprise a protective surface coating of a material such as LiAlO 2. Preferred dissociating agents for reaction mixtures comprising Li / N alloys or Na / N alloys are Pt or Pd on Al 2 O 3, Raney nickel (R—Ni) and Pt or Pd on carbon. If the dissociating agent support is Al 2 O 3, the reactor temperature may be maintained below the temperature causing substantial reaction with Li. The temperature may be in the range of about 250 ° C. to less than 600 ° C. In another embodiment, Li is in the form of LiH and the reaction mixture comprises one or more of LiNH 2, Li 2 NH, Li 3 N, NH 3, dissociating agent, hydrogen source such as H 2 gas or hydride, support and getter such as LiX (X is halide) Wherein the reaction of LiH with Al 2 O 3 is substantially endothermic. In other embodiments, the dissociating agent is not related to the balance of the reaction mixture, wherein the dissociating agent passes through the H atoms.

Two preferred embodiments include a first reaction mixture of LiH, LiNH2 and Pd on an Al2O3 powder and a second reaction mixture of Li, Li3N and hydrogenated Pd on an Al2O3 powder, which may further include H2 gas. The first reaction mixture can be regenerated by the addition of H2 and the second reaction mixture can be regenerated by removing H2 and hydrogenating the dissociating agent or reintroducing H2. The regeneration reaction as well as the reaction for regenerating the catalyst and H are shown below.

In one embodiment, LiNH 2 is added to the reaction mixture. LiNH2 produces not only a hydrogen atom but also a Li atom according to the following reversible reaction.

Li2 + LiNH2 → Li + Li2NH + H (37)

Li2 + Li2NH → Li + Li3N + H (38)

In one embodiment, the reaction mixture comprises about 2: 1 Li and LiNH 2. In the hydrino reaction cycle, Li-Li and LiNH 2 react to form Li atoms, H atoms and Li 2 NH, and the cycle continues according to equation (38). The reactants may be present in any weight percent.

The mechanism for forming Li 2 NH from LiNH 2 includes the first step of forming ammonia [42]:

2LiNH2 → Li2NH + NH3 (39)

When LiH is present, it reacts with ammonia to release H2,

* LiH + NH3 → LiNH2 + H2 (40)

The net reaction forms H2 with the consumption of LiNH2,

LiNH2 + LiH → Li2NH + H2 (41)

If Li is present, the amide is not consumed due to the much more energy efficient reverse reaction of Li with ammonia:

Li-Li + NH3 → LiNH2 + H + Li (42)

Thus, in one embodiment, the reactant comprises a mixture of Li and LiNH 2 to form Li and H atoms according to formulas (37) to (38).

The reaction mixture of Li and LiNH2 serving as Li catalyst and atomic hydrogen source can be regenerated. During the regeneration cycle, the reaction product mixture comprising species such as Li, Li 2 NH and Li 3 N can react with H to form LiH and LiNH 2. LiH has a melting point of 688 ° C., while LiNH 2 has a melting point at 380 ° C. and Li has a melting point at 180 ° C. The LiNH 2 liquid and any Li liquid formed can be physically removed from LiH at about 380 ° C. and then the LiH solids can be independently heated to form Li and H 2. The reaction mixture can be regenerated by recombining Li and LiNH 2. Then, excess H 2 from LiH pyrolysis is reused in the next regeneration cycle, and some supplemental H 2 replaces any H 2 consumed in hydrino formation.

In a preferred embodiment, competitive reactions in which one reactant is hydrogenated or dehydrogenated to another reactant are used to form the desired reaction mixture comprising the hydrogenated and non-hydrogenated compounds. For example, hydrogen is added under appropriate temperature and pressure conditions so that the reverse reactions of formulas (37) and (38) occur through a competitive reaction to form LiH such that the hydrogenated product is mainly Li and LiNH 2. Alternatively, LiH may be selectively dehydrogenated by hydrogenating a reaction mixture comprising compounds of the Li, Li 2 NH and Li 3 N groups to form hydrides and pumping in the temperature and pressure ranges while achieving selectivity based on differential kinetics. Can be.

In one embodiment, Li is deposited into a thin film over a high surface area and a mixture of LiH and LiNH 2 is formed by the addition of ammonia. The reaction mixture may further comprise excess Li. Li and H atoms are formed according to formulas (37) and (38), and subsequent reactions form a state having the energy given by formula (1). The mixture can then be regenerated by adding H2 followed by heating and pumping, where pumping and removal of H2 is optional.

The reversible system of the present invention for producing a lithium catalyst is a Li 3 N + H system and can be regenerated by pumping. The reaction mixture comprises at least one of Li 3 N, Li 3 N sources such as Li and N 2, H sources such as H 2, hydrogen dissociating agents, LiNH 2, Li 2 NH, LiH, Li, NH 3 and metal hydrides. The reaction of H2 with Li3N provides LiH and Li2NH, while the reaction of Li3N with a hydrogen atom source such as H2 and dissociating agent or H from a hydride carrying out the decomposition reaction is as follows.

Li3N + H → Li2NH + Li (43)

The Li atom catalyst may then react with additional H atoms to form hydrinos. Side products such as LiH, Li2NH and LiNH2 can be converted to Li3N by evacuating the reaction vessel of H2. A typical Li / N alloy reaction is as follows:

Li 3 N, H source and hydrogen dissociating agent are present in any desired molar ratio. Each is present in a molar ratio of greater than 0 and less than 100%. Preferably, the molar ratios are similar. In one embodiment, Li 3 N; At least one of LiNH 2, Li 2 NH, LiH, Li, and NH 3; And molar ratios of H sources such as metal hydrides are similar. In other embodiments, K, Cs and Na replace Li, with the catalyst being a K atom, a Cs atom and a NaH molecule.

In one embodiment, lithium amide and hydrogen react to form ammonia and lithium:

1 / 2H2 + LiNH2 → NH3 + Li (49)

The reaction can induce Li formation by increasing the H2 concentration. Alternatively, the forward reaction can be induced through the formation of H atoms using dissociating agents. The reaction by H atom is given by:

H + LiNH2 → NH3 + Li (50)

In an embodiment of a reaction mixture comprising at least one compound that reacts with a Li source to form a Li catalyst, the reaction mixture comprises at least one species from the group LiNH 2, Li 2 NH, Li 3 N, Li, LiH, NH 3, H 2 and dissociating agent. do. In one embodiment, the Li catalyst is produced from the reaction of LiNH 2 with hydrogen, preferably a hydrogen atom as given in Scheme (50). The ratio of reactants may be any desired amount. Preferably, the ratio is from about equivalence ratios to ratios as in equations (49) and (50). The catalysis reaction is reversible with an H source, such as H 2 gas addition, which replaces the reacted to form hydrinos, wherein the catalysis is given by equations (3) to (5), and lithium amide of ammonia and Li It is formed by the reaction:

NH3 + Li → LiNH2 + H (51)

In other embodiments, K, Cs and Na replace Li, with the catalyst being a K atom, a Cs atom and a NaH molecule. In a preferred embodiment, the reaction mixture comprises a hydrogen dissociating agent, a source of hydrogen atoms, and Na or K and NH 3. In one embodiment, ammonia reacts with Na or K to form NaNH 2 or KNH 2, which acts as a catalyst source. Another embodiment includes K catalyst sources such as K metal, hydrogen sources such as NH3, H2 and hydrides such as metal hydrides, and dissociating agents. Preferred hydrides are those containing R-Ni, which may act as a dissociating agent. In addition, hydrino getters such as KX may be present, wherein X is preferably a halide such as Cl, Br or I. The cell can run continuously with replacement of the hydrogen source. The NH 3 may serve as a source of K atoms by reversible formation of KN alloy compounds from one or more of K-K such as amides, imides or nitrides or by formation of KH by release of K atoms.

In further embodiments, the reactants comprise catalysts such as Li and hydrogen atom sources such as H2 and dissociating agents or hydrides such as hydrogenated R-Ni. H can react with Li-Li to form LiH and Li, which can also act as a catalyst to react with additional H to form hydrinos. Li can then be regenerated by removing H2 released from LiH. The plateau temperature at 1 Torr for LiH decomposition is about 560 ° C. LiH may decompose at about 500 ° C. below the alloy formation and sintering temperature of 0.5 Torr and R—Ni. The molten Li can be separated from R-Ni, R-Ni can be hydrogenated again, and Li and hydrogenated R-Ni can be recovered in another reaction cycle.

In one embodiment, Li atoms can be deposited on the surface. The surface can be a support or a source of H atoms. The surface may comprise one or more of a hydride and a hydrogen dissociating agent. The surface may be R-Ni, which may be hydrogenated. The deposition may be provided from a reservoir containing a Li atom source. The Li source can be controlled by heating. One source that provides Li atoms upon heating is Li metal. The surface can be kept at low temperature such as room temperature during deposition. The Li-coated surface can be heated to react Li with H to form the H state given by Equation (1). Other thin film deposition techniques that are well known in the art further include embodiments of the present invention. Such embodiments include physical spraying, electro-spraying, aerosols, electro-arc welding, Knudsen cell controlled release, dispenser-cathode injection, plasma deposition, sputtering and further coating methods and systems such as fine dispersion melting of Li , Electroplating of Li and chemical vapor deposition of Li. In other embodiments, K, Cs and Na replace Li, with the catalyst being a K atom, a Cs atom and a NaH molecule.

In the case of Li deposited on the hydride surface, it can be regenerated by removing LiH and Li by heating by pumping, the hydride can be hydrogenated again by introducing H2, and the cell is evacuated in certain embodiments. Li atoms can then be deposited again onto the regenerated hydride. In other embodiments, K, Cs and Na replace Li, with the catalyst being a K atom, a Cs atom and a NaH molecule.

Li and R-Ni are present in any desired molar ratio. Li and R-Ni are each present in a molar ratio of greater than 0 and less than 100%. Preferably, the molar ratios of Li and R-Ni are similar.

In a preferred embodiment, a competitive reaction is used to hydrogenate or dehydrogenate one reactant to another reactant to achieve a reaction mixture comprising the hydrogenated and non-hydrogenated compounds. For example, LiH formation is thermodynamically advantageous over R-Ni hydride formation. However, LiH formation rates are very low at low temperatures such as in the range of about 25 ° C. to 100 ° C., whereas R-Ni hydride formation is at high rates at suitable pressures such as about 100 Torr to 3000 Torr in this temperature range. Thus, the reaction mixture of Li and hydrogenated R—Ni dehydrogenates LiH by pumping at about 400 to 500 ° C., cooling the vessel to about 25 to 100 ° C., and hydrogen for a period of time to achieve the desired selectivity. Can be regenerated from LiH and R-Ni by preferential hydrogenation of R-Ni, followed by evacuation of the cell to remove excess hydrogen. While excess Li is present or added in excess, R-Ni can be used in repeated cycles by selectively hydrogenating alone. This is accomplished by adding hydrogen at a temperature and pressure range that results in selective hydrogenation of R-Ni, then heating the vessel to form H atoms and Li atoms and subsequently removing excess hydrogen before initiating the hydrino reaction. Can be. In this process additional hydride and catalyst sources can be used in place of Li and R-Ni. In further embodiments, the R—Ni is mostly hydrogenated in separate preparation steps using elevated temperature and high pressure hydrogen or using electrolysis. Electrolysis can occur in basic aqueous solutions. The base may be a hydroxide. The counter electrode may be nickel. In this case, R-Ni can provide H atoms for a long time by appropriate temperature, pressure and temperature ramp rate.

LiH has a high melting point of 688 ° C., which may be higher than the temperature at which the dissociating agent metal sinters or forms the alloy with the catalyst metal. For example, LiNi alloys can be formed at temperatures above about 550 ° C. when the dissociating agent is R—Ni and the catalyst is Li. Thus, in another embodiment, the reaction mixture can be regenerated by converting LiH to LiNH 2 which can be removed at a relatively low melting point. The reaction to form lithium amide from lithium hydride and ammonia is as follows:

LiH + NH3 → LiNH2 + H2 (52)

The molten LiNH 2 can then be recovered at a melting point of 380 ° C. LiNH 2 can be converted to Li by a decomposition reaction.

In one embodiment involving recovery of molten LiNH 2, gas pressure is applied to the mixture comprising LiNH 2 to increase its separation rate from the solid components. Separation nets or semi-permeable membranes may persist the solid components. The gas may be an inert gas such as rare gas or nitrogen which limits the decomposition of decomposition products such as LiNH 2. Molten Li can also be separated using gas pressure. To clean any residue from the dissociating agent, a gas stream can be used. Inert gases such as rare gases are preferred. If the residue Li is attached to a dissociating agent such as R-Ni, the residue can be removed by washing with a basic aqueous solution that can also regenerate R-Ni. Alternatively, Li can be hydrogenated to mechanically separate the solids of LiH and R-Ni and any additional solid compounds present by sieving. In another embodiment, dissociating agents such as R-Ni and other reactants may be physically separated, but may be kept in close proximity so that hydrogen atoms can act on the balance of the reaction mixture. The balance of the reaction mixture and the dissociating agent can be placed in an open juxtaposed boat, for example. In other embodiments, the reactor further comprises multiple compartments containing independently a balance of dissociating agent and reaction mixture. The separator in each compartment allows the hydrogen atoms formed in the dissociation compartment to flow into the balance compartment of the reaction mixture to maintain chemical separation. The separator may be a metal mesh or a semipermeable inert membrane, which may be metallic. The contents can be mechanically mixed during operation of the reactor. The separated balance of the reaction mixture and its product can be removed and reprocessed outside the reaction vessel to be independently recovered from the dissociating agent or independently in the reactor.

Other embodiments in which the system produces Li atom catalysts and H atoms include Li, ammonia and LiH. Li atom catalysts and H atoms can be produced by the reaction of Li 2 with NH 3:

Li2 + NH3 → LiNH2 + Li + H (53)

LiNH2 is the source of NH3 in the following scheme:

2LiNH2 → Li2NH + NH3 (54)

In a preferred embodiment, Li is dispersed on a support having a large surface area to react with ammonia. Ammonia also reacts with LiH to produce LiNH2:

LiH + NH3 → LiNH2 + H2 (55)

And, H2 can react with Li2NH to regenerate LiNH2:

H2 + Li2NH → LiNH2 + LiH (56)

In another embodiment, the reactant comprises a mixture of LiNH 2 and dissociation agent. The reaction to form a lithium atom is as follows:

LiNH2 + H → Li + NH3 (57)

Li may then react with additional H to form hydrinos.

Other embodiments of systems that produce Li atom catalysts and H atoms include Li and LiBH 4 or NH 4 X (where X is an anion such as a halide). Li atom catalysts and H atoms can be produced by the reaction of Li2 with LiBH4:

Li2 + LiBH4 → LiBH3 + Li + LiH (58)

NH 4 X can produce LiNH 2 and H 2:

Li2 + NH4X → LiX + LiNH2 + H2 (59)

Subsequently, Li atoms can be generated according to the formulas (32) and (37). In another embodiment, the reaction mechanism for the Li / N system to form a hydrino reactant of Li atoms and H is as follows:

NH4X + Li-Li → Li + H + NH3 + LiX (60)

Wherein X is a counter ion, preferably a halide.

Li atom catalysts may be produced by the reaction of Li atoms, formed by Li 2 NH or Li 3 N and dissociation of H 2:

Li2NH + H → LiNH2 + Li (61)

Li3N + H → Li2NH + Li (62)

In further embodiments, the reaction mixture comprises nitrides of metals other than Li such as Mg, Ca, Sr, Ba, Zn and Th. The reaction mixture may comprise a metal to form a metal compound substituted with Li or mixed with Li. The metal may be selected from the group of alkali metals, alkaline earth metals and transition metals. The compound may further comprise N such as amides, imides and nitrides.

In one embodiment, the Li catalyst is chemically produced by an anion exchange reaction such as a halide (X) exchange reaction. For example, one or more of the Li metal and Li-Li molecules react with the halide compound to form Li atoms and LiX. Alternatively, LiX reacts with metal M to form Li atoms and MX. In one embodiment, the lithium metal reacts with lanthanide element halides to form Li and LiX, where X is a halide. In one example, CeBr 3 and Li 2 react to form Li and LiBr. In other embodiments, K, Cs and Na replace Li, with the catalyst being a K atom, a Cs atom and a NaH molecule.

In another embodiment, the reaction mixture further comprises the reactants and products of the Haber procedure [43]. The product may be NHx (x = 0,1,2,3,4). These products can react with Li or a compound comprising Li to form Li atoms and H atoms. For example, Li-Li may react with NHx to form Li and possibly H:

Li-Li + NH3 → Li + LiNH2 + H (63)

Li-Li + NH2 → LiNH2 + Li (64)

Li-Li + NH2 → Li2NH + H (65)

In other embodiments, K, Cs and Na replace Li, with the catalyst being a K atom, a Cs atom and a NaH molecule.

Mixtures of compounds that melt at lower temperatures than the melting point of one or more individual compounds can be used. Preferably, an eutectic mixture, which is a molten salt mixed with reactants such as Li and LiNH 2, may be formed.

The chemistry of the reaction mixture can vary very substantially depending on the physical state of the reactants and the presence or absence of the solvent or solute or alloy species added. It is an object of the present invention to change the physical state to control the reaction rate and change the thermodynamics to achieve a sustainable low energy hydrogen reaction by H addition from the H source. Li / N alloy systems comprising reactants such as Li and LiNH 2, alkali metals, alkaline earth metals, and mixtures thereof may serve as solvents. For example, excess Li can include solvated Li and LiNH2 reactants that act as a molten solvent for LiNH2, resulting in relatively different reaction kinetics and thermodynamics from the solid-state mixture. The effect of the former, ie control of the low energy hydrogen reaction kinetics, can be adjusted by controlling the properties of the solute and solvent such as temperature, concentration and molar ratio. Following the reaction to produce the catalyst atoms and hydrogen atoms, the latter effect can be used to regenerate the initial reactants. This is the route through which the product can be directly regenerated by the hydrogenation reaction.

One embodiment where the regeneration of the reactants is facilitated by solvents or added solutes or alloy species includes lithium metal, wherein the hydrogenation of Li is not complete so that Li is present in the solvent and reactant. In Li solvents, the following regeneration reaction may occur by H addition from the source to form LiH:

LiH + Li2NH → 2Li + LiNH2 (66)

In the case of Li / N alloy systems comprising reactants such as Li and LiNH2, alkali metals, alkaline earth metals and mixtures thereof may serve as solvents. In one embodiment, the solvent is selected to reduce the reaction from LiH to Li and form an unstable solvent hydride with H release. Preferably, the solvent may be one or more of the group of Li (excess), Na, K, Rb, Cs and Ba with the corresponding hydrides having low thermal stability while being able to reduce Li +. If the melting point of the solvent is higher than desired, such as in the case of Ba having a high melting point of 727 ° C., the solvent is mixed with other solvents such as metal to form a solvent having a relatively low melting point such as including a eutectic mixture. can do. In one embodiment, one or more alkaline earth metals may be mixed with one or more alkali metals to lower the melting point, increase the likelihood of Li + reduction, and reduce the stability of the corresponding solvent hydride.

Another embodiment in which the regeneration of the reactants is promoted by solvents or added solutes or alloy species includes potassium metal. Potassium metals in a mixture of LiH and LiNH 2 may reduce the LiH to Li reaction and form KH. Since KH is thermally unstable at intermediate temperatures such as 300 ° C., it can further promote hydrogenation reactions from Li 2 NH to Li and LiNH 2.

Thus, K can catalyze the reaction given by equation (66). The reaction step is as follows:

LiH + K → Li + KH (67)

KH + Li2NH → K + Li + LiNH2 (68)

Here, H is added at a rate where H is consumed by low energy hydrogen production. Alternatively, K catalytically produces Li and H from LiH, wherein LiNH 2 is formed directly from the hydrogenation of Li 2 NH. The reaction step is as follows:

Li2NH + 2H → LiH + LiNH2 (69)

LiH + K → KH + Li (70)

KH → K + H (g) (71)

In addition to the preferred instability conditions of the hydride (KH), the amide (KNH2) is also unstable so that the exchange of lithium amide and potassium amide is thermodynamically undesirable. In addition to K, Na is also preferred as a metal solvent because it can reduce LiH and has a relatively low vapor pressure. Other examples of suitable metal solvents include Rb, Cs, Mg. Ca, Sr, Ba and Sn. The solvent may comprise a metal mixture such as a mixture of two or more alkali metals or alkaline earth metals. Preferred solvents are Li (excess) and Na above 380 ° C. because Li is miscible in Na above this temperature.

In another embodiment, the alkali metal or alkaline earth metal acts as a regeneration catalyst according to formulas (70) and (71). In one embodiment, LiNH 2 is first removed from the LiH / LiNH 2 mixture by melting LiNH 2. The metal M can then be added to catalyze the conversion of LiH to Li. M can be selectively removed by distillation. Na, K, Rb and Cs form hydrides that form amides that decompose and thermally decompose at relatively low temperatures, and in yet another embodiment, at least one is given by Formulas (67)-(71) Depending on the corresponding reaction for K, it may serve as a reactant for the catalytic conversion of LiH to Li and H. In addition, some alkaline earth metals such as Sr can form very stable hydrides and can act to convert LiH to Li by reacting LiH and alkaline earth metals to form stable alkaline earth hydrides. By operating at elevated temperatures, hydrogen can be supplied from alkaline earth hydrides through decomposition with lithium inclusions, mainly present as Li. The reaction mixture may include Li, LiNH 2, ×, and dissociating agent, where X has lithium compounds such as LiH, Li 2 NH and Li 3 N, and small amounts of alkaline earth metals that form stable hydrides to produce Li from LiH. The hydrogen source may be H2 gas. The operating temperature should be sufficient to make use of H.

In one embodiment, LiNO 3 may act to produce a source of Li and H LiNH 2 in a series of coupling reactions. Consider an embodiment of a catalytic reaction mixture comprising Li, LiNH 2 and LiNO 3. The reaction of Li and LiNH 2 to form Li 3 N and release H 2 is as follows:

LiNH2 + 2Li → H2 + Li3N (72)

The reaction in which the released H 2 (formula 72) and LiNO 3 form a balanced H 2 reduction reaction to form water and lithium amide is as follows:

4H2 + LiNO3 → LiNH2 + 3H2O (73)

Subsequently, Scheme (72) can proceed with the resulting LiNH2 and the balance Li, and the coupling reaction represented by Formulas (72) and (73) can occur until Li is completely exhausted. The overall response is given by:

LiNO3 + 8Li + 3LiNH2 → 3H2O + 4Li3N (74)

Water can be removed dynamically by methods such as condensation or react with the getter to prevent reaction with species such as Li, LiNH 2, Li 2 NH and Li 3 N.

Regeneration of Exemplary Li Catalyst Reactants

The present invention also includes methods and systems for producing or regenerating a reaction mixture to form a state given by formula (1) from any side product formed during the reaction. For example, in an embodiment of an energy reactor, the catalyst reactant mixtures such as Li, LiNH2 and LiNO3 may be prepared by any method known to those skilled in the art as given by Cotton and Wilkinson [43]. Regeneration from side products such as LiOH and Li2O. The components of the reactant mixture comprising the side products may be liquid or solid. The mixture is heated or cooled to the desired temperature and the product is physically separated by means known to those skilled in the art. In one embodiment, LiOH and Li 2 O are solids, Li, LiNH 2 and LiNO 3 are liquids, and the solid components are separated from the liquid components. LiOH and Li 2 O can be converted to lithium metals by reduction with H 2 at high temperatures or by electrolysis of molten compounds or mixtures containing them. The electrolysis cell may comprise a eutectic salt comprising one or more of LiOH, Li 2 O, LiCl, KCl, CaCl 2 and NaCl. The electrolysis cell is composed of a material resistant to attack by Li, such as BeO or BN containers. The Li product can be purified by distillation. LiNH 2 is formed by means known in the art, for example by reacting Li with nitrogen followed by hydrogen reduction. Alternatively, LiNH 2 can be formed directly by the reaction of Li with NH 3.

If the initial reaction mixture comprises at least one of Li, LiNH 2 and LiNO 3, the Li metal may be regenerated by a method such as electrolysis and LiNO 3 may be produced from the Li metal. One important step in removing the difficult nitrogen fixation step is to react Li metal with N 2 to form Li 3 N even at room temperature. Li 3 N may react with H 2 to form Li 2 NH and LiNH 2. Li 3 N may react with an oxygen source to form LiNO 3. In one embodiment, Li 3 N is a lithium nit comprising at least one reactant or intermediate of lithium (Li), lithium nitride (Li 3 N), oxygen (O 2), oxygen source, lithium imide (Li 2 NH) and lithium amide (LiNH 2). Used for the synthesis of rate (LiNO3).

In one embodiment, the oxidation reaction is as follows:

LiNH2 + 2O2 → LiNO3 + H2O (75)

Li2NH + 2O2 → LiNO3 + LiOH (76)

Li3N + 2O2 → LiNO3 + Li2O (77)

Lithium nitrate can be regenerated from Li 2 O and LiOH using one or more of NO 2, NO and O 2 by the following reactions:

3Li2O + 6NO2 + 3 / 2O2 → 6LiNO3 (78)

Li2O + 3NO2 → 2LiNO3 + NO (79)

NO + 1 / 2O2 → NO2 (80)

LiOH + NO2 + NO → 2LiNO2 + H2O (Industrial Process) (81)

2LiOH + 2NO2 → LiNO3 + LiNO3 + H2O (82)

Lithium oxide can be converted to lithium hydroxide by reaction with steam:

Li2O + H2O → 2LiOH (83)

In one embodiment, Li 2 O is converted to LiOH and then reacted with NO 2 and NO according to formula (81).

Both lithium oxide and lithium hydroxide can be converted to lithium nitrate by nitric acid treatment and drying:

Li2O + 2HNO3 → 2LiNO3 + H2O (84)

LiOH + HNO3 → LiNO3 + H2O (85)

LiNO 3 can be prepared by treating lithium oxide or lithium hydroxide with nitric acid. As shown by cotton and Wilkinson, nitric acid can also be produced by known industrial methods such as the Haber process, followed by the Ostwald process [43], and then by hydration and oxidation of NO. In one embodiment, the exemplary sequence of steps is as follows:

LiOH + HNO3 → LiNO3 + H2O (87)

In particular, the harbor process can be used to generate NH3 from N2 and H2 at elevated temperatures and pressures using a catalyst such as α-iron containing some oxides. Ammonia can be used to form LiNH 2 from Li. The Oswald process can be used to oxidize ammonia to NO in catalysts such as hot platinum or platinum-rhodium catalysts. The NO may further react with oxygen and water to form nitric acid, which may react with lithium oxide or lithium hydroxide to form lithium nitrate. Crystalline lithium nitrate is then obtained by drying. In another embodiment, NO and NO 2 react directly with one or more of lithium oxide and lithium hydroxide to form lithium nitrate. Regenerated Li, LiNH2 and LiNO3 are then recovered to the reactor in the desired molar ratio.

In a further exemplary regeneration reaction, embodiments of the reactor include reactants of Li, LiNH 2 and LiCoO 2. LiOH, Li 2 O, and Co and lower oxides thereof are side products. The reactants can be regenerated by electrolysis of LiOH and Li 2 O to Li. LiNH2 may be regenerated by reaction of Li with NH3 or N2 followed by H2. CoO 2 and its lower oxides can be regenerated by reaction with oxygen. LiCoO 2 may be formed by the reaction of Li and CoO 2. Li, LiNH2 and LiCoO2 are then returned to the cell in a batch or continuous regeneration process. If LiIO 3 or LiIO 4 is the reagent of the mixture, IO 3-and / or IO 4-can be regenerated by iodine or iodide reaction with a base, further electrolyzed to the desired anion and leached into LiIO 3 or LiIO 4, Can be dried and dehydrated.

NaH Molecular Catalyst

(여기서, m은 정수임) 중에서 하나가 되도록 하는 연속체 에너지 수준으로 촉매 시스템을 제공한다.In a further embodiment, a compound comprising hydrogen, such as MH, where H is hydrogen and M is another element, serves as a hydrogen source and a catalyst source. In one embodiment, the sum of the binding energy and the ionization energy of t electrons is approximately equal by the breakdown of the MH bond and the ionization of t electrons from the M atom.

Providing a catalyst system at a continuum energy level such that m is an integer.

One such catalyst system comprises sodium. The binding energy of NaH is 1.9245 eV [44]. The first and second ionization energies of Na are 5.13908 eV and 47.2864 eV, respectively [1]. Based on these energies, the binding energy of NaH + the double ionization energy (t = 2) for Na2 + of Na becomes 54.35 eV (2 × 27.2 eV), which is equivalent to the case of m = 2 in equation (2), NaH molecules can serve as catalysts and H sources. The catalytic reaction is given by the formula:

And the overall reaction is:

As set forth in Chapter 5 of Ref. [30] and Ref. [20], the hydrogen atom H (1 / p) (p = 1,2,3, ... 137) is also given by Formula (1) It can be transitioned to a low energy state, where the transition of one atom is catalyzed by a second atom that accepts m · 27.2 eV resonantly and non-radioactively while the potential energy is reversed. The general formula for the transition of H (1 / p) to H (1 / (p + m)) induced by the resonance transfer of m · 27.2 eV to H (1 / p ') is given by:

For high hydrogen concentrations, the transition of H (1/3) (p = 3) to H (1/4) (p + m = 4) by H catalyst (p = 1; m = 1) may be fast. :

Due to the stable binding of H- (1/4) in the halide and ionization stability to other reactive species thereof, 2H (1/4) → H2 (1/4) and H- (1/4) + H + → H2 H- (1/4) and the corresponding molecules formed by the (1/4) reaction are preferred products of hydrogen catalysts.

Since the sum of the binding energy of NaH, the double ionization energy from Na to Na2 + (t = 2) and the potential energy of H is 81.56 eV (3.27.2 eV), which is equivalent to the case of m = 3 in equation (2), NaH The catalytic reaction can be a harmonious reaction. The catalytic reaction is given by:

And the overall reaction is:

Here, H + fast is a fast hydrogen atom whose kinetic energy is 13.6 eV or more.

In one embodiment, the reaction mixture comprises one or more of NaH molecules and a hydrogen source. NaH molecules can act as catalysts to form the H state given by formula (1). The NaH molecular source may comprise one or more of a Na metal, a hydrogen source, preferably a hydrogen atom and NaH (s). The hydrogen source may be one or more of H 2 gas and dissociating agent and hydride. Preferably, the dissociating agent and hydride may be R-Ni. Preferably, the dissociating agent may also be Pt / Ti, Pt / Al 2 O 3 and Pd / Al 2 O 3 powder. Solid NaH may be one or more sources of NaH molecules, H atoms and Na atoms.

In a preferred embodiment, one of the sodium atoms and NaH molecules is provided by the reaction between the molecular form of the metal, ion or Na and one or more other compounds or elements. Sources of Na or NaH include metals Na, inorganic compounds including Na such as NaOH, and other suitable Na compounds such as NaNH2, Na2CO3 and Na2O (these are provided in CRC [41]), NaX (X is a halide) and NaH ( One or more). The other element may be H, a substituent or a reducing agent. The reaction mixture comprises (1) sodium sources such as Na (m), NaH, NaNH2, Na2CO3, Na2O, NaOH, NaOH doped R-Ni, NaX (X is halide), and NaX doped R-Ni, (2) Hydrogen sources such as H2 gas and dissociating agents and hydrides, (3) substituents such as alkali metals or alkaline earth metals, preferably Li, and (4) reducing agents such as metals such as alkali metals, alkaline earth metals, lanthanides, transition metals such as Ti, aluminum, B, metal alloys such as AlHg, NaPb, NaAl, LiAl and metals alone or in combination with reducing agents such as alkaline earth halides, transition metal halides, lanthanide halides and aluminum halides . Preferably, the alkali metal reducing agent is Na. Other suitable reducing agents include metal hydrides such as LiBH4, NaBH4, LiAlH4 or NaAlH4. Preferably, the reducing agent reacts with NaOH to form NaH molecules and Na products such as Na, NaH (s) and Na 2 O. The NaH source may be R-Ni, including NaOH and a reactant such as a reducing agent to form an Al intermetallic compound of a NaH catalyst such as an alkali metal or an alkaline earth metal or R-Ni. Further exemplary reactants are alkali or alkaline earth metals and oxidizing agents such as AlX 3, MgX 2, LaX 3, CeX 3 and TiXn where X is a halide, preferably Br or I. The reaction mixture may also comprise another compound comprising one or more of NaCO 3, Na 3 SO 4 and Na 3 PO 4 which may be doped into a dissociating agent such as a getter or a dispersant such as R—Ni. The reaction mixture may further comprise a support, wherein the support may be doped with one or more reactants of the mixture. The support may preferably have a large surface area desirable for the production of NaH catalyst from the reaction mixture. The support is R-Ni, Al, Sn, Al2O3 such as gamma, beta or alpha alumina, sodium aluminate (according to cotton [45], beta-alumina has other ions and provides Na +, an ideal composition Na2O.11Al2O3). ), Si, silica, silicates, zeolites, lanthanides, transition metals, metal alloys such as alkali and alkaline earth alloys with Na, rare earth metals, SiO2-Al2O3 or SiO2 supported Ni, and other supported metals such as alumina It may include one or more of the group consisting of one or more of supported platinum, palladium or ruthenium. The support has a large surface area and is a high surface area (HSA) material such as R-Ni, zeolites, silicates, aluminates, alumina, alumina nanoparticles, porous Al 2 O 3, Pt, Ru or Pd / Al 2 O 3, carbon, Pt or Pd / C, inorganic compounds such as Na 2 CO 3, silica and zeolite materials, preferably Y zeolite powders. In one embodiment, a support such as Al 2 O 3 (and, if present, an Al 2 O 3 support of the dissociating agent) reacts with a reducing agent such as a lanthanide element to form a surface-modified support. In one embodiment, the surface Al is substituted with lanthanide elements to form a lanthanide element-substituted support. This support is doped with a NaH molecular source such as NaOH and can react with a reducing agent such as lanthanide. Subsequent reaction of the lanthanide element-substituted support with the lanthanum element will not substantially change it, and NaOH doped on the surface can be reduced to a NaH catalyst by reaction with a reducing agent lanthanum element.

In one embodiment where the reaction mixture comprises a NaH catalyst source, the NaH source can be an alloy of Na and a hydrogen source. The alloy may be one or more 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 H source may be H2 or hydride.

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

A preferred embodiment comprises a reaction mixture of NaH and Pd on an Al 2 O 3 powder, wherein the reaction mixture can be regenerated by the addition of H 2.

In one embodiment, Na atoms are deposited on the surface. The surface may be a support or source of H atoms to form NaH molecules. The surface may comprise a hydride and at least one of hydrogen dissociable agents such as Pt, Ru or Pd / Al 2 O 3 which may be hydrogenated. Preferably, the surface area is large. The deposition may be formed from a reservoir containing a source of Na atoms. The Na source can be controlled by heating. One source for providing Na atoms upon heating is Na metal. The surface can be kept at low temperature such as room temperature during deposition. The Na-coated surface may be heated to react Na with H to form NaH, and the NaH molecules may be reacted to form an H state given by Formula (1). Other thin film deposition techniques known in the art further include embodiments of the present invention. Such embodiments include physical spraying, electro-spraying, aerosols, electro-arc welding, Knudsen cell controlled release, dispenser-cathode injection, plasma deposition, sputtering and further coating methods and systems such as fine dispersion melting of Na, of Na Electroplating and chemical vapor deposition of Na. Na metal is dispersed on a high-surface material, preferably Na 2 CO 3, carbon, silica, alumina, R-Ni and Pt, Ru or Pd / Al 2 O 3 to increase its activity upon reaction with another reagent such as H or H source. NaH can be formed. Other dispersing materials are known in the art as shown in cotton [46] et al.

In one embodiment, one or more reactants comprising a reducing agent or a NaH source such as Na and NaOH perform an aerosolization reaction to generate and react the corresponding reactant vapors to form a NaH catalyst. Na and NaOH can react in a cell to form a NaH catalyst, where one or more species undergo an aerosolization reaction. The aerosolized species can be transferred into the cell and reacted to form a NaH catalyst. The means for carrying the aerosolized species may be a carrier gas. Aerosolization of the reactants can be achieved using a mechanical stirrer and a carrier gas such as a rare gas to convey the reactants into the cell to form a NaH catalyst. In one embodiment, Na, which can act as a NaH source and reactant, is aerosolized by being charged and electrically dispersed. One or more of the reactants such as Na and NaOH may be mechanically aerosolized in the carrier gas or may be subjected to ultrasonic aerosolization. The reactant may also be passed through an orifice to form vapor. Alternatively, the reactants may be locally heated or evaporated to very high temperatures to form vapors. The reactant may further comprise a hydrogen source. The hydrogen may react with Na to form a NaH catalyst. Na may be in vapor form. The cell can form a hydrogen atom from H2 by including a dissociating agent. Another means of achieving aerosolization known in the art is part of the present invention.

In one embodiment, the reaction mixture comprises one or more species from the group comprising a Na or Na source, a source of NaH or NaH, a source of metal hydride or metal hydride, a reactant or a source of reactant, thereby It forms dissociating agents and hydrogen sources. The reaction mixture may further comprise a support. The reactant for forming the metal hydride may comprise a lanthanide element, preferably La or Gd. In one embodiment, La may be reversibly reacted with NaH to form LaHn (n = 1,2,3). In one embodiment, the hydride exchange reaction forms a NaH catalyst. The reversible general reaction can be given as follows:

MaH + M → Na + MH (96)

The reaction given by equation (96) also applies to the other MH-type catalysts provided in Table 2. The reaction is a hydrogen formation process, may be dissociated to form a hydrogen atom, and may react with Na to form a NaH catalyst. The dissociating agent is preferably at least one of Pt, Pd or Ru / Al2O3 powder, Pt / Ti and R-Ni. Preferably, the dissociating agent support, such as Al 2 O 3, comprises at least one surface where Al is replaced by La or comprises Pt, Pd or Ru / M 2 O 3 powder, where M is a lanthanide element. The dissociating agent can be separated from the rest of the reaction mixture, where the separator passes H atoms.

A preferred embodiment comprises a reaction mixture of LaH, La and Pd on Al 2 O 3, wherein the reaction mixture, in one embodiment, adds H 2, separates NaH and lanthanide hydride by sieving, and lanthanum The elemental hydride can be heated to form La and regenerated by mixing La and NaH. Alternatively, the regeneration melts Na and removes the liquid to separate Na and lanthanum element hydride, heat the lanthanum element hydride to form La, hydrogenate Na with NaH, and mix La and NaH It includes a step. The mixing can be by ball milling.

In one embodiment, a high surface area material such as R-Ni may be doped with NaX (X = F, Cl, Br, I). Doped R-Ni reacts with a reagent that displaces the halide to form one or more of Na and NaH. In one embodiment, the reactants are one or more alkali metal or alkaline earth metals, preferably one or more of K, Rb and Cs. In another embodiment, the reactants are at least one of alkali or alkaline earth hydrides, preferably KH, RbH, CsH, MgH2 and CaH2. The reactant may be both alkali metal and alkaline earth hydride. The reversible general reaction can be given as follows:

NaX + MH → NaH + MX (97)

NaOH catalysis to form NaH catalyst

The reaction from NaOH and Na to Na 2 O and NaH is as follows:

NaOH + 2Na → Na 2 O + NaH (98)

The exothermic reaction may lead to the formation of NaH (g). Thus, Na metal can act as a reducing agent to form catalyst NaH (g). Other examples of suitable reducing agents that provide high exothermic reduction reactions, similar to NaH sources, include at least one of alkali metals, alkaline earth metals such as Mg and Ca, metal halides such as LiBH4, NaBH4, LiAlH4 or NaAlH4, B, Al, transition metals such as Ti, lanthanide elements such as La, Sm, Dy, Pr, Tb, Gd and Er, preferably La, Tb and Sm. Preferably, the reaction mixture comprises a high surface area material (HSA material) having a dopant, such as NaOH, comprising a NaH catalyst source. Preferably, the conversion of the dopant to the catalyst on a material having a high surface area is achieved. The conversion may occur by a reduction reaction. The reducing agent may be provided in a gas stream. Preferably Na flows into the reactor as a gas stream. In addition to the preferred reducing agents, Na, other preferred reducing agents are other alkali metals, Ti, lanthanides or Al. Preferably, the reaction mixture comprises NaOH doped into an HSA material, preferably R-Ni, wherein the reducing agent is Na or intermetallic Al. The reaction mixture may further comprise an H source such as a hydride or H2 gas and a dissociating agent. Preferably, the H source is hydrogenated R—Ni.

In one embodiment, the reaction temperature is maintained below the temperature at which the reducing agent, such as lanthanide, forms an alloy with a catalyst source, such as R-Ni. In the case of lanthanum, the reaction temperature preferably does not exceed 532 ° C., which is the alloy temperature of Ni and La, as found by Gasser and Kefif. In addition, the reaction temperature is kept lower than the temperature at which the reaction of Al-O3 with R-Ni occurs to a significant extent, such as in the range of 100 ° C to 450 ° C.

In one embodiment, Na 2 O, formed into the reaction product, as given by Formula (98), to produce a NaH catalyst can be reacted with a hydrogen source to form NaOH, which can further act as a NaH catalyst source. In one embodiment, the regeneration reaction from Formula (98) to NaOH in the presence of a hydrogen atom is as follows:

Thus, small amounts of NaOH and Na, and hydrogen atom sources or hydrogen atoms act as catalyst sources for NaH catalysts, and in turn yield high yields of hydrinos through multiple cycles of regeneration reactions as given by formulas (98) to (101). To form. In one embodiment, from the reaction given by formula (102), Al (OH) 3 can serve as a source of NaOH and NaH, by performing the reaction given by formulas (98) to (101) by Na and H. Form hydrinos.

In one embodiment, the intermetallic Al acts as a reducing agent to form a NaH catalyst. The rest of the reaction is as follows:

This exothermic reaction can induce the formation of NaH (g) leading to a very exothermic reaction given by equations (88) to (92), wherein the regeneration of NaH is from Na in the presence of hydrogen atoms.

Two preferred embodiments comprise a first reaction mixture of Na and R-Ni comprising about 0.5% NaOH, wherein Na acts as a reducing agent and a second reaction mixture of R-Ni comprising about 0.5% NaOH. (In this case, intermetallic Al acts as a reducing agent). The reaction mixture can be regenerated by adding NaOH and NaH, which can act as H source and reducing agent.

In one embodiment of the energy reactor, the NaH source such as NaOH is regenerated by the addition of one or more of a hydrogen source such as hydride and hydrogen gas and dissociating agent. The hydride and dissociating agent can be hydrogenated R-Ni. In another embodiment, a NaH source such as NaOH-doped R-Ni is regenerated by one or more of rehydrogenation, addition of NaH, and addition of NaOH, wherein the addition may be by physical mixing. The mixing can be carried out mechanically, for example by means of ball milling.

In one embodiment, the reaction mixture further comprises an oxide-forming reactant that reacts with NaOH or Na 2 O to form a very stable oxide and NaH. Such reactants include cerium, magnesium, lanthanides, titanium or aluminum or compounds thereof such as AlX3, MgX2, LaX3, CeX3 and TiXn, where X is a halide, preferably Br or I, and a reducing compound such as an alkali metal Or alkaline earth metals. In one embodiment, the NaH catalyst source comprises R-Ni that includes a sodium compound, such as NaOH, on its surface. Subsequently, the reaction of NaOH with oxide-forming reactants such as AlX 3, MgX 2, LaX 3, CeX 3 and TiXn, and alkali metal M forms NaH, MX and Al 2 O 3, MgO, La 2 O 3, Ce 2 O 3 and Ti 2 O 3, respectively.

In one embodiment, the reaction mixture comprises NaOH doped R-Ni and an alkali metal or alkaline earth metal added to form one or more of the Na and NaH molecules. Na may further react with a source such as H2 gas or with a hydride such as R-Ni to form a NaH catalyst. Subsequent catalytic reaction of NaH forms the H state given by Formula (1). The addition of alkali metal or alkaline earth metal M can reduce Na + to Na by the following reactions:

NaOH + M → MOH + Na (104)

2NaOH + M → M (OH) 2 + 2Na (105)

M may also react with NaOH to form H and Na:

2NaOH + M → Na 2 O + H 2 + MO (106)

Na2O + M → M2O + 2Na (107)

The catalyst NaH is then reacted with:

Na + H → NaH (108)

By reacting with H and any added H source from the reaction as given in equation (106) and from R-Ni. Na is a preferred reducing agent because it is an additional source of NaH.

Hydrogen may be added to reduce NaOH and form a NaH catalyst:

NaOH + H2 → NaH + H2O (109)

H in R-Ni can reduce NaOH to Na metal and water which can be removed by pumping.

In one embodiment, the reaction mixture comprises one or more compounds that react with a NaH source to form a NaH catalyst. The source may be NaOH. The compound may comprise one or more of LiNH 2, Li 2 NH and Li 3 N. The reaction mixture may further comprise a hydrogen source such as H2. In an embodiment, the reaction in which sodium hydroxide and lithium amide form NaH and lithium hydroxide is as follows:

NaOH + LiNH2 → LiOH + NaH + 1 / 2N2 + LiH (110)

The reaction in which sodium hydroxide and lithium imide form NaH and lithium hydroxide is as follows:

NaOH + Li2OH → Li2O + NaH + 1 / 2N2 + 1 / 2H2 (111)

And the reaction of sodium hydroxide and lithium nitride to form NaH and lithium oxide is as follows:

NaOH + Li3N → Li2O + NaH + 1 / 2N2 + Li (112)

Alkaline Earth Hydroxide Catalytic Reaction to Form NaH Catalyst

In one embodiment, a H source is provided to a Na source to form a catalyst NaH. The Na source may be a metal. The H source may be a hydroxide. The hydroxide may be one or more of alkali, alkaline earth hydroxides, transition metal hydroxides and Al (0H) 3. In one embodiment, Na reacts with the hydroxide to form its corresponding oxide and NaH catalyst. In an embodiment where the hydroxide is Mg (OH) 2, the product is MgO. In an embodiment where the hydroxide is Ca (OH) 2, the product is CaO. Alkaline earth oxides can react with water to regenerate hydroxides as shown in cotton [48]. The hydroxide may be collected into the precipitate by means such as filtration and centrifugation.

For example, in one embodiment, the NaH catalyst formation reaction and the Mg (OH) 2 regeneration cycle are given by the following reactions:

3Na + Mg (OH) 2 → 2NaH + MgO + Na 2 O (113)

MgO + H 2 O → Mg (OH) 2 (114)

In one embodiment, the NaH catalyst formation reaction and the Ca (OH) 2 regeneration cycle are given by the following reactions:

4Na + Ca (OH) 2 → 2NaH + CaO + Na 2 O (115)

CaO + H 2 O → Ca (OH) 2 (116)

Na / N alloy reaction to form NaH catalyst

In the solid and liquid states sodium is a metal and the gas contains covalent N2 molecules. To produce a NaH catalyst, the reaction mixture of solid fuels includes a Na / N alloy reactant. In one embodiment, the reaction mixture, solid-fuel reaction, and regeneration reaction include those of a Li / N system, wherein Na replaces Li and the catalyst is molecular NaH, provided that the solid fuel reaction is atomic Li and It produces molecules NaH rather than H. In one embodiment, the reaction mixture comprises one or more compounds that react with a NaH source to form a NaH catalyst. The reaction mixture may comprise one or more from the group of Na, NaH, NaNH 2, Na 2 NH, Na 3 N, NH 3, dissociating agents, hydrogen sources such as H 2 gas or hydrides, supports and getters such as NaX (X is halide). The dissociating agent is preferably a Pt, Ru or Pd / Al 2 O 3 powder. For high temperature operation, the dissociating agent may comprise Pt or Pd on a high surface area support that is suitably inert to Na. The dissociating agent may be Pt or Pd on carbon or Pd / Al 2 O 3. The latter support may comprise a protective surface coating of a material such as NaAlO 2. The reactants may be present in any weight percent.

Preferred embodiments include a reaction mixture of Na or NaH, NaNH 2 and Pd on Al 2 O 3, wherein the reaction mixture can be regenerated by the addition of H 2.

In one embodiment, NaNH 2 is added to the reaction mixture. NaNH2 produces NaH according to the following reversible reaction:

Na2 + NaNH2 → NaH + Na2NH (117)

And

2NaH + NaNH2 → NaH (g) + Na2NH + H2 (118)

In the hydrino reaction cycle, Na-Na and NaNH 2 react to form NaH molecules and Na 2 NH, and NaH forms hydrinos and Na. Thus, the reaction is reversible according to the following reaction:

Na2NH + H2 → NaNH2 + NaH (119)

And

Na2NH + Na + H → NaNH2 + Na2 (120)

In one embodiment, this reaction is another reaction that produces a catalyst because NaH in formula (119) is a molecule.

The reaction of sodium amide and hydrogen to form ammonia and sodium hydride is as follows:

H2 + NaNH2 → NH3 + NaH (121)

In one embodiment, the reaction is reversible. The reaction can be induced to form NaH by increasing the H2 concentration. Alternatively, the forward reaction can be induced through the formation of H atoms using dissociating agents. The response is given by:

2H + NaNH2 → NH3 + NaH (122)

Exothermic reactions can lead to the formation of NaH (g).

In one embodiment, the NaH catalyst is produced from the reaction of NaNH 2 with hydrogen, preferably hydrogen atoms as given in formulas (121) and (122). The ratio of reactants may be any desired amount. Preferably, the ratio is an approximate equivalence ratio for that of equations (121) and (122). The reaction for forming the catalyst is reversible by supplementing the reaction with the addition of an H source such as H2 gas or hydride, wherein the catalytic reaction is given in equations (88) to (95), and the sodium amide of ammonia and Na Formed by additional NaH catalyst by reaction:

NH3 + Na2 → NaNH2 + NaH (123)

In one embodiment, the HSA material is doped with NaNH 2. The doped HSA material reacts with a reactant which will replace the amide group to form one or more of Na and NaH. In one embodiment, the reactant is an alkali metal or alkaline earth metal, preferably Li. In another embodiment, the reactants are alkali or alkaline earth hydrides, preferably LiH. The reactant may be both alkali metal and alkaline earth hydride. H sources such as H2 gas may also be provided in addition to those provided by any other reactants of the reaction mixture such as hydrides, HSA materials and substitution reagents.

In one embodiment, the sodium amide reacts with lithium to form lithium amide, imide or nitride and Na or NaH catalyst. The reaction of sodium amide and lithium to form lithium imide and NaH is as follows:

2Li + NaNH2 → Li2NH + NaH (124)

The reaction of sodium amide and lithium hydride to form lithium amide and NaH is as follows:

LiH + NaNH2 → LiNH2 + NaH (125)

The reaction of sodium amide, lithium and hydrogen to form lithium amide and NaH is as follows:

Li + 1 / 2H2 + NaNH2 → LiNH2 + NaH (126)

In one embodiment, the reaction of the mixture forms Na, and the reactant further comprises an H source that reacts with Na to form the catalyst NaH by the following reaction:

Li + NaNH 2 → LiNH 2 + Na (127)

And

Na + H → NaH (128)

LiH + NaNH2 → LiNH2 + NaH (129)

In one embodiment, the reactant comprises a reactant such as an alkali metal or an alkaline earth metal, preferably Li, for substituting NaNH2, an amide group of NaNH2, and also an H source such as MH (M = Li, Na, K, Rb, Cs). , Mg, Ca, Sr and Ba), H2 and hydrogen dissociating agents, and hydrides.

Reagents such as M, MH, NaH, NaNH 2, HSA materials, hydrides and dissociating agents of the reaction mixture are present in any desired molar ratio. Each of M, MH, NaNH 2 and dissociating agent is present in a molar ratio of greater than 0 and less than 100%, preferably the molar ratios are similar.

Another embodiment of a system for producing a molecular catalyst NaH includes Na and NaBH 4 or NH 4 X (X is an anion such as a halide). Molecular NaH catalysts can be produced by the reaction of Na2 with NaBH4:

Na2 + NaBH4 → NaBH3 + Na + NaH (130)

NH 4 X can produce NaNH 2 and H 2:

Na2 + NH4X → NaX + NaNH2 + H2 (131)

Subsequently, a NaH catalyst may be produced according to the reaction of formulas (117) to (129). In another embodiment, the reaction mechanism for the Na / N system to form hydrino-catalyzed NaH is as follows:

NH4X + Na-Na → NaH + NH3 + NaX (132)

Preparation and Regeneration of NH Catalytic Reactants

In one embodiment, NaH molecules or Na and hydrogenated R—Ni may be regenerated by the systems and methods following the systems and methods disclosed for Li-based reactant systems. In one embodiment, Na may be regenerated from solid NaH by venting H 2 released from NaH. The ballast temperature at about 1 Torr for NaH decomposition is about 500 ° C. NaH may decompose at about 500 ° C., below the alloy formation and sintering temperatures of about 1 Torr and R—Ni. The molten Na can be separated from R-Ni, R-Ni can be hydrogenated again, and Na and hydrogenated R-Ni can be recovered in another reaction cycle. In the case of Na deposited on the hydride surface, it can be regenerated by removing Na by heating by pumping, the hydride can be hydrogenated again by introducing H2, and after evacuating the cell in certain embodiments Na atoms can be deposited again onto the regenerated hydride.

In a preferred embodiment, a competitive reaction in which one reactant is hydrogenated or dehydrogenated to another reactant is used to form a reaction mixture comprising the hydrogenated and non-hydrogenated compounds. For example, the formation of NaH solids is thermodynamically advantageous over the formation of R-Ni hydrides. However, NaH formation rates are low at low temperatures such as in the range of about 25 ° C. to 100 ° C., whereas R-Ni hydride formation is at high rates at suitable pressures such as about 100 Torr to 3000 Torr in this temperature range. Thus, the reaction mixture of Na and hydrogenated R—Ni is pumped at about 400 to 500 ° C. to dehydrogenate NaH, the vessel is cooled to about 25 to 100 ° C. and hydrogen is added for a period of time to achieve the desired selectivity. Can be regenerated from NaH solids and R-Ni by preferentially hydrogenating R-Ni and then evacuating the cell to remove excess hydrogen. While excess Na is present or added in excess, R-Ni can be used in repeated cycles by selectively hydrogenating alone. This is followed by addition of hydrogen at a temperature and pressure range to achieve selective hydrogenation of R-Ni, followed by heating the vessel to form H atoms and NaH molecules and subsequent reaction to obtain the H state given by formula (1). Can be achieved by removing hydrogen. Alternatively, the reaction mixture comprising Na and a hydrogen source such as R—Ni can be hydrogenated to form hydrides, and selectively NaH solids are pumped in the temperature and pressure ranges while achieving selectivity based on differential kinetics. Can be dehydrogenated.

In one embodiment having a powder reactant such as a powder source of catalyst and reducing agent, the reducing agent powder is mixed with the catalyst source powder. For example, NaOH-doped R-Ni providing a NaH catalyst is mixed with a metal or metal hydride powder such as lanthanide or NaH, respectively. In embodiments of the reaction mixture having a solid material such as a dissociating agent, a support, or an HSA material that is doped or coated with one or more other species in the reaction mixture, the mixing may be accomplished by ball milling or initial wetting. In one embodiment, the surface may be coated by infiltration of the surface into a solution of a species such as NaOH or NaX (X is a counter anion such as a halide) and then drying. Alternatively, NaOH can be etched by Ni / Al alloy or by etching with concentrated (deoxygenated) NaOH using the same procedure [49] as used to etch R-Ni as is well known in the art. It can be incorporated into R-Ni. In one embodiment, an HSA material such as R-Ni doped with a species such as NaOH reacts with a reducing agent such as Na to form a NaH catalyst that forms hydrinos. Excess reducing agent such as Na can then be removed from the product, preferably by evaporation under vacuum at elevated temperature. The reaction can be condensed and recycled. In another embodiment, at least one of the reducing agent and the product species is removed using a carrier medium such as a gas or a liquid such as a solvent, and the removed species is isolated from the carrier medium. The species can be isolated by means well known in the art, such as precipitation, filtration or centrifugation. The species may be directly recycled or further reacted to take a chemical form suitable for recycling. The NaOH can also be regenerated by H reduction or by reaction with a steam gas stream. In the case of the former, excess Na can be removed by evaporation, preferably under vacuum at elevated temperature. Alternatively, the reaction product may be removed by washing with a suitable solvent such as water, the HSA material may be dried, and the initial reactant may be added. Independently, the product can be regenerated into the original reactants by methods known to those skilled in the art. Alternatively, a reaction product such as NaOH separated by washing of R-Ni may be used in a process of etching R-Ni to regenerate it. In one embodiment that includes a reactant that reacts with the HSA material, the product, such as an oxide, may be treated with a solvent such as dilute acid to remove the product. The removed product may then be recycled by known methods while re-doping and reusing the HSA material.

As shown in cotton [48], methods and systems known to those skilled in the art can be used to regenerate reducing agents such as alkali metals from products comprising the corresponding compounds, preferably NaOH or Na 2 O. One method involves electrolysis in a mixture such as a eutectic mixture. In further embodiments, the reaction product may include at least some oxides such as lanthanide element metal oxides (such as La 2 O 3). The hydroxide or oxide can be dissolved in a weak acid such as hydrochloric acid to form the corresponding salt such as NaCl or LaCl 3. The gases may be stream streams at low pressure. The salts can be treated with product reducing agents such as alkali or alkaline earth metals to form the original reducing agent. In one embodiment, the second reducing agent is an alkaline earth metal, preferably Ca, wherein NaCl or LaCl 3 is reduced to Na or La metal. Methods known to those skilled in the art are presented in Cotton [48], the entire disclosure of which is incorporated herein by reference. Additional CaCl3 products are also recovered and recycled. In another embodiment, the oxide is reduced by H 2 at high temperature.

In one embodiment where NaAlH 4 is a reducing agent, the product includes Na and Al that do not need to be separated from the R-Ni product. R-Ni is regenerated as a catalyst source without separation. Regeneration can be by addition of NaOH. NaOH can partially etch [49] Al of R-Ni for drying and reusing [50]. Alternatively, Na and Al react or separate in situ from the reaction product mixture and react with H2 as shown by cotton [51] or by the reaction of recovered NaH and Al to form NaAlH4. Form.

R-Ni is a preferred HSA material with NaOH as the source of NaH catalyst. In one embodiment, the Na content obtained from the manufacturer is about 0.01 mg to 100 mg per gram of R-Ni, preferably about 0.1 mg to 10 mg per gram of R-Ni, most preferably about gram per R-Ni. 1 mg to 10 mg. The alloy of R-Ni or Ni may also further comprise one or more of promoters such as Zn, Mo, Fe and Cr. R-Ni or alloy is W. R. Grace Davidson Raney 2400, Raney 2800, Raney 2813, Raney 3201 and Raney 4200, preferably 2400, or may be one or more of the etched or Na-doped embodiments of these materials. The NaOH content of R-Ni can be increased in multiples from about 1.01 to 1000 times. Solid NaOH can be added by mixing by means such as ball milling or can be dissolved in solution to achieve the desired concentration or pH. Doping can be achieved by adding the solution to R-Ni and evaporating water. Doping may range from about 0.1 μg to 100 mg per gram of R-Ni, preferably from about 1 μg to 100 μg per gram of R-Ni, most preferably from about 5 μg to 50 μg per gram of R-Ni. have. In one embodiment, 0.1 g of NaOH is dissolved in 100 ml of distilled water and 10 ml of NaOH is available from 500 g of non-decanted R-Ni (double oil. R. Grace Chemical Company) Lot # 2800/05310) with a total content of about 0.1% by weight. The mixture is then dried. Drying can be accomplished by heating to 50 ° C. under vacuum for 65 hours. In another embodiment, doping may be accomplished by ball milling NaOH, such as about 1-10 mg NaOH per gram of R-Ni with R-Ni.

R-Ni can be dried according to the standard R-Ni drying procedure [50]. R-Ni can be decanted and dried in a temperature range of about 10 to 500 ° C. under vacuum, preferably at 50 ° C. The duration may range from about 1 hour to 200 hours, preferably about 65 hours. In one embodiment, the H content of the dried R-Ni is about 1 ml to 100 ml H / g R-Ni, preferably about 10 to 50 ml H / g R-Ni, where the ml gas is in STP state. ) Range. Drying temperature, time, vacuum pressure and flow of gas (such as He, Ar or H2, if present) during and after drying are controlled to achieve drying and the desired H content.

In one embodiment of R-Ni doped with a NaH catalyst source such as NaOH, the preparation of R-Ni from Ni / A alloys includes etching the alloy with an aqueous NaOH solution. The concentration of NaOH, etch time and wash exchange can be varied to achieve the desired level of NaOH incorporation. In one embodiment, the NaOH solution is oxygen free. The molar concentration is in the range of about 1 to 10 M, preferably in the range of about 5 to 8 M, most preferably about 7 M. In one embodiment, the alloy is reacted with NaOH at about 50 ° C. for about 2 hours. The solution is then diluted with water such as deionized water until an Al (OH) 3 precipitate is formed. In this case, NaOH and Al (OH) 3 at least partially prevent the reaction of forming water-soluble Na [Al (OH) 4] to allow NaOH to be incorporated into R-Ni. The incorporation can be accomplished by drying R-Ni without decanting. The pH of the diluted solution may range from 8 to 14, preferably from 9 to 12, most preferably from about 10 to 11. Argon can be bubbled through the solution for about 12 hours, and then the solution can be dried.

Following the reaction in which the reducing agent and catalyst source form hydrino (H having the state given by Formula (1)), the reducing agent and catalyst source are regenerated. In one embodiment, the reaction product is separated. The reducing agent product may be separated from the product of the catalyst source. In one embodiment where at least one of the reducing agent and catalyst source is a powder, the product is mechanically separated based on at least one of particle size, shape, weight, density, magnetic force or dielectric constant. Particles with significant differences in size and shape can be separated mechanically using a sieve. Particles with large differences in density can be separated by buoyancy differences. Particles with large differences in dielectric constant can be electrostatically separated. In one embodiment, the product is milled to reverse any sintering. The grinding may be by a ball mill.

Methods known to those skilled in the art can be applied to the separation of the present invention by the application of conventional experiments. In general, mechanical separation can be separated into sedimentation, centrifugation, filtration, and sieving as described in the four groups, Earle [52], the entire disclosure of which is incorporated herein by reference. . In a preferred embodiment, separation of the particles is achieved by one or more of the use of a sieving and granulator. The size and shape of the particles can be chosen from the starting materials to achieve the desired product separation.

In further embodiments, the reducing agent is a powder or is converted to a powder and mechanically separated from other components of the reaction product mixture, such as HSA material. In an embodiment, Na, NaH and lanthanide elements comprise one or more of a reducing agent and a reducing agent source and the HSA material component is R-Ni. The reducing agent product may be separated from the product mixture by converting any unreacted non-powder reducing agent metal to hydride. The metal hydride may be ground to form a powder. The powder can then be separated from that of another product such as a catalyst source based on the size difference of the particles. The separation can be carried out by shaking the mixture on a series of sieves that select and separate a particular size range. Alternatively, or in combination with the sieving, R-Ni particles are separated from metal hydrides or metal particles based on large magnetic susceptibility differences between the particles. The reduced R-Ni product may be magnetic. The unreacted lanthanide element metals and hydrogenated metals and optional oxides such as La 2 O 3 are weak paramagnetic and diamagnetic materials, respectively. The product mixture is shaken in a series of strong magnets alone or in a strong magnet combined with one or more sieves, based on one or more of a relatively strong adhesion or attachment of R-Ni product particles to the magnet and the size difference of the two classes of particles. Can be separated. In one embodiment where a sieve is used and a magnetic field is applied, the latter adds additional force to gravity to attract smaller R-Ni product particles through the sieve, while the weak paramagnetic or diamagnetic properties of the reducing agent product are of relatively large size. Because it stays on the sieve. Alkali metals can be recovered from their corresponding hydrides by heating and optionally applying vacuum. The released hydrogen may react with the alkali metal in another batch of repeated reaction-regeneration cycles. There may be at least one batch in the cycle in the various stages. The hydride and any other compound (s) may be separated and then reacted to form a metal separately from the metal formation from the hydride.

In one embodiment, the reaction mixture is regenerated by deposition techniques, preferably when the reactants are on the surface of an HSA material such as R-Ni. In a further embodiment having another coated preferred reactant comprising at least one of a NaH catalyst source on the surface and a material that supports the formation of a NaH catalyst, such as an HSA material, the reactant may react the gas stream with an HSA material such as R-Ni. By reacting. The deposited reactants are Na, NaH, Na 2 O, NaOH, Al, Ni, NiO, NaAl (OH) 4, β-alumina, Na 2 O.nAl 2 O 3 (n is an integer from 1 to 1000, preferably 11), Al ( OH) 3 and alpha, beta, and gamma forms of Al 2 O 3. In addition to being preferred reactants or preferred reactants, the deposited elements, compounds, intermediates and species that are converted to the order and composition and chemistry of the gas stream to form reactants from the gas stream are well known to those skilled in the deposition arts. For example, alkali metal can be deposited directly, and any metal with low vapor pressure, such as Al, can be deposited from the gas halide or hydride. Moreover, oxide products such as Na 2 O can be reacted with a hydrogen source to form hydroxides such as NaOH. The hydrogen source may comprise a steam gas stream to regenerate NaOH. Alternatively, NaOH can be formed using H2 or H2 sources. In addition, hydrogenation of HSA materials such as R-Ni can be accomplished by supplying hydrogen gas and removing excess hydrogen by means such as pumping. NaOH can be stoichiometrically regenerated by precisely controlling the total moles of H reacted from sources such as water vapor or hydrogen gas. Any additional Na or NaH formed in this stage can be removed by evaporation and decomposition and evaporation, respectively. Alternatively, oxides or hydroxide products such as Na 2 O or excess NaOH can be removed. This can be achieved by conversion to a halide such as NaI which can be removed by distillation or evaporation. The evaporation can be accomplished by heating and by maintaining a vacuum at elevated temperature. Conversion to halides can be accomplished by reaction with an acid such as HI. The treatment may be by a gas stream comprising the acid gas. In another embodiment, any excess NaOH is removed by sublimation. This occurs under vacuum in the temperature range of 350-400 ° C. as shown by cotton [53]. Any evaporation, distillation, conveying, gas stream process or related reactant process may further comprise a carrier gas. The carrier gas may be an inert gas such as a rare gas. Additional steps may include mechanical mixing or separation. For example, NaOH and NaH may also be deposited or mechanically removed by methods such as ball milling and sieving, respectively.

When the reducing agent is a preferred first element such as an element other than Na, other elements can be substituted by the second element such as Na using methods known in the art. One step may include evaporation of excess reducing agent. It is possible to etch high surface area materials such as R-Ni. The etching may be by base, preferably NaOH. The etched product may be decanted with virtually any solvent such as, for example, water mechanically removed by decanting and possibly centrifugation. The etched R-Ni can be dried and recycled under vacuum.

Additional MH-Type Catalysts and Reactions

Another catalyst system of the MH type comprises aluminum. The binding energy of AlH is 2.98 eV [44]. The first and second ionization energies of Al are 5.985768 eV and 18.82855 eV, respectively [1]. Based on these energies, AlH molecules are catalysts and H, since the binding energy of AlH + double ionization (t = 2) of Al to Al2 + is equivalent to m = 1 in equation (2), 27.79 eV (27.2 eV). Can serve as a source. The catalytic reaction is given by:

And the overall reaction is:

In one embodiment, the reaction mixture comprises one or more of AlH molecules and AlH molecule sources. The AlH molecular source may comprise an Al metal and a hydrogen source, preferably a hydrogen atom. The hydrogen source may be a hydride, preferably R-Ni. In another embodiment, the catalyst AlH is produced by the reaction of an oxide or hydroxide of Al with a reducing agent. The reducing agent comprises at least one of the NaOH reducing agents set forth above. In one embodiment, the H source is provided to an Al source to form a catalyst AlH. The Al source may be a metal. The H source may be a hydroxide. The hydroxide may be one or more of alkali, alkaline earth hydroxides, transition metal hydroxides and Al (OH) 3.

Raney nickel can be prepared by two reaction steps:

Na [Al (OH) 4] is readily soluble in concentrated NaOH. It can be washed in deoxygenated water. Ni produced contains Al (about 10% by weight, can vary), is porous and has a large surface area. It contains a large amount of H in both the Ni lattice and Ni-AlHx (x = 1,2,3).

R-Ni reacts with another element to cause chemical release of the AlH molecule, followed by catalysis according to the reactions shown in equations (133) to (135). In one embodiment, AlH release is caused by a reduction reaction, etching or alloy formation. One such other element, M, is an alkali or alkaline earth metal, releasing AlH molecules that subsequently undergo catalysis by reacting with the Ni portion of R—Ni to form an AlHx component. In one embodiment, M reacts with Al hydroxide or oxide to form Al metal, which may also react with H to form AlH. The reaction can be initiated by heating and the speed can be controlled by controlling the temperature. M (alkaline or alkaline earth metal) and R-Ni are present in any desired molar ratio. Each M and R-Ni is present in molar ratios greater than 0 and less than 100%. Preferably, the molar ratios of M and R-Ni are similar.

In one embodiment, Al atoms are deposited on the surface. The surface may be a support or an H atom source for forming AlH molecules. The surface may comprise one or more of a hydride and a hydrogen dissociating agent. The surface may be R-Ni, which may be hydrogenated. The deposition may be formed from a reservoir containing a source of Al atoms. The Al source can be controlled by heating. One source that provides Al atoms upon heating is Al metal. The surface can be kept at low temperature such as room temperature during deposition. The Al-coated surface may be heated to react Al and H to form AlH, and the AlH molecules may also be reacted to form the H state given by Equation (1). Other thin film deposition techniques well known in the art for forming Al and other elements such as one or more metal layers further include embodiments of the present invention. Such embodiments include physical spraying, electro-spraying, aerosols, electro-arc welding, Knudsen cell controlled release, dispenser-cathode injection, plasma deposition, sputtering and further coating methods and systems such as fine dispersion melting of Al, of Al Electroplating and chemical vapor deposition of Al.

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

The AlH source may further comprise AlH 3. AlH 3 may be deposited on or with Ni to form a NiAlHx alloy. The alloy can be activated by the addition of a metal such as an alkali metal or an alkaline earth metal. In one embodiment, the reaction mixture comprises AlH 3, R-Ni and a metal such as alkali metal. The metal can be supplied by evaporation from the reservoir or by gravity from a source flowing into the R-Ni phase at elevated temperature. In one embodiment, AlH molecules or Al and hydrogenated R—Ni may be regenerated by systems and methods following the disclosed systems and methods for other reactant systems. Another catalyst system of the MH type includes chlorine. The binding energy of HCl is 4.4703 eV [44]. The first, second and third ionization energies of Cl are 12.96764 eV, 23.814 eV and 39.61 eV, respectively [1]. Based on these energies, HCl is a catalyst and since the binding energy of HCl + Cl of tri-ionization (t = 3) to Cl3 + is 80.86 eV (3.27.2 eV) equivalent to m = 3 in equation (2) Can act as an H source. The catalytic reaction is given by:

And the overall reaction is:

In one embodiment, the reaction mixture comprises HCl or an HCl source. The source can be NH 4 Cl or a solid acid and chlorine such as alkali or alkaline earth chlorides. The solid acid may be one or more of MHSO 4, MHCO 3, MH 2 PO 4 and MHPO 4, where M is a cation such as an alkali or alkaline earth cation. Other such solid acids are known to those skilled in the art. In one embodiment, the reactants comprise HCl catalyst in the ionic lattice such as alkali or alkaline earth halides, preferably HCl in chloride. In one embodiment, the reaction mixture comprises a strong acid such as H 2 SO 4 and an ionic compound such as NaCl. The reaction of an acid with an ionic compound such as NaCl produces HCl in the crystal lattice, acting as a hydrino catalyst and H source.

Generally, hydrinos provided by the breakdown of MH bonds are produced at a continuum energy level such that the sum of the binding energy and the ionization energy of t electrons is approximately m · 27.2 eV, where m is the integral number in Table 2. The MH type hydrogen catalyst and ionization from each M atom of t electrons are given in Table 2 below. Each MH catalyst is shown in the first column and the corresponding M-H binding energy is shown in the second column. The atoms M of the MH species presented in the first column are ionized to provide a net reaction enthalpy of m · 27.2 eV along with the binding energy of the second column. The enthalpy of the catalyst is shown in the eighth column, where m is shown in the ninth column. Electrons participating in ionization are presented as ionization potentials (also called ionization energies or binding energies). For example, the binding energy of NaH, 1.9245 eV [44], is shown in the second column. The ionization potential of the nth electron of an atom or ion is expressed in IPn and is given in CRC [1]. For example, Na + 5.13908 eV-> Na + + e- and Na + 47.2864 eV-> Na2 + + e-. The first ionization potential, IP1 = 5.13908 eV and the second ionization potential, IP2 = 47.2864, are presented in the second and third columns, respectively. The net reaction enthalpy and the double ionization of Na for breaking NaH bonds are 54.35 eV as shown in the eighth column and m = 2 as shown in the ninth column. In addition, H reacts with each of the MH molecules shown in Table 2 below to form a hydrino with a quantum number p that increases by one relative to the catalytic reaction product of MH alone, as shown in Exemplary Formula (92). (Eq. (1)).

Table 2 below shows an MH type hydrogen catalyst capable of providing a net reaction enthalpy of about m · 27.2 eV.

In another embodiment of the MH type catalyst, the reactant comprises a source of SbH, SiH, SnH and InH. In an embodiment providing the catalyst MH, the source comprises an M, H2 source and MHx such as Sb, Si, Sn and In and H2 sources, and one or more of SbH3, SiH4, SnH4 and InH3.

The reaction mixture further comprises an H source and a catalyst source, wherein H and one or more sources of catalyst may be a solid acid or NH 4 X (where X is a halide, preferably Cl) forming an HCl catalyst. Preferably, the reaction mixture may comprise one or more of NH4X, solid acid, NaX, LiX, KX, NaH, LiH, KH, Na, Li, K, support, hydrogen dissociating agent and H2, wherein X Is a halide, preferably Cl. The solid acid may be NaHSO4, KHSO4, LiHSO4, NaHCO3, KHCO3, LiHCO3, Na2HPO4, K2HPO4, Li2HPO4, NaH2PO4, KH2PO4 and LiH2PO4. The catalyst may be one or more of NaH, Li, K and HCl. The reaction mixture may further comprise one or more of a dissociating agent and a support.

Other thin film deposition techniques that are well known in the art further include embodiments of the present invention. Such embodiments include physical spraying, electro-spraying, aerosols, electro-arc welding, Knudsen cell controlled release, dispenser-cathode injection, plasma deposition, sputtering and further coating methods and systems such as M's fine dispersion melting, Electroplating and chemical vapor deposition of M, wherein MH comprises a catalyst.

For M alloys such as MH sources comprising AlH and Al, respectively, the alloys can be hydrogenated by H2 sources such as H2 gas. H2 may be supplied to the alloy during the reaction, or H2 may be supplied to form an alloy of the desired H content with the H pressure varying during the reaction. In this case, the initial H2 pressure may be about zero. The alloy can be activated by the addition of a metal such as an alkali metal or an alkaline earth metal. For MH catalysts and MH sources, the hydrogen gas may be maintained in the range of about 1 Torr to 100 atm, preferably about 100 Torr to 10 atm, more preferably about 500 Torr to 2 atm. In other embodiments, the hydrogen source is provided from hydrides such as alkali metal or alkaline earth metal hydrides or transition metal hydrides.

High-density hydrogen atoms undergo a three-body-collision reaction to form hydrinos, when two additional H atoms ionize, one H atom transitions and is given by equation (1) To form. The response is given by:

And the overall reaction is:

In another embodiment, the reaction is given as follows:

And the overall reaction is:

In one embodiment, the material providing high density H atoms is R-Ni. H atoms may be provided from one or more of the decomposition of H in R-Ni and the dissociation of H2 from H2 sources such as H2 gas provided to the cell. R-Ni can be catalyzed by reacting with alkali metal or alkaline earth metal M to promote the formation of H atomic layers. R-Ni can be regenerated by evaporating the metal M followed by the addition of hydrogen to rehydrogenate the R-Ni.

references

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13. RL Mills, Y. Lu, M. Nansteel, J. He, A. Voigt, B. Dhandapani, "Energetic Catalyst-Hydrogen Plasma Reaction as Potential New Energy Source", Division of Fuel Chemistry, Session: Chemistry of Solid, Liquid, and Gaseous Fuels, 227th American Chemical Society National Meeting, March 28- April 1, 2004, Anaheim, CA.

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16. R. Mills, B. Dhandapani, N. Greenig, J. He, "Synthesis and Characterization of Potassium Iodo Hydroxide", Int. J. of Hydrogen Energy, Vol. 25, Issue 12, December, (2000), pp. 1185-1203.

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24. RL Mills, P. Ray, B. Dhandapani, J. He, "Comparison of Excessive Balmer Line Broadening of Inductively and Capacitively Coupled RF, Microwave, and Glow Discharge Hydrogen Plasmas with Certain Catalysts", IEEE Transactions on Plasma Science, Vol. . 31, No. (2003), pp. 338-355.

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46. F. A. Cotton, G. Wilkinson, C. A. Murillo, M. Bochmann, Advanced Weapon Chemistry, Sixth Edition, John Wiley & Sons, Inc., New York, (1999), p. 95.

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Experiment

The number of equations, number of sections, and references given later in this experimental section refer to those described in the experimental section of the present disclosure.

summary

(p ≤ 137 는 정수임) 는 수소 여기 상태에 대해 리드베리 방정식에서 공지된 파라미터 n = 정수를 대신함) 이다. 리튬 원자 및 NaH 분자는 촉매로서 사용되기 때문에, 촉매 기준에 부합한다 - 수소 원자의 포텐셜 에너지, 27.2 eV 의 정수 배수 m (예, Li 에 대해서는 m = 3 및 NaH 에 대해서는 m = 2) 와 같은 엔탈피 변화를 갖는 화학적 또는 물리적 공정. 신규 알칼리 할리도 하이드리노(hydrino) 수소화물 화합물 (MH*X; M = Li 또는 Na,×= 할라이드) 및 디하이드리노 분자 H2(1/4) 의 상응하는 하이드리노(hydrino) 수소화물 이온 H-(1/4) 의 에너지 준위의 폐쇄형 방정식에 기반을 둔 구체적인 예상을, 화학적으로 발생된 촉매작용 반응물을 사용하여 테스트했다.The data from the broad spectrum of the irradiation technique shows firmly and consistently that hydrogen may be present in a lower energy state than previously conceivable. The expected reaction involves non-release resonance energy transfer from other stable hydrogen atoms to the energy acceptable catalyst. The product is H (1 / p), a fractional Rydberg state of hydrogen atoms called " hydrino atoms "

(p ≦ 137 is an integer), replacing the parameter n = integer known in the Lidbury equation for the hydrogen excited state. Since lithium atoms and NaH molecules are used as catalysts, they meet the catalyst criteria-enthalpy such as potential energy of hydrogen atoms, integer multiples of 27.2 eV (e.g. m = 3 for Li and m = 2 for NaH). Chemical or physical process with change. Novel Alkali Halide Hydrino Hydride Compounds (MH * X; M = Li or Na, × = halide) and the corresponding hydrino hydride ions H of the dihydrino molecule H2 (1/4) Specific predictions based on closed equations of energy levels of-(1/4) were tested using chemically generated catalysis reactants.

) 및 약 1-2 V/cm 의 아주 낮은 필드(field) 강도에서 공명 전달, 즉 rt-플라즈마로 불리는 플라즈마의 형성의 관찰이었다. H Balmer α 라인의 시간 의존성 라인 넓어짐(증대)이 아주 빠른 H (>40 eV) 에 대응하여 관찰되었다.First, the Li catalyst was tested. Li and LiNH 2 were used as sources of lithium atoms and atomic hydrogen. Using water flow batch calorimetry, the measured power from 1 g Li, 0.5 g LiNH 2, 10 g LiBr, and 15 g Pd / Al 2 O 3 was about 160 W with an energy balance of ΔH = −19.1 kJ. The observed energy balance was 4.4 times the maximum theory based on known chemistry. Raney nickel (R-Ni) is then used as a dissociating agent when the power reaction mixture is used in chemical synthesis, where LiBr not only captures H 2 (1/4) in the crystal but also forms LiH * X. It acted as a getter for the catalysis product H (1/4). ToF-SIMs showed LiH * X peaks. 1 H MAS NMR LiH * Br and LiH * I showed large and distinct top field resonance at about −2.5 ppm corresponding to H- (1/4) in the LiX matrix. The NMR peak at 1.13 ppm corresponds to the invasive H2 (1/4) and the rotational frequency of 42 times H2 (1/4) of conventional H2 was observed at 1989 cm-1 of the FTIR spectrum. XPS spectra recorded for LiH * Br crystals show peaks at about 9.5 eV and 12.3 eV that cannot be assigned to any known element based on the absence of other primary element peaks, but in two chemical environments It corresponds to a binding energy of-(1/4). A further signature of the energy process is that low temperatures (e.g.,

) And observation of resonance transfer, ie the formation of a plasma called rt-plasma, at very low field strengths of about 1-2 V / cm. Time dependent line broadening (increase) of the H Balmer α line was observed corresponding to very fast H (> 40 eV).

NaH uniquely achieves kinetics because the catalytic reaction depends on the intrinsic release of H, which forms an additional H (1/3) that reacts to form H (1/4). Suffer incidental transmission. Hot differential scanning calorimetry (DSC) was performed on ionic NaH under helium atmosphere at a very slow temperature ramp rate (0.1 ° C./min) to increase the amount of molecular NaH formation. Novel exothermic effects of -177 kJ / mole NaH were observed in the temperature range of 640 ° C-825 ° C. To achieve high power, R-Ni having a surface area of about 100 m 2 / g is surface-coated with NaOH and reacts with Na metal to form NaH. Using water flow batch calorimetry, the measured power from 15 g of R-Ni was obtained when ΔH = -36 kJ compared to ΔH 0 kJ from the R-Ni starting material, R-NiAl alloy when reacted with Na metal. It was about 0.5 kW with energy balance. The observed energy balance of the NaH reaction was -1.6 x 10 4 kJ / mole H 2, at least 66 times the -241.8 kJ / mole H 2 combustion enthalpy.

ToF-SIMs showed sodium hydrino hydride, NaHx, peak. The 1 H MAS NMR spectra of NaH * Br and NaH * Cl showed large and distinct upper field resonances at -3.6 ppm and -4 ppm corresponding to H- (1/4), respectively, and the NMR peak at 1.1 ppm showed H2 (1 / 4) in accordance with. NaH * Cl from the reaction of solid acid KHSO 4, the only source of NaCl and hydrogen, contained two fractional hydrogen states. H- (1/4) NMR peaks were observed at -3.97 ppm and H- (1/3) peaks were also present at -3.15 ppm. Corresponding H2 (1/4) and H2 (1/3) peaks were observed at 1.15 ppm and 1.7 ppm, respectively. XPS spectra recorded for NaH * Br showed H- (1/4) peaks at about 9.5 eV and 12.3 eV corresponding to the results from LiH * Br and KH * I, whereas sodium hydrino ) Hydride showed two fractional hydrogen states with additional H- (1/3) XPS peak at 6 eV in the absence of halide peaks. The expected rotational transfer with 42 times the energy of conventional H2 was also observed from H2 (1/4) excited using a 12.5 keV electron beam.

I. Introduction

Mills [1–12] interpreted the structure of the combined electrons using classical principles, and continued to unfold with results consistent with observations of basic phenomena of physics and chemistry from the quark scale to the universe. We developed a single theory based on a principle called Theory of Classical Physics (GUTCP). This paper is first in two series containing two specific projections of GUTCP that pollinate the presence of a low energy state of hydrogen atoms, indicating a powerful new energy source and the transfer of hydrogen atoms to low energy states [2]. ].

GUTCP anticipates reactions involving non-emitting resonance energy transfer from other stable hydrogen atoms to energy-acceptable catalysts to form hydrogen at lower energy states than previously conceivable. Specifically, the product is H (1 / p), a fractional Rydberg state of a hydrogen atom called a "hydrino atom", where (p ≦ 137 is an integer) is read for a hydrogen excited state Parameter n = replaces integer. Since He +, Ar +, Sr +, Li, K, and NaH are expected to be used as catalysts, they meet the catalyst criteria-chemical or physical processes with enthalpy changes such as potential energy of hydrogen atoms, integer multiples of 27.2 eV. Data from a broad spectrum of irradiation techniques firmly and consistently support these states, referred to as hydrinos, and the presence of corresponding biatomic molecules called dihydrino molecules for "small hydrogen". Some of these previous related studies supporting the possibility of new reactions of hydrogen atoms to generate hydrogen in fractional quantum states, which are less energy than conventional "ground" (n = 1) states, are found in extreme ultraviolet (EUV) spectroscopy. Characteristic emissions from catalysts and hydride ion products, low energy hydrogen emissions, chemically formed plasmas, Balmer α line enhancement, H line inversion distribution, high electron temperature, anomalous plasma persistence period, power generation, and analysis of new compounds [13-40].

Recently, there have been announcements of some unexpected astrophysical results supporting the presence of hydronose. In 1995, Mills published the GUTCP projection [41] that the expansion of the universe is accelerating from the same equation that accurately predicts the mass of Top Quark before it is measured. Surprisingly, the cosmology confirmed this until 2000. Mills made other predictions about the nature of dark matter based on the almost identifiable GUTCP. Based on recent evidence, Bournaud et al. [42-43] suggested that dark matter is hydrogen in a dense molecular form that behaves differently by what cannot be observed except by gravitational effects. The theoretical model predicted that dwarfs formed from collision fragments of large mass galaxies should be free of nonbaryonic dark matter. As such, his gravity must coincide with the stars and gas within them. Analyzing the observed gas kinematics of such recirculating galaxies, Bournaud et al. [42–43] described the gravitational mass of a series of dwarf galaxies lying in rings around large mass galaxies that have recently experienced collisions. Was measured. Contrary to the expectations of the Cold Dark Matter (CDM) theory, its results demonstrate that it contains a large mass of dark components that is calculated at about twice the visible material. Although this baryonic dark matter is claimed to be cold hydrogen molecules, it is distinguished from conventional hydrogen molecules in that it is not traced at all by conventional methods such as the release of CO lines. These results are consistent with the expectation that the dark matter is a dihydrino molecule.

Emission lines recorded on cold interstellar zones containing dark matter corresponded to the fractional Rydberg state of hydrogen atoms given by H (1 / p), equations (2a) and (2c) [29]. Such emission lines with an energy of q · 13.6 eV (where q = 1, 2, 3, 4, 6, 7, 8, 9, or 11) are also subject to microwave discharge of helium with 2% hydrogen. Observed by extreme ultraviolet (EUV) spectroscopy [27-29]. These He + s complete the chemical or physical process with an enthalpy change, such as an integer multiple of 27.2 eV on the basis of the catalyst, because they ionize at 54.417 eV, which is 2 · 27.2 eV. The product of the He + catalysis reaction, H (1/3), can also be used as a catalyst to transition to another state H (1 / p).

J. R. Rydberg showed that every spectral line of hydrogen atoms is given by a complete empirical relationship:

(1)

(One)

Where R = 109,671 cm-1, nf = 1,2,3, ..., nj = 2,3,4, ... and ni> nf. Bohr, Schroedinger, and Heisenberg, respectively, developed a theory for hydrogen atoms that provide energy levels according to the Rydberg equation.

(2a)

(2a)

n = 1,2,3, ... (2b)

(Where e is the basic charge, εo is the permittivity of the vacuum and aH is the radius of the hydrogen atom). The excited energy state of the hydrogen atom is given by equation (2a) for n> 1 in equation (2b). The n = 1 state is the "ground" state for "pure" photons before (ie, the n = 1 state can absorb photons and go to the excited electron state, but cannot emit photons and low energy electrons) Can't go into state). However, electron transition from ground state to low energy state may be possible by resonant non-emitting energy transfer, such as multipole coupling or resonance collision mechanism. Processes such as forming hydrogen molecule bonds that occur without photons and require collisions are common [44]. In addition, some commercially available phosphors are based on resonant non-emitting energy shear with multipole coupling [45].

The previously reported theory [1, 13-40] states that the hydrogen atom is any atom, excimer, ion and dihydrogen atom (potential energy of hydrogen atom, Eh = 27.2 eV, where Eh is one Hartree It can be expected that the reaction can be subjected to catalytic reaction). Specific classes that can be identified based on known electron energy levels (eg, He +, Ar +, Sr +, K, Li, HCl, and NaH) need to be present with hydrogen atoms to facilitate the process. The reaction involves the delivery of non-emission energy to form hydrogen atoms that are significantly less energetic than the unreacted hydrogen atoms corresponding to the extremely hot excited state H [13-17, 19-20, 32-39], and fractional donor numbers. Then involves q · 13.6 eV release or q · 13.6 eV transfer to H. In other words,

(2c)

(2c)

Replaces the known parameter n = integer in the Rydberg equation for hydrogen excited state. The n-1 state of hydrogen and the n = 1 / integer state of hydrogen are non-emissions, but a transition between two non-emission states, where n = 1 to n = 1/2, is possible through non-emission energy transfer Do. Thus, the catalyst provides a net positive enthalpy of the reaction of m · 27.2 eV (ie, the catalyst resonantly allows non-emission energy transfer from hydrogen atoms and releases energy around to the injected quantum energy level). Affects electronic transitions). As a result of the non-emission energy transfer, the hydrogen atoms become unstable and further release energy until a low energy non-emission state with a main energy level according to equations (2a) and (2c) is achieved.

The catalyst product, H (1 / p), may be reacted with the electrons to form a new hydride ion H- (1 / p) having a binding energy EB [1, 13-14, 18, 30].

(여기서, mp 는 양성자의 질량임) 로 표시되는 환산 전자 질량, ao 는 Bohr(보어) 반경이고, 이온 반경은

이다. 방정식 (3)으로부터, 수소 이온의 계산된 이온화는 0.75418 eV 이고, 리케(Lykke) [46] 에 의해 주어진 실험값은 6082.99 ± 0.15 cm-1 (0.75418 eV)이다.Where p = integer> 1, S = 1/2, h is plaque constant bar, μo is the permeability of vacuum, me is the mass of electron, μe is

(Where mp is the mass of the proton), the converted electron mass, ao is the Bohr radius, and the ionic radius is

to be. From equation (3), the calculated ionization of hydrogen ions is 0.75418 eV and the experimental value given by Lykke [46] is 6082.99 ± 0.15 cm-1 (0.75418 eV).

The upfield shifted NMR peak is direct evidence of the presence of low energy state hydrogen with a reduced radius for conventional hydrogen ions and with an increase in the diamagnetic shielding of the protons. The shift is given by the sum of the common hydride ions H- and the components due to the low energy state [1, 15]:

(4)

(4)

Where p = 0 for H-, p = integer> 1 for H- (1 / p), and is a microstructural constant.

H (1 / p) can react with protons and two H (1 / p) can react to form H2 (1 / p) + and H2 (1 / p), respectively. Hydrogen molecular ions and molecular charge and current density functions, bond distances, and energy have been described from Laplacian in ellipsoid coordinates with suppression of non-emissions [1, 6].

The total energy ET of the hydrogen molecular ion with the central field of + pe at each focal ellipsoid molecular orbit is:

Where p is an integer, c is the speed of light in vacuum, μ is the equivalent nuclear mass, and k is the harmonic load constant previously described in a closed equation with only a basic constant [1, 6]. The total energy of a hydrogen molecule with a central field of + pe at each focal ellipsoid molecular orbit is:

The bond dissociation energy of the hydrogen molecule H2 (1 / p), ED, is the difference between the corresponding hydrogen atom and the total energy of ET:

ED = E (2H (1 / p))-ET (8)

Here [47],

E (2H (1 / p)) = -p227.20eV (9)

ED is given by equations (8-9) and (7):

The calculations and measurement parameters of H2, D2, H2 +, and D2 + from references [1, 6] are given in Table 3 below.

[1, 6]은 H2 와 H2(1/p)에 대한 p = 정수 > 1 에 의존하는 용어의 이동의 합에 의해 주어진다:The 1 H NMR resonance of H 2 (1 / p) is expected to be high field from the resonance of H 2 due to the fractional radius in elliptical coordinates [1, 6], where the electrons are quite close to the nucleus. Expected shift for previously derived H2 (1 / p),

[1, 6] is given by the sum of the shifts in terms that depend on p = integer> 1 for H2 and H2 (1 / p):

Where p = 0.

The molecular vibration energy, Evib, for the transition υ = 0 to υ = 1 of hydrogen H2 (1 / p) is [1, 6].

Evib = p20.55902 eV (13)

Where p is an integer and the experimental vibrational energy for the υ = 0 to υ = 1 transition is given by Beutler [48] and Herzberg [49].

The rotational energy, Erot, for the J to J + 1 transition of hydrogen type H2 (1 / p) is [1, 6].

Where p is an integer, I is the moment of inertia, and the experimental rotational energy for the J = 0 to J = 1 transition of H2 is given by Atkins [50].

The p2 dependence of rotational energy arises from the internuclear distance on the moment of inertia I and the inverse p dependence of the corresponding impact. The expected internuclear distance 2c 'for H2 (1 / p) is:

(15)

(15)

The formation of new states of hydrogen is very vigorous. New chemically generated or enhanced plasma sources have been developed that are based on a novel resonance energy transfer mechanism (rt-plasma) and may be new power sources. One such source operates by heating a hydrogen dissociating agent and a catalyst with an incandescent lamp to provide a hydrogen atom and a gaseous catalyst, respectively, whereby the catalyst reacts with the hydrogen atoms to produce a plasma. Surprisingly, the strong EUV emission has a surprising low electric field strength of about 1-2 V / cm from the potential energy of hydrogen atoms, hydrogen atoms that simply or vary ionize at integer multiples of 27.2 eV and from any atomizing element or any gas phase ion. As well as by Mills et al. [13-21, 38-39] at low temperatures (eg 103 K).

K-K3 + gives the reaction a net enthalpy of three times the potential of the hydrogen atom. It has been previously reported that the presence of this gaseous atom with thermally dissociated hydrogen forms an rt-plasma with strong EUV emission with normal inversion Lyman density [13-21, 38-39]. Other noncatalytic metals such as Mg did not produce plasma. Significant line enhancement of the Balmer α, β and γ lines of 18 eV was observed. Emission from rt-plasma occurred even when the electric field applied to the plasma was zero. Since no conventional discharge power source exists, the formation of plasma required a vigorous reaction. The cause of the Doppler linewidth increase is the relative thermal motion of the emitter relative to the observer. Linewidth enhancement is a measure of atomic temperature and a significant increase was expected and was observed for K [13-21, 38-39] as well as catalyst, Sr + or Ar + with hydrogen. Observation of high hydrogen temperatures without prior description indicates that the rt-plasma should have a source of free energy. The vigorous chemical reactions were even more involved because they knew that augmentation was time dependent [13-14, 20]. Therefore, the thermal power balance was measured in calories. Since the reaction is exothermic, an excess power of 20 mW cm-3 was measured by Calvet calorimetry [20]. In further experiments, KNO 3 and Raney nickel were used as sources of K catalyst and atomic hydrogen, respectively, resulting in corresponding exothermic reactions. The energy balance is due to the combustion of hydrogen by atmospheric oxygen, ΔH = -17,925 kcal / mole KNO3, 300 times that expected for the most active known chemistry of KNO3, assuming the maximum possible list of H2 [14]. ΔH = −3585 kcal / mole H2, which is more than 60 times the maximum enthalpy of the assumption of −57.8 kcal / mole H2. Further substantial evidence of a vigorous catalytic reaction is described above, involving resonance energy transfer between hydrogen atoms and K to form highly stable novel hydride ions and molecules H- (1/4) and H2 (1/4), respectively. Reported [13-15, 24-26, 30-31]. Characteristic release was observed from K3 +, which confirmed a resonance non-emission energy transfer of 3 · 27.2 eV from K to the hydrogen atom used as the expected catalyst. From equation (3), the binding energy EB of H- (1/4) is:

The product hydride ion H- (1/4) was observed by EUV spectroscopy at 10 nm corresponding to the expected binding energy of 11.2 eV [13-15, 24-26, 30-31]. The identity of H- (1/4) was previously confirmed by XPS measurement of its binding energy. With additional features at 8.9 eV and 10.8 eV, the XPS spectra of KH * I different from KI are consistent with H- (1/4) Eb = 11.2 eV in two different chemical environments without corresponding any other primary element peaks. did. The 1 H MAS NMR spectrum of the novel compound KH * Cl for external tetramethylsilane (TMS) shows large and distinct upper field resonance at -4.4 ppm, corresponding to an absolute resonance shift of -35.9 ppm consistent with the theoretical prediction of p = 4. [13-15, 25-26, 30-31]. Elemental analysis identified these compounds containing alkali metals, halogens and hydrogen, and the unknown hydride compounds of this composition could be found in the literature with higher field shift hydride NMR peaks. Conventional alkali hydrides, alone or mixed with alkali halides, showed subfield shift peaks [13-15, 25-26, 30-31]. From the above, the list of alternatives of H- (1 / p) as a possible source of higher field NMR peaks has been limited to H at the center of kJ. This was eliminated by the absence of a strong and characteristic infrared oscillation band at 530 cm −1 due to the substitution of Cl— by H— for KCl [51].

As a further feature, an FTIR analysis of the KH * I crystals by H- (1/4) was performed and an invasive H2 (1/4) with the expected rotational energy given by equation (14) was observed. Rotating lines were observed in the 145-300 nm region from atmospheric electron beam excitation argon-hydrogen plasma [13-14]. The unprecedented energy interval, 42 times that of hydrogen, established the internuclear distance as one-quarter of the H2 distance and confirmed H2 (1/4) (equation (13-15)). The spectra were asymmetrical with the P branch dominant corresponding to the absence of dense rotation in the excited v = 1 oscillation state. This was due to the high rotational energy (10 times the thermal energy), the short lifespan of the rotational excited state and the low cross-sectional area of the electron beam rotational excitation, while oscillating dipole excitation was allowed. Thus, only the ν = 1, J = O state is quite dense from the electron beam excitation, and the transition occurred with AJ> 0 during the υ = l to υ = 0 transitions. KH * Cl with H- (1/4) by NMR was incident on a 12.5 keV electron beam, which excited the similar emission of invasive H2 (1/4) as observed in the argon-hydrogen plasma. [13-14]. Specifically, H2 (1/4) trapped in the lattice of KH * Cl is the electron beam of the crystal using a 12.5 keV electron gun below the pressure at which a gas can produce a detectable emission (<10-5 Torr). It was investigated by windowless EUV spectroscopy for this. The rotational energy of H 2 (1/4) was likewise confirmed by this technique. These results include intense hydrogen Lyman release, normal reverse Lyman density, excessive afterglow persistence, very vigorous hydrogen atoms, characteristic alkali-ion release due to catalysis, expected new spectral lines, and more stable hydr Transfer of the catalytic reaction of atomic hydrogen to form reno ion-designated H- (1 / p) from plasma formed by vigorous hydrino-forming reactions with power measurements beyond any conventional chemistry [13-40] in line with expectations. Confirmed the observation. Since the comparison of ions with experimental energies is direct evidence of low energy hydrogen with unclear large exotherms during the formation of hydrogen, the results when these experiments are additionally repeated with the expected catalysts Li and NaH are reported in this paper.

The catalyst system produced, used and analyzed for the expected hydride compounds involves lithium atoms. The primary and secondary ionization energies of lithium are 5.39172 eV and 75.64018 eV, respectively [52]. At that time, the double ionization (t-2) reaction of Li-Li 2+ has a net enthalpy of the reaction of 81.0319 eV corresponding to 3 · 27.2 eV.

And, total reaction is

Lithium is a metal in the solid and liquid state, and the gas is a covalent Li2 molecule [53], each with a binding energy of 110.4 kJ / mole [54]. In order to yield lithium atoms, LiNH 2 was added to the reaction mixture. LiNH2 also yields hydrogen atoms following a reverse reaction [55-64]:

Li2 + LiNH2 → Li + Li2NH + H (20)

* And

Li2 + Li2NH → Li + Li3N + H (21)

The reaction energy of lithium amide to lithium nitride and lithium hydride is an invention [65-66]:

4Li + LiNH2 → Li3N + 2LiH ΔH = -198.5 kJ / mole LiNH2 (22)

Thus, the reaction must occur to a significant extent. The specific prediction of the vigorous response given by equation (17-19) was tested by rt-plasma formation and H line enhancement. The developed power was measured by water flow batch calorimetry. Then, the expected products of H- (1/4) and H2 (1/4) with energies given by equations (3) and (5-15), respectively, were obtained by magic angle solid proton nuclear magnetic resonance spectroscopy (MAS 1H). NMR), X-ray photoelectron spectroscopy (XPS), time-of-flight secondary ion mass spectroscopy (ToF-SIMs), and Fourier transform infrared spectroscopy (FTIR).

Compounds containing hydrogen, such as MH, where M is an element other than hydrogen, are used as a source of hydrogen and a source of catalyst. Catalytic reactions are provided by the breakage of M-H bonds plus ionization of t electrons from each atom M to the continuous energy level, whereby the sum of the binding energy and the ionization energy of t electrons is about m · 27.2 eV (where M is an integer). One such catalyst system involves sodium. The binding energy NaH is 1.9245 eV [54] and the primary and secondary ionization energies of Na are 5.13908 eV and 47.2864 eV, respectively [52]. Based on these energies, NaH molecules are used as catalysts and H sources because the binding energy of the double ionization (t = 2) of the binding energy NaH + Na-Na 2+ is 54.35 eV (2.27.2 eV). Catalytic reaction is given by:

And the overall reaction is:

As given in Chapter 5 of Ref. [1] and Ref. [29], the hydrogen atom H (1 / p) p = l, 2,3, .. 137 is given by equations (2a) and (2c) Additional transitions to the low energy state can be experienced, where the transition of one atom is facilitated by the other, which accepts m · 27.2 eV non-emissions resonantly with an incidental opposite change in potential energy. The overall general equation for the transition from H (1 / p) to H (l / (p + m)) induced by resonance transfer from m · 27.2 eV to H (1 / p ') is shown below.

In the case of high hydrogen atom concentrations, the transition from H (1/3) (p = 3) to H (1/4) (p + m = 4) by H as catalyst (p = 1; m = 1) Can be faster:

 The NaH catalysis can be matched because the binding energy NaH, the double ionization of Na-Na 2+ (t = 2), and the potential energy of H are 81.56 eV (3.27.2 eV).

And the overall reaction is:

Here, H + fast is a fast hydrogen atom with a kinetic energy of at least 13.6 eV. H- (1/4) forms a stable halide hydride and reacts with 2H (1/4) to H2 (1/4) and H- (1/4) + H + → H2 (1/4). Crushed product with the corresponding molecule formed by [13-15, 24-26, 30-31]. Corresponding hydrino atom H (1/4) is the preferred end product consistent with the observation that p = 4 quantum states have higher polypolarity than quadrupoles which give long theoretical life. H (1/4) may be formed directly from H (eg, equations (36-38)) or via multiple transitions (eg, equations (23-27)). In the latter case, the quantum numbers p = 2 corresponding to dipole and quadrupole transitions, respectively; l = 0 and p = 3; High-energy H (Mp) states with l = 0,1,2 have a fast transition that is theoretically acceptable.

Sodium hydride is generally in the form of an ionic crystalline compound formed by the reaction of gaseous hydrogen with metal sodium. In the gas phase, sodium also contains covalent Na2 molecules with a binding energy of 74.8048 kJ / mole [53]. When NaH (s) is heated at a very slow temperature gradient (0.1 ° C./min) under helium atmosphere to form NaH (g), the expected exothermic reaction given by equation (23-25) is determined by differential scanning calorimetry ( DSC) was observed at high temperatures. In order to achieve high power, the chemical system was designed to greatly increase the amount of NaH (g) and the rate of formation. The reaction of NaOH and Na to Na 2 O and NaH (s) calculated from the heat of formation [54, 65] releases ΔH = -44.7 kJ / mole NaOH:

NaOH + 2Na → Na 2 O + NaH (s) ΔH = -44.7 kJ / mole NaOH (31)

This exothermic reaction can form NaH (g) and is used for the exothermic reaction given by equation (23-25). The regeneration reaction in the presence of hydrogen atoms is as follows:

Na 2 O + H → NaOH + Na ΔH = -11.6 kJ / mole NaOH (32)

NaH → Na + H (1/3) ΔH = -10,500 kJ / mole H (33)

* And

NaH → Na + H (1/4) ΔH = -19,700 kJ / mole H (34)

Thus, small amounts of NaOH, Na, and hydrogen atoms are used as catalyst sources for NaH catalysts which in turn form large yields of hydrins of hydrino through multiple cycles of regeneration reactions as given by equations (31-34). R-Ni having a high surface area of about 100 m 2 / g and containing H was coated with NaOH and reacted with Na metal to form NaH (g). Since the energy balance in the formation of NaH (g) can be neglected due to the small amount involved, the energy and power due to the hydrino reaction given by equation (23-25) is clearly measured by water flow batch calorimetry. It became. Then, R-Ni 2400 was prepared containing about 0.5 wt% NaOH, and Al of the intermetallic compound was used as a reactant to form a NaH catalyst during calorimetry. The reaction of NaOH + Al-Al 2 O 3 + NaH [65] calculated from the heat of formation is exothermic with ΔH = -189.1 kJ / mole NaOH. The balance reaction is given by:

3NaOH + 2Al → Al2O3 + 3NaH ΔH = -189.1 kJ l mole NaOH (35)

This exothermic reaction can form NaH (g) and is used for that exothermic reaction given by equation (23-25), where the regeneration of NaH takes place from Na in the presence of hydrogen atoms. For 0.5 wt% NaOH, the exothermic reaction given by equation (35) provided a myriad of ΔH = -0.024 kJ background heat during the measurement.

It has been reported above [28-29] that the reaction product H (1 / p) can undergo further reaction to a low energy state. For example, the catalytic reaction of Ar +-Ar2 + forms H (1/2), which is further used as both catalyst and reactant to produce H (1/4) [1, 13-14, 28-29] and corresponding Preferred molecule H 2 (1/4), which can be observed with different catalysts [13-14]. Thus, the expected products of NaH catalysts from Equations (23-25) and Table 1 of Ref. [29] are H- (1/3) and each having the energy given by Equations (3) and (5-15), respectively; H2 (1/4). The product was tested by MAS 1H NMR and ToF-SIMs.

Other catalyst systems of the MH type involve chlorine. The binding energy of HCl is 4.4703 eV [54]. The primary, secondary, and tertiary ionization energies of Cl are 12.96764 eV, 23.814 eV, and 39.61 eV, respectively [52]. Based on these energies, HCl can be used as a catalyst and H source because the binding energy of HCl + triple ionization (t = 3) of Cl to Cl3 + is 80.86 eV (3.27.2 eV). Catalytic reactions are given by:

Cl3 + + 3e- + Η → HCl + 80.86 eV (37)

And the overall reaction is as follows:

At that time, the expected product is H 2 (1/4).

Alkali chlorides generally contain both Cl and H from H2O contaminants. Thus, some HCl can be formed intrusive in the crystalline matrix. Since H + is the most easily substituted for Li + and the substitution is likely to be the case for Cs +, H2 (1/4) tends to form in the order of Group 1 elements, forming HCl where alkali chlorides undergo catalysis. It was expected that it could form. Due to the difference in lattice structure, MgCl 2 cannot form an HCl catalyst; Therefore, it is used as a goat control. This condition applies to halides of copper that can be used as a control for the formation of other alkaline earth halides and transition metal halides such as H 2 (1/4). One exception from this set is Mg 2+ in a suitable lattice, since the ionization of Mg 2+ -Mg 3+ is 80.1437 eV with nearly 3 · 27.2 eV [52]. This hypothesis is based on alkali halides, MgX 2 (X = F, Cl, Br, I), with the aim of determining whether the expected release of H 2 (1/4) is selectively observed when a catalytic reaction is possible or not. And CuX2 (X = F, Cl, Br) by electron beam-excited emission spectroscopy. NMR was recorded for phase compounds to find the corresponding expected H 2 (1/4) peak to be compared with the release result.

II. Experiment method

Rt-plasma and line broadening method. LiNH2 argon-hydrogen (95/5%) and LiNH2 hydrogen rt-plasma were generated in the experimental apparatus described above [15-21] (FIG. 1), which provided a stopper with passages to gas inlets and outlets. And thermally insulated stainless steel cells. Titanium filaments (55 cm long, 0.5 mm diameter) were used as heaters and hydrogen dissociators in the cell. 1 g of LiNH2 (Alfa Aesar, 99.95%) was placed in the center of the cell in a glove box at 1 atm argon. The cell was sealed and taken out of the glove box. Helium was flowed at 1 Torr pressure at a rate of 30 sccm while maintaining the cell at 50 ° C. for 4 hours. The filament power was increased by 20 W every 20 minutes to reach 200 W. At 120 W, the filament temperature was estimated to range from 800 to 1000 ° C. The outer wall temperature of the cell was about 700 ° C. The cell was then operated with or without flowing argon-hydrogen (95/5%) maintained at 1 Torr at a rate of 5.5 sccm. The cells were also operated with flowing hydrogen gas instead of argon-hydrogen (95/5%). LiNH2 was evaporated using a filament heater to verify the presence of Li lines. The presence of argon-hydrogen or the presence of hydrogen plasma was determined by recording in the visible spectrum in the ballmer region, for which the CCD detector using the aforementioned inlet / outlet slit of 80/80 μm and an integration time of 3 seconds [15- 21] was used (Jobin Yvon Horiba 1250 M). The width of the 656.3 nm Ballmer series line emitted from argon-hydrogen (95/5%)-LiNH2 or hydrogen-LiNH2 rt-plasma with titanium filaments was measured periodically during the initial and test periods. As a control, each of the above experiments was conducted by flowing a gas containing LiNH 2.

Differential scanning calorimetry (DSC). Differential Scanning Calorimetry (DSC) measurements were performed using the DSC mode of the calorimeter (HT-1000, Setaram, France). Two alumina gloves were used for the sample and reference compartments, respectively. Two globes allowed atmospheric reactions to be controlled. 0.067 g of NaH was placed in a flat-bottom Al-23 crucible (Alfa-Aesar, 15 mm height × 10 mm outer diameter × 8 mm inner diameter). The crucible was then placed at the bottom of the sample group alumina glove cells. As a reference group, an aluminum oxide sample (Alfa-Aesar, -400 mesh powder, 99.9%) was put in the same kind of Al-23 crucible with the same mass as the sample group. All samples were handled in a glove box. Each alumina glove cell was sealed in a glove box, taken out of the glove box, and quickly attached to the calorimeter. They immediately depressurized to a pressure of 1 mTorr or less. The cell was refilled with 1 atm of helium, recompressed and then with 760 Torr of helium. The cells were then placed in an oven and their positions fixed in the DSC equipment. The oven temperature was set at 100 ° C., the desired starting temperature. The temperature of the oven was raised from 100 ° C. to 750 ° C. at a rate of 0.1 ° C./min. As a control, MgH 2 was used instead of NaH. A MgH 2 sample (Alfa-Aesar, 90%, residual Mg) was added to the sample group cell, and the same mass of aluminum oxide (Alfa-Aesar) was added to the reference group cell. All samples were handled in a glove box.

Water-flow, batch calorimeter. A cylindrical stainless steel reactor of about 60 cm 3 in volume (outer diameter 1.0 ", length 5.0", and outer wall thickness 0.065 ") is shown in Figure 2. The cell has an inner welded cylindrical thermocouple having a length of 2.5" and an outer wall thickness of 0.035 ". It was additionally provided at the center with a thermocouple (Type K, Omega) read by the instrument (DAS). For cells sealed with high temperature valves, the outer diameter welded to the end 1/4 "inch from the center. A 3/8 ", 0.065" thick tube was used as a passageway for introducing the following reagents: (i) 1 g of Li, 0.5 g of LiNH2, 10 g of LiBr, and 15 g of Pd / Al2O3, (ii) 3.28 g of Naney, Raney 15 g of (R-) Ni / Al alloy, (iii) 15 g of NaOH doped R-Ni, and (iv) 3 wt% Al (OH) 3 doped Ni / Al alloy. When sealing the passage by spot welding, a tube having an outer diameter of 1/4 "and an outer wall thickness of 0.02" SS was used. The reaction was loaded into a glove box, the valve was attached to the passage tube to seal the cell, and the cell was taken out of the glove box and connected to a vacuum pump. The cell was decompressed by reducing the pressure to 10 mTorr. The cell was then sealed with a valve or sealed with 1/2 "spot welding of the cell which blocked the remaining tube.

The reactor was installed in the cylindrical calorimeter chamber shown in FIG. The stainless steel chamber was to have an inner diameter of 15.2 cm, an outer wall thickness of 0.305 cm, and a length of 40.4. Removable stainless steel plates and VitonTM o-rings were used to seal both ends of the chamber. The space between the reactor and the inner wall of the cylindrical chamber was filled with a high temperature insulator. The gas composition and pressure in the chamber were controlled by adjusting the thermal conductivity between the reactor and the chamber. The interior of the chamber was first filled with 1000 Torr of helium to bring the cell to room temperature and then decompressed during calorimetry to increase the temperature of the cell. Then, 1000 Torr of helium was added to increase the thermal conductivity from the hot cell to the coolant and to control the thermal change associated with the pressure-volume change. The relative dimensions of the reactor and chamber were adjusted such that the heat flowing from the reactor to the chamber was primarily radial. The chamber was cooled using fast flowing coolant through a copper tube with an inner diameter of 6.35 mm, which was wound tightly about 63 times on the outer cylindrical surface of the chamber. The reactor and chamber were designed to safely absorb 50 kW of thermal power pulses for 1 minute. The absorbed energy was sequentially released to the coolant stream in a manner determined for calorimetry. The temperature rise of the cooling water was measured at the cooling coil inlet and outlet using a precision thermistor probe (Omega, OL-703-PP, 0.01 ° C.). The temperature of the inlet water was controlled by a constant temperature bath (Cole Parmer, digital Polystat, model 12101-41) with 0.01 C temperature stability and a cooling capacity of 900 W at 20 ° C. Insulated 8 liter tanks were installed only at the bottom of the tank to reduce temperature fluctuations caused by circulation in the tank. Cooling water flow in the equipment was maintained by the FMI model QD variable flow rate positive displacement test pump. Cooling water flow rate was controlled by a high resolution variable area flow meter. The flow meter was adjusted by its own flow sorting. Secondary flow rate measurements were performed by a turbine flow meter (McMillan, G111 Flometer, 1%) that continuously sent the flow rate to the data acquisition device. The calorimeter chamber was installed in a closed HDPE tank filled with melamine foam insulator to minimize the heat loss rate of the device. A precise measurement of the thermal power dissipation into the cooling water and comparison with the measured input power shows that the heat loss rate is 2-3%.

The calorimeter is adjusted by a precision heater acting during the adjustment time to determine the percent recovery of the total energy added by the heater. Energy recovery was calculated by integrating the total output power Pr during that time. The power was calculated by the following equation.

(39)*

(39)

Where is the total flow rate, Cp is the specific heat of water, is the absolute value of the temperature difference between the inlet and the outlet, where the two thermistors compensate for the difference in constant flow rate without input power. As a step in the calibration test, the hollow reaction cell (which is the same as the power cell containing the reactant tested next) was decompressed to less than 1 Torr and inserted into the calorimeter vacuum chamber. The chamber was depressurized and filled with helium to reach 1000 Torr. The unpowered device reached equilibrium after approximately two hours, at which time the temperature difference between thermistors became constant. The apparatus was run for another hour to obtain a difference according to the calibration values of the two sensors. The degree of correction was 0.036 ° C. and the correction was constant when looking at the data collected during the entire run of the test.

In order to increase the temperature of the cell per input power, during the last 10 minutes of the 10 hour equilibrium time, helium in the chamber was evacuated through a vacuum pump and the pump was continuously maintained at a pressure of less than 1 Torr. Power of 100.00 W was supplied to the heaters (50.23 V and 1.991 A) for 50 minutes. During this time, the cell temperature increased to approximately 650 ° C. and the maximum value of the difference in water temperature (water temperature difference between the outlet and the inlet) was about 1.2 ° C. After 50 minutes, the power pointed to zero. In order to increase the heat transfer rate to the cooling water, the chamber was repressurized to 100 Torr of helium and the device was brought to full equilibrium after 24 hours as confirmed by the equilibrium observation in the flow thermistor.

The hydrino reaction followed the procedure when performing the calibration, but the cell contained a sample. The equilibration time in the chamber with 1000 Torr helium was 90 minutes. Power of 100.00 W was supplied to the heater, and after 10 minutes, helium was discharged from the chamber. The cell was heated faster than the evacuation rate and at 57 minutes the reagents reached 190 ° C., the limit temperature of the hydrino reaction. Initiation of the reaction was confirmed as the cell temperature rapidly increased to about 378 ° C. in about 58 minutes. After 10 minutes, power was cut off and helium was slowly injected into the cell at a rate of 150 sccm for 1 hour.

0.1 wt% NaOH-doped R-Ni 2800 or 0.5 wt% NaOH-doped R-Ni 2400 (elemental analysis was performed by WR Grace Davidson, manufacturer, wt% of NaOH for samples in an inert atmosphere Obtained by performing elemental analysis (Galbraith) and reaction of these reactants with Li (1 g) and LiNH2 (0.5 g), LiBr (10 g) (Alfa Aesar, ACS grade 99 +%), and Pd / Al2O3 ( The products obtained from the reaction of the reaction mixture containing 15 g) (1% Pd, Alfa Aesar) were analyzed, which was quantified using a sealed sample holder (Bruker, Model # A100B3) loaded in a glove box under argon. Diffractometer using X-ray diffraction analysis (XRD) and using Cu radiation with a power of 40 kV / 30 mA over a range of 10 ° to 70 ° with a step interval of 0.02 ° and an 8 hour calculation time (Siemens, D5000 ). In addition, in a 16.5 cc stainless steel cell connected to a vacuum device with a total volume of 291 cc, a sample of weighed R-Ni is heated from 25 ° C. to 550 ° C. to decompose and release it into a physically adsorbed or chemisorbed gas. The gas being identified was measured and measured. Mass spectrometer, quantitative gas chromatography (HP 5890 Series II-microfill column (2 m length, 1/16 "outer diameter, ShinCarbon, ST 100/120), N2 carrier gas (flow rate 14 ml / min), oven temperature 80 And the measured pressure, volume, and temperature were substituted into the ideal gas equation to derive the hydrogen content. Hydrogen was most dominant in each analysis with water, and less than 2% of methane was measured by gas chromatography.R-Ni and traces of water were each measured with hydrogen, which was measured at room temperature. 0.5 g of the sample did not increase to saturated moisture-steam pressure at liquefaction, followed by liquefaction of H2O in the liquid nitrogen trap, dehydrogenation and evaporation of moisture.

Synthesis and solid phase 1H MAS NMR of LiH * Br, LiH * I, NaH * Cl and NaH * Br. As further reactants, Li (1 g) and LiNH2 (0.5 g) (Alfa Aesar, 99%) were reacted with hydrogen to synthesize lithium bromo and iodohydrinohydrides (LiH * Br and LiH * I). It was. The compound was prepared in a stainless steel gas cell (FIG. 4) to further contain Raney Ni (15 g) (W. R. Grace Davidson) as the hydrogen dissociating agent according to the aforementioned method [13-14]. The reactor was operated in a kiln at 500 ° C. for 72 hours with hydrogen to cyclically change the pressure between 1 Torr and 760 Torr. The reactor was then cooled under helium gas. The sealed reactor was opened under argon gas in a glove box. The NMR sample was placed in a glass ampoule, sealed with a rubber stopper and then moved out of the glove box to make it nonflammable. 1H MAS NMR was performed on LiH * X (X is halide) solid samples as described above [Spectral Data Services, Inc., Champaign, Illinois). Chemical shifts were referenced to external TMS. In addition, XPS was performed on crystalline samples that were treated as air sensitive materials.

Since the synthetic reaction comprises LiNH 2 and Li 2 NH is the reaction product, both materials were used alone and as controls in LiBr or LiI substrates. LiNH2 is a commercial starting material, Li2NH is synthesized by the reaction of LiNH2 and LiH [67] and also by the decomposition of LiNH2, and [68] the product Li2NH is identified by X-ray diffraction analysis (XRD). . LiH (Aldrich Chemical, 99%), LiNH2, and Li2NH, in order to eliminate the possibility of alkali halides being affected by local quantum environments or generating NMR resonances shifted relative to any known species, A control comprising the same molar ratio mixture of LiX was utilized. Controls were prepared by mixing the same moles of compound in a glove box under argon. Electron spins on LiH * Br and LiH * I samples to remove F centers that are likely to provide a local quantum environment of any known species, making it impossible to generate upfield-shifted NMR resonances Resonance spectroscopy (ESR) was performed. For ESR analysis, the samples were loaded into quartz tubes (Suprasil) with a diameter of 4 mm and decompressed to a final pressure of 10-4 Torr. ESR spectra were recorded at room temperature and 77 K using an X-band spectrometer (ESP 300, Bruker). The magnetic field was adjusted using a magnetic flux meter (Varian, E-500 gauss meter). The microwave frequency was measured using a frequency measuring instrument (HP company, 5342A).

Elemental analysis was performed (Galbraith Laboratories) to confirm the resulting composition and to eliminate the possibility of NMR detection of transition metal hydrides or other hydrides that could generate high field-shift peaks. In particular, the presence of all elements (Li, H, X) and all elements (Ni, Fe, Cr, Mo, Mn, Al) present in the product and stainless steel reaction vessels were analyzed.

Na (3.28 g) and NaH (1 g) (Aldrich Chemical, 99%) as a raw material of the NaH catalyst are reacted with hydrogen, and as a further reactant, the corresponding alkali halide (15 g, NaCl or NaBr) (Alfa Aesar, ACS grade 99 +%) was reacted with native atom H to synthesize NaH * Cl and NaH * Br. Pt / Ti (Pt coated Ti (15 g); Titan Metal Fabricators, platinum-plated titanium mini-expanded cathode, 0.089 cm × 0.5 cm × 2.5 cm, platinum layer 2.54 μm) as hydrogen dissociating agent Compounds were prepared in a containing stainless steel gas cell (FIG. 4). Each synthesis was carried out according to the method described for Li except for the kiln maintained at 500 ° C., and NaH * Cl synthesis was repeated without addition of hydrogen gas to measure the effect of using NaH (s) as a single hydrogen source. . XPS was performed on NaH * Cl and no NMR irradiation was performed on both products as there were no possible elemental peaks in the region of H- (1/4).

In addition, NaH * Cl, the only source of hydrogen, was synthesized from NaCl (10 g) and KHSO 4 (1.6 g), a solid acid, using a kiln maintained at 580 ° C. When the dissociation agent with H2 or hydride is free of high concentrations of H and the fast reaction to H- (1/4) according to equation 27 is partially inhibited, the reaction of H- (1/3) NMR was performed to see if) could be formed.

Silicon wafer (2 g, 0.5 × 0.5 × 0.05 cm, Silicon Quest International, Silicon (100), boron-doped, heated to 700 ° C. under vacuum) was transferred to Na (1.7 g), NaH (0.5 g), NaCl ( 10 g), and Pt / Ti (15 g) were placed in the reaction and coated with the products NaH * Cl and NaH *, where NaCl was initially heated to 400 ° C. under vacuum to H 2 (1/4). ) Was used. The reaction was carried out in a kiln at 550 ° C. for 19 hours at 760 Torr initial hydrogen pressure conditions. XPS was performed using a silicon wafer (NaH * -coated Si) coated only with sodium hydrino hydride. NaH * Cl-coated silicon wafers (NaH * Cl-coated Si) were analyzed by electron beam excitation spectroscopy. In addition, emission spectra of pressed pellets of NaH * Cl crystals were recorded.

ToF-SIMS Spectrum. Crystal samples of LiH * Br, LiH * I, NaH * Cl, NaH * Br, and corresponding alkali halide controls are scattered on the surface of the double-sided adhesive tape and used a ToF-SIMS device (Physical Electronics, TFS-2000). And analyzed. The primary ion gun used 69Ga + liquid metal raw material. (60 μm) 2 regions of each sample were analyzed. Samples were sputtered for 60 seconds using raster (80 μm × 100 μm) to remove surface impurities and expose clean surfaces. The gap setting was 3, the ion current was 600 pA, and the total ion addition amount was 1015 ions / cm 2.

During capture, the ion gun was operated using a 15 kV beam of bundles (pulsing 4 ns of pulse width into 1 ns) [69-70]. The total ion addition amount was 1012 ions / cm 2. The charge was neutralized and the post acceleration voltage was 8000 V. Positive and negative SIMS spectra were obtained. Representative late sputtering data was recorded.

In addition, 0.1 g Na, 0.5 g NaH, and 15 g Pt / Ti were loaded into a water flow calorimetry cell and water-flow calorimetry was performed under the same conditions as described for Na and R-Ni. It was. The cell produced an excess energy of 15 kJ while the theoretical energy balance resulting from the decomposition of NaH was an endotherm on the order of +1.2 kJ. Therefore, in order to confirm the presence of hydrino hydride corresponding to the reaction given by Equation 23-25 as a source of excess heat, sodium hydride was followed by the same procedure as for the crystalline sample except for sputtering for 100 seconds. Samples of Pt / Ti coated with lino hydride (NaH * -coated Pt / Ti) were analyzed directly. Unreacted Pt / Ti was coated with starting material and used as a control. XPS was also performed.

ToF-SIMS of R-Ni 2400 which had been reacted at 50 ° C. for 48 hours was carried out by the same procedure as for the above crystalline sample. The reaction to form hydrinos is given in Equations 32-35. Since the surface was coated with NaOH, a sodium hydrino hydride composition with NaOH was predicted.

FTIR spectroscopy. FTIR analysis was performed on solid-sample-KBr pellets of LiH * Br (mode: transmittance; test site: Department of Chemistry, Princeton University, New Jersey FTIR spectrometer with DTGS detector with 4 cm-1 resolution (Nicolet, 730) The procedure is as described above [13-14]). Samples were handled under inert gas. The resolution was 0.5 cm −1. Controls include LiNH2, Li2NH, and Li3N, which are commercially available, of which Li2NH has been synthesized by reaction of LiNH2 with LiH or by decomposition of LiNH2 [68] and the Li2NH product is X-ray diffraction Confirmed by analysis (XRD).

XPS Spectrum. A series of XPS analyzes were performed on the crystal samples using an XPD spectrometer (Scienta 300). The transmission mode of the analyzer and the sweep acquisition mode were used. The step energy in the general scan was 0.5 eV and the step energy in the high resolution scan was 0.15 eV. In the general scan, the step time was 0.4 seconds and the number of sweeps was four. In the high resolution scan, the step time was 0.3 seconds and the number of cathode rays was 30. C 1s at 284.5 eV was used as internal standard.

UV spectral analysis of electron beam excited interstitial H2 (1/4). The electron bombardment of the crystals analyzed the lattice of alkali halides (MgCl 2), and the vibration-rotating emission electrons of H 2 (1/4) trapped in the silicon wafer. A windowless UV spectroscopy of electrons emitted from the electron beam excitation of the crystal was performed using a 12.5 keV electron gun at a pressure below Torr and a beam current of 10 to 20 mA. . UV spectra were recorded using a photomultiplier tube (PMT). The wavelength resolution was about 2 nm (FWHM) when the inlet and outlet slit widths were 300 μm. The increase amount was 0.5 nm, and the residence time was 1 second.

III. Results and Discussion

A. RT-plasma emission and Ballmer series α line width.

From atomic hydrogen produced in LiNH2 and titanium filaments that were evaporated by heating, argon-hydrogen (95/5%)-lithium rt-plasma was formed at low field (1 V / cm) low temperature (eg) conditions. Lithium and H-emitting electrons were detected to identify LiNH2 and Li, which is a decomposition product thereof, used as raw materials for atoms Li and H. Argon in the argon-hydrogen mixture increased the amount of atoms H, which is evidenced by the apparent reduction in H release in the absence of argon. H Balmer-based emission electrons corresponding to populations with energy levels> 12 eV were observed as shown in FIGS. 5 and 6, which also required the presence of the Riemann-based emission electrons.

Plasma is not formed with argon / hydrogen alone. It is not possible for a titanium filament, vaporized LiNH 2, and 0.6 Torr argon-hydrogen mixture to undergo chemical reactions that can explain ballmer-based emission electrons at 700 ° C. cell temperature. Indeed, no chemical reaction is known to release enough energy to excite the Ballmer and Lehmann emission electrons from hydrogen. In addition to known chemical reactions, electron collision excitation, resonance photon transfer, and lowering of ionization and excitation energy due to "nonideal" states in strong plasmas also include ionization or excitation energy sources that form hydrogen plasma. Not suitable [21]. The energy resulting from the vigorous reaction of atomic hydrogen satisfied the energy source liberated by Li from the catalyst of atomic hydrogen.

) 및 기기(

)에 따른 반진폭(half-width)으로부터 얻어진 각각의 가우시안 결과값의 총 반진폭(

)은 다음과 같다:The active hydrogen atom energy was calculated using the width of the 656.3 nm Balmer series α-rays emitted from RF rt-plasma. Doppler

) And devices (

The total half amplitude of each Gaussian result obtained from half-width according to

)Is as follows:

(40)

40

 Was ± 0.006 nm in this experiment. The temperature was calculated from the Doppler half amplitude using the following equation:

(41)

(41)

는 선 파장이고, T는 K (1 eV = 11,605 K)에서의 온도이며, μ는 분자량(원자수소=1로 함)이다. 각 경우에서, 평균 도플러 반진폭은 압력에 따라 쉽게 변하지 않았으나, ±10%의 에너지 오차에 대응하여 ±5% 범위에서 변화하였다.here,

Is the line wavelength, T is the temperature at K (1 eV = 11,605 K), and μ is the molecular weight (atomic hydrogen = 1). In each case, the average Doppler half amplitude did not change easily with pressure, but varied in the range of ± 5% in response to an energy error of ± 10%.

For argon-hydrogen (95/5%)-lithium rt-plasma, a Ballmer sequence α linewidth of 656.3 nm was recorded after the initial and 70 h trials, as shown in FIGS. 5A and 5B. The Balmer sequence α-ray following plasma release at both time points contains two separate Gaussian peaks, which are internal narrow peaks corresponding to slow components below 0.5 eV and external very corresponding to fast components above 40 eV. It is a broad peak. The fast component reaches 90% of the initial n = 3 excited state H number and increases to 97% after 70 hours. Only the hydrogen line was widened. As seen earlier, the fast H energy source is not related to the added energy field and can be explained by the mechanism of the hydrogen catalyst in the low energy state. [32-37]

In addition, lithium rt-plasma is formed when pure H2 gas at a pressure of 1 Torr, except that at the initial and 70 hour points, only 27% population is small in line width and number to about 6 eV. As shown in 6A and 6B, respectively. This result was expected because excess H2 and Li can react to form LiH, which promotes the collapse of LiNH2 as follows:

(42)

(42)

Therefore, the reaction to produce the atoms Li and H was attenuated. In addition, argon of the argon-hydrogen mixture can prevent its recombination to increase the amount of atomic hydrogen, and Ar + produced by the plasma can act as a catalyst, as is Li.

In the present invention, it is assumed that Doppler widening due to heat change is the main reason, and other causes are insignificant. This assumption became clear when each causal factor was considered. In general, the experimental design should take into account a combination of two Doppler effects, mechanical, natural (life), Stark, Van der Waals, resonance, and microstructures. The effect of each causal factor depends on the limit of detection [13-21, 38-39].

The rapid formation of H can be explained by the resonance energy transfer from the hydrogen atom to the Li atom, which is three times the potential energy of atomic hydrogen, resulting in a central field four times the proton and radius H * (1/4) which is an intermediate of the same life span as this hydrogen atom is formed. When the radius is reduced to by collisions or space energy transitions, the intermediates spontaneously decrease because they produce fast H (n = 1), as is the case for photon emission previously reported [27–29]. Collision energy transitions, including through-space coupling, are common. For example, the formation of H2 by a chemical exothermic reaction of H + H does not occur with the emission of photons. Rather, it collides with another entity M to remove the binding energy— [44]. The other individual distributes energy from the exothermic reaction, producing H2 and raising the temperature of the system. In the case of the catalytic reaction for the formation of the state given by equations 2a and 2c, the temperature of H becomes very high.

B. Differential Scanning Calorimetry (DSC). DSC of NaH (100-750 ° C.) is shown in FIG. 7. A wide endothermic peak was observed at 350 ° C. to 420 ° C., which corresponds to 47 kJ / mol. Sodium hydride decomposes corresponding to an enthalpy of 57 kJ / mol in the above temperature range [71]. Large exotherms were observed in the range of 640 ° C. to 825 ° C., which corresponds to −177 kJ / mol. DSC of MgH 2 (100-750 ° C.) is as shown in FIG. 8. Two clear endothermic peaks were observed. The first peak was observed at the center at 351.75 ° C., corresponding to 68.61 kJ / mol MgH 2. Decomposition of MgH 2 was observed in the center at 440 ° C. to 560 ° C., corresponding to 744 kJ / mol MgH 2 [71]. In FIG. 8, the second peak was observed at the center at 647.66 ° C., which corresponds to 6.65 kJ / mol MgH 2. The known melting point of Mg (m) is 650 ° C. which corresponds to a melt enthalpy of 8.48 kJ / mol Mg (m) [72]. Therefore, the expected results were observed during the degradation of the control non-catalytic hydride. In contrast, new exothermic phenomena of at least -177 kJ / mol NaH or at least -354 kJ / mol H2 were observed under the conditions of forming NaH catalyst with some H via the catalytic reaction given in Equations 23-25. The enthalpy observed was greater than that of almost all possible exothermic reactions for H, i.

는 에너지 공급량

및 임의의 초과 에너지

의 합과 동일해야 한다:C. Water-Flow Calorimetry Power Measurements. In each test, the energy supply and energy release were calculated by the integration of the corresponding power. In the power supplied, the voltage and current measured at the end of each time interval were multiplied by the time interval (usually 10 seconds) to obtain the amount of energy increase in Joules. All energy gains were summed over the entire experiment after the equilibrium period to get total energy. For the amount of energy released, thermistor difference values were calculated after each test, assuming that the final values of the inlet and outlet temperatures were the same. This difference was calculated to be 0.036 ° C. The heat energy increase with cooling water flow was calculated using Equation 39 at each cycle, which was determined by the flow rate of water at 19 ° C, density of water (0.998 kg / liter), specific heat of water (4.181 kJ / kg- ℃), and corrected temperature difference. , And time intervals. The values were summed over the entire experiment to obtain the total energy release. Total energy of the cell

Is the energy supply

And any excess energy

Must equal the sum of:

(43)

(43)

From the energy balance equation, excess calorific value was derived.

The calibration test results are as shown in FIGS. 9 and 10. 10, it can be seen that there is a time when the inclination of the coolant power changes almost discontinuously. This point in time, approximately one hour, corresponds to the addition of helium, which enhances the heat transfer from the cell to the chamber wall. The numerical integration of the input and output power curves yields an output energy of 292.2 kJ and an input energy of 303.1 kJ, corresponding to a combination of flow rates of 96.4% of the resistance input to the exhaust coolant.

Cell temperature and time-dependent cooling water power for the hydrino reaction with a cell containing a sample containing 1 g of Li, 1 g of LiNH2, 10 g of LiBr, and 15 g of Pd / Al2O3, respectively, are shown in FIGS. As shown in 12. The numerical integration of the input and output power curves with the correction applied yields an output energy of 227.2 kJ and an input energy of 208.1 kJ. Therefore, from equation 43, the amount of excess energy was calculated to be 19.1 KJ. 12, it can be seen that there is a point where the gradient of temperature changes almost discontinuously. The change in slope occurs after 1 hour, which corresponds to the rapidly increasing cell temperature with the onset of the reaction. Based on the system response to the power pulses, an excess amount of energy of 19.1 kJ occurred within 2 minutes as the power to the reaction was higher than 160 W.

Quantitative XRD analysis of the composition resulting from the reaction showed that LiBr and Pd / Al 2 O 3 did not change. Therefore, assuming 100% yield, the maximum value of theoretical energy released from known compounds is 4.3 kJ, which is calculated according to equation 22 from the formation of lithium nitride and hydride, whereas the resulting energy balance The value reached 4.4 times the maximum value. Only exothermic reactions that can explain the energy balance are given in equations 17-19. The hydrogen content in 0.5 g of LiNH2 was 22 mmol H2. Therefore, the resulting energy balance is -870 kJ / mol H2, which is more than 3.5 times the enthalpy of combustion enthalpy of -241.8 kJ / mol H2, the most active hydrogen reaction, assuming a list of the best possible H2.

In the R-Ni power test using a cell containing a sample containing 15 g of R-Ni / Al alloy powder and 3.27 g of Na as starting materials for R-Ni, , As shown in FIGS. 13 and 14, respectively. The curves for temperature and coolant power time are very similar to the correction values. The numerical integration of the input and output power curves with the correction values yielded an output power value of 384 kJ and an input power value of 385 kJ. Energy balance was obtained.

In the hydrino reaction using a cell containing a sample containing 15 g of NaOH-doped R-Ni, which is a catalyst material, and 3.28 g of Na, the cell temperature with time and the coolant power with time are shown in FIGS. 15 and 16, respectively. As shown. The numerical integration of the input and output power curves with the corrections yielded an output energy of 185.1 kJ and an input energy of 149.1 kJ. Therefore, from equation 43, the excess energy amount was calculated to be 36 kJ. Referring to the schematic of FIG. 15, it can be seen that there is a point where the gradient of temperature changes almost discontinuously. This change in slope occurs from 1 hour before, which corresponds to the rapidly increasing cell temperature with the onset of the reaction. Based on the system response to the power pulses, an excess amount of energy of 36 kJ occurred within 1.5 minutes as the power to the reaction was higher than 0.5 kW.

[75] 및

[65])이다. Quantitative XRD analysis of the composition consisting of NaOH-doped R-Ni reactants and products by reaction with alkali metals showed that Ni with trace amounts of Bayrite and Ni with trace amounts of alkali hydroxides. Were analyzed respectively. The formation of sodium-Ni alloys or the reaction of R-Ni with Al2O3 and sodium [73-74] have obvious endothermic reactions (each

[75] and

[65]).

[65, 76])은, 초기의 미량의 배이어라이트 및 Na와의 반응으로부터 생성되는 NaOH를 보여주는 XRD 분석에 기초하여, 에너지 균형값에 거의 영향을 미치지 않음을 알 수 있다. 문헌 [74]에 나타난 바와 같이, 배이어라이트 분해물 내의 H2O 함량은 47.7 μmole H2O/g R-Ni이며, 이는 Al(OH)3의 분해 (

)에 기인한 NaOH의 형성 (

[65])에 의해 거의 영향을 미치지 않는 것이다. 전체 반응은 배이어라이트와 나트륨이 반응하여 NaOH를 형성하는 것이다 (

).When using the heat of formation, the formation of NaOH through the reaction of Bayrite with sodium (

[65, 76]) show little effect on the energy balance value based on XRD analysis showing NaOH resulting from the reaction with the initial trace amount of valite and Na. As shown in [74], the H2O content in the baitrite lysate is 47.7 μmole H2O / g R-Ni, which results in the decomposition of Al (OH) 3 (

Formation of NaOH due to

[65]) has little effect. The overall reaction is the reaction of the salts with sodium to form NaOH (

).

An exothermic reaction that can explain the energy balance is given in Equations 23-25. The hydrogen content of R-Ni derived using the quantitative GC analysis and using the ideal gas laws of measured P, V, and T states was 150 μmole H2 / g R-Ni. Therefore, the resulting energy balance is -1.6 x 104 kJ / mol H2, which is more than 66 times the enthalpy of combustion enthalpy of -241.8 kJ / mol H2, the most active reaction of hydrogen, assuming the list of the best possible H2. The theoretical conservation energy value calculated for the reaction of equation 44 is 259 eV / H2 or 25 mJ / mol H2 [7].

(44)

(44)

The most active of the oxidation reactions involving solid fuels is, which has a heat of combustion of 24 kJ / g and little fuel / oxidant systems producing more than 10 kJ / g are known [65]. In comparison, even if not completed, H contained in the renewable catalyst NaH produced 300 times more energy per unit weight of the well-known solid fuel.

By increasing NaOH doping and converting to R-Ni 2400, the catalytic material produced high power and energy without the need to add Na. The cell temperature over time and the coolant power over time for the hydrino reaction with a cell containing 15 g of NaOH-doped R-Ni 2400 as the catalyst material are shown in FIGS. 17 and 18, respectively. The numerical integration of the input and output power curves with the correction values yielded an output energy of 195.7 kJ and an input energy of 184.0 kJ, which corresponds to an excess energy of 11.7 kJ, with power exceeding 0.25 kW.

Quantitative XRD analysis of the product after reaction with the composition of the reactant NaOH-doped R-Ni revealed R-Ni and R-Ni with 3.7 wt% Baerite, respectively. The H2O content measured from the initial R-Ni's Baylite decomposition was 32.8 μmole, which resulted in a 34.0 μmoles H2O // H2O content measured from the Baylite decomposition of 3 wt% Al (OH) 3-doped Ni / Al alloy This is the value to compare with g. Most possible exothermic reactions were from Al (OH) 3 to Al 2 O 3. The balanced equation is given by [65, 75, 77]:

(45)

(45)

이다. 이는 3 wt% Al(OH)3-도핑된 Ni/Al 알로이 15g의 열측정에 의해 확인되었는데, 상기 열측정에서 평균 에너지는

로 나타났으며, 이는 이론적인 에너지값인

과 비교되는 값이다 (식 45 에서

일 때

[75]). 그러므로, NaOH-도핑된 R-Ni로부터 관찰된 에너지는 이론값의 4.4배였으며 이는 식 23 내지 25에서 주어진 촉매 반응에 더 많은 영향을 줄 수 있었다.At 3.7 wt% Al2O3, the maximum value of theoretical energy in the reaction given by equation 45 is

to be. This was confirmed by thermometry of 15 g of 3 wt% Al (OH) 3 -doped Ni / Al alloy, in which the average energy was

, Which is the theoretical energy value

Is the value to be compared to

when

[75]). Therefore, the energy observed from NaOH-doped R-Ni was 4.4 times the theoretical value, which could have more influence on the catalytic reaction given in Equations 23-25.

D. ToF-SIMS Spectrum. Positive ToF-SIMS spectra obtained from LiBr and LiH * Br crystals are shown in FIGS. 19 and 20, respectively. In the positive ion spectra of LiH * Br crystals and LiBr controls, Li + ions were mainly observed. Other Li 2+, Na +, Ga +, and Li (LiBr) + were also observed.

Anion ToF-SIMS of LiBr and LiH * Br crystals is shown in FIGS. 21 and 22. In the LiH * Br spectra, H- and Br- peaks were mainly observed and the intensities were H-> Br-. Only bromine ions were observed in the anion ToF-SIMS of the LiBr control group. In both cases, O-, OH-, Cl-, and LiBr- were also observed. In addition to the increased hydride, other characteristic peaks of the LiH * Br samples were observed LiHBr- and Li2H2Br- which satisfied the formation of new lithium borohydride.

Positive ToF-SIMS spectra obtained from LiI and LiH * I crystals are shown in FIGS. 23 and 24, respectively. Li + ions were mainly observed in the positive ion spectra of LiH * I crystal and LiI control. Li +, Na +, Ga +, and a series of zwitterions Li [LiI] n + were also observed. Characteristic peaks of LiH * I samples were LiHI +, Li2H2I +, Li4H2I +, and Li6H2I +.

Anion ToF-SIMS of LiI and LiH * I crystals are shown in FIGS. 25 and 26, respectively. H- and I- peaks were mainly observed in the LiH * I spectrum, and the intensity was H-> I-. Iodine ions were mainly observed in the anion ToF-SIMS for the LiI control. In both cases, O-, OH-, Cl-, and a series of anion I [LiI] n- were observed together. In addition to the increased hydride, LiHI-, Li2H2I-, and NaHI- were observed to satisfy the formation of novel lithium iodohydrides as characteristic peaks of LiH * I samples.

)을 도 27에 나타내었다. 일련의 하이드리노-하이드라이드-화합물인 NaHx-도 관찰되었는데, 이 때 고성능 (10,000) 질량 결정법으로부터 얻은 질량 손실량을 통해 대조군에서 관찰된 일련의 C2Hx-에 대한 이의 작용을 명확히 알 수 있었다. XPS 스펙트럼에 따르면 NaH*-코팅된 Pt/Ti는 두 개의 수소 상태, 즉 H-(1/3) 및 H-(1/4)을 포함하고 있다 (Sec. IIIF).Negative ToF-SIMS spectrum for NaH * -coated Pt / Ti following generation of excess heat of 15 kJ (

) Is shown in FIG. 27. A series of hydrino-hydride-compounds, NaHx-, were also observed, with mass loss obtained from high performance (10,000) mass determinations clearly revealing its action on the series of C2Hx- observed in the control group. According to the XPS spectrum, NaH * -coated Pt / Ti contains two hydrogen states, H- (1/3) and H- (1/4) (Sec. IIIF).

In the spectrum of R-Ni obtained by performing Na / R-Ni water-flow calorimetric, NaHx- with a series of mass defects was observed to produce excess heat of 36 kJ. Positive ToF-SIMS spectra obtained from R-Ni reacted at 50 ° C. for 48 hours are shown in FIG. 28. The main ion on the surface was Na + along with NaOH doped on the surface. Ions of other major elements of R—Ni 2400 such as Al +, Ni +, Cr +, and Fe + were also observed.

과의 결합이온에 해당한다. 그 외 관찰되는 다른 특징적인 피크는 NaOH, NaO, OH- 및 O-과 결합된 소듐 하이드리노 하이드라이드 NaHx-에 해당한다.29 shows the anion ToF-SIMS results of R-Ni reacted at 50 ° C. for 48 hours. In the spectrum, OH- and O-, which are free hydroxyl groups, were also observed with very large H- peaks. The two other major peaks correspond to the high resolution masses of NaH 3-and NaH 3 NaOH- corresponding to 10,000, which is sodium hydrino hydride and its

Corresponds to the combined ion with. Other characteristic peaks observed correspond to sodium hydrino hydride NaHx- in combination with NaOH, NaO, OH- and O-.

E. H- (1/3), H- (1/4), H2 (1/3) and H2 (NMR identification of 1/4. 1H of LiH * Br and LiH * I using relative values with external TMS MAS NMR spectra are shown in Figures 30A and 30B, respectively.LiH * X samples showed very large upfield resonances corresponding to X = Br and X = I at -2.51 ppm and -2.09 ppm, respectively. No high field-shift peaks were seen in any of the controls comprising equal molar ratios of LiH and LiBr or LiI, LiNH2, Li2NH, and equal molar ratios of LiNH2 or Li2NH and LiBr or LiI. Since the high field peak of LiH * X is very wide, these results may be compared with the above-mentioned identification results of H- (1/4) of KH * Cl and KH * I.

TMS and relative 1H MAS NMR spectra (FIG. 31A) for KH * Cl samples obtained from individual synthesis and controls were described above [13-15, 24-26]. The experimental absolute resonant shift value of TMS is -31.5 ppm compared to both rotor magnetic frequencies [78-79]. The experimental shift of KH with reference to TMS is +1.1 ppm, which corresponds to an absolute resonance shift of -30.4 ppm, and the expected shift of H- (1/1) calculated by Equation 4 when p = 0. Fits very well with -30 ppm phosphorus. The shift value of the new peak for TMS is -4.46 ppm, which corresponds to an absolute resonance shift value of -35.96 ppm, telling p = 4 in equation (4). H- (1/4) is a hydride ion predicted using K as catalyst [1, 15, 30]. In addition, very narrow peak widths refer to small hydride ions that are free rotors. In contrast, for KH * I (FIG. 31B), a very wide peak appears at -2.31 ppm. The hydride ion H- (1/4), the expected product of the reaction with the K catalyst forming KH * I, was observed by XPS at its expected binding energy of 11.2 eV [13-15, 26, 30]. Therefore, the diamagnetic shift by large halide ions is +2.15 ppm. The corrected high field NMR peaks for LiH * X are about −4.46 ppm each, which is consistent with the expected shift of free ions given by equation (4).

Elemental analysis of LiH * Br in weight percent yields Li (8%), H (1.1%), and I (90.9%), which correlates to the detectable stoichiometric ratio of LiHBr in stainless steel and R-Ni components. The corresponding value. Elemental analysis of LiH * I in weight percent yielded Li (5.2%), H (0.8%) and I (94%), which were related to the detectable stoichiometric ratio of LiHI in stainless steel and R-Ni components. The corresponding value. Therefore, hydrides other than hydrides of Li cannot be applied. U H does not have a [13-14] high-shift NMR peak as before. The F center cannot be the cause because there is no detectable ESR signal in LiH * Br or LiH * I at room temperature or at a temperature of 77 K. 1 H MAS NMR spectra obtained from LiNH2, Li2NH, and compounds thereof in LiBr or LiI substrates, did not show any of these compounds with high-shifted NMR peaks. To further remove LiNH2 and Li2NH, which are responsible for the -2.5 ppm peak, LiH * Br samples with a -2.5 ppm peak were heated to 600 ° C under dynamic vacuum to decompose LiNH2 and Li2NH. The heat-treated samples were analyzed by FTIR spectroscopy, which confirmed that the amides and imides were removed, corresponding to 3314, 3259, 2079 (wide peak), 1567, and 1541 cm-1 and imide peaks corresponding to amide peaks. The peaks were found at 3172 (wide peak), 1953, and 1578 cm −1, and the -2.5 ppm peak was reanalyzed by NMR. The FTIR spectrum shown in FIG. 45B showed that these species were removed and the corresponding NMR spectrum showed a -2.5 ppm peak. Past and present NMR and FTIR analyzes showed that the -2.5 ppm peak in the 1H NMR spectrum was not associated with UH, LiNH2, Li2NH, or other known species, and the -2.5 ppm peak in the 1H NMR spectrum was consistent with theoretical expectations. Corresponds to-(1/4) ions, confirming direct evidence of hydride ions in the low-energy state.

In addition to the -2.5 ppm and -2.09 ppm peaks corresponding to H- (1/4), 1.3 ppm peaks were observed in the 1H MAS NMR spectra of LiH * Br and LiH * I, which are shown in FIGS. 30A and 30B, respectively. None of the controls showed this peak to remove all starting compounds or possible known products. However, this peak may be due to H2 (1/4) molecules corresponding to H- (1/4).

H2 was analyzed via gaseous 1H NMR. The experimental absolute resonant shift value of gaseous TMS compared to both rotor magnetic frequencies is -28.5 ppm [80]. H2 was observed at 0.48 ppm compared to gaseous TMS set at 0.00 ppm [81]. Therefore, the corresponding absolute H2 gas phase resonance shift value of -28.0 ppm (-28.5 + 0.48) ppm was exactly in agreement with the expected absolute gas phase shift value of -28.01 ppm given in (12).

The absolute H 2 gas phase shift value can be used to determine the substrate shift value for H 2 in the lithium-compound substrate. The correction for substrate shift can then be compared to Equation 12 by adding a 1.3 ppm peak and determining the gas phase absolute shift. The shift values of all peaks were compared to the liquid phase TMS, which had -31.5 ppm, the experimental absolute resonance shift value for both rotor magnetic frequencies. The experimental shift of H2 in the lithium compound substrate at 4.06 ppm relative to liquid TMS is shown in FIG. 7 (Lu et al.), Which corresponds to the absolute resonance shift of -27.44 ppm (-31.5 ppm + 4.06 ppm). . Using an absolute H2 gas phase resonance shift of -28.0 ppm corresponding to 3.5 ppm (-28.0 ppm-31.5 ppm) for liquid TMS, the lithium-compound substrate effect is +0.56 ppm (4.06 ppm-3.5 ppm), which is It needs to be calibrated to -0.56 ppm, the measured shift. The high field peak of H2 at the 1.26 ppm peak for TMS then corresponds to a substrate-corrected absolute resonance shift of -30.8 ppm (-31.5 ppm + 1.26 ppm-0.56 ppm). When assigning data to Eq. 12, p = 4 and matches H2 (1/4):

(46)

(46)

에 대한 상대적인 강도가 증가된 것이다. 도 6 및 7에서 알려지지 않은 피크에 대해서는 확인할 수 없었다. H2(1/4)의 이론적인 이동값과 정확히 일치하는 피크에 대한 확인은, FTIR (Sec. IIIG)과 전자 빔-여기 방출 분광법 (Sec. IIIH)에 의해 실시하였다.Lu et al. [82] observed a peak at this location, as LiH + LiNH2 (1.1 / 1) was heated.

The relative strength to is increased. Unknown peaks were not found in FIGS. 6 and 7. Identification of peaks that exactly match the theoretical shift of H 2 (1/4) was performed by FTIR (Sec. IIIG) and electron beam-excited emission spectroscopy (Sec. IIIH).

The presence of H- (1/4) ions in LiH * X was determined by the polarization of the halide ions. 1 H MAS NMR spectra of LiH * F and LiH * Cl are as shown in FIGS. 32A and 32B. The peaks of 4.3 ppm and 1.2 ppm were consistent with the theoretical estimates of molecular hydrogen in two different quantum states [1, 6]. 4.3 ppm was consistent with Lu et al. [82] 's expectations for H2, and 1.2 ppm was consistent with H2 (1/4) not disclosed in Lu et al. [82]. The presence of H2 (1/4) can be seen by observing the rotational transition estimates in the FTIR spectrum (Sec. IIIG) and the rotational distance estimates by electron beam-excited emission spectroscopy (Sec. IIIH). H- (1/4) ion peaks were not found in LiH * F containing unpolarized fluorine and LiH * Cl containing unpolarized chlorine, while they were the major peaks in both LiH * Br and LiH * I. 30A and 30B, respectively. These results indicate that the polarized halides form the corresponding lithium halidehydride by reaction of LiX and H- (1/4) ions. Because molecular species are unspecifically trapped in the crystal lattice, the H-content selectivity of LiH * X for molecular species alone or in combination with H- (1/4) ions is determined by the degree of polarization of the halide and the corresponding H- (1 / 4) responsiveness. Potassium catalysts form H 2 (1/4) very well, but not in KCl and KI substrates with H- (1/4), as shown in FIGS. 31A and 31B.

1H MAS NMR spectra of NaH * Br with reference to external TMS are shown in FIG. 32. NaH * Br showed large and clear high field resonance at -3.58 ppm. None of the controls containing NaH or the same molar ratio mixture of NaH and NaBr showed high intestinal peaks. The high field peak of NaH * Br, -3.58 ppm, is wider but less obvious than in the case of KH * I, so the substrate may not have the same effect as the previous case of identifying H- (1/4) in KH * I. Can be. Therefore, the measured shift value is directly compared with the expected theory that the peak shifts low field due to the substrate effect. The experimental absolute resonance shift of TMS is -31.5 ppm with respect to the quantum rotor magnetic frequency [78-79]. The new peak at -3.58 ppm for TMS corresponds to the absolute resonance shift value of -35.08 ppm, which tells p = 4 in Equation 4. H- (1/4) is the preferred hydride ion expected when using the catalyst NaH (Equations 3-4 and 23-27). Similar to the case of LiH * X, the 4.3 ppm peak shown in FIG. 33 corresponds to H2 and the 1.13 ppm peak corresponds to H2 (1/4). The latter is generally observed as the preferred catalyst molecular product [29].

NaH * Cl 1H MAS NMR spectra referring to external TMS, showing the effect of hydrogenation on the relative strengths of H2, H2 (1/4), and H- (1/4), are shown in FIGS. 34A-34B. The addition of hydrogen increases the H- (1/4) peak and decreases H2 (1/4) as H2 increases. (A) NaH * Cl synthesized by hydrogenation is -4 ppm high field shift peak corresponding to H- (1/4), 1.1 ppm peak corresponding to H2 (1/4), and corresponding to H2 The main peak of 4 ppm is shown. (B) NaH * Cl synthesized without hydrogenation has a high field peak of -4 ppm corresponding to H- (1/4), a main peak of 1.0 ppm corresponding to H2 (1/4), and corresponding to H2 Show a small peak of 4.1 ppm.

The effect of hydrogenation on the relative 1 H MAS NMR of H 2, H 2 (1/4), and H- (1/4) in NaH * Cl is as shown in FIGS. 34A and 34B. The conversion of the main peak from H2 to H2 (1/4) by the addition of external hydrogen shows that H2 can occupy the space in the lattice filled by H2 (1/4) when H2 is not abundant. However, the addition of hydrogen increases the relative intensity of the H- (1/4) peak, which may be due to the increased hydrino reactant concentration.

Since there is no high concentration of H obtained by dissociating H2 or hydride, H- (1 / formed by the reaction of Equations 23 to 25 when the fast reaction of H- (1/4) according to Equation 27 is partially suppressed. NMR was performed on NaH * Cl synthesized from KHSO4 solid acid, the only source of NaCl and hydrogen, to see if 3) could be observed. NaH * Cl formed using a solid acid was subjected to 1H MAS NMR spectra referring to external TMS and is shown in FIG. 35. The peaks at -3.97 ppm and 1.15 ppm matched the peaks at -4 ppm and 1.1 ppm in Figures 34A and 34B, which correspond to H- (1/4) and H2 (1/4), respectively, which are H2 And NaH * Cl synthesized using H obtained by dissociating hydride. Since the content of KHSO4 in the mixture with NaCl is only 6.5 mol%, precise analysis was performed to ensure that the substrate effect was always constant between samples. Specifically, peaks at -3.15 ppm and 1.7 ppm were observed in the solid acid product. The previous substrate shift values for NaH * Cl were used in Equations 4 and 12, and these peaks corresponded to H- (1/3) and H2 (1/3), respectively. The curve fit of the two peaks yielded peaks of about -3 ppm and -4 ppm, which are theoretical values taking into account experimental errors. Therefore, both partial hydrogen states were present and the H2 peak did not appear at 4.3 ppm, due to the synthesis of NaH * Cl with the solid acid, the only source of H, which was the reaction given by Equations 23-30. To confirm. The presence of H 2 (1/4) and H- (1/4) in NaH * Cl obtained from the reaction of NaCl with solid acid KHSO 4 was confirmed by XPS and electron beam-excited emission spectroscopy.

로의 전이 반응을 유발할 수 있는 다른 촉매이며, 이는 이차 이의 이온화에너지가 54.4 eV, (

)이기 때문이다. 촉매 반응은 다음과 같다:Helium silver

It is another catalyst that can induce a transition reaction to a secondary ion, which has a secondary ionization energy of 54.4 eV, (

) The catalytic reaction is as follows:

(47)

(47)

(48)

(48)

And the overall reaction is:

(49)

(49)

의

로의 순차적인 빠른 전이는, 식 27에서 주어진 바와 같이

에서 일차적으로 27.2 eV을 받아들이는 원자 수소에 의한 추가적인 촉매 반응을 통해 일어날 수 있다. 46.5 nm에서 시작되고 짧은 파장으로 이어지는 특징적으로 넓은 방출선은 활발한 H 촉매 분해로 인한 전이 반응 때문인 것으로 예상할 수 있다. 2% 수소를 갖는 헬륨의 마이크로파 방출을 기록하는 EUV 분광법을 이용하여 방출선을 관찰하였다[27-29]. 분광분석 및 NMR 데이터를 통해

의 형성과

으로의 순차 전이의 촉매 메카니즘을 확신할 수 있다. 추가적인 증거로서는 Sec. IIIF에서 주어진 바와 같이 NaH*Cl 내에서 H-(1/3) 및 H-(1/4) 모두가 관찰되는 것이다. As can be seen in the case of NaH catalysis, the He + catalyst product

of

Sequential fast transition to

This can occur through an additional catalytic reaction with atomic hydrogen which initially accepts 27.2 eV. Characteristically wide emission lines starting at 46.5 nm and leading to short wavelengths can be expected to be due to transition reactions due to active H catalysis. The emission line was observed using EUV spectroscopy, which records the microwave emission of helium with 2% hydrogen [27-29]. Through spectroscopic and NMR data

With the formation of

The catalytic mechanism of sequential transition to can be assured. Further evidence is provided by Sec. Both H- (1/3) and H- (1/4) are observed in NaH * Cl as given in IIIF.

영역에 걸쳐 각각의 LiBr 및 LiH*Br에 대한 스펙트럼 분석이 실시되었다 (도 36A 내지 36B). LiH*Br 결정과 LiBr 대조군 내에 존재하는 모든 원소를 결정하기 위해 주 원소 피크를 조사하였다. 스캔 결과, 다음 피크를 제외하고는 낮은 결합 에너지 영역 (도 37) 내에서 피크를 확인할 수 있는 원소는 존재하지 않았다: Li 1s (55 eV, LiBr과 비교하여 1 eV 낮게 이동), O 2s (23 eV), Br 3d5/2 및 Br 3d3/2 (각각 69 eV 및 70 eV), Br 4s (15 eV), 및 Br 4d (5 eV). 따라서, 이 영역에서 나타나는 다른 피크는 새로운 종일 수 밖에 없다. 도 37에 나타난 바와 같이, LiH*Br의 XPS 스펙트럼은 LiBr과 비교할 때 9.5 eV 및 12.3 eV에서 추가적인 피크를 가지는 점에서 차이가 있으나, 이는 다른 어떠한 주 원소 피크와도 관련된 것도 아니며

하이드라이드 이온과 일치하는 것이다 (식 4 및 16). 이들 피크를 알아보기 위하여 원자가-밴드 영역에서 피크를 가지는 원소에 대하여 문헌을 검색하였다. 현재 알려진 주원소 피크로서는 이를 확인할 수가 없었다. 그러므로, 알려진 원소에는 해당하지 않으며 다른 어떠한 주원소 피크에도 대응하지 않는 9.5 eV 및 12.3 eV 피크는, 두 개의 다른 화학적 환경에 존재하는 H-(1/4)임을 알 수 있었다. 이러한 사실은 KH*I의 H-(1/4)에 대하여 이전에 보고된 바와 매우 유사하다 [13-15, 26, 30].F. XPS Identification of H- (1/4) and H- (1/3).

Spectral analysis was performed for each LiBr and LiH * Br over the region (FIGS. 36A-36B). Main element peaks were examined to determine all elements present in the LiH * Br crystals and the LiBr control. As a result of the scan, no element was found in the low binding energy region (FIG. 37) except for the following peak: Li 1s (55 eV, shifted 1 eV lower compared to LiBr), O 2s (23 eV), Br 3d5 / 2 and Br 3d3 / 2 (69 eV and 70 eV, respectively), Br 4s (15 eV), and Br 4d (5 eV). Thus, other peaks appearing in this region are inevitably new species. As shown in FIG. 37, the XPS spectrum of LiH * Br differs in that it has additional peaks at 9.5 eV and 12.3 eV when compared to LiBr, but it is not related to any other main element peak.

Coincides with hydride ions (Equations 4 and 16). In order to identify these peaks, the literature was searched for elements having peaks in the valence-band region. This could not be confirmed with the present known major element peak. Therefore, it was found that the 9.5 eV and 12.3 eV peaks, which do not correspond to known elements and do not correspond to any other main element peak, are H- (1/4) present in two different chemical environments. This fact is very similar to previously reported for H- (1/4) of KH * I [13-15, 26, 30].

영역에 걸쳐 각각의 NaBr 및 NaH*Br에 대해 스펙트럼을 얻었다 (도 38A 내지 38B). NaH*Br 결정 및 NaBr 대조군 내에 존재하는 모든 원소를 결정하기 위해 주 원소 피크를 조사하였다. 그 결과, 다음 피크를 제외하고는 낮은 결합 에너지 영역에서 확인할 수 있는 원소가 없었다: Na 2p 및 Na 2s (30 eV 및 63 eV, NaBr과 비교하여 1 eV 낮게 이동), O 2s (23 eV), Br 3d5/2 및 Br 3d3/2 (각각 69 eV 및 70 eV), Br 4s (15.2 eV), 및 Br 4d (5 eV). 따라서, 이 영역에서 나타나는 다른 피크는 새로운 종일 수 밖에 없다. 도 39에 나타난 바와 같이, NaH*Br의 XPS 스펙트럼은 NaBr과 비교할 때 9.5 eV 및 12.3 eV에서 추가적인 피크를 가지는 점에서 차이가 있으나, 이는 다른 어떠한 주 원소 피크와도 관련된 것도 아니며

하이드라이드 이온과 일치하는 것이다 (식 4 및 16). 이들 피크를 알아보기 위하여 원자가-밴드 영역에서 피크를 가지는 원소에 대하여 문헌을 검색하였다. 현재 알려진 주원소 피크로서는 이를 확인할 수가 없었다. 그러므로, 알려진 원소에는 해당하지 않으며 다른 어떠한 주원소 피크에도 대응하지 않는 9.5 eV 및 12.3 eV 피크는, 두 개의 다른 화학적 환경에 존재하는 H-(1/4)임을 알 수 있었다.

Spectra were obtained for each NaBr and NaH * Br over the region (FIGS. 38A-38B). Main element peaks were examined to determine all elements present in the NaH * Br crystals and the NaBr control. As a result, no elements were found in the low binding energy region except for the following peaks: Na 2p and Na 2s (30 eV and 63 eV, 1 eV lower compared to NaBr), O 2s (23 eV), Br 3d5 / 2 and Br 3d3 / 2 (69 eV and 70 eV, respectively), Br 4s (15.2 eV), and Br 4d (5 eV). Thus, other peaks appearing in this region are inevitably new species. As shown in FIG. 39, the XPS spectrum of NaH * Br differs in that it has additional peaks at 9.5 eV and 12.3 eV when compared to NaBr, but it is not related to any other main element peak.

Coincides with hydride ions (Equations 4 and 16). In order to identify these peaks, the literature was searched for elements having peaks in the valence-band region. This could not be confirmed with the present known major element peak. Therefore, it was found that the 9.5 eV and 12.3 eV peaks, which do not correspond to known elements and do not correspond to any other main element peak, are H- (1/4) present in two different chemical environments.

NaBr 영역에 걸쳐 15 kJ의 초과 열의 생성에 따르는 각각의 Pt/Ti 및 NaH*-코팅된 Pt/Ti에 대해 스펙트럼을 얻었다 (도 40A 내지 40B). NaH*-코팅된 Pt/Ti 및 Pt/Ti 대조군 내에 존재하는 모든 원소를 결정하기 위해 주 원소 피크를 조사하였다. 그 결과, 다음 피크를 제외하고는 낮은 결합 에너지 영역 (도 41A 내지 41B) 내에서 확인할 수 있는 원소가 없었다: Pt 4f7/2 및 Pt 4f5/2 (각각 70.7 eV 및 74 eV), 및 O 2s (23 eV). NaH*-코팅된 Pt/Ti에 대해 Na 2p 및 Na 2s 피크가 31 eV 및 64 eV에서 관찰되었으며, 원자가 밴드는 단지 Pt/Ti에 대해서만 관찰되었다. 따라서, 이 영역에서 나타나는 다른 피크는 새로운 종일 수 밖에 없다. 도 42A 내지 42B에 나타난 바와 같이, NaH*-코팅된 Pt/Ti의 XPS 스펙트럼은 Pt/Ti과 비교할 때 6 eV, 10.8 eV, 및 12.8 eV 에서 추가적인 피크를 가지는 점에서 차이가 있으나, 이는 다른 어떠한 주 원소 피크와도 관련된 것도 아니며

및

하이드라이드 이온과 일치하는 것이다 (식 4 및 16). 이들 피크를 알아보기 위하여 원자가-밴드 영역에서 피크를 가지는 원소에 대하여 문헌을 검색하였다. 현재 알려진 주원소 피크로서는 이를 확인할 수가 없었다. 그러므로, 알려진 원소에는 해당하지 않으며 다른 어떠한 주원소 피크에도 대응하지 않는 10.8 eV 및 12.8 eV 피크는, 두 개의 다른 화학적 환경에 존재하는 H-(1/4)임을 알 수 있었다. 6 eV 피크는 H-(1/3)에 해당하였다. 그러므로, 이 영역에서 할라이드 피크의 부재하에서, 부분적인 수소 상태 (1/3 및 1/4)는 식 27에서 예상된 바와 같이 관찰되었다. 높은 결합 에너지에 기인한 원자가 밴드의 부재는 NaH*-코팅된 Pt/Ti의 하이드리노 하이드라이드의 선별을 또한 만족하였다.

Spectra were obtained for each Pt / Ti and NaH * -coated Pt / Ti following generation of excess heat of 15 kJ over the NaBr region (FIGS. 40A-40B). Principal element peaks were examined to determine all elements present in the NaH * -coated Pt / Ti and Pt / Ti controls. As a result, no elements were found within the low binding energy region (FIGS. 41A-41B) except for the following peaks: Pt 4f7 / 2 and Pt 4f5 / 2 (70.7 eV and 74 eV, respectively), and O 2s ( 23 eV). Na 2p and Na 2s peaks were observed at 31 eV and 64 eV for NaH * -coated Pt / Ti, and valence bands were only observed for Pt / Ti. Thus, other peaks appearing in this region are inevitably new species. As shown in Figures 42A-B, the XPS spectra of NaH * -coated Pt / Ti differ in that they have additional peaks at 6 eV, 10.8 eV, and 12.8 eV when compared to Pt / Ti, but this Nor is it related to the main element peak

And

Coincides with hydride ions (Equations 4 and 16). In order to identify these peaks, the literature was searched for elements having peaks in the valence-band region. This could not be confirmed with the present known major element peak. Therefore, it was found that the 10.8 eV and 12.8 eV peaks, which do not correspond to known elements and do not correspond to any other main element peak, are H- (1/4) present in two different chemical environments. The 6 eV peak corresponded to H- (1/3). Therefore, in the absence of halide peaks in this region, partial hydrogen states (1/3 and 1/4) were observed as expected in equation 27. The absence of valence bands due to high binding energy also satisfied the selection of hydrino hydrides of NaH * -coated Pt / Ti.

The results of NaH * -coated Pt / Ti are shown in FIG. 42B, which is the same as that of NaH * -coated Si. As shown in Figures 43 and 44, the XPS spectra of NaH * -coated Si showed peaks at 6 eV, 10.8 eV, and 12.8 eV, which do not correspond to known elements and do not correspond to any other main element peaks. But is identical to H- (1/3) and H- (1/4). Therefore, the partial hydrogen states 1/3 (H- (1/3) at 6 eV) and 1/4 (H- (1/4) at 10.8 eV and 12.8 eV) are expected as shown in equation 27. exist.

G. FTIR identification of H2 (1/4). High performance FTIR spectroscopy on samples with high-shifted 1H NMR peaks at -2.5 ppm corresponding to H- (1/4) and NMR peaks at 1.3 ppm corresponding to corresponding H2 (1/4) molecules Was carried out. As shown in FIG. 45B, a single narrow peak was observed at 1989 cm −1. Considering the starting materials and expected reactions, compounds of LiNH 2, Li 2 NH, and Li 3 N are possible, but none of these compounds show peaks in the region of 1989 cm −1. No other peak was observed other than the peaks that were easily assumed to be LiBr (FIG. 45A). All species that could be found in this region, such as heterogeneous materials such as azide, metal carbonyl, and metaborate ions, have been thoroughly investigated. Azide and metal carbonyl were excluded because the bands on the spectrum must be very wide. Metaborate ions could be excluded by ToF-SIMS analysis. ToF-SIMS analysis revealed a total boron content that was not detected at the ppb level, which is below the FTIR detection limit. NA) and 2B corresponding to 11B (80% NA).

Considering possible substrate effects, the peak at 1989 cm −1 (0.24 eV) was consistent with 1947 cm −1, which is the theoretical estimate for H 2 (1/4). As can be seen from Equations 14 to 15, a very large rotational energy of four times the normal hydrogen means the internuclear distance of H 2 (1/4) corresponding to one quarter of H 2. Intrusive H2 in silicon and GaAs is close to a free rotor showing a single rotational vibration transition [83–87]. H2 is not only FTIR activity but also Raman activity, which is due to induced dipoles by interaction with the crystal lattice [83]. The crystal lattice can also influence the law of selection to allow other forbidden transitions in H2 (1/4). Considering the substrate effect, having a peak of 1943 cm −1 and having a relatively narrow peak width means that H 2 (1/4) can freely rotate inside the crystal and correspond to a quarter of the dimensions of a typical hydrogen It means that it has a small size. Typical hydrogen shows an ortho-para ratio of 3: 1 at non-cold temperatures, whereas a single peak of H2 (1/4) formed under synthetic conditions has a relative internuclear spacing of 1/4, resulting in a 64x increase in stability. Only paratypes can be seen. Since the frequency obtained matches the 1989 cm-1 peak and hydrogen is the only element known to show a single rotational vibrational transition in a solid substrate, no other suitable one can be found, so the 1989 cm-1 peak is J of para H2 (1/4). Corresponds to the rotational transition of = 0 to J = 1.

H. H2 (1/4) rotational UV spectrum by electron beam excitation. H2 (1/4), MgX2 (X = F, Cl, Br, I), and CuX2 (X = F, Cl, Br) trapped in the alkali halide lattice were analyzed by windowless UV spectroscopy As an analytical condition, an electron beam excited state of the crystal was measured using a 12.5 keV electron gun at a beam current of 10-20 mA and a pressure range of less than 10-5 Torr. In the case of alkali metals, only alkali chlorides were found to show the peaks expected by Equation 14, and the strength was approximately in line with the estimate as the strength increased towards the bottom of the group 1 elemental column. In all cases, the Lehmann alpha α peak and other peaks were removed by heating and were not observed in the UV. In hydrogen mass spectrometry only hydrogen was recorded. Of the series of compounds of MgX2 (X = F, Cl, Br, I) and CuX2 (X = F, Cl, B), the expected bands were only detected in MgI2, which in this case could be affected by the catalyst Mg2 + have. NMR for these crystals showed the H2 (1/4) peak at a relative intensity of F, Cl, Br, << I at 1.13 ppm only for MgX2, indicating that the bands due to electron beam-excited emission of MgI2 alone Coincides with the detection line.

(

는 최종 상태의 회전 양자수)를 갖는 회전 에너지 간격의 예상치인 0.241 eV (식 14; p=4)와 일치한다. H2(1/4)는 자유 회전자이나, 자유 진동자는 아니며 이는 앞서 예를 든 실리콘 내의 침입형 수소 [83-87]의 경우와 유사하다. 5.73 eV의 측정 경사값은 8.25 eV (식 13)의 진동에너지(

) 예상치로부터 실리콘 내의 침입형 H2의 백분율에 비하여 2배 정도 이동하였다. 후자의 경우에는, 자유 H2의 진동 에너지가 4161 cm-1인 반면, 실리콘 내의 진동 피크가 오르쏘 및 파라-H2에 대응하여 3618 및 3627 cm-1에서 각각 관찰된다 [83]. 전자의 경우에는 이동치가 약 30% 낮은데, 이는 분자 진동 모드가 결정 격자와 결합함에 따라 질량이 두드러지게 상승하기 때문인 것으로 볼 수 있다. The spectrum of the 100-350 nm region for electron beam-excited CsCl crystals with captured H 2 (1/4) is shown in FIG. 46. A series of uniform lines were observed in the 220-300 nm region as shown in FIG. 46. These lines approximately corresponded to the spacing and intensity of the P branches of H2 (1/4) given in Eq. P (1), P (2), P (3), P (4), P (5), and P (6) at 226.0 nm, 237.0 nm, 249.5 nm, 262.5 nm, 277.0 nm, and 292.5 nm Each was observed. The slope of the linear curve with respect to the energy of the peak is 0.25 eV, as shown in FIG. 46, with an intercept of 5.73 eV and a residual error sum of r2 <0.0000. Slope

(

Corresponds to 0.241 eV (Equation 14; p = 4), which is an estimate of the rotational energy interval with the final state of rotational quantum number. H2 (1/4) is a free rotor, but not a free oscillator, which is similar to the case of intrusive hydrogen [83-87] in the above-described silicon. The measured slope of 5.73 eV is the vibration energy of 8.25 eV (Equation 13)

) Shifted approximately two times compared to the percentage of invasive H2 in silicon from the estimate. In the latter case, the vibrational energy of free H 2 is 4161 cm −1, while vibration peaks in silicon are observed at 3618 and 3627 cm −1, respectively, corresponding to Ortho and para-H 2 [83]. In the former case, the movement is about 30% lower, which is probably due to the significant increase in mass as the molecular vibration mode combines with the crystal lattice.

Using equations 14 and 15 with a measured rotational energy interval of 0.25 eV, an internuclear distance that is 1/4 of the normal H2 internuclear distance relative to H2 (1/4) is derived. Corresponding weak bands were observed from NaH * Br, and stronger bands were observed from NaH * Cl. Considering the latter case, the emission intensity was significantly increased by H2 (1/4) trapped in the silicon substrate. A 100-550 nm spectrum of NaH * Cl coated electron beam-excited silicon wafer with trapped H2 (1/4) is shown in FIG. 47. What was observed was roughly consistent with the spacing and intensity of the P branches of H2 (1/4) given in equation (14). P (1), P (2), P (3), P (4), P (5), and P (6) at 222.5 nm, 233.4 nm, 245.2 nm, 258.2 nm, 272.2 nm, and 287.4 nm Each was observed. The slope of the linear curve with respect to the energy of the peak is 0.25 eV as shown in FIG. 47, with an intercept of 5.82 eV and a residual error sum of r2 <0.0000. Linearity is a property of rotation, and the result is again in line with H2 (1/4). This technique is Secs. Confirm the solid state NMR and FTIR results given in IIIE and IIIG. As already known, when [13-14] KH * Cl having H- (1/4) is projected on an electron beam of 12.5 keV by NMR, electron beam excited alkali chloride, NaH * Cl-coated Si, and argon Excitation release of invasive H2 (1/4) similar to that observed in hydrogen plasma was observed [13-14]. It was also observed that the band corresponding to H 2 (1/4) was removed from the KCl starting material by high temperature heating. After KH * Cl was synthesized from the heat treated KCl, KH * Cl trapped in the lattice of KH * Cl was observed in addition to H- (1/4), indicating that multiple catalysts such as HCl, NaH, K, and Ar + Tells us that we can generate H2 (1/4).

Experiment reference

R. Mills, The Grand Unified Theory of Classical Quantum Mechanics October 2007 Edition, posted at http://www.blacklightpower.com/theory/bookdownload.shtml.

2. R. Mills, K. Akhar, Y. Lu, "Spectroscopic Observation of Helium- and Hydrogen-Catalyzed Hydrino Transitions", to be submitted.

3. R. L. Mills, "Classical Quantum Mechanics", Physics Essays, Vol. 16, No. 4, December, (2003), pp. 433-498.

4. R. Mills, "Physical Solutions of the Nature of the Atom, Photon, and Their Interactions to Form Excited and Predicted Hydrino States", in press.

5. R. L. Mills, "Exact Classical Quantum Mechanical Solutions for One-Through Twenty-Electron Atoms", Physics Essays, Vol. 18, (2005), pp. 321-361.

6. R. L. Mills, "The Nature of the Chemical Bond Revisited and an Alternative Maxwellian Approach", Physics Essays, Vol. 17, (2004), pp. 342-389.

7.R. L. Mills, "Maxwell's Equations and QED: Which is Fact and Which is Fiction", in press.

8. R. L. Mills, "Exact Classical Quantum Mechanical Solution for Atomic Helium Which Predicts Conjugate Parameters from a Unique Solution for the First Time", submitted.

9. R. L. Mills, "The Fallacy of Feynman's Argumenton the Stability of the Hydrogen Atom According to Quantum Mechanics," Annales de la Fondation Louis de Broglie, Vol. 30, no. 2, (2005), pp. 129-151.

10. R. Mills, "The Grand Unified Theory of Classical Quantum Mechanics", Int. J. Hydrogen Energy, Vol. 27, No. 5, (2002), pp. 565-590.

11.R. Mills, The Nature of Free Electrons in Superfluid Helium-a Test of Quantum Mechanics and a Basis to Review its Foundations and Make a Comparison to Classical Theory, Int. J. Hydrogen Energy, Vol. 26, No. 10, (2001), pp. 1059-1096.

12. R. Mills, "The Hydrogen Atom Revisited", Int. J. of Hydrogen Energy, Vol. 25, Issue 12, December, (2000), pp. 1171-1183.

13. R. L. Mills, J. He, Y. Lu, M. Nansteel, Z. Chang, B. Dhandapani, "Comprehensive Identification and Potential Applications of New States of Hydrogen", Int. J. Hydrogen Energy, Vol. 32 (14), (2007), pp. 2988-3009.

14.R. Mills, J. He, Z. Chang, W. Good, Y. Lu, B. Dhandapani, "Catalysis of Atomic Hydrogen to Novel Hydrogen Species H- (1/4) and H2 (1/4) as a New Power Source ", Int. J. Hydrogen Energy, Vol. 32, no. 12, (2007), pp. 2573-2584.

15.R. Mills, P. Ray, B. Dhandapani, W. Good, P. Jansson, M. Nansteel, J. He, A. Voigt, "Spectroscopic and NMR Identification of Novel Hydride Ions in Fractional Quantum Energy States Formed by an Exothermic Reaction of Atomic Hydrogen with Certain Catalysts ", European Physical Journal-Applied Physics, Vol. 28, (2004), pp. 83-104.

16. R. Mills and M. Nansteel, P. Ray, "Argon-Hydrogen-Strontium Discharge Light Source", IEEE Transactions on Plasma Science, Vol. 30, no. 2, (2002), pp. 639-653.

17. R. Mills and M. Nansteel, P. Ray, "Bright Hydrogen-Light Source due to a Resonant Energy Transfer with Strontium and Argon Ions", New Journal of Physics, Vol. 4, (2002), pp. 70.1-70.28.

18. R. Mills, J. Dong, Y. Lu, "Observation of Extreme Ultraviolet Hydrogen Emission from Incandescently Heated Hydrogen Gas with Certain Catalysts", Int. J. Hydrogen Energy, Vol. 25, (2000), pp. 919-943.

19. R. Mills, M. Nansteel, and P. Ray, "Excessively Bright Hydrogen-Strontium Plasma Light Source Due to Energy Resonance of Strontium with Hydrogen", J. of Plasma Physics, Vol. 69, (2003), pp. 131-158.

20. R. L. Mills, J. He, M. Nansteel, B. Dhandapani, "Catalysis of Atomic Hydrogen to New Hydrides as a New Power Source", International Journal of Global Energy Issues (IJGEI), Special Edition in Energy Systems, Vol. 28, Nos. 2/3 (2007), pp. 304-324.

21. H. Conrads, R. Mills, Th. Wrubel, "Emission in the Deep Vacuum Ultraviolet from a Plasma Formed by Incandescently Heating Hydrogen Gas with Trace Amounts of Potassium Carbonate", Plasma Sources Science and Technology, Vol. 12, (3003), pp. 389-395.

22. J. Phillips, R. L. Mills, X. Chen, "Water Bath Calorimetric Study of Excess Heat in 'Resonance Transfer' Plasmas", Journal of Applied Physics, Vol. 96, No. 6, pp. 3095-3102.

23. R. L. Mills, X. Chen, P. Ray, J. He, B. Dhandapani, "Plasma Power Source Based on a Catalytic Reaction of Atomic Hydrogen Measured by Water Bath Calorimetry", Thermochimica Acta, Vol. 406 / 1-2, (2003), pp. 35-53.

24. R. Mills, B. Dhandapani, M. Nansteel, J. He, T. Shannon, A. Echezuria, "Synthesis and Characterization of Novel Hydride Compounds", Int. J. of Hydrogen Energy, Vol. 26, No. 4, (2001), pp. 339-367.

25. R. Mills, B. Dhandapani, M. Nansteel, J. He, A. Voigt, "Identification of Compounds Containing Novel Hydride Ions by Nuclear Magnetic Resonance Spectroscopy", Int. J. Hydrogen Energy, Vol. 26, No. 9, (2001), pp. 965-979.

26. R. Mills, B. Dhandapani, N. Greenig, J. He, "Synthesis and Characterization of Potassium Iodo Hydride", Int. J. of Hydrogen Energy, Vol. 25, Issue 12, December, (2000), pp. 1185-1203.

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Claims (119)

A reaction cell for catalysis of atomic hydrogen, forming a composition of matter comprising new hydrogen species and a new form of hydrogen; Reaction vessels constructed and arranged to contain pressures that are less than, equal to, or greater than atmospheric pressure; A vacuum pump; A hydrogen atom source in communication with said reaction vessel; A source of hydrogen catalyst in communication with the reaction vessel comprising at least one reactant comprising the element or elements forming the catalyst and a reaction mixture with at least one other element, whereby the catalyst is formed from the source; And Heater that heats the vessel to initiate the formation of a catalyst in the reaction vessel if the reaction is not spontaneous at room temperature, whereby the catalysis of atomic hydrogen releases an amount of energy greater than about 300 kJ per mole of hydrogen Power source and hydride reactor comprising a. The method of claim 1, An energy cell for catalysis of atomic hydrogen to form a composition of matter comprising a novel hydrogen species and a novel form of hydrogen, a source of hydrogen catalyst and a source of atomic hydrogen, the source of hydrogen catalyst being hydrogen and at least one At least one reactant having another element of, Wherein said at least one reactant experiences a reaction wherein the energy released is greater than the difference between the standard enthalpy of formation of the compound having a stoichiometric or elemental composition of the product and the energy of formation of the at least one reactant. The method of claim 1, The source of the hydrogen catalyst comprises at least one reactant having hydrogen and at least one other element, The at least one reactant experiences a reaction where the energy released is greater than the theoretical standard enthalpy required to regenerate the at least one reactant from the product, wherein the energy for returning any reacted hydrogen is a standard power supply and hydride Reactor. The method of claim 1, A power source for generating electricity comprising a reactant of hydrogen and at least one other element, wherein the released energy experiences a reaction greater than the difference between the standard enthalpy of the formation of the compound having a stoichiometric or elemental composition of the product and the energy of formation of the reactant; and Hydrogenated water reactor. The method of claim 1, The released energy includes a reactant of hydrogen and at least one other element that experiences a reaction greater than the theoretical standard enthalpy required to regenerate the reactant from the product, and the energy for returning any reacted hydrogen is a standard value for the combustion of hydrogen. Power source and hydride reactor for power generation. The method of claim 1, The catalyst is about

A power supply and a hydride reactor capable of receiving energy from hydrogen atoms in one integer unit of either. The method of claim 1, The catalyst comprises one atom or ion M, wherein the ionization of t electrons from each atom or ion M to the continuous energy level is approximately the sum of the ionization energies of the t electrons.

Power source and hydride reactor, wherein m is an integer. The method of claim 7, wherein And the catalyst atom M is at least one of the groups Li, K, and Cs. The method of claim 8, Wherein said source of catalyst comprises a biatomic molecule of catalyst atoms and a hydride reactor. The method of claim 8, The reaction mixture comprises an atomic catalyst comprising one of Li, K, Cs, and H groups and at least a first reactant as a source of atomic hydrogen; The reaction mixture further comprises at least one other reactant, wherein the atomic hydrogen and atomic catalyst are formed by the reaction of at least one primary and at least one other reactant. The method of claim 10, The source of catalyst comprises MH, wherein M is a catalyst atom so that the atomic catalyst is formed from the source by reaction with a species comprising at least one other element. The method of claim 1, The catalyst comprises a diatomic molecule MH, The breakage of MH bond + the ionization of t electrons from each of the atoms M to the continuous energy level is approximately the sum of the binding energy and the ionization energy of t electrons.

Power source and hydride reactor, wherein m is an integer. The method of claim 12, The power source and hydride reactor of claim 1, wherein the source of catalyst comprises a reaction resulting in a biatomic molecule comprising hydrogen and other elements. The method of claim 13, The catalyst is a power source and a hydride reactor comprising hydrogen and other elements than hydrogen. The method of claim 14, Wherein the source of catalyst and reactant atomic hydrogen comprises a biatomic molecule of hydrogen and other elements. The method of claim 15, Said catalyst comprising at least one of molecular AlH, BiH, ClH, CoH, GeH, InH, NaH, RuH, SbH, SeH, SiH, and SnH. The method of claim 1, A power source and a hydride reactor comprising at least one of an element (s) of said catalyst, another element, and a composition of material having the same composition as the catalyst but different in physical state from the catalyst. The method of claim 1, The source of catalyst is a power source and a hydride reactor comprising hydrogen and other elements than hydrogen. The method of claim 1, The reaction mixture comprises a catalyst or a source of catalyst and atomic hydrogen or a source of atomic hydrogen (H), wherein at least one of the catalyst and atomic hydrogen is a chemical reaction between at least one species of the reaction mixture or two or more species of reaction mixture Power source and hydride reactor emitted by. The method of claim 19, The species may be at least one of an element, a complex, an alloy, or a compound such as a molecular or inorganic compound, each of which may be at least one of a reagent or a product in the reactor. The method of claim 20, Wherein said species is capable of forming a complex, an alloy, or a compound having at least one of hydrogen and a catalyst. The method of claim 21, The element or alloy is a power source and hydride comprising at least one of M (catalyst atom), H, Al, B, Si, C, N, Sn, Te, P, S, Ni, Ta, Pt, and Pd Reactor. The method of claim 22, Wherein said catalyst atoms M are at least one of Li, K, Cs, and Na groups and the catalysts are atoms Li, K, and Cs, and molecules NaH. The method of claim 23, wherein At least one of the reaction mixture species is capable of forming at least one reaction product species such that H or the energy for releasing the free catalyst is low in the absence of formation of reaction product species. The method of claim 24, The reaction resulting in at least one of the atom H and the catalyst is a reversible power source and a hydride reactor. The method of claim 25, Wherein said complex, alloy, or compound comprises a lithium alloy or compound. The method of claim 26, The reaction mixture is LiAlH4, Li3AlH6, LiBH4, Li3N, Li2NH, LiNH2, NH3, H2, LiNO3, Li / Ni, Li / Ta, Li / Pd, Li / Te, Li / C, Li / Si, and Li / Sn A power source and a hydride reactor comprising at least one of the group of alloys or compounds. The method of claim 27, The reaction mixture comprises one or more compounds that react with a source of Li to form a Li catalyst, Wherein said reaction mixture comprises at least one species from the group LiNH2, Li2NH, Li3N, Li, LiH, NH3, H2, and dissociating agent. The method of claim 28, Wherein the reaction mixture comprises Pd, LiH, and LiNH 2 on Al 2 O 3 powder. The method of claim 29, Wherein the reaction mixture comprises hydrogenated Pd, Li, and Li 3 N, and any H 2 gas on an Al 2 O 3 powder. The method of claim 25, The source of catalyst comprises a source of NaH catalyst, wherein the source of NaH is an alloy of a source of Na and hydrogen. The method of claim 31, wherein The alloy source of the catalyst is sodium metal and one or more nitrogen-based compounds, alkali metals or alkaline earth metals, transition metals, Al, Sn, Bi, Ag, In, Pb, Hg, Si, Zr, B, Pt, Pd, or other A power source and hydride reactor comprising at least one of a metal and the H source comprises H 2 or hydride. 33. The method of claim 32, And a source of hydrogen catalyst comprising a Na-containing inorganic compound. The method of claim 33, wherein The reaction mixture comprises one or more compounds that react with a source of NaH to form a NaH catalyst; At least one of the source of NaH catalyst and the reaction mixture is Na, NaH, alkali metal or alkaline earth metal hydroxide, aluminum hydroxide, alkali metal, alkaline earth metal, NaOH doped R-Ni, NaOH, Na2O, and Na2CO3 A power source and hydride reactor comprising at least one and at least one of NaNH 2, Na 2 NH, Na 3 N, Na, NaH, NH 3, H 2 and dissociating agent groups. The method of claim 33, wherein The reaction mixture comprises one or more compounds that react with a source of NaH to form a NaH catalyst; Wherein said reaction mixture comprises at least one of a group of NaNH 2, Na 2 NH, Na 3 N, Na, NaH, NH 3, H 2 and a dissociating agent. 36. The method of claim 35 wherein The reaction mixture comprises one or more compounds that react with a source of NaH to form a NaH catalyst; The reaction mixture is a power source and hydride comprising at least one species of the group of NaH, Na, metals, metal hydrides, lanthanum metals, lanthanum metal hydrides, lanthanum, lanthanum hydrides, H2, and dissociating agents. Reactor. The method of claim 34, wherein The reaction mixture comprises at least one of a NaH molecule and a source of NaH molecules and the NaH molecule

Used as a catalyst to form an H state given by an integer greater than 1, preferably 2 to 137; The source of NaH molecules is: (a) Na metal, atom Na, source of hydrogen, atomic hydrogen, and NaH (s); (b) R-Ni comprising NaOH and a reactant to form NaH comprising a reducing agent and a source of hydrogen; A power source and a hydride reactor comprising at least one of. The method of claim 34, wherein The reaction mixture, A reactant comprising a reducing agent to form NaH from NaOH; Source of hydrogen including at least one of NaH, H2 gas and dissociating agent and hydride A power source and a hydride reactor comprising at least one of. The method of claim 34, wherein The atomic sodium and one of the molecules NaH are provided by a reaction between the metal, ion or molecular type of Na and at least one compound or element; The source of Na or NaH is at least one of metals Na, NaNH 2, NaOH, NaX (X is a halide), and NaH (s); And other elements are H, substituents, or reducing agents. The method of claim 34, wherein The reaction mixture is at least one of a power source and a hydride reactor: (1) a source of sodium; (2) support materials; (3) a source of hydrogen; (4) a substituent, and (5) reducing agents. The method of claim 40, Sources of sodium include Na, NaH, NaNH 2, NaOH, NaOH coated R-Ni, NaX (X is halide), and NaX coated R-Ni. 42. The method of claim 41 wherein The reducing agent comprises at least one of a metal, such as an alkali metal, an alkaline earth metal metal, a lanthanum element, a transition metal such as Ti, aluminum, B, a metal alloy such as AlHg, NaPb, NaAl, LiAl, and a metal or a reducing agent Such as alkaline earth halides, transition metal halides, lanthanide element halides, aluminum halides, metal hydrides such as LiBH4, NaBH4, LiAlH4, or NaAlH4, and alkali or alkaline earth metals and oxidizing agents such as AlX3, MgX2, LaX3, CeX3 And a TiXn, where x is a halide, preferably Br or I. The method of claim 42, wherein Wherein the source of hydrogen comprises H2 gas and a dissociating agent and a hydride. The method of claim 43, And the substituent comprises at least one of an alkali metal, an alkaline earth metal metal, an alkali metal hydride, and an alkaline earth metal metal hydride. The method of claim 44, The support may be R-Ni, Al, Sn, Al2O3, such as gamma, beta, or alpha alumina, aluminate, sodium aluminate, alumina nanoparticles, porous Al2O3, Pt, Ru, or Pd / Al2O3, carbon, Pt or Pd / C, inorganic compounds such as Na 2 CO 3, lanthanide oxides such as M 2 O 3 (preferably M = La, Sm, Dy, Pr, Tb, Gd, and Er), Si, silica, silicate, zeolite, Y zeolite powder, lanthanum At least one of elemental elements, transition metals, metal alloys such as alkali and alkaline earth metal alloys with Na, rare earth metals, SiO2-Al2O3 or SiO2 supported Ni, and other supported metals such as alumina supported platinum, palladium, and ruthenium Power source and hydride reactor comprising one. The method of claim 45, The dissociating agent comprises at least one of Raney nickel (R-Ni), a noble metal, and a noble metal on a support, wherein the noble metal may be Pt, Pd, Ru, Ir, and Rh, and the support is Ti, Nb , Al2O3, SiO2 and combinations thereof; Pt or Pd on carbon, hydrogen rich catalyst, nickel fiber mat, Pd sheet, Ti sponge, Pt or Pd, TiH, Pt black, and Pd black, refractory metals such as molybdenum and electroplated on Ti or Ni sponge or mat and A power source and hydride reactor in which tungsten, transition metals such as nickel and titanium, internal transition metals such as niobium and zirconium, and refractory metals such as tungsten or molybdenum, and separation materials can be maintained at high temperatures. The method of claim 40, The source of NaH may be R-Ni comprising NaOH and a reactant to form NaH, and the reactant is a power source that is a reducing agent comprising at least one of an alkali metal, an alkaline earth metal metal, and an intermetallic Al of R-Ni. And hydride reactors. A reaction cell for catalysis of atomic hydrogen, forming a composition of matter comprising new hydrogen species and a new form of hydrogen; Reaction vessels constructed and arranged to contain pressures that are less than, equal to, or greater than atmospheric pressure; A vacuum pump; A hydrogen atom source in communication with said reaction vessel; Source of hydrogen catalyst M in communication with the reaction vessel, whereby t electrons are ionized from the catalyst to each continuum energy level, and the sum of the ionization energies of the t electrons is approximately

Wherein m is an integer; If the catalyst is not yet present, reaction mixture to form catalyst from catalyst source; And If the reaction is not spontaneous at room temperature, the vessel is heated to initiate at least one of a hydrino reaction and a reaction for the formation of a catalyst in the reaction vessel, wherein the H atoms catalyzed by hydrogen Emits more than about 300 kJ of energy per mole) Power source and hydride reactor comprising a. The method of claim 48, And the catalyst atom M is at least one of the groups Li, K, and Cs. A reaction cell for catalysis of atomic hydrogen, forming a composition of matter comprising new hydrogen species and a new form of hydrogen; Reaction vessels constructed and arranged to contain pressures that are less than, equal to, or greater than atmospheric pressure; A vacuum pump; A hydrogen atom source in communication with said reaction vessel; A source of at least one of the group of Li, K and Cs catalyst atoms in communication with the reaction vessel; If the catalyst is not yet present, a reaction mixture forming an atomic catalyst from an atomic catalyst source; And If the reaction is not spontaneous at room temperature, the vessel is heated to initiate the formation of at least one of Li, K and Cs atomic catalysts in the reaction vessel, whereby the catalytic reaction with H is about 1 mole of hydrogen during the catalysis of atomic hydrogen. Emits more than 300 kJ of energy) Power source and hydride reactor comprising a. 51. The method of claim 50, Wherein the reaction mixture comprises Pd, LiH, and LiNH 2 on Al 2 O 3 powder. 51. The method of claim 50, Wherein the reaction mixture comprises hydrogenated Pd, Li, and Li 3 N, and any H 2 gas on an Al 2 O 3 powder. A reaction cell for catalysis of atomic hydrogen, forming a composition of matter comprising new hydrogen species and a new form of hydrogen; Reaction vessels constructed and arranged to contain pressures that are less than, equal to, or greater than atmospheric pressure; A vacuum pump; Hydrogen catalyst source in communication with the reaction vessel comprising MH, whereby ionization of t electrons from atom M to each continuum energy level occurs, as well as MH bonds, and the sum of the binding energy and the ionization energy of t electrons is approximately

Where m is an integer; If molecular MH is not present yet, reaction mixture to form molecular MH from a source of molecular catalyst; And A heater that heats the vessel and initiates the formation of molecular MH in the reaction vessel if the reaction is not spontaneous at room temperature, whereby the molecular MH functions as a hydrogen catalyst and the source of H reactant per mol of hydrogen during catalysis of atomic hydrogen Emits more than about 300 kJ of energy) Power source and hydride reactor comprising a. The method of claim 53, And a hydride reactor further comprising a source of atomic hydrogen from said source in communication with said reaction vessel. The method of claim 53, Wherein said MH comprises at least one of AlH, BiH, ClH, CoH, GeH, InH, NaH, RuH, SbH, SeH, SiH, and SnH groups. A reaction cell for catalysis of atomic hydrogen, forming a composition of matter comprising new hydrogen species and a new form of hydrogen; Reaction vessels constructed and arranged to contain pressures that are less than, equal to, or greater than atmospheric pressure; A vacuum pump; A molecular NaH catalyst source in communication with the reaction vessel; If molecular NaH is not yet present, reaction mixture to form molecular NaH from a source of molecular NaH; And A heater that heats the vessel and initiates the formation of molecular NaH in the reaction vessel if the reaction is not spontaneous at room temperature, whereby the molecular NaH functions as a hydrogen catalyst and the source of H reactant per mol of hydrogen during catalysis of atomic hydrogen. Emits more than about 300 kJ of energy) Power source and hydride reactor comprising a. The method of claim 56, wherein And a hydride reactor further comprising a source of atomic hydrogen from the source in communication with the reaction vessel. The method of claim 56, wherein Said reaction mixture comprising Pd and NaH on Al2O3 powder. The method of claim 56, wherein Said reaction mixture comprising R-Ni and Na comprising about 0.5 wt% NaOH, wherein Na is used as a reducing agent and a hydride reactor. The method of claim 56, wherein Wherein said reaction mixture comprises R-Ni comprising about 0.5 wt% NaOH, wherein intermetallic Al is used as a reducing agent. The method of claim 56, wherein Wherein the reaction mixture comprises Pd, NaH, and La on an Al 2 O 3 powder. The method of claim 56, wherein Wherein the reaction mixture comprises Pd, NaH, and NaNH 2 on Al 2 O 3 powder. At least one reaction vessel constructed and arranged to contain a range of pressures lower than, equal to, or greater than atmospheric pressure; A vacuum pump in communication with the reaction vessel; A reaction mixture comprising a first source of hydrogen atoms in communication with the reaction vessel; A catalyst source in communication with the reaction vessel; A heater to initiate the catalysis; Means for regenerating the reaction mixture; And Power converter Power plant comprising a. The method of claim 63, wherein The converter includes a steam generator in communication with the reaction vessel, a steam turbine in communication with the steam generator, and an electrical generator in communication with the steam turbine. The method of claim 1, A power source and hydride reactor wherein the composition of matter comprising the new hydrogen species and the new form of hydrogen comprises: (a) hydrogen species with increased binding energy of at least one neutral, positive or negative, the binding energy being (i) greater than the binding energy of the corresponding common hydrogen species, or (ii) the hydrogen species having a binding energy greater than that of any hydrogen species in which the corresponding generic hydrogen species are unstable or unobservable since the binding energy of the common hydrogen species is less than or negative to thermal energy at room temperature; And (b) at least one other element. The method of claim 65, The compound is characterized by increased binding energy hydrogen paper

Wherein n is a positive integer, provided that when H has a positive charge, n is greater than one. 67. The method of claim 66, Wherein said compound is an increased binding energy hydrogen species is selected from the group consisting of: (a) a hydride having a binding energy greater than the binding energy of a typical hydride ion (about 0.8 eV) for p = 2 to 23, wherein the binding energy is

Where p is an integer greater than 1, s = 1/2, π is pi, h is Planck's constant bar, μ0 is vacuum permeability, me is the mass of electrons, μe is

Is the reduced electron mass given by, where mp is the mass of protons, aH is the radius of the hydrogen atom, a0 is the Bohr radius, and e is the basic charge; (b) hydrogen atoms having a binding energy greater than about 13.6 eV; (c) hydrogen molecules having a binding energy greater than about 15.3 eV; And (d) hydrogen molecular ions having a binding energy greater than about 16.3 eV. The method of claim 67, The compound has an increased binding energy hydrogen species of about 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 And hydride ions having a binding energy of 34.7, 19.3, and 0.69 eV. The method of claim 68, The compound is a power source and hydride reactor wherein the increased binding energy hydrogen species is a hydride ion having the following binding energy:

Where p is an integer greater than 1, s = 1/2, π is pi, h is Planck's constant bar, μ0 is vacuum permeability, me is the mass of electrons, μe is

Is the reduced electron mass given by, where mp is the mass of protons, aH is the radius of the hydrogen atom, a0 is the Bohr radius, and e is the basic charge. The method of claim 69, wherein Wherein said compound is selected from the group consisting of increased binding energy hydrogen species: (a) about

A hydrogen atom having a binding energy of (where p is an integer), (b) about

Where p is an integer greater than 1, s = 1/2, π is pi, h is Planck's constant bar, μ0 is vacuum permeability, me is the mass of electrons, μe is

Is the reduced electron mass given by, where mp is the mass of protons, aH is the radius of the hydrogen atom, a0 is the Bohr radius, and e is the basic charge. (H-); (c) increased binding energy hydrogen species

; (d) approximately

Increased binding energy hydrogen species trihydrino molecular ions having a binding energy of (where p is an integer),

; (e) about

Increased binding energy hydrogen molecules with a binding energy of; And (f) about

Increased binding energy of hydrogen molecule ions with a binding energy of. The method of claim 1, The catalyst is a power source and number comprising a chemical or physical process providing a net enthalpy of m.27.2 ± 0.5 eV, where M is an integer or m / 2 · 27.2 ± 0.5 eV and M is an integer greater than one. Digestion reactor. The method of claim 1, In the catalyst system, the sum of the ionization energies of t electrons is about m · 27.2 ± 0.5 eV, where M is an integer or m / 2 · 27.2 ± 0.5 eV, M is an integer greater than 1, and t is an integer. Power source and hydride reactor provided by ionization of participating species such as atoms, ions, molecules, and t-electrons from ionic or molecular compounds to continuous energy levels. The method of claim 1, The catalyst is provided by the transfer of t electrons between participating ions; The transfer of t electrons from one ion to another provides a net enthalpy of the reaction, and the sum of the ionization energy of the electron donor ion minus the ionization energy of the electron accepting ion is about m.27.2 ± 0.5 eV, where M is an integer. ) Or m / 2 · 27.2 ± 0.5 eV, where M is an integer greater than 1 and t is an integer. The method of any one of claims 71, 72, and 73, wherein m is an integer less than 400 power source and hydride reactor. The method of claim 74, wherein The catalyst is 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, 2K +, He +, Na +, Rb +, Sr +, Fe3 +, Mo2 +, Mo4 +, and In3 +, Ar +, Xe +, Ar2 + and H +, and Ne + and H + Power source and hydride reactor selected. 76. The method of claim 75, The catalyst of atomic hydrogen can provide a net enthalpy of m.27.2 ± 0.5 eV (where M is an integer) or m / 2 · 27.2 ± 0.5 eV (where M is an integer greater than 1) and about

(Where p is an integer), wherein the net enthalpy is such that the breakdown of the molecular bonds of the catalyst and the sum of the ionization energies of the t electrons is about m.27.2 ± 0.5 eV ( Where M is an integer or m / 2 · 27.2 ± 0.5 eV and M is an integer greater than 1), the power supply and hydride provided by ionization of t electrons from the atom of each broken molecule to the continuous energy level Reactor. 77. The method of claim 76, The catalyst is a power source and hydride comprising at least one of AIH, BiH, CIH, CoH, GeH, InH, NaH, RuH, SbH, SeH, SiH, SnH, C2, N2, O2, CO2, NO2, and NO3 Reactor. 78. The method of claim 77 wherein Said catalyst comprising a molecule in combination with an ionic or atomic catalyst. The method of claim 78, The catalyst combination is Li, Be, K, Ca, Ti, V, Cr, Mn, Fe, Co, Ni, Cu, Zn, As, Se, Kr, Rb, Sr, Nb, Mo, Pd, Sn, Te, Consisting of Cs, Ce, Pr, Sm, Gd, Dy, Pb, Pt, 2K +, He +, Na +, Rb +, Sr +, Fe3 +, Mo2 +, Mo4 +, In3 +, He +, Ar +, Xe +, Ar2 + and H +, and Ne + and H + A group consisting of AIH, BiH, CIH, CoH, GeH, InH, NaH, RuH, SbH, SeH, SiH, SnH, C2, N2, O2, CO2, NO2, and NO3 in combination with one or more atoms or ions selected from the group A power source and a hydride reactor comprising at least one molecule selected from. The method of claim 79, The catalyst absorbs at least one of 27.21 eV and 54.4 eV and is ionized to 2H + so that it is (p) a hydrogen atom from at least one of the (p + 1) and (p + 2) energy levels given by at least one of the following: A power supply and hydride reactor comprising two hydrogen atoms to facilitate the delivery of:

Where the overall response is

And

ego, Where the overall response is

to be. The method of claim 80, The catalyst comprises hydrinos in a catalyst disproportionation reaction, wherein hydrinos, which are low-energy hydrogen atoms, act as catalysts for each metastable excitation, resonance excitation, and ionization energy of the hydrino atoms.

Power source and hydride reactor. Providing a reaction vessel constructed and arranged to contain a range of pressures lower than, equal to, or greater than atmospheric pressure; Maintaining the pressure in a range lower than, equal to, or greater than atmospheric pressure; Providing a hydrogen atom in the reaction vessel from a first source of hydrogen atoms in communication with the reaction vessel; Providing a source of hydrogen catalyst atoms in communication with the reaction vessel, the reaction mixture comprising at least one reactant comprising the element or elements forming the catalyst and a reaction mixture of at least one other element such that a catalyst is formed from the source; If the catalyst is not yet present or the reaction to form the catalyst is not spontaneous at room temperature, heating the reaction mixture to produce an atomic catalyst from an atomic catalyst source; If the reaction is not spontaneous at room temperature, heating the reaction mixture to initiate the catalysis of atomic hydrogen in the reaction vessel, whereby the catalysis of atomic hydrogen is an amount of energy greater than about 300 kJ per mole of hydrogen Emits) Power production method comprising a. 83. The method of claim 82, Wherein said catalyst is atomic Li. 84. The method of claim 83, And reacting Pd, LiH, and LiNH 2 on Al 2 O 3 powder in the reaction vessel to form an atomic Li catalyst and atomic hydrogen. 85. The method of claim 84, Further comprising the addition of H2 to regenerate LiH and LiNH2. 83. The method of claim 82, Reacting the hydrogenated Pd, Li, and Li3N and any H2 gas on Al2O3 powder in the reaction vessel to form an atomic Li catalyst and atomic hydrogen. 87. The method of claim 86, further comprising removing H2 to regenerate Li and Li3N and then hydrogenating the dissociating agent or reintroducing H2. Providing a reaction vessel constructed and arranged to contain a range of pressures lower than, equal to, or greater than atmospheric pressure; Maintaining the pressure in a range lower than, equal to, or greater than atmospheric pressure; Providing a source of a molecular hydrogen catalyst in communication with a reaction vessel comprising at least one reactant comprising the element or elements forming the catalyst and a reaction mixture with at least one other element, whereby the catalyst is formed from a source ); And If the catalyst is not yet present or the reaction forming the catalyst is not spontaneous at room temperature, heating the reaction mixture to produce a molecular catalyst from a source of molecular catalyst; If the reaction is not spontaneous at room temperature, heating the reaction mixture to initiate the catalysis of atomic hydrogen in the reaction vessel, whereby the catalysis of atomic hydrogen is an amount of energy greater than about 300 kJ per mole of hydrogen Emits) Power production method comprising a. 89. The method of claim 88, And providing hydrogen atoms to the reaction vessel from a first source of hydrogen atoms in communication with the reaction vessel. 89. The method of claim 88, The catalyst is a method of producing power that is a molecular NaH. 91. The method of claim 90, Wherein said source of molecule NaH comprises a source of Na metal and hydrogen. 91. The method of claim 90, Wherein said reaction mixture comprises Pd and NaH on an Al 2 O 3 powder. 92. The method of claim 92, Further comprising regenerating NaH by adding H2. 91. The method of claim 90, Wherein said reaction mixture comprises R-Ni and Na comprising about 0.5 wt% NaOH and said Na is used as a reducing agent. 91. The method of claim 90, Wherein said reaction mixture comprises R-Ni comprising about 0.5 wt% NaOH, wherein intermetallic Al is used as a reducing agent. 95. The method of claim 94 or 95, The reaction mixture is regenerated by the addition of NaOH and NaH, wherein NaH can be used as H source and reducing agent. 91. The method of claim 90, Wherein the reaction mixture comprises Pd on NaH, lanthanide metal, and Al 2 O 3 powder. 97. The method of claim 97, The reaction mixture is regenerated by adding H2, separating NaH and lanthanum element hydrides by sieving, heating lanthanum element hydrides to form lanthanum metals, and mixing lanthanum metals and NaH Way. 97. The method of claim 97, The reaction mixture melts Na to separate Na and lanthanum element hydride, removes the liquid, and heats the lanthanum element hydride to form a lanthanide metal, hydrogenated from Na to NaH, and a lanthanum metal and A method of producing power that is regenerated by mixing NaH. 91. The method of claim 90, Wherein the reaction mixture comprises Pd, NaH and NaNH 2 on Al 2 O 3 powder. 101. The method of claim 100, Further comprising regenerating NaH and NaNH2 by adding H2. 91. The method of claim 90, And reacting NaOH with a reducing agent in the reaction vessel to form molecular NaH. 91. The method of claim 90, Further comprising reacting at least one of the following: (1) a source of sodium; (2) support materials; (3) a source of hydrogen; (4) a substituent, and (5) a reducing agent for forming a molecule NaH. 103. The method of claim 103, The source of sodium comprises Na, NaH, NaNH 2, NaOH, NaOH coated R-Ni, NaX (X is a halide), and NaX coated R-Ni. 103. The method of claim 103, The reducing agent comprises at least one of a metal, such as an alkali metal, an alkaline earth metal metal, a lanthanum element, a transition metal such as Ti, aluminum, B, a metal alloy such as AlHg, NaPb, NaAl, LiAl, and a metal or a reducing agent Such as alkaline earth halides, transition metal halides, lanthanide element halides, aluminum halides, metal hydrides such as LiBH4, NaBH4, LiAlH4, or NaAlH4, and alkali or alkaline earth metals and oxidizing agents such as AlX3, MgX2, LaX3, CeX3 , And TiXn, where x is a halide, preferably Br or I. 103. The method of claim 103, The source of hydrogen comprises H2 gas and dissociating agent and hydride. 103. The method of claim 103, Wherein said substituent comprises an alkali or alkaline earth metal metal. 103. The method of claim 103, Providing a source of NaH on a large surface area support that aids in the generation of molecular NaH from said source, and further reacting the source of NaH to form molecular NaH. 108. The method of claim 103 or 108, The support may be R-Ni, Al, Sn, Al2O3, such as gamma, beta, or alpha alumina, aluminate, sodium aluminate, alumina nanoparticles, porous Al2O3, Pt, Ru, or Pd / Al2O3, carbon, Pt or Pd / C, inorganic compounds such as Na 2 CO 3, lanthanide oxides such as M 2 O 3 (preferably M = La, Sm, Dy, Pr, Tb, Gd, and Er), Si, silica, silicate, zeolite, Y zeolite powder, lanthanum At least one of elemental elements, transition metals, metal alloys such as alkali and alkaline earth metal alloys with Na, rare earth metals, SiO2-Al2O3 or SiO2 supported Ni, and other supported metals such as alumina supported platinum, palladium, and ruthenium Power production method comprising one. 91. The method of claim 89 wherein Wherein the source of atomic hydrogen comprises hydrogen molecules and the hydrogen atoms are formed from hydrogen molecules using a dissociating agent. 112. The method of claim 103 or 110, The dissociating agent comprises at least one of Raney nickel (R-Ni), a noble metal, and a noble metal on a support, wherein the noble metal may be Pt, Pd, Ru, Ir, and Rh, and the support is Ti, Nb , Al2O3, SiO2 and combinations thereof; Pt or Pd on carbon, hydrogen rich catalyst, nickel fiber mat, Pd sheet, Ti sponge, Pt or Pd, TiH, Pt black, and Pd black, refractory metals such as molybdenum and electroplated on Ti or Ni sponge or mat and Tungsten, transition metals such as nickel and titanium, internal transition metals such as niobium and zirconium, and refractory metals such as tungsten or molybdenum, and separation materials can be maintained at high temperatures. 91. The method of claim 90, And forming Na 2+ in the reaction vessel from molecules NaH. 89. The method of claim 82 or 88, Removing the reaction product from the vessel and regenerating a source of catalyst from at least a portion of the reaction product. 89. The method of claim 82 or 88, Further comprising converting the emitted energy into electrical energy. 89. The method of claim 82 or 88, The source of the hydrogen catalyst comprises at least one reactant having hydrogen and at least one other element, Wherein said at least one reactant experiences a reaction wherein the energy released is greater than the difference between the standard enthalpy of formation of a compound having a stoichiometric or elemental composition of the product and the energy of formation of said at least one reactant. 89. The method of claim 82 or 88, The source of the hydrogen catalyst comprises at least one reactant having hydrogen and at least one other element, Wherein said at least one reactant experiences a reaction where the energy released is greater than the theoretical standard enthalpy required to regenerate the at least one reactant from the product, wherein the energy for returning any reacted hydrogen is a standard value. The at least one reactant includes providing hydrogen and at least one other element that experiences a reaction where the energy released is greater than the difference between the standard enthalpy of formation of the compound having the stoichiometry or elemental composition of the product and the formation energy of the reactant. Power production method. Energy that provides hydrogen and at least one other element that experiences a reaction that is greater than the theoretical standard enthalpy required to regenerate the reactants from the product, wherein the energy for returning any reacted hydrogen may Power production method that is the standard value for 89. The method of claim 82 or 88, Further comprising preparing or regenerating the reaction mixture, wherein the preparing or regenerating comprises at least one of mechanical mixing or separation, melting, filtration, hydrogenation, dehydrogenation, decomposition, deposition, evaporation, vaporization and sublimation, and ball milling. Power production method achieved by.

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