ELECTROCHEMICALLY ASSISTED EXCESS HEAT PRODUCTION

Abstract: Electrochemically assisted nuclear reaction that produces excess heat at elevated temperatures by immersing a metal in an electrolyte solution comprising a molten salt containing an alkali deuteride and applying a potential and current to the electrolyte and the metal to enhance diffusion of deuterium into the metal. A recycling system utilizing metals that do not form compounds with lithium and also have very limited solubilities for lithium will increase the usefulness of the invention by recombining lithium with deuterium gas that has not diffused into the metal. Torched palladium having a very porous structure increases efficiency as well.

Description: DESCRIPTION Electrochemicallv Assisted Excess Heat Production Technical Field This invention relates to electrochemically-assisted excess heat production. Recent reports of excess heat production in electrochemically-assisted metal-deuterium systems have been attributed to fusion. Nuclear fusion occurs when two nuclei of a light element combine in order to form a single nucleus of a heavier element. Nuclear fusion is the process that causes the sun to shine and a hydrogen bomb to explode. The simplest fusion reactions between two deuterium atoms are to form (i) a helium-3 nucleus and a neutron or (ii) a tritium nucleus and a proton. The nucleus of a hydrogen atom consists only of a single positively charged particle, the proton. A hydrogen atom's nucleus may also contain a single neutron and a single proton to form the hydrogen isotope deuterium. A hydrogen atom containing two neutrons and one proton is the hydrogen isotope tritium. The energy in a helium nucleus is less than the energy in two deuterium nuclei, so that if two deuterium nuclei fuse to form a helium nucleus, the excess energy is released; this is the source of energy for a deuterium fusion reaction. However, because deuterium nuclei are positively charged, they repel each other. Accordingly, in order to induce fusion, this repulsion must be overcome. Background Art Scientists have sought a method for inducing controlled fusion reactions for decades. At this time, at least four major methods have been proposed and are being studied. The first method, magnetic confinement, requires the creation of high temperature plasmas in a confined electromagnetic field in order to overcome the electrostatic repulsion between deuterium nuclei to cause them to fuse. The second method, inertial confinement, attempts to overcome the electrostatic repulsion between deuterium nuclei by simultaneously compressing a deuterium cluster from all directions with powerful laser beams. The third method, muon-assisted fusion, involves thδ use of muon particles to assist deuterium fusion. Magnetic confinement and inertial confinement fusions require very high energies or extremely expensive equipment. However, the fourth method, electrochemically-assisted "cold fusion", appears to require only readily available materials and relatively inexpensive equipment. Electrochemically-assisted "cold fusion" has been attributed to deuterium-deuterium or deuterium-hydrogen fusion within a metal's crystal lattice. In this application, the term "metal" shall be deemed to mean and include metals and alloys that absorb hydrogen and its isotopes. A deuteride is a compound with deuterium and a tritide is a compound with tritium. The term "elevated temperatures" shall mean above ambient temperatures, say 20 degrees Celsius. Metals usually form crystal lattices in which the nuclei of the metals are packed closely together. The crystal lattice of a metal also can have two or more phases, depending on such factors as temperature, pressure and impurities. Hydrogen, including its heavy isotopes deuterium and tritium, can diffuse into the interstices of the crystal lattice. Further, if a suitable potential is applied to the crystal lattice, the diffusion of deuterium can be enhanced so that extremely high effective pressures or activities of deuterium can be obtained in the crystal lattice. The relationship between the applied voltage and the effective pressure or activity of the deuterium within the crystal lattice can be calculated using the Nernst equation. If the effective pressure or activity of the deuterium is sufficiently great, the deuterium nuclei may undergo fusion or some other nuclear process and produce excess heat. Pons and Fleischmann claim to hcve achieved electrochemical-fusion by immersing a palladium electrode in heavy water with a supporting electrolyte, lithium deuteroxide (LiOD), and then using electrolysis to dissociate the heavy water. See "Electrochemically Induced Nuclear Fusion of Deuterium," J. Electroanal. Che . 261 (1989) 301-308, and more recently, in the same journal 287 (1990) 293-348. However, the Pons and Fleischmann method of electrochemical fusion has several disadvantages. First, Pons and Fleischmann employed an aqueous solution, which limits the usefulness of their invention to a temperature range below the boiling point of water (approximately 100 degrees Celsius at 1 atmosphere pressure). This low-temperature operation leads to low efficiency in commercial applications. Second, the Pons and Fleischmann invention requires the use of expensive materials such as Pd and its alloys because the aqueous solution will result in an oxide film on almost all other host metals. This oxide film will normally impede diffusion of the deuterium into the metal. Accordingly, the host metal must be a noble metal that will not form diffusion-impeding oxide films in the presence of water or oxygen. Third, Pons and Fleischmann used a negative Pd electrode which will cause positive deuterium ions and positive alkali ions to migrate to the negative Pd electrode to form alloys with Pd and impede diffusion of the deuterium into the metal. Fourth, the Pons and Fleischmann invention dissociates its solvent, heavy water, and therefore requires substantial amounts of solvent in order to function, unless recombined. Fifth, the Pons and Fleischmann invention creates substantial amounts of deuterium and oxygen gas, thereby creating a danger of a chemical explosion. Sixth, the Pons and Fleischmann invention might not work efficiently with metals including palladium. At the temperatures employed by Pons and Fleischmann, palladium has two single crystalline phases. However, at elevated temperatures, Pd as well as many other metals have only one crystalline phase. Each crystalline phase has a different packing density and atomic arrangement and it is therefore unlikely that fusion or other possible nuclear processes will take place under the same conditions for the different crystalline phases. Thus, having multiple crystalline phases might reduce the efficiency of any nuclear reaction that was induced. Attempts to achieve electrochemical fusion, as claimed by Pons and Fleischmann, have reportedly been unable to detect fusion by-products consistently. The present inventors are unable to determine whether their invention employs fusion or some other reaction or principle. Accordingly, the present inventors describe their invention only as relating to a "nuclear process"; the determination of the theory of the reaction taking place is left to others. It is therefore an object of this invention to provide an electrochemical method of inducing a nuclear reaction at a temperature that will be commercially useful for power generation. It is a further object of this invention to provide such a method that will avoid the formation of diffusion-impeding oxide films on the host metal. It is a further object of this invention to provide such a method that will enable operation at a temperature sufficiently high that the host metal is in a single phase. It is a still further object of this invention to provide such a method that will use negatively charged deuterium ions. It is a still further object of this invention to provide such a method that will not dissociate the solvent of the electrolyte. It is a still further object of this invention to provide such a method that will employ inexpensive materials. It is a still further object of this invention to provide such a method that will not generate oxygen so that the risk of a chemical explosion may be avoided. It is a still further object of this invention to provide a recycling system for deuterium and lithium. Disclosure of Invention These and other objects are achieved by dissolving a hydrogen isotope-containing component capable of providing a source of a hydrogen isotope (preferably an alkali deuteride) into a substantially non-aqueous molten salt to form an electrolytic solution, immersing a metal into the electrolytic solution and then applying a sufficiently high electrical potential and current density to the metal and the electrolytic solution to dissociate the alkali deuteride and to force sufficient amounts of deuterium into the metal at sufficient pressures to increase the activity of the deuterium and to initiate the nuclear reaction. Using a liquid salt avoids oxidation of the host metal because of the lack of oxygen and also provides an extremely reducing environment that eliminates any oxides that may form on the metal's surface. Use of a liquid salt also permits a wide range of working temperatures, depending on the particular salt selected. For example, a salt could be selected that was solid at room temperature, but would melt at operating temperatures. The avoidance and elimination of oxidation allows the use of many different metals because no oxide film will impede diffusion of the deuterium into the metal. Thus, less expensive metals can be used. The lack of oxygen also avoids the possibility of a chemical explosion from accumulated oxygen with hydrogen and its isotopes. The ability to use a higher temperature allows the generation of heat at commercially valuable temperatures ar. i also enhances deuterium diffusion into the metal. It als^ allows operation at a temperature in which the host metai . - in a single phase. Because the source for deuterium is the alkali deuter. :•< dissolved in the liquid salt, the salt can be selected s that dissociation of the alkali deuteride will not dissociate the salt. Further, the dissociation potently, the alkali deuteride (preferably lithium deuteride) is * ■ lower than the dissociation potential of heavy water. Therefore, the power required for the electrolysis is reduced substantially. Brief Description of the Drawings Figure 1 is a schematic view of an apparatus according to this invention. Figure 2 is a cross sectional view of the apparatus in Figure 1 through the line 2-2. Figure 3 is a schematic view of an improved mass and energy flow arrangement according to this invention incorporating a lithium deuteride recycling system. Figure 4 is a schematic diagram of the lithium deuteride recycling system incorporated into the electrolysis cell. Best Mode for Carrying Out the Invention Referring to Figure 1, a crucible 10 (preferably aluminum) is filled with a eutectic lithium chloride- potassium chloride (LiCl-KCl) salt and heated above 350 degrees Celsius (and preferably between 370 and 400 degree Celsius) in an inert gas environment (preferably argon or helium) at atmospheric pressure or greater to form a molten salt solution. Alternatively, the salt could be heated in an evacuated environment or in a deuterium environment. Sufficient alkali deuteride (preferably lithium deuteride ( iD)) is then dissolved into the molten salt to form a saturated electrolytic solution 12. However, the solution is not required to be saturated and is expected to be unsaturated under operating conditions. A positive electrode 14 made of a transition metal, preferably palladium, which has been thermally annealed (preferably torched and remelted), is immersed in the electrolytic solution 12, as is a negative electrode 16, preferably made of aluminum. At the preferred temperature, the palladium positive electrode 14 will be in a single phase during reaction. 2 A constant current density (preferably 200 milliamps/cm or higher) is passed at a sufficiently high rate between the electrodes 14 and 16 to dissociate the lithium deuteride and to increase the activity of the deuterium in the positive electrode 14 so that a nuclear reaction takes place. Experimental results indicate that reaction takes place at 1.8 volts or higher. The experiments have been reproduced, but not consistently. The preferred salt for the practice of this invention is a lithium chloride-potassium chloride eutectic molten salt, the preferred electrolyte is lithium deuteride and the preferred host metal is palladium, as indicated above. However, other salts and other alkali deuterides may be employed in the practice of this invention, as may other metals. For example, the molten salt could be an organometallic salt, an alkali halide, or an alkali hydroxide, and their mixtures. The alkali deuteride could be lithium deuteride, sodium deuteride or potassium deuteride. Alternatively, alkaline earth metal (Group IIA) deuterides (such as magnesium deuteride, calcium deuteride, or strontium deuteride) or Group IIIA metal deuterides (such as aluminum deuteride) could be employed. The metal also could be a transition metal, such as titanium, palladium, vanadium, tantalum, niobium, zirconium, hafnium, nickel, iron, or cobalt, and their alloys, and intermetallics based on the lanthanum and actinium series. Many of the advantages of using a molten salt solution in forcing hydrogen into a metal lattice are described and discussed in the article entitled "Controlled Electrolyte Environments and Their Use For Studying and Modifying Materials Properties: Potentials for Employment in Practical Devices," Solid State Ionics 28-30 (1988) 1078-1083. RECYCLING SYSTEM A problem that arises with use of the cell structure depicted in Fig. 1 is that deuterium gas evolved from the palladium anode escapes. Further, lithium is depleted from the system and combines with the aluminum cathode to form Li Al (nominally "LiAl"), which is a by-product of no further use in this application. These reactions make the system discontinuous because it runs down relatively quickly; it is anticipated that the system would run down in a matter of hours or days instead of months or years. This also results in a low efficiency in the use of LiD electrolyte and adds to the cost of the system. Accordingly, it would be desirable to provide some type of recycling system for the deuterium gas and lithium. Figure 3 shows a schematic mass and energy flow chart for a lithium and deuterium recycling system. This recycling is preferably achieved by using tungsten, molybdenum, nickel or iron for the cathode, preferably molybdenum. These metals do not form compounds with lithium and also have very limited solubilities for lithium, so that the lithium will plate on the surface. As indicated above, the excess heat from the fusion cell is used to generate useful electricity. Some of this electricity is used by the cell for electrolysis of the lithium deuteride solution. Unused deuterium- gas evolves from the palladium electrode and, because the cell's temperature is higher than the melting point of lithium, liquid lithium plates on the cathode. The deuterium gas and liquid lithium are recombined to form lithium deuteride. This recombination should release additional heat due to the negative enthalpy of formation and could be used for additional power generation. The lithium deuteride then is recycled through the fusion cell. A separate deuterium gas supply is preferred in order to insure proper formation of lithium deuteride because deuterium will be consumed in the reaction creating excess heat. Figure 4 shows a cell similar to the cell shown in Figure 1, with a lithium and deuterium recycling system. As is the case in Figure 1, a crucible 20 (preferably of the same material as the cathode, namely molybdenum) is filled with a lithium chloride-potassium chloride (LiCl-KCl) eutectic salt and initially heated by a heating element 24 above 350 degrees Celsius (and preferably between 370 and 400 degrees Celsius) in an inert gas environment (preferably argon or helium) at atmospheric, pressure or greater to form a molten salt solution. A similar system using pure deuterium gas or an evacuated environment can also be employed. Sufficient lithium deuteride (LiD) is dissolved into the molten salt to form a saturated electrolytic solution 22. A positive electrode 26 preferably made of torched and annealed palladium, but having a significant horizontal extent, is immersed in the electrolytic solution 22. A negative electrode 30, comprising a metallic sponge (to present a large reaction surface) made of a metal that does not form alloys with lithium and has little lithium solubility, such as tungsten, molybdenum, nickel or iron (and preferably molybdenum) is also immersed in the electrolytic solution but spaced apart from and above the positive electrode. The negative electrode 30 is approximately horizontally coextensive with the interior of the crucible 20. The positive electrode 26 should be electrically isolated from the rest of the cell. In operation, excess deuterium D~ that does not react with the positive electrode 26 bubbles upwards into the negative electrode 30. Simultaneously, lithium Li that has been dissociated from the lithium deuteride plates onto the negative electrode 30 and is held in its absorbent structure. The electrochemically-generated deuterium D- gas that is not incorporated into the host lattice then reacts with the lithium Li to form lithium deuteride LiD, which redissolves into the electrolytic solution 22. Preferably, a source of additional deuterium S is provided below the negative electrode 30 to react with the lithium Li in the negative electrode 30. Any lithium Li that does not react with deuterium D 2 gas in the negative electrode 30 will float to the surface as a liquid because the electrolytic solution 22 is heated above lithium's melting point. Excess deuterium or deuterium from the source S then can react with the lithium Li floating on the surface of the electrolytic solution 22. It is anticipated that this recycling system would increase the lifetime of a system by at least one, and perhaps more, orders of magnitude. TORCHED PALLADIUM It is preferable that the palladium used in the cell be torched palladium which has a very porous structure. It appears to be much more effective than other forms of palladium. Any other means to prepare such a porous structure may be obvious in this application and may be usable as well. 1 Industrial Applicability The apparatus and process of this invention have a wide range of applications. In the utility industry, these applications include electric power generation, dwelling 5 heating, and self-sustaining power generation for remote areas. In the manufacturing and processing industries, the applications could include chemical production and materials production. In transportation, the applications could include vehicles, such as cars, trains, buses, trucks, 10 ships, and aircraft. Other applications are limited only by the imagination. It will be apparent to those skilled in the art that many modifications may be made without departing from the scope and spirit of this invention. The term "transition 15 metals" shall include transition metals and their alloys and also shall include elements in the lanthanum and actinium series and intermetallics based thereon. The term "molten salt" shall mean and include mixtures of salts. The invention has been described only with respect to single 20. preferred embodiment and no limitation is to be implied or inferred except as may be set forth in the appended claims.

Claims: CLAIMS What is claimed is: 1. A process for inducing nuclear reactions at temperatures above ambient temperature, comprising: applying an electrical potential and current density to an electrolytic solution having a hydrogen isotope- containing component capable of providing a source of a hydrogen isotope and a metal, by applying an electrical potential and current density to said metal and solution to diffuse the hydrogen isotope into the metal to initiate the nuclear reaction; and enhancing the rate of diffusion and activity of said hydrogen isotope by minimizing oxide formation on the metal. 2. A process for effecting enhanced diffusion and dissolution of deuterium into a metal using electrochemically assisted means, comprising: dissolving an alkali deuteride into a substantially non- aqueous molten salt to form an electrolytic solution; immersing a metal in said electrolytic solution; and applying a sufficiently high electrical potential and current density to said metal and said electrolytic solution to enhance the diffusion and dissolution of deuterium into said metal and activity of said deuterium in said metal. 3. A process as in claim 2 wherein the metal is selected from the group consisting of transition metals and their alloys. 4. A process as in claim 3, wherein said transition metal is torched palladium having a porous structure. 5. A process as in claim 2, wherein said alkali deuteride is lithium deuteride. 6. An electrolytic cell comprising: a substantially non-aqueous molten salt; an alkali deuteride dissolved in said salt to form an electrolytic solution; a metal immersed in said electrolytic solution; -nd means for applying an electrical potential and current density to said metal and said electrolytic solution. 7. A cell as in claim 6 wherein said metal is selected from the group consisting of transition metals and their alloys. 8. A process for electrochemically-assisted nuclear reaction,comprising: dissolving an alkali deuteride into a substantially non- aqueous liquid salt to form an electrolytic solution; immersing a metal in said electrolytic solution; and applying a sufficiently high electrical potential and current density to said metal and said electrolytic solution to diffuse sufficient amounts of deuterium into said metal at sufficient activity to initiate the nuclear reaction. 9. A process for electrochemically-assisted nuclear reaction, comprising: dissolving an alkali earth metal deuteride into a substantially non-aqueous liquid salt to form an electrolytic solution; immersing a metal in said electrolytic solution; and applying a sufficiently high electrical potential and current density to said metal and said electrolytic solution to diffuse sufficient amounts of deuterium into said metal at sufficient activity to initiate the nuclear reaction. 10. A process for electrochemically-assisted nuclear reaction ,comprising: dissolving a Group IIIA metal deuteride into a substantially non-aqueous liquid salt to form an electrolytic solution; immersing a metal in said electrolytic solution; and applying a sufficiently high electrical potential and current density to said metal and said electrolytic solution to diffuse sufficient amounts of deuterium into said metal at sufficient activity to initiate the nuclear reaction. 11. A process for electrochemically-assisted nuclear reaction, comprising: dissolving an alkali tritide into a substantially non- aqueous liquid salt to form an electrolytic solution; immersing a metal in said electrolytic solution; and applying a sufficiently high electrical potential and current density to said metal and said electrolytic solution to diffuse sufficient amounts of tritium into said metal at sufficient activity to initiate the nuclear reaction. 12. A process for electrochemically-assisted nuclear reaction, comprising: dissolving an alkali earth metal tritide into a substantially non-aqueous liquid salt to form an electrolytic solution; immersing a metal in said electrolytic solution; and applying a sufficiently high electrical potential and current density to said metal and said electrolytic solution to diffuse sufficient amounts of tritium into said metal at sufficient activity to initiate the nuclear reaction. 13. A process for electrochemically-assisted nuclear reaction, comprising: dissolving a Group IIIA metal tritide into a substantially non-aqueous liquid salt to form an electrolytic solution; immersing a metal in said electrolytic solution; and applying a sufficiently high electrical potential and current density to said metal and said electrolytic solution to diffuse sufficient amounts of tritium into said metal at sufficient activity to initiate the nuclear reaction. 14. A process as in any one of claims 8 to 13, wherein said substantially non-aqueous liquid salt comprises a molten salt. 15. A process as in claim 14, wherein said molten salt is selected from the group consisting of organo etallic salts, alkali halides, alkali hydroxides and mixtures of them. 16. A process as in any one of claims 8 to 13 wherein said metal is selected from the group consisting of transition metals and their alloys. 17. A process as in claim 16 wherein said transition metal is selected from the group consisting of titanium, palladium, vanadium, tantalum, niobium, zirconium, nickel, cobalt, iron and their alloys. 18. A process as in claim 8, wherein: said applying step dissociates said alkali deuteride into an alkali and deuterium gas; wherein only a diffused portion of said deuterium gas initiates said nuclear reaction leaving a remaining portion of said deuterium gas which evolves out of said solution; and wherein said alkali accumulates in said solution; further comprising: reacting said alkali with said remaining deuterium gas and with additional deuterium gas to form an alkali deuteride; and dissolving said alkali deuteride into said electrolytic 0 solution to recycle said alkali and said deuterium. 19. A process as in claim 18, wherein said alkali is lithium. 20. A process as in claim 19, wherein said salt is a lithium chloride-potassium chloride eutectic salt heated 5 above 350 degrees Celsius. 21. A process as in claim 20, wherein said metal is palladium. 22. A process as in claim 21, wherein said palladium is torched palladium having a porous structure. o 23. A process as in claim 22, wherein said electrical potential is at least 1.8 volts and said current density is at least 200 milliamps per square centimeter. 24. An electrolytic cell having a recycling system, comprising: 5 a crucible; an inert gas contained in said crucible providing an inert gas atmosphere; a substantially non-aqueous molten salt melted in said crucible in said inert gas atmosphere; 0 an alkali deuteride dissolved in said salt to form an electrolytic solution; a first electrode comprising a metal selected from the group consisting of tungsten, molybdenum, nickel, iron and their alloys, immersed in said electrolytic solution; 5 a second electrode comprising a metal selected from the group consisting of palladium, titanium, tantalum, vanadium, nickel, niobium, iron, cobalt, zirconium, and their alloys, immersed in said electrolytic solution; and means for applying an electrical potential and current density to said electrodes and said electrolytic solution, whereby: said alkali deuteride is electrolyzed into an alkali and deuterium, whereby: a diffused portion of said deuterium is diffused into said second electrode to generate excess heat; a remaining portion of said deuterium is evolved as deuterium gas; and said alkali is deposited onto said first electrode; a source of additional deuterium gas; means for combining said remaining deuterium gas and said additional deuterium gas with said alkali to form an alkali deuteride; and means for dissolving said alkali deuteride into said electrolytic solution. 25. A cell as in claim 24 wherein said alkali is lithium. 26. A cell as in claim 24, wherein said first electrode comprises molybdenum. 27. A cell as in claim 24, wherein said second electrode comprises palladium. 28. A cell as in claim 27, wherein said palladium is • torched palladium having a porous structure. 29. An electrolytic cell, comprising: a molybdenum crucible; a lithium chloride-potassium chloride eutectic salt in said crucible, wherein said salt has been heated above 350 degrees Celsius to form a molten salt; sufficient amounts of lithium deuteride dissolved into said molten salt to form an electrolytic solution; a positive electrode comprising torched and remelted palladium immersed in said electrolytic solution; a negative electrode comprising molybdenum immersed in said electrolytic solution and spaced apart from said first electrode; a source of electrical current density and voltage capable of applying a current density of at least 200 milliamps per square centimeter at a voltage of at least 1.8 volts between said first and second electrodes; whereby said electrical current density and voltage dissociate said lithium deuteride into lithium and deuterium; whereby a diffused portion of said deuterium diffuses into said palladium in said positive electrode and a remaining portion of said deuterium evolves as deuterium gas at said positive electrode; whereby said lithium is deposited as liquid lithium metal at said negative electrode and floats to said surface; means for combining said liquid lithium metal and said remaining portion of said deuterium gas to create recycled lithium deuteride; and means for introducing said recycled lithium deuteride into said electrolytic solution. 30. An electrolytic cell, comprising: a crucible; a heat source for heating said crucible; a lithium chloride-potassium chloride eutectic salt in said crucible, wherein said salt has been heated by said heat source above 350 degrees Celsius to form a molten salt; sufficient amounts of lithium deuteride dissolved into said molten salt to form an electrolytic solution; a negative electrode comprising porous molybdenum immersed in said electrolytic solution; a positive electrode comprising torched and remelted palladium immersed in said electrolytic solution underneath said negative electrode; a source of electrical current density and voltage capable of applying a current density of at least 200 milliamps per square centimeter at a voltage of at least 1.8 volts between said positive and negative electrodes; whereby said electrical current density and voltage dissociate said lithium deuteride into lithium and deuterium; whereby a diffused portion of said deuterium diffuses into said palladium in said positive electrode and a remaining portion of said deuterium evolves into unused deuterium gas bubbles at said positive electrode and said unused deuterium gas bubbles float upwards into said negative electrode; whereby said lithium is deposited as liquid lithium metal in said negative electrode; whereby said unused deuterium gas reacts with said liquid lithium metal to form recycled lithium deuteride and whereby said recycled lithium deuteride dissolves into said electrolytic solution. 31. An electrolytic cell, according to claim 29 or 30, wherein said salt is heated in an inert gas environmen . 32. An electrolytic cell, according to claim 31, wherein said environment is at least at atmospheric pressure. 33. An electrolytic cell, according to claim 31, wherein said environment is below atmospheric pressure. 34. An electrolytic cell, according to claim 29 or 30, wherein said salt is heated in a deuterium environment. 35. An electrolytic cell, according to claim 34 wherein said environment is at least at atmospheric pressure. 36. An electrolytic cell, according to claim 34, wherein said environment is below atmospheric pressure. 37. An electrolytic cell, according to claim 29 or 30, wherein said salt is heated in an evacuated environment. 38. An electrolytic cell, according to claim 29 or 30, further comprising: means for introducing additional deuterium gas below the surface of said electrolytic solution whereby additional deuterium gas bubbles to the surface of said electrolytic solution. 39. An electrolytic cell, according to claim 38, wherein said solution is an unsaturated electrolytic solution. 40. An electrolytic cell, according to claim 38, wherein said solution is a saturated electrolytic solution.

Inventors: LIAW BOR YANN, LIEBERT BRUCE E, LIAW, BOR, YANN, LIEBERT, BRUCE, E.
Applicants: UNIV HAWAII, UNIVERSITY OF HAWAII
Application year: 1990
Main classification: G21B1
IPC codes: G21B3