Abstract:
A method and apparatus is disclosed for utilizing sulfur as a consumable fuel in an electrochemical cell. The principal of the above described invention is that sulfur is oxidized or acts as an oxidizing agent to produce energy while avoiding the production of harmful gases and other byproducts, traditionally associated with the burning of sulfur.

Description:
CROSS-REFERENCE TO RELATED APPLICATIONS 
       [0001]    This application claims the benefit of U.S. Provisional Application No. 60/885,642 filed Oct. 31, 2006 in the United States Patent and Trademark Office and U.S. Provisional Application No. 60/899,270 filed Feb. 1, 2007 in the United States Patent and Trademark Office, which are hereby incorporated by reference herein in their entirety, including but not limited to those portions that specifically appear hereinafter, the incorporation by reference being made with the following exception: In the event that any portion of the above-referenced provisional application is inconsistent with this application, this application supercedes said above-referenced provisional application. 
     
    
     STATEMENT REGARDING FEDERALLY SPONSORED RESEARCH OR DEVELOPMENT 
       [0002]    Not Applicable. 
       BACKGROUND 
       [0003]    1. The Field of the Invention 
         [0004]    This disclosure relates generally to the use of sulfur as a consumable fuel in an electrochemical cell. More particularly, this invention produces energy by oxidizing sulfur in the presence of a liquid electrolyte. In the alternative, this invention can be configured to produce energy by using sulfur as the oxidizing agent to oxidize a metal in the presence of a liquid electrolyte. Thus, this invention allows sulfur to be utilized as a consumable fuel while avoiding the harmful gaseous by-products associated with burning sulfur. 
         [0005]    2. Description of Related Art 
         [0006]    The search for an effective utilization of energy sources has been of critical importance to civilization since the beginning of the industrial age. At the present time, most usable energy comes from the following principal sources: solar, in the form of photovoltaic cells and in growing vegetable and other organic matter that is either burned by humans or consumed by living organisms as a primary energy source; nuclear, in which the heat of a controlled nuclear fission reaction is used to generate electricity; and, the burning or “oxidation” of hydrocarbons contained in fossil fuels such as coal and oil. (wind and hydroelectric can also be considered a subcategory of the solar group in that it is the heat produced by solar radiation on the earth&#39;s surface that supplies the energy to drive these processes). 
         [0007]    Of these sources, the burning of fossil fuels is by far the most significant to industrialized societies in terms of the percentage of energy produced and consumed. However, the burning of fossil fuels as the primary energy source for modern civilization possesses severe limitations that include the following. First, the supply of fossil fuels is finite. Thus, as a theoretical matter, fossil fuels will eventually become depleted. Second, the burning of fossil fuels produces deleterious byproducts including carbon dioxide. For example, because carbon dioxide in the atmosphere can theoretically slow the radiation of heat from the earth&#39;s surface, it is thought that an increased level of carbon dioxide in the atmosphere can result in an increase in the mean temperature of the earth&#39;s surface and surrounding atmosphere. Finally, fossil fuels are not distributed evenly throughout the earth&#39;s surface. This uneven distribution of an essential resource is associated with certain social and political dislocations observed in the world today. 
         [0008]    Thus, it would be helpful to industrialized society to discover and utilize an additional energy source, currently existing on earth that can be utilized in place of, or in addition to, the existing energy sources in use today. Most of the elements contained at or below the earth&#39;s surface are not suitable as energy sources. Energy is most readily extracted from an atom or molecule by oxidizing it—usually in the form of burning. As used herein, burning refers to the combination with oxygen in the atmosphere to produce heat. When a molecule is burned, some, or all of its atoms combine with oxygen and, in the process release some of the potential energy contained within the electron bonds of the molecule in the form of heat. 
         [0009]    The problem in finding a new fuel source to replace or supplement hydrocarbons is that most of the elements capable of being oxidized are already in an oxidized state due to their exposure to oxygen in the atmosphere. Hence, elements such as silicon, aluminum, zinc and iron, although plentiful at or near the earth&#39;s surface, already exist primarily in an oxidized state. Because they are already in and oxidized they are not usable as consumable fuels in any type of oxidation/reduction reaction. As used herein, a consumable fuel is defined as and element or compound as to which the following two conditions apply:
       1. The element or compound that yields more energy in an oxidation/reduction reaction than was required to put the element or compound in a state suitable for participating in the oxidation/reduction reaction; and,   2. once the element or compound is utilized in an oxidation reduction reaction, it is not recovered, but rather is discarded.
 
For the purposes of this disclosure, any element or compound which is being used in a manner consistent with these two conditions is being used as a consumable fuel. By way of example, hydrocarbons qualify as consumable fuels under this definition. In their natural state, or with minimal refining, hydrocarbons can take part in oxidation/reduction reactions that yield more energy than was required to put the hydrocarbon in a state suitable for participating in the oxidation/reduction reaction. As a consequence, hydrocarbons are utilized in oxidation/reduction reactions, and the products of these reaction, principally water and carbon dioxide, are generally not recovered but are discarded into the environment.
       
 
         [0012]    In contrast, elements such as silicon aluminum, zinc and iron, although plentiful at or near the earth&#39;s surface, already exist primarily in an oxidized state. Therefore, these elements must be refined in order to put them in a state suitable for participating in an oxidation/reduction reaction. And, the energy necessary to refine these elements is at least as great as or greater than the energy released in their oxidation/reduction reactions. Therefore, while these elements can serve as energy storage media in their refined states, they do not represent consumable fuels as that term is used in this disclosure. 
         [0013]    Of all the oxidizable elements present in large quantities at or near the earth&#39;s surface, sulfur is the only one that exists in relatively large quantities in an unoxidized state. In addition, according to present day geological theory, sulfur is constantly being produced in an unoxidized or “reduced” state by the volcanic activity within the earth. Sulfur is a major product of volcanic eruptions, and is constantly being pumped to the surface through volcanic structures such as volcanic heat vents on the ocean floor. Large deposits of sulfur are also produced by bacterial action where they remain in an unoxidized form. Sulfur also occurs in varying quantities in conjunction with various hydrocarbons such as crude oil and coal. Sulfur dioxide emissions associated with the burning of sulfur containing coal and oils and gas has resulted in mandated removal of sulfur either prior to the burning of the hydrocarbon or after burning via scrubbing of the emissions. Government mandated sulfur removal from fuels has created a glut of sulfur that is presenting increasing disposal problems for oil and gas refiners. This problem will probably become exacerbated as refiners rely more and more on high sulfur content crude oil as supplies of lower sulfur crude oil become depleted. Finally, Sulfur occurs in very large quantities in oil shale regions of the world. For example, it is estimated that the Colorado Plateau region contains approximately 600 billion tons of sulfur. Assuming this sulfur can be economically extracted, it would provide a tremendous source of zero emission energy. Because of these characteristics, sulfur fits the definition of a consumable fuel as defined herein. 
         [0014]    It is well known that sulfur can be readily burned and is thus readily oxidizable in an exothermic reaction. The potential energy it possesses makes it a theoretical source of consumable fuel. The drawback to utilizing sulfur as a consumable fuel in this manner is that the by-products of burning sulfur in the atmosphere are extremely toxic. Burning sulfur produces sulfur dioxide and sulfur trioxide gas, both of which are toxic. When these gases react with water, they produce sulfuric acid, the principal component of acid rain. Because of the harmful byproducts of burning sulfur, it has never qualified as a useful energy source, despite the potential energy it possesses. Thus, it would be desirable to develop a way to release the potential energy in sulfur by oxidizing it without producing the harmful by-products associated with burning it in the atmosphere. Thus, the current invention teaches using sulfur as a consumable fuel by harvesting its energy in an electrochemical oxidation/reduction reaction. 
       SUMMARY 
       [0015]    The current disclosure teaches an effective way to utilize sulfur as a consumable fuel in an electrochemical cell. 
     
    
     
       BRIEF DESCRIPTION OF THE DRAWINGS  
         [0016]    The features and advantages of the disclosure will become apparent from a consideration of the subsequent detailed description presented in connection with the accompanying drawings in which: 
           [0017]      FIG. 1  is an apparatus capable of carrying out a storage battery type oxidation/reduction reaction. 
           [0018]      FIG. 2  is an apparatus capable of carrying out a hydrogen fuel cell oxidation/reduction reaction. 
           [0019]      FIG. 3  is a perspective view of the apparatus comprising an electrochemical cell that utilizes sulfur as a consumable in conjunction with oxygen. 
           [0020]      FIG. 4  is a cross section of one embodiment of a sulfur electrode. 
           [0021]      FIG. 5  is a perspective view an embodiment of a sulfur electrode. 
           [0022]      FIG. 6  is a cross section view of an electrochemical cell that utilizes sulfur as a consumable fuel in an oxidation/reduction reaction with aluminum. 
           [0023]      FIG. 7  is an apparatus that utilizes sulfur as a consumable fuel to produce hydrogen. 
       
    
    
     DETAILED DESCRIPTION  
       [0024]    At the outset, it should be appreciated that like drawing numbers on different views identify identical structure elements of the disclosure. While the present disclosure is described with respect to what is presently considered to be exemplary embodiments, it is understood that the disclosure is not limited to the disclosed embodiments. 
         [0025]    Furthermore, it is understood that this disclosure is not limited to the particular methodology, materials and modifications described and as such may, of course, vary. It is also understood that the terminology used herein is for the purpose of describing particular aspects only, and is not intended to limit the scope of the present disclosure, which is limited only by the appended claims. 
         [0026]    Unless defined otherwise, all technical and scientific terms used herein have the same meaning as commonly understood to one of ordinary skill in the art to which this disclosure belongs. Although any methods, devices or materials similar or equivalent to those described herein can be used in the practice or testing of the disclosure, the preferred methods, devices, and materials are now described. 
         [0027]    As used herein, a consumable fuel is defined as an element or compound as to which the following two conditions apply:
       1. The element or compound that yields more energy in an oxidation/reduction reaction than was required to put the element or compound in a state suitable for participating in the oxidation/reduction reaction; and,   2. once the element or compound is utilized in an oxidation reduction reaction, it is not recovered, but rather is discarded.
 
For the purposes of this disclosure, any element or compound which is being used in a manner consistent with these two conditions is being used as a consumable fuel. By way of example, hydrocarbons qualify as consumable fuels under this definition. In their natural state, or with minimal refining, hydrocarbons can take part in oxidation/reduction reactions that yield more energy than was required to put the hydrocarbon in a state suitable for participating in the oxidation/reduction reaction. As a consequence, hydrocarbons are utilized in oxidation/reduction reactions, and the products of these reaction, principally water and carbon dioxide, are generally not recovered but are discarded into the environment.
       
 
         [0030]    One alternative to burning a fuel in the atmosphere is to oxidize the fuel in an electrochemical cell. It is a well known phenomenon that electrical energy can be produced by the chemical reaction that takes place when a reducing element is combined with an oxidizing element in an oxidation/reduction reaction in an electrochemical cell. Whereas the byproduct of atmospheric oxidation/reductions is heat energy, the byproduct of an electrochemical oxidation/reduction reaction is electric current. 
         [0031]    There are a wide variety of electrochemical cells known in the art. Some of the more common electrochemical cells include what are commonly called storage batteries. Batteries of the Lead/acid, zinc/copper and sodium/sulfur type are some of the more commonly known types of storage batteries.  FIG. 1  is an illustration of an apparatus  2  capable of carrying out an electrochemical reaction of the type that takes place within the average storage battery. 
         [0032]    In the apparatus  2  of  FIG. 1 , a container  4  contains a liquid electrolyte solution  6 . In this case, the liquid electrolyte solution is sulfuric acid having a chemical formula of H2 2+  SO4 2−  dissolved in water. The apparatus  2  has a first electrode  8  comprised of Lead. This first electrode  8  is immersed in the electrolyte solution  6 . The first electrode  8  has an electron conductor  10  whose first end  11  is attached to the first electrode&#39;s  8  upper end  12 . This electron conductor  10  is made of a material that conducts electricity and thus allows the first electrode  8  to be in electrical contact with a second electrode  14  when the second end  16  of the electron conductor  10  is attached to the second electrode  14 . In this instance, the second electrode  14  is comprised of lead oxide. The second electrode  14  is also immersed in the electrolyte solution  6 . The first electrode  8  reacts with the SO4 2−  ions to form PbSO4+2e−. The electrons produced by this reaction travel through the electron conductor  10  to the second electrode  14  where the following reaction takes place PbO2+4H + +SO4 2− +2e − −          PBSO4+H2O. The energy of this reaction drives the electrons that are produce through the electron conductor  10  with a force that allows the electrons to do work on the resistor  18  located at a point along the electron conductor. 
         [0033]    A defining characteristic of Storage batteries of the type depicted in  FIG. 2  is that their energy is stored in their electrodes and/or electrolyte. The materials from which they derive their energy output like lead, originally existed in an oxidized form. Thus, in order to be put into a condition where they could participate in an oxidation/reduction reaction, they had to be refined in a process that requires at least as much energy as they produce in an oxidation/reduction reaction. Once the energy the electrodes store is depleted via the oxidation/reduction reaction that takes place within the storage battery, the storage battery must be either recharged, by introducing sufficient electrical energy to reverse the oxidation/reduction reaction, or thrown away, depending on whether the battery is rechargeable or not. In either case, storage batteries, do not utilize consumable fuel as that term is defined herein. Thus, a storage battery is not an energy source. It is merely an energy storage medium, with the energy that is stored generally coming from nuclear, fossil fuel or hydroelectric driven power plants. 
         [0034]    Another type of electrochemical cell is known as the fuel cell. In a fuel cell, the electrical energy is continually produced by constantly introducing a fuel into the system. The fuel reacts in the presence of an electrolyte in an oxidation/reduction reaction to produce an electric current. 
         [0035]    The most common fuel cell is the hydrogen fuel cell.  FIG. 2  is a depiction of an apparatus  24  capable of carrying out a hydrogen/oxygen fuel cell reaction. In this apparatus  24 , a container  26  contains a liquid electrolyte solution  28 . In this case, the liquid electrolyte solution  28  is sodium hydroxide having a chemical formula of Na +  OH −  dissolved in water. The apparatus  24  has a first electrode  30  comprised of a cylindrical tube  34 , open at both ends and containing stainless steel fibers  36  in its interior. The first electrode  30  is immersed in the electrolyte solution  28  such that the stainless steel fibers  36  are immersed in the electrolyte solution  28 . A hollow tube  38  extends into the electrolyte solution  28  such that its first end  40  extends into the bottom opening  42  of the cylindrical tube  34 . A second end (not shown) of the hollow tube  38  is attached to an oxygen source (not shown) such that the hollow tube  38  channels oxygen from the oxygen source (not shown) into the bottom opening  42  of the cylindrical tube  34 . The oxygen, upon being released into the bottom opening  42  of the cylindrical tube  34  bubbles up through the electrolyte solution  28 , past the stainless steel fiber  36 , such that the oxygen molecules make intermittent contact with the stainless steel fiber  36 . 
         [0036]    The apparatus  24  has a second electrode  46  comprising a cylindrical tube  48 , open at both ends and containing platinum fibers  50  in its interior. The second electrode  46  is immersed in the electrolyte solution  28  such that the platinum fibers  50  are immersed in the electrolyte solution  28 . A hollow tube  52  extends into the electrolyte solution  28  such that its first end  54  extends into the bottom opening  56  of the cylindrical tube  48 . A second end (not shown) of the hollow tube  52  is attached to a hydrogen source (not shown) such that the hollow tube  52  channels hydrogen from the hydrogen source (not shown) into the bottom opening  56  of the cylindrical tube  48 . The hydrogen, upon being released into the bottom opening  56  of the cylindrical tube  48  bubbles up through the electrolyte solution  28 , past the platinum fibers  50 , such that the hydrogen molecules make intermittent contact with the platinum fibers  50 . 
         [0037]    The first electrode  30  has an electron conductor  60  inserted through the top opening  62  of the cylindrical tube  34  such that the electron conductor  60  makes electrical contact with the stainless steel fiber  36 . This electron conductor  60  is made of a material that conducts electricity. A second electron conductor  64  is inserted through the top opening  66  of the cylindrical tube  46  such that the second electron conductor  64  makes electrical contact with the platinum fibers  50 . Both the first electron conductor  60  and the second electron conductor  64  are in electrical contact with a resistor  68 . 
         [0038]    As oxygen is introduced into the first electrode  30  it reacts with the electrolyte solution  28  as it contacts the stainless steel fibers  36  according to the following reaction: O2+2H2O+4e−−          4OH − . The OH −  ions produced by this reaction travel through the electrolyte solution  28  to react with the hydrogen where it contacts the platinum fibers  50  according to the following reaction 2OH+H2           2H2O+2e − . The electrons generated by this reaction travel through the second electron conductor  64  where they do work on a resistor  68 . The electrons then travel through the first electron conductor  60  to the first electrode  30  where they participate in the reaction whereby the oxygen goes into reaction whereby the oxygen goes into solution as OH − . 
         [0039]    Unlike storage batteries, fuel cells do not need to be recharged. A fuel cell is “recharged” by reloading it with fuel. In the apparatus of  FIG. 2 , the fuel is hydrogen. However, hydrogen does not represent a consumable fuel in every instance. Where the hydrogen is derived from a hydrocarbon such as methane, it can constitute a consumable fuel to the extent the energy required to separate the hydrogen from the carbon in the methane molecule is less than the energy produced in the fuel cell reaction. However, where the hydrogen is derived from water, the energy required to liberate the hydrogen from the water is greater than the energy obtained in the reaction. Therefore, hydrogen derived from water does not constitute a consumable fuel. A fuel cell that utilizes a hydrocarbon as a fuel is an example of an electrochemical reaction that utilizes a consumable fuel. 
         [0040]      FIG. 3 , is an illustration of an apparatus that utilizes sulfur as a consumable fuel in an electrochemical reaction.  FIG. 3 , depicts an electrochemical cell  70  comprising a container  72  capable of holding an electrolyte solution  74 . This compartment can be constructed of glass, plastic, fiberglass, rubber, or any other material that will generally not react with the electrolyte solution  74 . The container  72  may also be constructed initially of one or more materials that will generally react with the electrolyte solution  74  so long as the inner surface  76  of the container  72  is lined with a non reactive material. The electrolyte solution  74  can be any ph between 0 and 14. In the embodiment depicted in  FIG. 3 , the electrolyte solution  74  comprises a combination of Na+ OH− and Na+ Cl− dissolved in H2O. Suspended in the electrolyte solution  74  is a first electrode  78 . This first electrode  78  is comprised of elemental sulfur impregnated with one or more other elements or compounds capable of conducting electricity. 
         [0041]      FIG. 4  depicts a cross section view of one embodiment of the first electrode  78 . In this embodiment, the first electrode  78  comprises a core of stainless steel  80 . The core of stainless steel  80  is coated with a mixture comprising elemental sulfur mixed with powdered graphite  82 . Such electrode  78  can be made, among other ways, by melting sulfur and mixing in powdered graphite. The stainless steel core  80  is then dipped into the molten sulfur graphite mixture  82  and then allowed to cool. The sulfur graphite mixture  82  hardens as it cools in the form of a shell of solid sulfur graphite mixture around the stainless steel core  80 . A length of exposed stainless steel  84  exists at one end of the electrode  78  to which is attached a conductor  86 . The core can also be comprised of aluminum steel, iron, copper, zinc, carbon, carbon compound, metal alloy or any metal or other material capable of conducting electricity. While the embodiment depicted in  FIG. 4  utilizes stainless steel, the core can be copper, zinc, aluminum, carbon or carbon nano tubes or any other metal, alloy or material capable of conducting electricity. The electrode can also consist solely of a mixture of graphite and sulfur with no metal or other core. 
         [0042]      FIG. 5  depicts yet another alternative embodiment of the sulfur electrode  78  in which the sulfur electrode  78  is comprised of sulfur which is impregnated with very fine strands of an electron conducting material  90  such as steel, copper, aluminum, steel, zinc, carbon, carbon alloy, carbon nano tubes or any other material capable of both conducting electrons and being formed into thin filaments. Elemental sulfur  92  is located within the sulfur electrode  78  so as to fill all the spaces between the strands of electron conducting material  90 . The sulfur electrode  78  depicted in this embodiment works best as the distance between the strands of electron conducting material  90  approach the width of two sulfur molecules. The sulfur electrode  78  also contains a post  94  that is situated such that a first end  96  is in contact with one or more of the strands of electron conducting material  90 . The second end  98  of the post  94  extends beyond the sulfur electrode  78 . 
         [0043]    The strands of electron conducting material  90  are also situated so that each strand of electron conducting material  90  is in contact with at least one other strand of electron conducting material  90  such that each strand of electron conducting material  90  is ultimately in electrical contact with the post  94 . 
         [0044]    Returning now to  FIG. 3 , the apparatus  70  has a second electrode  100  comprised of a cylindrical tube  102 , open at both ends and containing fibers  104  capable of conducting electrons in its interior. These fibers can be stainless steel, platinum, carbon, or any metal, alloy, compound or other material capable of conducting electricity. The second electrode  100  is immersed in the electrolyte solution  74  such that the fibers  104  are immersed in the electrolyte solution  74 . A hollow tube  108  extends into the electrolyte solution  74  such that its first end  110  extends into the bottom opening  112  of the cylindrical tube  102 . A second end (not shown) of the hollow tube  108  is attached to an oxygen source (not shown) such that the hollow tube  108  channels oxygen from the oxygen source (not shown) into the bottom opening  112  of the cylindrical tube  102 . The oxygen, upon being released into the bottom opening  112  of the cylindrical tube  102  bubbles up through the electrolyte solution  74  past the fibers  104 , such that the oxygen molecules make intermittent contact with the fibers  104 . 
         [0045]    The second electrode can also be in any form and comprise any material known in the art sufficient to ionize oxygen in an electrolyte solution. 
         [0046]    The second electrode  100  is connected to the first electrode  78  via an electron conductor  114 . As oxygen is pumped into the second electrode  100 , electrons  116  travel via the electron conductor  114  to the second electrode  100  where they ionize the oxygen molecules in contact with the second electrode  100  according to the following formula: O2+2H2O+4e−          4OH−. The OH− ions migrate through the electrolyte to combine with the elemental sulfur in the first electrode  78  according to the following reaction S+2OH−−          SO2+H2+2e−. The electrons  116  produced via this reaction travel again through the electron conductor  114 . A resistor  120  is located within path of the electron conductor  114  on which the electrons  116  do work before returning to the second electrode  100 . When the sulfur in the first electrode has been reacted, the first electrode can be replaced. It is also important to note that sulfur in a solid, liquid or gaseous state could be used in conjunction with this electrodes as well as various sulfur compounds. 
         [0047]      FIG. 6  is an illustration of an apparatus that utilizes sulfur as a consumable fuel in an electrochemical reaction to produce electricity and hydrogen. As depicted in  FIG. 6 , the electrochemical cell  130  comprises a container  132  capable of holding an electrolyte solution  134 . This container  132  can be constructed of glass, plastic, fiberglass, rubber, or any other material that will generally not react with the electrolyte solution  134 . The container  132  may also be constructed initially of one or more materials that will generally react with the electrolyte solution  134  so long as the inner surface  136  of the container  132  is lined with a non reactive material. The electrolyte solution  134  can contain be of any ph between 0 and 14. In the embodiment depicted in  FIG. 6 , the electrolyte solution  134  comprises a combination of Na+ OH− and Na+ Cl− dissolved in H2O. Immersed in the electrolyte solution  134  is a first electrode  138 . This first electrode  138  is comprised of sulfur in combination with one or more other elements or compounds capable of conducting electricity. In this embodiment, the first electrode  138  comprises a copper core  140  having an outer coating  142  comprising a mixture of sulfur and powdered graphite. However, the core  140  can also be zinc, steel, lead, aluminum or any other metal, metal alloy or any other material capable of conducting electricity. An electron conductor  144  material extends from the top of the first electrode  146 . While the sulfur in this embodiment is mixed with powdered graphite, the sulfur can be mixed with any material capable of conducting electricity. The apparatus  130  has a second electrode  148  immersed in the electrolyte solution  134  and in electrical contact with the first electrode  146  via the electron conductor  144 . In this embodiment, the second electrode  148  is comprised of aluminum. However, the second electrode  148  can also be comprised of iron, steel, zinc, or any other electron conducting material capable of being oxidized by sulfur. It is also important to note that the electrolyte  134  can have any ph between 0 and 14. 
         [0048]    Without being bound to any single theory, it appears that the reaction at the first electrode involves the ionization of sulfur in the presence of the electrolyte to form one or more forms of Sulfur Hydroxide ions or one or more hydroxide ions containing Sulfur or copper. These ions then react to oxidize the aluminum to form one or more of the Sulfate class of compounds in which one or more sulfur atoms or combination of sulfur and copper atoms are bonded to one or more aluminum atoms. Generally, however, it appears that the principal reaction products are aluminum sulfate, electrical energy and hydrogen. When the sulfur in the first electrode has been reacted, the first electrode can be replace. 
         [0049]    An alternative embodiment of this invention is depicted in  FIG. 7 . In this embodiment, a copper core  160  has a first end  162  that is coated with aluminum  164 . A second end  168 , is coated with sulfur mixed with powdered graphite  170 . The entire electrode  174  is immersed in an electrolyte solution  176  comprising NaCl and NaOH dissolved in H20. The resulting oxidation/reduction reaction of the sulfur and aluminum produces hydrogen gas which bubbles out of the electrolyte solution. While in this embodiment, the electrode  174  comprises a copper core  160 , the core  160  can be comprised of aluminum, iron, steel, zinc or any other metal, alloy or other material capable of conducting electricity. In addition, while the core  160  in this embodiment is coated in part with aluminum, the core  160  can also be coated with zinc, iron, steel or any other metal, alloy or other electricity conducting material capable of being oxidized by sulfur. Finally, while the sulfur in this embodiment is mixed with powdered graphite, the sulfur can be mixed with any material capable of conducting electricity. 
         [0050]    The publications and other reference materials referred to herein to describe the background of the disclosure, and to provide additional detail regarding its practice, are hereby incorporated by reference herein in their entireties, with the following exception: In the event that any portion of said reference materials is inconsistent with this application, this application supercedes said reference materials. The reference materials discussed herein are provided solely for their disclosure prior to the filing date of the present application. Nothing herein is to be construed as a suggestion or admission that the inventors are not entitled to antedate such disclosure by virtue of prior disclosure, or to distinguish the present disclosure from the subject matter disclosed in the reference materials. 
         [0051]    In the foregoing Detailed Description, various features of the present disclosure are grouped together in a single embodiment for the purpose of streamlining the disclosure. This method of disclosure is not to be interpreted as reflecting an intention that the claimed disclosure requires more features than are expressly recited in each claim. Rather, as the following claims reflect, inventive aspects lie in less than all features of a single foregoing disclosed embodiment. Thus, the following claims are hereby incorporated into this Detailed Description of the Disclosure by this reference, with each claim standing on its own as a separate embodiment of the present disclosure. 
         [0052]    It is to be understood that the above-described arrangements are only illustrative of the application of the principles of the present disclosure. Numerous modifications and alternative arrangements may be devised by those skilled in the art without departing from the spirit and scope of the present disclosure and the appended claims are intended to cover such modifications and arrangements. Thus, while the present disclosure has been shown in the drawings and described above with particularity and detail, it will be apparent to those of ordinary skill in the art that numerous modifications, including, but not limited to, variations in size, materials, shape, form, function and manner of operation, assembly and use may be made without departing from the principles and concepts set forth herein.