Patent Application
20060183008
The present invention relates to liquid fuel compositions for use in electrochemical fuel cells, a method of producing electricity with the fuel compositions, and a fuel cell using the fuel compositions to generate electricity.
A fuel cell is a device that converts the energy of a chemical reaction into electricity. Amongst the advantages that fuel cells have over other sources of electrical energy are high efficiency and environmental friendliness. Although fuel cells are increasingly gaining acceptance as electrical power sources, there are technical difficulties that prevent the widespread use of fuel cells in many applications.
A fuel cell produces electricity by bringing a fuel and an oxidant in contact with a catalytic anode and a catalytic cathode, respectively. When in contact with the anode, the fuel is catalytically oxidized on the catalyst, producing electrons and protons. The electrons travel from the anode to the cathode through an electrical circuit connected between the electrodes. The protons pass through an electrolyte with which both the anode and the cathode are in contact. Simultaneously, the oxidant is catalytically reduced at the cathode, consuming the electrons and the protons generated at the anode.
A common type of fuel cell uses hydrogen as a fuel and oxygen as an oxidant. Specifically, hydrogen is oxidized at the anode, releasing protons and electrons as shown in equation 1:
H2→2H++2e− (1)
The protons pass through an electrolyte towards the cathode. The electrons travel from the anode, through an electrical load and to the cathode. At the cathode, the oxygen is reduced, combining with electrons and protons produced from the hydrogen to form water as shown in equation 2:
½O2+2H++2e−→H2O (2)
Although fuel cells using hydrogen as a fuel are simple, clean and efficient the extreme flammability and the bulky high-pressure tanks necessary for storage and transport of hydrogen mean that hydrogen powered fuel cells are inappropriate for many applications.
In general, the storage, handling and transport of liquids is simpler than of gases. Thus liquid fuels have been proposed for use in fuel cells. Methods have been developed for converting liquid fuels such as methanol into hydrogen, in situ. These methods are not simple, requiring a fuel pre-processing stage and a complex fuel regulation system.
Fuel cells that directly oxidize liquid fuels are the solution for this problem. Since the fuel is directly fed into the fuel cell, direct liquid-feed fuel cells are generally simple. Most commonly, methanol has been used as the fuel in these types of cells, as it is cheap, available from diverse sources and has a high specific energy (5025 Wh/kg).
In direct-feed methanol fuel cells, the methanol is catalytically oxidized at the anode producing electrons, protons and carbon monoxide, equation 3:
CH3OH→CO+4H++4e− (3)
Carbon monoxide tightly binds to the catalytic sites on the anode. The number of available sites for further oxidation is reduced, reducing power output. One solution is to use anode catalysts which are less susceptible to CO adsorption, such as platinum/ruthenium alloys.
Another solution has been to introduce the fuel into the cell as an “anolyte”, a mixture of methanol with an aqueous liquid electrolyte. The methanol reacts with water at the anode to produce carbon dioxide and hydrogen ions, equation 4:
CH3OH+H2O→6H++CO2+6e− (4)
In fuel cells that use anolytes, the composition of the anolyte is an important design consideration. The anolyte must have both a high electrical conductivity and high ionic mobility at the optimal fuel concentration. Acidic solutions are most commonly used. Unfortunately, acidic anolytes are most efficient at relatively high temperatures, temperatures at which the acidity can to passivate or destroy the anode. Anolytes with a pH close to 7 are anode-friendly, but have an electrical conductivity that is too low for efficient electricity generation. Consequently, most prior art direct methanol fuel cells use solid polymer electrolyte (SPE) membranes.
In a cell using SPE membrane, the cathode is exposed to oxygen in the air and is separated from the anode by a proton exchange membrane that acts both as an electrolyte and as a physical barrier preventing leakage from the anode compartment wherein the liquid anolyte is contained. One membrane commonly used as a fuel cell solid electrolyte is a perfluorocarbon material sold by E. I. DuPont de Nemours of Wilmington, Del. under the trademark “Nafion.” Fuel cells using SPE membranes have a higher power density and longer operating lifetimes compared to other anolyte based cells. One disadvantage SPE membrane fuel cells have arises from the tendency of methanol to diffuse through the membrane. As a result, much methanol is not utilized for generation of electricity but is lost through evaporation. In addition, if the methanol comes in contact with the cathode, a “short-circuit” occurs as the methanol is oxidized directly on the cathode, generating heat instead of electricity. Further, depending upon the nature of the cathode catalyst and of the oxidant, catalyst poisoning or cathode sintering often occurs.
The diffusion problem is overcome by using anolytes with a low (up to 5%) methanol content. The low methanol content limits the efficiency of the fuel cell as the methanol diffusion rate limits electrical output. Efficiency is also limited when measured in terms of electrical output as a function of volume of fuel consumed and raises issues of fuel transportation, dead weight and waste disposal.
Lastly, despite a high specific energy, methanol is rather unreactive. As a result, the performance of direct-feed liquid methanol fuel cells is limited to about 5 mWcm−2.
An alternative fuel to consider is one composed of hydrogen-containing compounds with a high reduction potential such as metal hydrides, hydrazine and hydrazine derivatives. Such compounds have a high specific energy and are highly reactive. One such compound is NaBH4. In water, NaBH4 dissociates to give BH4−. In a neutral solution BH4− is oxidized at the anode according to equation 5:
BH4−+2H2O→BO2−+8H++8 e− (5)
The greatest drawbacks of hydrogen-containing compounds with a high reduction potential as fuel is the spontaneous decomposition of these compounds in acidic and neutral solutions, equation 6:
BH4−+2H2O→BO2−+4H2 (6)
In a basic solution BH4− is oxidized at the anode according to equation 7:
BH4−+8OH−→BO2−+6H2O+8 e− (7)
Although stable in basic solutions, BH4− decomposes on contact with a catalyst, such as found on the anode of a fuel cell, even when the circuit is broken.
There is a need for a liquid fuel composition for fuel cells that can produce high power and is stable in contact with the catalytic anode when the electrochemical circuit is broken.
The above and other objectives are achieved by the innovative fuel composition provided by the invention. The fuel composition is made up of a combination of a primary fuel and an auxiliary fuel. The primary fuel is a mixture of one or more compounds, of which at least one is a surface-active compound, most preferably an alcohol such as methanol. Preferably, the primary fuel includes at least one compound from amongst CH4O, C2H6O, C3H8O, C4H10O, C5H12O, C6H14O, ethylene glycol and glycerine. The auxiliary fuel is a reducing compound that is, a compound with a standard reduction potential more negative than the reduction potential of hydrogen gas. Compounds suitable for use as components of the auxiliary fuel of the present invention include hydrides, formates (COOH1−), thiosulfates (S2O32−), sulfites (SO32−), phosphates (PO33−), and hypophosphites (PO23−). Exceptionally suitable compounds include LiAlH4, NaBH4, LiBH4, (CH3)3NHBH3, NaAlH4, NaCNBH3, CaH2, LiH, NaH, KH, Na2S2O3, Na2SO3, Na2HPO3, Na2HPO2, K2S2O3, K2SO3, K2HPO3, K2HPO2, NaCOOH and KCOOH.
According to a feature of the present invention, the fuel composition includes an additional compound, for example, a stabilizing agent.
The invention further provides the fuel composition as an “anolyte” where the electrolyte component of the fuel composition has a pH above 7, preferably above 8 and is most preferably an aqueous solution of an alkali metal hydroxide such as KOH.
According to a feature of the present invention the concentration of the alkali metal hydroxide in the electrolyte is between about 3 M and about 12 M, most preferably substantially 6 M.
According to a further feature of the present invention, the fuel composition includes between 2 weight percent and 60 weight percent of the primary fuel and between 1 weight percent and saturation of the auxiliary fuel.
The invention further provides a fuel cell for the generation of electrical power, made up of an anode, a cathode, and a fuel composition as described herein.
Still further, the invention provides a method of producing electricity through the steps of providing a fuel cell with an anode, a cathode and a fuel composition as described herein, bringing the fuel composition in contact with the anode, oxidizing the fuel composition, and obtaining electricity from the fuel cell.
The invention is herein described, by way of example only, with reference to the accompanying drawings, where:
a is a graph showing experimental results of current as a function of time generated by a cell as in
b is a graph showing experimental results of current as a function of time generated by a cell as in
The fuel composition provided by the present invention is a liquid and is made up of at least two components: a primary fuel and an auxiliary fuel.
The primary fuel is composed of a mixture of one or more compounds, of which at least one is a surface-active compound, most preferably an alcohol such as methanol.
The auxiliary fuel is made up of one or more reducing compounds. By reducing compound is meant a compound with a standard reduction potential more negative than the reduction potential of hydrogen gas. A table of such compounds is found, for example, on pp. 8-22 to 8-23 in “Handbook of Chemistry and Physics, 71st edition” D. R. Lide, Ed., CRC Press, Inc., Boca Raton (1990) which is included by way of reference as if fully set forth herein.
Amongst the most preferable compounds are those described in co-pending U.S. patent application Ser. No. 09/752,551. In U.S. Ser. No. 09/752,551 is taught the use of hydrogen containing compounds with a high reduction potential, that is to say, with a reduction potential greater than that of hydrazine. A compound having a high reduction potential in U.S. Ser. No. 09/752,551 is therefore defined as having a reduction potential such that a thermodynamic reversible potential of an electrochemical cell including that compound at an anode and with an oxygen cathode is greater than or equal to about 1.56 V, 1.56 V being the thermodynamic reversible potential of a hydrazine/oxygen cell (page 593, Bockris, J. O. M. and Srinivasan, S. “Fuel Cells: Their Electrochemistry” McGraw-Hill, Inc., NY (1969)), equation 8:
N2H2+O2→N2+2H2O (8)
Specifically described in U.S. Ser. No. 09/752,551 is the use of metal hydrides such as LiAlH4, NaBH4, LiBH4, (CH3)2NHBH3, NaAlH4, B2H6, NaCNBH3, CaH2, LiH, NaH, KH or sodium bis (2-methoxyethoxo)dihydridaluminate as auxiliary fuels.
Also specifically described in U.S. Ser. No. 09/752,551 is the use of hydrazine and hydrazine derivatives as auxiliary fuels. By hydrazine derivatives is meant compounds having a nitrogen-nitrogen single bond. The purpose of the primary fuel is two-fold, to be a source of electrical energy by undergoing oxidation at the anode and to prevent undesired decomposition of the auxiliary fuel. For the latter function, the primary fuel must have some level of surface activity. As used herein, surface activity is defined as the property of substantially preventing contact between the auxiliary fuel and the catalytic sites of the anode. While not wishing to be held to any theory, it is believed that the primary fuel of the present invention prevents unwanted spontaneous oxidation of the auxiliary fuel when the electrical circuit is open by two mechanisms. The first mechanism is that effective adsorption of molecules of the primary fuel to the anode catalytic sites sterically obstructs access of the auxiliary fuel to the sites, preventing decomposition. The second mechanism is that the molecules of the primary fuel effectively solvate the auxiliary fuel species. As long as a shell of primary fuel molecules surrounds the auxiliary fuel species, it cannot make contact with the anode catalytic sites and does not decompose.
Once the electrical circuit is closed, oxidation of the adsorbed primary fuel molecules commences. The anode catalytic sites become free for access of other species. At least one primary fuel molecule solvating the auxiliary fuel molecule is likely be oxidized before the auxiliary fuel species can approach the catalytic sites of the anode to be oxidized.
Many classes of compounds can be countenanced when selecting the primary fuel for the purpose of being a source of energy, most preferably alcohols. Methanol is a prime candidate due to its availability and high specific energy. For the purpose of adsorption onto the anode catalytic sites, bulkier alcohols or other surface-active compounds can be considered as primary fuels. For instance, isopropanol or glycerol are likely more suitable for this purpose than methanol. For the purpose of auxiliary fuel solvation, the ideal primary fuel is dependent on the identity of the auxiliary fuel.
The compounds making up the auxiliary fuel of the present invention, in contrast to the compounds making up the auxiliary fuel compounds taught in copending U.S. Ser. No. 09/752,551, are selected from reducing compounds, that is compounds with a standard reduction potential more negative than the reduction potential of hydrogen gas. As noted hereinabove, a table of such compounds is found, for example, in the CRC “Handbook of Chemistry and Physics, 71st edition”.
Compounds suitable for use as components of the auxiliary fuel of the present invention include hydrides, formates (COOH1−), thiosulfates (S2O32−), sulfites (SO32−), phosphates (PO33−) and hypophosphites (PO23−). Exceptionally suitable compounds include LiAlH4, NaBH4, LiBH4, (CH3)3NHBH3, NaAlH4, NaCNBH3, CaH2, LiH, NaH, KH, Na2S2O3, Na2SO3, Na2HPO3, Na2HPO2, K2S2O3, K2SO3, K2HPO3, K2HPO2, NaCOOH and KCOOH.
Reducing compounds tend to be unstable and over-reactive in the presence of a fuel cell anode even when the fuel cell circuit is open. When the reducing compounds are found in the presence in solution with the primary fuel of the present invention and thus prevented from contact with the anode catalytic centers, the reducing compounds are stable.
Additionally, the presence of the auxiliary fuel increases the rate of catalytic oxidation of the primary fuel. While not wishing to be held to any theory, it is believed that primary fuel oxidation products such as CO and CO2 are effectively removed from the anode catalytic sites by the oxidation of the auxiliary fuel.
Thus the combination of the primary fuel and the auxiliary fuel of the invention has a synergistic effect on catalytic oxidation in a fuel cell using a fuel composition of the invention.
It is clear to one skilled in the art that there are a number of factors that influence the exact composition of a fuel composition of the invention. Instead of choosing one compound as the primary fuel, a mixture of compounds is often preferred. Similarly, a mixture of compounds is often preferable to form the auxiliary fuel.
Factors to be considered when formulating a fuel composition according to the invention are solubility, stability, safety and factors that arise from the desired qualities of the generated electrical current. Conceivably, additives that are neither primary nor auxiliary fuel can be added to the fuel composition. Additives that stabilize the fuel composition, directly modify the qualities of the generated electricity, modify the solubility of the components so as to indirectly modify the qualities of the electricity generated or in some other way improve the performance of the fuel composition used in a fuel cell, can be used. Engineering issues also dictate the exact composition of the fuel composition: for example, a fuel composition composed of methanol and NaBH4 could contain sodium methoxide as a stabilizing agent.
In one embodiment of the invention, the fuel composition as described above is supplied as an anolyte, that is, an electrolytic liquid is added in addition to the primary and auxiliary fuel. The preferred electrolytic liquid is a basic aqueous solution, preferably of an alkali metal hydroxide, such as KOH (See, for example, Hirchenhofer, J. H., Staufer, D. B. and Engleman, R. R. Fuel Cells—A Handbook (revision 3) DOE/METC-94-1006, January 1994). The alkali metal hydroxide concentration in the anolyte is typically between 2 and 12 M. In the art, 6 M KOH has been shown to be ideal for fuel cell operation at ambient temperatures (see, for example, Appelby, A. J. and Foulkes, F. R., Fuel Cell Handbook, Krieger Publishing, Malabar, Fla. 1993, Chapters 8, 10, 11, 12, 13, 16). The addition of the electrolytic liquid has a positive effect on ion mobility within the anolyte fuel and helps ensure the stability of the auxiliary fuel component of the fuel. When considering the exact composition of the fuel composition of the invention when supplied as an anolyte, factors such as stability and solubility are taken into account.
The principles and operation of a fuel cell and generation of electricity according to the invention may be better understood with reference to the figures and accompanying description.
In
When switch 30 is open, methanol in fuel chamber 22 is adsorbed onto the catalytic sites on anode 20, preventing contact between the BH4− species in fuel composition 24 and the catalytic sites. The methanol also solvates the BH4− species, further isolating the BH4− species from the catalytic sites. When switch 30 is closed, the methane molecules at the catalytic sites are oxidized, clearing the sites for contact with and oxidation of more fuel including BH4− species. Electrons formed by catalytic oxidation of fuel composition 24 are transported through electrical circuit 26 to cathode 14. Simultaneously, protons formed by catalytic oxidation are transported from anode 20, through electrolyte 16 and to cathode 14. At cathode 14, oxidant 12 is reduced by the action of cathode 14 and the electrons coming through circuit 26, and combines with the protons to form water.
In an additional embodiment, appearing in
When switch 60 is open, methanol from fuel composition 52 is adsorbed onto the catalytic sites on anode layer 50, preventing contact between the BH4− species and the catalytic sites. Similarly, the methanol solvates the BH4− species, further isolating the BH4− species. When switch 60 is closed, the methanol molecules at the catalytic sites are oxidized, clearing the catalytic sites for contact with and oxidation of the all fuel components. Electrons formed by catalytic oxidation are transported through electrical circuit 56 to cathode layer 46. Protons formed by the catalytic oxidation are transported through anode layer 50, through electrolyte layer 48 and to cathode layer 46. At cathode layer 46, oxidant 42 is reduced by the action of catalytic cathode layer 46 and the electrons coming through circuit 56, and combines with the protons to form water.
Many other embodiments of the invention can be countenanced. Whereas the embodiments above are described using oxygen from air as an oxidant, with the necessary modifications a liquid oxidant can be used, for example, an organic fluid with a high oxygen concentration (see U.S. Pat. No. 5,185,218) or a hydrogen peroxide solution.
Similarly, the choice of catalyst for anode and cathode construction is not limited to those made of precious metals as in the embodiments described above. (See, for example, Fuel Cell Systems, (eds. Blomen, L. J. M. J and Mugerwa, M. N.), Plenum Press, New York, 1993, Chapter 2: pp. 42-52, 63-69, Chapter 3: pp. 88-97, p. 110, Chapters 7, 8, 11)
A fuel cell, similar to that described in
The current at U=0.5 V was measured as a function of time in a fuel cell as in Example 1, wherein to the methanol/KOH solution 5 weight percent NaBH4 was added. A current of 240±5 mA was measured over 90 minutes. The graph of the measured current as a function is time is presented in
While the invention has been described with respect to a limited number of embodiments, it will be appreciated that many variations, modifications and other applications of the invention may be made.
This is a Divisional of U.S. patent application Ser. No. 10/445,355, which is a Divisional of U.S. patent application Ser. No. 10/162,564 filed on Jun. 6, 2002, which is a continuation in part of U.S. patent application Ser. No. 09/752,551 filed on Jan. 3, 2001.
| Number | Date | Country | |
|---|---|---|---|
| Parent | 10445355 | May 2003 | US |
| Child | 11400175 | Apr 2006 | US |
| Parent | 10162564 | Jun 2002 | US |
| Child | 10445355 | May 2003 | US |
| Number | Date | Country | |
|---|---|---|---|
| Parent | 09752551 | Jan 2001 | US |
| Child | 10162564 | Jun 2002 | US |
