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Energies 2010, 3 1500 Keywords: alcohol oxidation; oxygen reduction; anion exchange membranes; fuel cells; catalysts; power output 1. Introduction Easy storage and handling, high energy density and wide availability are features that make alcohols attractive liquid fuels for the most promising alternative power sources for transportation, portable electronics and stationary applications. One of the first investigations of alcohol in fuel cells was conducted by Palve in 1954. He demonstrated that methanol acted as a fuel in aqueous electrolytes [1]. Since the development of perfluorinated cation exchange membranes, such as Nafion®(DuPont), proton exchange membranes (PEM) have dominated as the electrolyte for fuel cells. Ethanol [2–7], 2-propanol [8,9], ethylene glycol [10–13] and glycerol [14] have all been considered for fuel cell applications. In direct alcohol fuel cells (DAFCs), alcohol is directly oxidised at the anode in an acidic medium using a proton exchange membrane (PEM). Direct methanol fuel cells are the most advanced and studied systems since methanol, with only one carbon in its molecule and no C-C bonds, is the simplest alcohol. Electrooxidation of methanol is relatively simple compared to other alcohols. However, two major obstacles have restrained the more rapid development and applications of DAFCs, even for methanol systems: Alcohol crossover from the anode to the cathode The relatively low activity and complex reaction mechanism of most alcohols Apart from methanol, it is particularly difficult to break the C-C bond in alcohols during electrochemical oxidation. In addition to these two major issues, the high costs of proton exchange membranes and precious metal catalysts (Pt and Pt/Ru based catalysts), and CO poisoning of Pt catalysts at lower temperature in acidic media have further hampered development of DAFCs. It is known that for many reactions, electrocatalysts perform better in alkaline electrolytes. In fact, one of the first direct methanol fuel cells (DMFCs) developed in 1955 by Justi and Winsel were operated in alkaline media and used porous nickel for the anode and porous nickel-silver for the cathode [1]. A problem with alkaline fuel cells is the carbonation of the solution due to CO2 production of the fuel oxidation and from air: 2OH− + CO2→CO32− + H2O (1) This can cause solid precipitation of carbonate salts on the porous electrode and a pH decrease in the alkaline electrolyte solution [15]. Consequently, it leads to a reduction in reactivity for fuel oxidation in the system [16]. The application of anion exchange membranes (AEMs) as the solid polymer electrolyte can reduce formation of carbonate from carbon dioxide, compared to aqueous electrolyte. It was also discovered that the electro-oxidation of methanol in alkaline electrolytes is structure insensitive [17], which opens up the opportunity for use of non-precious metals, such as Pd, Ag, Ni and perovskite-type oxides [18–20], which are significantly cheaper than Pt based catalysts, in alkaline fuel cells. Furthermore, the ionic current in the alkaline fuel cell is due to conduction ofPDF Image | Aspects of Direct Alkaline Alcohol Fuel Cells
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