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2.2 Ideal Performance The Nernst potential, E, gives the ideal open circuit cell potential. This potential sets the upper limit or maximum performance achievable by a fuel cell. The overall reactions for various types of fuel cells are presented in Table 2-1. The corresponding Nernst equations for those reactions are provided in Table 2-2. Table 2-1 Electrochemical Reactions in Fuel Cells Fuel Cell Polymer Electrolyte and Phosphoric Acid Alkaline Molten Carbonate CO - carbon monoxide CO2 - carbon dioxide CO3= - carbonate ion Anode Reaction H2 → 2H+ + 2e- H2 +2(OH)- →2H2O+2e- H2 +CO3= →H2O+CO2 +2e- CO+CO3= →2CO2 +2e- Cathode Reaction 1⁄2 O2 + 2H+ + 2e- → H2O 1⁄2O2 +H2O+2e- →2(OH)- 1⁄2O2 +CO2 +2e- →CO3= Solid Oxide H2 +O= →H2O+2e- CO+O= →CO2 +2e- CH4 +4O= →2H2O+CO2 +8e- 1⁄2O2 +2e- →O= e- - electron H+ - hydrogen ion H2 - hydrogen H2O - water O2 - oxygen OH- - hydroxyl ion The Nernst equation provides a relationship between the ideal standard potential (E°) for the cell reaction and the ideal equilibrium potential (E) at other partial pressures of reactants and products. For the overall cell reaction, the cell potential increases with an increase in the partial pressure (concentration) of reactants and a decrease in the partial pressure of products. For example, for the hydrogen reaction, the ideal cell potential at a given temperature can be increased by operating at higher reactant pressures, and improvements in fuel cell performance have, in fact, been observed at higher pressures. This will be further demonstrated in Chapters 3 through 7 for the various types of fuel cells. The reaction of H2 and O2 produces H2O. When a carbon-containing fuel is involved in the anode reaction, CO2 is also produced. For MCFCs, CO2 is required in the cathode reaction to maintain an invariant carbonate concentration in the electrolyte. Because CO2 is produced at the anode and consumed at the cathode in MCFCs, and because the concentrations in the anode and cathode feed streams are not necessarily equal, the CO2 partial pressures for both electrode reactions are present in the second Nernst equation shown in Table 2-2. 2-4PDF Image | Fuel Cell Handbook (Seventh Edition)
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