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Uf = H2, consumed (2-42) H2,in + COin where the H2 consumed originates from the H2 present at the fuel cell inlet (H2,in) and any H2 produced in the cell by the water gas shift reaction (COin). Gas composition changes between the inlet and outlet of a fuel cell, caused by the electrochemical reaction, lead to reduced cell voltages. This voltage reduction arises because the cell voltage adjusts to the lowest electrode potential given by the Nernst equation for the various gas compositions at the exit of the anode and cathode chambers. Because electrodes are usually good electronic conductors and isopotential surfaces, the cell voltage can not exceed the minimum (local) value of the Nernst potential. In the case of a fuel cell with the flow of fuel and oxidant in the same direction (i.e., co-flow), the minimum Nernst potential occurs at the cell outlet. When the gas flows are counterflow or crossflow, determining the location of the minimum potential is not straightforward. The MCFC provides a good example to illustrate the influence of the extent of reactant utilization on the electrode potential. An analysis of the gas composition at the fuel cell outlet as a function of utilization at the anode and cathode is presented in Example 9-5. The Nernst equation can be expressed in terms of the mole fraction of the gases (Xi) at the fuel cell outlet: RT XX1⁄2X P1⁄2 E = Eo + 2F ln H2 O2 CO2,cathode XH2O,anodeXCO2,anode (2-43) where P is the cell gas pressure. The second term on the right side of Equation (2-43), the so-called Nernst term, reflects the change in the reversible potential as a function of reactant utilization, gas composition, and pressure. Figure 2-8 illustrates the change in reversible cell potential as a function of utilization using Equation (2-43). 2-22PDF Image | Fuel Cell Handbook (Seventh Edition)
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