Question

In a hydrogen fuel cell, oxygen and hydrogen are combincd to produce water and a small potential differ- ence. The steps of the chemical reaction are: at-electrode: at + electrode: H2 + 20H-→ 2H2O + 2e-; O2 + H2O + 2e-→ 2OH-, Use the table of chemical values to calculate a) the work that can be produced from this fuel cell, b) the 'waste' heat produced during standard operation, c) the voltage of the cell, and d) the minimum voltage required for the electrolysis of water (i.e. the minimum voltage required to run this reaction backwards and charge this fuel cell), e) The total entropy change for both the forward and the backward reaction Comment on engine efficiencies and the 2nd law of thermodynamics

Answer 1

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