Question: The overall reaction and equilibrium constant value for a hydrogenoxygen fuel cell at 298 K is 2H 2 (g) + O 2 (g) 2H

The overall reaction and equilibrium constant value for a hydrogen–oxygen fuel cell at 298 K is 2H₂(g) + O₂(g) → 2H₂O(l) K = 1.28 × 10⁸³

a. Calculate E°_cell and ΔG⁸ at 298 K for the fuel cell reaction.

b. Predict the signs of ΔH^o and ΔS^o for the fuel cell reaction.

c. As temperature increases, does the maximum amount of work obtained from the fuel cell reaction increase, decrease, or remain the same? Explain.

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