The overall reaction and equilibrium constant value for a hydrogenoxygen fuel cell at 298 K is 2H
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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 ΔHo and ΔSo 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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2 H 2 g O 2 g 2 H 2 Oloxygen goes from the zero oxidation st...View the full answer
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