The overall reaction and equilibrium constant value for a hydrogenoxygen fuel cell at 298 K is 2H 2 (g) O 2 (g) 2H 2 O(l) K 1 28 10 83 a Calculate E cell and G 8 at 298 K for the fuel cell reaction b Predict the signs of H o and S o for the fuel cell reaction c As temperature increases, does the ma...

2 H 2 g O 2 g 2 H 2 Oloxygen goes from the zero oxidation st ...

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 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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Chemical Principles

ISBN: 978-1111580650

7th edition

Authors: Steven S. Zumdahl, Donald J. DeCoste

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Question Posted: May 05, 2015 02:24 AM

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The overall reaction and equilibrium constant value for a hydrogenoxygen fuel cell at 298 K is 2H

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