The overall reaction and equilibrium constant value for a hydrogen-oxygen fuel cell at 298 K is given below. 2 H₂(g) + O₂(g) →→ 2 H₂O(l) K = 1.34 x 1083 (a) Calculate 8 and AG at 298 K for the fuel-cell reaction. V kJ 8⁰ AGⓇ (b) Predict the signs of AH and AS for the fuel-cell reaction. AH°: Opositive O negative AS°: O positive O negative (c) As temperature increases, does the maximum amount of work obtained from the fuel-cell reaction increase, decrease, or remain the same? Explain. Since AS is ---Select---, as T increases, AG becomes more ---Select--- . Therefore, the maximum work obtained will ---Select--- Bas T increases.

The overall reaction and equilibrium constant value for a hydrogen-oxygen fuel cell at 298 K is given below. 2 H₂(g) + O₂(g) →→ 2 H₂O(l) K = 1.34 x 1083 (a) Calculate 8 and AG at 298 K for the fuel-cell reaction. V kJ 8⁰ AGⓇ (b) Predict the signs of AH and AS for the fuel-cell reaction. AH°: Opositive O negative AS°: O positive O negative (c) As temperature increases, does the maximum amount of work obtained from the fuel-cell reaction increase, decrease, or remain the same? Explain. Since AS is ---Select---, as T increases, AG becomes more ---Select--- . Therefore, the maximum work obtained will ---Select--- Bas T increases.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 122AE: The overall reaction and equilibrium constant value for a hydrogen-oxygen fuel cell at 298 K is...

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