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The free energy change for the following reaction at 25 °C, when [H+] = 1.14 M and [Cr3+] = 5.01×10-3 M, is -442 kJ: 6H+(1.14 M) + 2Cr(s)3H2(g) + 2Cr3+(5.01×10-3 M)     ΔG = -442 kJ What is the cell potential for the reaction as written under these conditions? ____________ V Would this reaction be spontaneous in the forward or the reverse direction?

The free energy change for the following reaction at 25 °C, when [H+] = 1.14 M and [Cr3+] = 5.01×10-3 M, is -442 kJ: 6H+(1.14 M) + 2Cr(s)3H2(g) + 2Cr3+(5.01×10-3 M)     ΔG = -442 kJ What is the cell potential for the reaction as written under these conditions? ____________ V Would this reaction be spontaneous in the forward or the reverse direction?

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter17: Chemcial Thermodynamics
Section: Chapter Questions
Problem 17.59QE: Calculate G for the following reactions and state whether each reaction is spontaneous under...
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The free energy change for the following reaction at 25 °C, when [H+] = 1.14 M and [Cr3+] = 5.01×10-3 M, is -442 kJ:

6H+(1.14 M) + 2Cr(s)3H2(g) + 2Cr3+(5.01×10-3 M)     ΔG = -442 kJ

What is the cell potential for the reaction as written under these conditions?

____________ V

Would this reaction be spontaneous in the forward or the reverse direction? 

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