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The free energy change for the following reaction at 25 °C, when [Sn2+] = 1.13 M and [Ni2+] = 4.56×10-3 M, is -34.9 kJ: Sn2+(1.13 M) + Ni(s)→ Sn(s) + Ni2+(4.56×10-3 M)     ΔG = -34.9 kJ What is the cell potential for the reaction as written under these conditions? Answer: ____  V Would this reaction be spontaneous in the forward or the reverse direction? _________. (forward or reverse)

The free energy change for the following reaction at 25 °C, when [Sn2+] = 1.13 M and [Ni2+] = 4.56×10-3 M, is -34.9 kJ: Sn2+(1.13 M) + Ni(s)→ Sn(s) + Ni2+(4.56×10-3 M)     ΔG = -34.9 kJ What is the cell potential for the reaction as written under these conditions? Answer: ____  V Would this reaction be spontaneous in the forward or the reverse direction? _________. (forward or reverse)

Chemistry
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
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The free energy change for the following reaction at 25 °C, when [Sn2+] = 1.13 M and [Ni2+] = 4.56×10-3 M, is -34.9 kJ:

Sn2+(1.13 M) + Ni(s)→ Sn(s) + Ni2+(4.56×10-3 M)     ΔG = -34.9 kJ

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

Answer: ____  V

Would this reaction be spontaneous in the forward or the reverse direction? _________. (forward or reverse)

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