The free energy change for the following reaction at 25 °C, when [Cu2+] = 1.11 M and [Cr3+] = 3.59×10-3 M, is -638 kJ: 3Cu2+(1.11 M) + 2Cr(s) → 3Cu(s) + 2Cr3+(3.59×10-3 M) ΔG = -638 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?
The free energy change for the following reaction at 25 °C, when [Cu2+] = 1.11 M and [Cr3+] = 3.59×10-3 M, is -638 kJ: 3Cu2+(1.11 M) + 2Cr(s) → 3Cu(s) + 2Cr3+(3.59×10-3 M) ΔG = -638 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?
Chemistry by OpenStax (2015-05-04)
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Chapter17: Electrochemistry
Section: Chapter Questions
Problem 25E: Determine the overall reaction and its standard cell potential at 25 C for this reaction. Is the...
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The free energy change for the following reaction at 25 °C, when [Cu2+] = 1.11 M and [Cr3+] = 3.59×10-3 M, is -638 kJ:
3Cu2+(1.11 M) + 2Cr(s) → 3Cu(s) + 2Cr3+(3.59×10-3 M) ΔG = -638 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?
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