The free energy change for the following reaction at 25 °C, when [Cu2+] = 1.71×10-3 M and [Fe3+] = 1.13 M, is 75.7 kJ:Cu2+(1.71×10-3 M) + Fe2+(aq) Cu+(aq) + Fe3+(1.13 M) ΔG = 75.7 kJWhat is the cell potential for the reaction as written under these conditions?Answer: VWould this reaction be spontaneous in the forward or the reverse direction?
The free energy change for the following reaction at 25 °C, when [Cu2+] = 1.71×10-3 M and [Fe3+] = 1.13 M, is 75.7 kJ:Cu2+(1.71×10-3 M) + Fe2+(aq) Cu+(aq) + Fe3+(1.13 M) ΔG = 75.7 kJWhat is the cell potential for the reaction as written under these conditions?Answer: VWould this reaction be spontaneous in the forward or the reverse direction?
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 24E: For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is...
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The free energy change for the following reaction at 25 °C, when [Cu2+] = 1.71×10-3 M and [Fe3+] = 1.13 M, is 75.7 kJ:
Cu2+(1.71×10-3 M) + Fe2+(aq) Cu+(aq) + Fe3+(1.13 M) ΔG = 75.7 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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