For the following redox reaction, calculate the E°cell, ΔG°, and equilibrium constant (K) for the reaction below. All species are in their standard state. (F = 96,500 C • mol –1) MnO4–(aq) + 8H+(aq) + 5Fe2+(aq) Mn2+(aq) + 4 H2O(l) + 5Fe3+(aq) MnO4–(aq) + 8H+(aq) + 5e– Mn2+(aq) + 4H2O(l) E° = 1.51 V Fe3+(aq) + e– Fe2+(aq) E° = 0.77 V
For the following redox reaction, calculate the E°cell, ΔG°, and equilibrium constant (K) for the reaction below. All species are in their standard state. (F = 96,500 C • mol –1) MnO4–(aq) + 8H+(aq) + 5Fe2+(aq) Mn2+(aq) + 4 H2O(l) + 5Fe3+(aq) MnO4–(aq) + 8H+(aq) + 5e– Mn2+(aq) + 4H2O(l) E° = 1.51 V Fe3+(aq) + e– Fe2+(aq) E° = 0.77 V
General Chemistry - Standalone book (MindTap Course List)
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Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.128QP: a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4...
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| For the following |
|
(F = 96,500 C • mol –1) MnO4–(aq) + 8H+(aq) + 5Fe2+(aq) Mn2+(aq) + 4 H2O(l) + 5Fe3+(aq) |
| MnO4–(aq) + 8H+(aq) + 5e– Mn2+(aq) + 4H2O(l) | E° = 1.51 V |
| Fe3+(aq) + e– Fe2+(aq) | E° = 0.77 V |
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