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20. Electrochemistry - Part 2 of 3
20. Electrochemistry - Part 2 of 3
20. Electrochemistry / Cell Potential and Equilibrium / Problem 6
Given the following E°red
Cl2(g) + 2 e− → 2 Cl− (aq) E°red = 1.36 V
MnO4−(aq) + 8 H+(aq) + 5 e− → Mn2+(aq) + 4 H2O(l) E°red = 1.51 V
What is the value of the equilibrium constant for the reaction at 298 K?
10 Cl− (aq) + 2 MnO4−(aq) + 16 H+(aq) → 2 Mn2+(aq) + 8 H2O(l) + 5 Cl2(g)
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