We are asked to calculate the equilibrium constant for each of the following reaction at 298 K
10Br- (aq) + 2MnO4 - (aq) + 16H+ (aq) → 2Mn2 + (aq) + 8H2 O (l) + 5Br2 (l)
We can solve this using the formula below:
Ecell = cell potential under non-standard conditions
E°cell = standard cell potential
n = number of e- transferred
K = equilibrium constant = [products]/[reactants]
Using the standard reduction potentials listed in Appendix E in the textbook, calculate the equilibrium constant for each of the following reactions at 298 K.
10Br- (aq) + 2MnO4 - (aq) + 16H+ (aq) → 2Mn2 + (aq) + 8H2 O(l) + 5Br2 (l)
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