Problem: 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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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:

E°cell = 0.0592 Vnlog K

Ecell = cell potential under non-standard conditions
cell = standard cell potential
n = number of e- transferred
K = equilibrium constant = [products]/[reactants] 


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Problem Details

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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