How many moles of electrons (n) are transferred between the oxidizing agent and the reducing agent in the following overall redox reaction?

Question

5 Ag+(aq) + Mn2+(aq) + 4H2O(l) → 5 Ag(s) + MnO4-(aq) + 8H+(aq)

Answer 1

5 moles of electrons

You can verify this by looking at the electrons transferred during the reduction and the oxidation reactions as follows:

Reduction: 5 Ag⁺ + 5e- ==> 5 Ag so 5 moles of electrons transferred

Oxidation: Mn²⁺ ==> Mn⁷⁺ + 5e- so 5 moles electrons transferred