Predict the products of electrolysis of the following. An aqueous solution of AgNO3 with silver electrodes.

An aqueous solution of AgNO3 with silver electrode, when undergoes electrolysis, two oxidation and two reduction half-reactions must be considered.Oxidation (at anode) (A) Ag(s)⟶Ag+(aq)+e-;E°=-0.80 V (B) 2H2O(l)⟶O2(g)+4H+(aq)+4e-;E°=-1.23 VReduction (at cathode) (C) Ag+(aq)+e-⟶Ag(s);E°=+0.80 V (D) 2H2O(l)+2e-⟶H2(g)+2OH-(aq);E°=-0.83 VBy E° values of (A ) and (B ) it appears that at anode silver of silver anode gets oxidized more readily because oxidation potential of Ag is greater than that of H2Omolecule. Similarly by E° values of (C) and (D), it appears that at cathode reduction potential of Ag+ ions is higher than that of H2O molecules. Therefore, on electrolysis of aq. AgNO3 solution with silver electrodes, Ag from silver anode dissolves while Ag+(aq) ions present in the solution get reduced and deposited at cathode.