The standard e.m.f of a galvanic cell involving cell reaction with n =2 is found to be 0.295 ~V at 25^ C . The equilibrium constant of the reaction would be: (Given F =96500 C mol ⁻¹, R =8.314 ~J K ⁻¹ ~mol ⁻¹

Step-by-step solution

E = E ^ - 0.0591 n ₁₀ Q at 25^ C At equilibrium, E =0, Q = K 0= E ^ - 0.0591 n ₁₀ ~K or, K = Antilog [ n E ^ 0.0591 ] or, K = Antilog [ 2 0.295 0.0591 ] aligned & = Antilog [ 0.590 0.0591 ] & = Antilog 10=1 10¹⁰ . aligned Related Theory The cell potential is the difference between the electrode potentials (reduction potentials) of the cathode and anode. It is called the standard electromotive force (emf) of the cell when no current is drawn through the cells.