Electro Chemistry

Question

Calculate the ΔGO (in kJ/mol) for the following reaction at 25.0℃.

Sn^+2(aq) + Mn(s) ---> Sn(s) + Mn^+2(aq)

Answer 1

∆Gº = -nFEºcell

n = mols electrons = 2 (see below)

F = Faraday constant = 96,485 C/mol e-

Eº = standard potential of the galvanic cell (see below)

Sn2+ + 2e- ==Sn(s) Eº = -0.14 V

Mn2+ + 2e- ==> Mn(s) Eº = -1.18 V

Eº = -0.14 - (-1.18) = 1.04 V

∆Gº = - (2 mol e-)(96,485 C/ mol e-)(1.04 V) = -200,689 C-V = -200,689 Joules

∆Gº = -201 kJ