ΔG is 133kJ
ΔG = –nFE°cell
ΔG = free energy of the reaction = ?
n = no of moles of electrons exchanged in the reaction = 3
F = Faraday's constant (9.648456 x [tex] 10^{4} [/tex]C/mol)[tex] E_{0} [/tex] = cell potential = –0.46 v
⇒ ΔG = –nFE°cell
⇒ ΔG = - (3 mol)(9.648456 x [tex] 10^{4} [/tex] C/mol) (-0.46 J/C) ⇒ ΔG = +133148 J ≈ 133 kJ
