<span>ΔG is 133kJ
</span>
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
C/mol)
= cell potential = <span>–0.46 v
</span>
⇒ ΔG = –nFE°cell
⇒ ΔG = - (3 mol)(9.648456 x C/mol) (-0.46 J/C) ⇒ ΔG = +133148 J ≈ 133 kJ
</span>
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
</span>
⇒ ΔG = –nFE°cell
⇒ ΔG = - (3 mol)(9.648456 x