Question

For a cell whose potential is –0.46 v with 3 moles of electrons exchanged, what is ΔG ? ΔG = –nFE°cell

Answer 1

Answer:

133kj

Explanation:

Answer 2

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 $10^{4}$C/mol)$E_{0}$ =  cell potential = –0.46 v

⇒ ΔG = –nFE°cell
⇒ ΔG = - (3 mol)(9.648456 x $10^{4}$ C/mol) (-0.46 J/C) ⇒ ΔG = +133148 J ≈ 133 kJ