Question

For the cell reaction

\[\ce{2Fe^{3+}_{( aq)} + 2l^-_{( aq)} -> 2Fe^{2+}_{( aq)} + l2_{( aq)}}\]

\[\ce{E^0_{cell}}\] = at 298 K. The standard Gibbs energy (∆G°) of the cell reactions is:

Options

• – 46.32 KJ mol⁻¹

• – 23.16 KJ mol⁻¹

• 46.32 KJ mol⁻¹

• 23.16 KJ mol⁻¹

Answer 1

– 46.32 KJ mol⁻¹

Explanation:

n = 2; \[\ce{E^0_{cell}}\] = 0.24 V; ∆G° = ?; F = 96500 C

∆G° = – nFE°

∆G°= – 2 × 96500 × 0.24

∆G° = – 46320 J mol⁻¹

∆G° = – 46.32 KJ mol⁻¹