Question

An oxidation-reduction reaction in which 3 electrons are transferred has a \(\Delta G^\circ\) of 17.37 kJ \(\mathrm{mol^{-1}}\) at 25 \(^\circ\)C. The value of \(E^\circ_{\mathrm{cell}}\) (in V) is ______ \(\times\) \(10^{-2}\).
(1 F = 96,500 C \(\mathrm{mol^{-1}}\))

Hint:

Use \(\Delta G^\circ = -nFE^\circ_{\mathrm{cell}}\) with n = 3; the positive \(\Delta G^\circ\) gives a negative \(E^\circ\).

Answer 1

Correct Answer: -6

\(\Delta G^\circ = -nFE^\circ_{\mathrm{cell}}\)
\(E^\circ_{\mathrm{cell}} = -\frac{\Delta G^\circ}{nF} = -\frac{17.37\times 10^3}{3\times 96500}\)
\(= -\frac{17370}{289500} = -0.06\) V \(= -6\times 10^{-2}\) V.
Answer: -6