43. Given the standard electrode potentials: V and V. Calculate the standard electrode potential for — Electrochemistry Chemistry Question

💡 Solution & Explanation

$\Delta G_1^\circ (Au^+ \rightarrow Au) = -1F(1.69)$. $\Delta G_2^\circ (Au^{3+} \rightarrow Au) = -3F(1.40) = -4.20F$. The target is $Au^{3+} \rightarrow Au^+$. $\Delta G_3^\circ = \Delta G_2^\circ - \Delta G_1^\circ = -4.20F - (-1.69F) = -2.51F$. Since $n=2$ for this step, $-2FE^\circ_3 = -2.51F \implies E^\circ_3 = 2.51 / 2 = 1.255$ V.