A reaction occurring under standard conditions is represented by the following equation

CHEMISTRY · Multi-part · A Level · Chemistry · Electrode potentials · Electrode potentials

Problem

A reaction occurring under standard conditions is represented by the following equation.

2\,\text{Ag}^+(aq) + \text{Ni}(s) \rightarrow 2\,\text{Ag}(s) + \text{Ni}^{2+}(aq)

E^\circ_{\text{cell}} = 1.03\,\text{V}

The Faraday constant is

F = 9.65 \times 10^4\,\text{C mol}^{-1}

. (a) Identify the value of

n

for the overall reaction. (b) Calculate the standard Gibbs free energy change,

\Delta G^\circ

, in

\text{kJ}

per mole of Ni consumed. (c) If the stoichiometric coefficients in the balanced equation were doubled, state whether

E^\circ_{\text{cell}}

and

\Delta G^\circ

would change, and justify your answer quantitatively or conceptually.