At the following reaction is carried out under standard conditions: The standard…

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

Problem

25\,^{\circ}\text{C}

the following reaction is carried out under standard conditions:

Fe(s) + 2\,\text{H}^{+}(aq) \rightarrow \text{Fe}^{2+}(aq) + \text{H}_{2}(g)

The standard molar Gibbs free-energy change for this reaction is

\Delta G^\circ = +54.9\,\text{kJ}

. Faraday’s constant:

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

. (a) Calculate the standard cell potential, including proper units and sign, for the reaction as written. (b) Interpret the sign of the value you obtained in part (a) in terms of the thermodynamic favorability of the reaction at

25\,^{\circ}\text{C}

. (c) The reaction in part (a) is written in the opposite direction (the products become reactants and vice versa). Determine the numerical values of

\Delta G^\circ

and the standard cell potential for the reversed reaction and discuss its spontaneity under standard conditions.

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