A battery manufacturer needs a galvanic cell that delivers at least under standard…

CHEMISTRY · Multi-part · CBSE · Chemistry · Electrochemistry · Electrochemistry

Problem

A battery manufacturer needs a galvanic cell that delivers at least

1.50\,\text{V}

under standard conditions. Three candidate metal–ion couples are available, with their standard reduction potentials listed below. Half-Reaction E° (V)

M^{2+}(aq) + 2e^{-} \rightarrow M(s)

-0.13\,\text{V}

N^{2+}(aq) + 2e^{-} \rightarrow N(s)

+0.79\,\text{V}

O^{2+}(aq) + 2e^{-} \rightarrow O(s)

-0.56\,\text{V}

Only combinations of these three electrodes may be employed. (a) For every possible pairing of two different electrodes, calculate the standard cell potential,

E^\circ_{\text{cell}}

. Present your results in an organized manner. (b) Identify all electrode combinations that satisfy the manufacturer’s requirement of

E^\circ_{\text{cell}} \geq 1.50\,\text{V}

. For each qualifying pair, write the balanced overall redox equation including physical states. (c) Choose one of the qualifying pairs and calculate the value of

\Delta G^\circ

(in kJ) when exactly

2.0\,\text{mol}

of electrons are transferred under standard conditions. Use

F = 96\,485\,\text{C mol}^{-1}

. (d) Justify, with thermodynamic reasoning, why the chosen electrode pair is suitable for the intended battery application. Include a brief comment on how material abundance or cost might influence the final selection in practice.

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