The Gibbs energy for the decomposition of at 500°C is as follows: The potential difference needed for electrolytic reduction of at 500° is at least

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The Gibbs energy for the decomposition of ${Al}_{2}O_{3}$ at
500°C is as follows:
$\frac{2}{3}{Al}_{2}O_{3} \rightarrow \frac{4}{3}Al + O_{2};\Delta_{r}G = + 966{kJmol}^{- 1}$
The potential difference needed for electrolytic reduction of
${Al}_{2}O_{3}$ at 500° is at least

Show answer and solution

\frac{2}{3}{Al}_{2}O_{3} \longrightarrow \frac{4}{3}Al + O_{2}

\Delta_{r}G = + 966kJ{mol}^{- 1} = 966 \times 10^{3}J{mol}^{- 1}

\Delta G = - nFE_{cell\ }

966 \times 10^{3} = - 4 \times 96500 \times E_{cell\ }

E_{cell\ } = 2.5V

Source: Grass-G / CH-28 Chemistry Paper FST 16 Jan.docx

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