Chemistry · 2012
NEET 2012 · Mains · Code C · Q91
The Gibbs' energy for the decomposition of Al_2 O_3 at 500°C is as follows: 2/3 Al_2 O_3 → 4/3 Al + O_2; Δ_r G =+960 kJ mol^-1. The potential…
The Gibbs' energy for the decomposition of $\displaystyle \mathrm{Al}_2 \mathrm{O}_3$ at $\displaystyle 500$°C is as follows :
$$\begin{aligned}
& \frac{2}{3} \mathrm{Al}_2 \mathrm{O}_3 \rightarrow \frac{4}{3} \mathrm{Al}+\mathrm{O}_2 ; \\
& \Delta_{\mathrm{r}} \mathrm{G}=+960 \mathrm{~kJ} \mathrm{~mol}^{-1} .
\end{aligned}
$$
The potential difference needed for the electrolytic reduction of aluminium oxide $\displaystyle \left(\mathrm{Al}_2 \mathrm{O}_3\right)$ at $\displaystyle 500$°C is at least :
Official answer
(1)
2.$\displaystyle 5$ V
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