The Gibbs energy for the decomposition of Al_ | vedclass

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(D) The reaction is $\frac{2}{3}Al_2O_3 	o \frac{4}{3}Al + O_2$.In $Al_2O_3$,the oxidation state of $Al$ is $+3$. The reduction half-reaction is $Al^

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$2.5$

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(D) The reaction is $\frac{2}{3}Al_2O_3 	o \frac{4}{3}Al + O_2$.In $Al_2O_3$,the oxidation state of $Al$ is $+3$. The reduction half-reaction is $Al^{3+} + 3e^- 	o Al$.For the overall reaction,the number of electrons transferred $(n)$ is $4$ (since $\frac{4}{3} 	imes 3 = 4$).Using the formula $\Delta_rG = -nFE^o$,where $\Delta_rG = 940 	imes 10^3\,J\,mol^{-1}$,$n = 4$,and $F = 96500\,C\,mol^{-1}$:$E^o = -\frac{\Delta_rG}{nF} = -\frac{940 	imes 10^3}{4 	imes 96500} \approx -2.43\,V$.The potential difference required for the electrolytic reduction is the magnitude of this value,which is approximately $2.5\,V$.

$LIST$-$I$ (Cell)	$LIST$-$II$ (Use/Property/Reaction)
$A$. Leclanche cell	$I$. Converts energy of combustion into electrical energy
$B$. Ni-Cd cell	$II$. Does not involve any ion in solution and is used in hearing aids
$C$. Fuel cell	$III$. Rechargeable
$D$. Mercury cell	$IV$. Reaction at anode $Zn \rightarrow Zn^{2+} + 2e^-$

The Gibbs energy for the decomposition of $Al_2O_3$ at $500\,^oC$ is as follows:
$\frac{2}{3}Al_2O_3 \to \frac{4}{3}Al + O_2, \Delta_rG = +940\,kJ\,mol^{-1}$
The potential difference needed for the electrolytic reduction of aluminium oxide is ............... $V$.

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The Gibbs energy for the decomposition of $Al_2O_3$ at $500\,^oC$ is as follows:$\frac{2}{3}Al_2O_3 \to \frac{4}{3}Al + O_2, \Delta_rG = +940\,kJ\,mol^{-1}$The potential difference needed for the electrolytic reduction of aluminium oxide is ............... $V$.