For the equilibrium 2H_2O rightleftharpoons H | vedclass

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(C) The equilibrium constant for the auto-ionization of water is $K_w = [H_3O^+][OH^-] = 10^{-14}$ at $298 \ K$.The relationship between standard Gibb

Vedclass · Accepted Answer

$80$

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(C) The equilibrium constant for the auto-ionization of water is $K_w = [H_3O^+][OH^-] = 10^{-14}$ at $298 \ K$.The relationship between standard Gibbs free energy change and the equilibrium constant is given by $\Delta G^o = -RT \ln K_{eq} = -2.303RT \log K_{eq}$.Substituting the values: $\Delta G^o = -2.303 	imes 8.314 	imes 10^{-3} \ kJ \ K^{-1} \ mol^{-1} 	imes 298 \ K 	imes \log(10^{-14})$.$\Delta G^o = -2.303 	imes 8.314 	imes 10^{-3} 	imes 298 	imes (-14) \ kJ \ mol^{-1}$.$\Delta G^o \approx 79.88 \ kJ \ mol^{-1} \approx 80 \ kJ \ mol^{-1}$.

List-$I$	List-$II$
$A$. $Aq.$ solution of $AlCl_3$	$I$. Basic
$B$. $Aq.$ solution of $CH_3COONa$	$II$. Acidic
$C$. $Aq.$ solution of $KCl$	$III$. Highly conductive
$D$. $Al_2O_3$	$IV$. Strongly basic
	$V$. Amphoteric

For the equilibrium $2H_2O \rightleftharpoons H_3O^{+} + OH^{-}$,the value of $\Delta G^o$ at $298 \ K$ is approximately ....... $kJ \ mol^{-1}$.

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$A$. $Aq.$ solution of $AlCl_3$ $I$. Basic
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