The standard Gibbs energy change in the react | vedclass

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(C) The standard Gibbs energy change is given by the formula $\Delta G^{\circ} = -RT \ln K_w = -2.303 	imes RT 	imes \log K_w$. At $25\ ^oC$ $(298 \

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$90$

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(C) The standard Gibbs energy change is given by the formula $\Delta G^{\circ} = -RT \ln K_w = -2.303 	imes RT 	imes \log K_w$. At $25\ ^oC$ $(298 \ K)$,the ionic product of water $K_w = 10^{-14}$. Substituting the values: $\Delta G^{\circ} = -2.303 	imes (8.314 	imes 10^{-3} \ kJ \ K^{-1} \ mol^{-1}) 	imes 298 \ K 	imes \log(10^{-14})$. $\Delta G^{\circ} = -2.303 	imes 8.314 	imes 10^{-3} 	imes 298 	imes (-14) \approx 79.9 \ kJ/mol$. The closest integer value provided in the options is $90 \ kJ/mol$.

The standard Gibbs energy change in the reaction $H_2O \rightleftharpoons H^{+} + OH^{-}$ at $25\ ^oC$ is.....$kJ/mol$.

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