Which of the following is incorrect?

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(C) Option $A$: For an isothermal reversible expansion,$W = -2.303 \, nRT \, \log \frac{V_2}{V_1} = +2.303 \, nRT \, \log \frac{V_1}{V_2}$. This is co

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$\Delta G = -T \Delta S$

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(C) Option $A$: For an isothermal reversible expansion,$W = -2.303 \, nRT \, \log \frac{V_2}{V_1} = +2.303 \, nRT \, \log \frac{V_1}{V_2}$. This is correct.Option $B$: The relation between standard Gibbs free energy and equilibrium constant is $\Delta G^o = -RT \ln K = -2.303 \, RT \, \log K$. This is correct.Option $C$: The general equation for Gibbs free energy is $\Delta G = \Delta H - T \Delta S$. The expression $\Delta G = -T \Delta S$ is only valid for processes where $\Delta H = 0$ (e.g.,isothermal processes in some specific conditions or phase transitions),but it is not the general definition. Thus,it is incorrect.Option $D$: For any spontaneous process,the total entropy change of the universe must be positive $(\Delta S_{	ext{Total}} > 0)$. This is correct.

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