Which of the following equations is incorrect | vedclass

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(D) The relationship between the equilibrium constant $K$ and standard Gibbs free energy change is $\Delta G^\circ = -RT \ln K$. Rearranging this,we g

Vedclass · Accepted Answer

$\ln K = \frac{\Delta H^\circ - T\Delta S^\circ}{RT}$

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(D) The relationship between the equilibrium constant $K$ and standard Gibbs free energy change is $\Delta G^\circ = -RT \ln K$. Rearranging this,we get $\ln K = -\frac{\Delta G^\circ}{RT}$,which implies $K = e^{-\Delta G^\circ / RT}$. Thus,option $A$ is correct. For any process,$\Delta G_{	ext{system}} = -T\Delta S_{	ext{total}}$. Therefore,$\frac{\Delta G_{	ext{system}}}{\Delta S_{	ext{total}}} = -T$. Thus,option $B$ is correct. For an isothermal process,the definition $\Delta G = \Delta H - T\Delta S$ is correct. Comparing this with the expression in option $D$,we know $\Delta G^\circ = \Delta H^\circ - T\Delta S^\circ$. Substituting this into $\Delta G^\circ = -RT \ln K$,we get $-RT \ln K = \Delta H^\circ - T\Delta S^\circ$,which simplifies to $\ln K = -\frac{\Delta H^\circ - T\Delta S^\circ}{RT}$. The expression given in option $D$ is $\ln K = \frac{\Delta H^\circ - T\Delta S^\circ}{RT}$,which lacks the negative sign. Therefore,option $D$ is the incorrect equation.

Which of the following equations is incorrect?

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