Assertion (A): For every chemical reaction at | vedclass

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(D) The standard Gibbs energy change of a reaction is given by $\Delta G^\circ = -RT \ln K$. At equilibrium,the reaction quotient $Q = K$,but the stan

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$(A)$ is not correct but $(R)$ is correct

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(D) The standard Gibbs energy change of a reaction is given by $\Delta G^\circ = -RT \ln K$. At equilibrium,the reaction quotient $Q = K$,but the standard Gibbs energy change $\Delta G^\circ$ is not necessarily zero unless the equilibrium constant $K = 1$. Therefore,Assertion $(A)$ is incorrect. The reason statement is correct because for a spontaneous process at constant temperature and pressure,the Gibbs energy of the system must decrease $(\Delta G < 0)$. Thus,$(A)$ is incorrect but $(R)$ is correct.

Assertion $(A)$: For every chemical reaction at equilibrium,standard Gibbs energy change of the reaction is zero.
Reason $(R)$: At constant temperature and pressure,chemical reactions are spontaneous in the direction of decreasing Gibbs energy.

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Assertion $(A)$: For every chemical reaction at equilibrium,standard Gibbs energy change of the reaction is zero. Reason $(R)$: At constant temperature and pressure,chemical reactions are spontaneous in the direction of decreasing Gibbs energy.