Assertion :When $Q_{c} = K_{c}$ , reaction is at equilibrium. Reason: At equilibrium, ${Δ G}^{\circ}$ is 0.

Both Assertion and Reason are correct and Reason is the correct explanation for Assertion

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Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion

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Assertion is correct but Reason is incorrect

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Both Assertion and Reason are incorrect

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Solution

The correct option is B Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
The reaction is in equilibrium as long as there is no change in the temperature. When $Q_{c}$ = $K_{c}$ reaction is said to be in equilibrium, this means that the initial concentrations are equilibrium concentrations.
As the reaction reaches equilibrium, the standard Gibbs free energy becomes less negative and finally reaches zero.
Thus both assertion and reason are correct, but the assertion is not the correct explanation for the assertion.

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Assertion :When Qc=Kc, reaction is at equilibrium. Reason: At equilibrium, ΔG∘ is 0.

Assertion :When $Q_{c} = K_{c}$ , reaction is at equilibrium. Reason: At equilibrium, ${Δ G}^{\circ}$ is 0.