Question

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

• A. If both (A) and (R) are correct, and (R) is the correct explanation for (A)
• B. If the both (A) and (R) are correct, but (R) is not the correct explanation for (A)
• C. If (A) is correct, but (R) is incorrect
• D. IF (A) is incorrect, but (R) is correct

Answer 1

The correct option is D

IF (A) is incorrect, but (R) is correct

Don't get confused in the question here. During equilibrium, $△G^{\ominus }$ = 0 Standard Gibbs energy of the reaction is not zero.
And for the second statement,
It is given reaction is spontaneous.
Therefore, $△G$ = -ve
$G_{final}-G_{initial}$ = -ve
Therefore, $G_{final}$ < $G_{initial}$
So, this statement is correct.