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.
IF (A) is incorrect, but (R) is correct
Don't get confused in the question here. During equilibrium, △G⊖ = 0 Standard Gibbs energy of the reaction is not zero.
And for the second statement,
It is given reaction is spontaneous.
Therefore, △G = -ve
Gfinal−Ginitial = -ve
Therefore, Gfinal < Ginitial
So, this statement is correct.