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

Options

A. `S` is correct but `E` is wrong.
B. `S` is wrong but `E` are correct and `E`
C. Both `S` and `E` are correct but `E` is correct explanation of `S`.
D. Both `S` and `E` are correct but `E` is not correct explanation of `S`.

Answer

b

Explanation

AT equilibrium `DeltaG=0`, but standard Gibbs energy `(DeltaG^(2))` of a reaction may or may not be zero. For reaction to be spontaneousn `DeltaG`(Gibbs energy) should be more negative, i.e., `DeltaGgt0`.