STATEMENT-1: For every chemical reaction at equilibrium, standard Gibbs energy of reaction is zero. and STATEMENT-2: At constant temperature and pressure, chemical reactions are spontaneous in the direction of decreasing Gibbs energy.

Question

STATEMENT-1: For every chemical reaction at equilibrium, standard Gibbs energy of reaction is zero. and STATEMENT-2: At constant temperature and pressure, chemical reactions are spontaneous in the direction of decreasing Gibbs energy. (A) STATEMENT - 1 is True, STATEMENT-2 is True; STATEMENT - 2 is correct explanation for STATEMENT-1 (B) STATEMENT - 1 is True, STATEMENT-2 is True; STATEMENT -2 is NOT a correct explanation for STATEMENT-1 (C) STATEMENT - 1 is True, STATEMENT-2 is False (D) STATEMENT - 1 is False, STATEMENT-2 is True

Tardigrade Admin · Accepted Answer

At equilibrium Δ G =0, Δ G ° of a reaction may or may not be zero. For a spontaneous process Δ G <0

Q. STATEMENT-1: For every chemical reaction at equilibrium, standard Gibbs energy of reaction is zero.
and
STATEMENT-2: At constant temperature and pressure, chemical reactions are spontaneous in the direction of decreasing Gibbs energy.

STATEMENT - 1 is True, STATEMENT-2 is True; STATEMENT - 2 is correct explanation for STATEMENT-1

STATEMENT - 1 is True, STATEMENT-2 is True; STATEMENT $- 2$ is NOT a correct explanation for STATEMENT-1

STATEMENT - 1 is True, STATEMENT-2 is False

STATEMENT - 1 is False, STATEMENT-2 is True

At equilibrium $Δ G = 0,$
$Δ G^{\circ}$ of a reaction may or may not be zero.
For a spontaneous process $Δ G < 0$

Q. STATEMENT-1: For every chemical reaction at equilibrium, standard Gibbs energy of reaction is zero. and STATEMENT-2: At constant temperature and pressure, chemical reactions are spontaneous in the direction of decreasing Gibbs energy.