Question

Statement-I: For every chemical reaction at equilibrium, standard Gibbs’ energy of reaction is zero. 

Statement-II: At constant temperature and pressure, chemical reactions are spontaneous in the direction of decreasing Gibbs’ energy

(A) Statement-I is true; statement-II is true; statement-II is the correct explanation of statement-I. 

(B) Statement-I is true; statement-II is true; statement-II is not the correct explanation of statement-I. 

(C) Statement-I is true; statement-II is false. 

(D) Statement-I is false; statement-II is true

Answer 1

Correct option (D) Statement-I is false; statement-II is true

Explanation:

Statement-I is false. At equilibrium, ∆G = 0, G ≠ 0. 

Statement-II is true, spontaneous direction of reaction is towards lower Gibb’s free energy.