Consider the graph of Gibbs free energy G vs extent of reaction. The number of statement/s from the following which are true with respect to points (a), (b) and (c) is _ _ _ _ _ _ A. Reaction is spontaneous at (a) and (b) B. Reaction is at equilibrium at point (b) and non-spontaneous at point (c) C. Reaction is spontaneous at (a) and non-spontaneous at (c) D. Reaction is non-spontaneous at (a) and (b)

Step-by-step solution

For spontaneous process, ∆ G = - ve , at equilibrium ∆ G = 0 and for non-spontaneous process ∆ G = + ve . The relation between the change in Gibbs reaction energy and Gibbs energy can be defined as the slope of the Gibbs energy plotted against the extent of reaction at constant pressure and temperature. At point a: Slope = - ve ∆ G = - ve Hence, reaction is spontaneous at point a. At point b: Slope = 0 ∆ G = 0 Hence. it is the equilibrium condition. At point c: Slope = + ve ∆ G =