Consider the following reaction : N2O4 2NO2 (g) ; Hº = +58 kJ For each of the following cases (a,b), the direction in which the equilibrium shifts is : (a) Temperature is decreased. (b) Pressure is in

Question

Consider the following reaction : N2O4 2NO2 (g) ; Hº = +58 kJ For each of the following cases (a,b), the direction in which the equilibrium shifts is : (a) Temperature is decreased. (b) Pressure is increased by adding N2 at constant T.

(A) (a) towards reactant, (b) no change
(B) (a) towards product, (b) no change
(C) (a) towards product, (b) towards reactant
(D) (a) towards reactant (b) towards product

Prashant Kotian · Accepted Answer

Correct answer: A. (i) As reaction is endothermic so on decrease in temperature equilibrium shift in reactant side. (ii) On increase in pressure by adding inert gas at same temperature, no shifting will take place

💡 Solution & Explanation

Practice 22,000+ questions like this