consider-the-following-reaction-2-nobr-g-cl2-g-2-no-g-2-brcl-g-h-47-4-kj-how-wil

Question

Consider the following equilibrium reaction: 2 NOBr(g) + Cl₂(g) ⇌ 2 NO(g) + 2 BrCl(g), ΔH° = +47.4 kJ.

(a) How will the concentration of NO change when the temperature of the system is lowered?

(b) How will the equilibrium constant (K_c) change when the temperature of the system is increased?

Explain your answer using Le Chatelier's principle.

Accepted Answer

(a) [NO] will decrease when the temperature is lowered because the reaction is endothermic.

(b) K_c will increase because the concentration of the reactants will increase and the concentrations of the products will decrease when the temperature is increased.

Answer

(a) [NO] will increase when the temperature is increased because the reaction is exothermic.

(b) K_c will decrease because the concentration of the reactants will decrease and the concentrations of the products will increase when the temperature is increased.

Answer

(a) [NO] will decrease when the temperature is increased because the reaction is exothermic.

(b) K_c will increase because the concentration of the reactants will increase and the concentrations of the products will decrease when the temperature is increased.

Answer

(a) [NO] will increase when the temperature is increased because the reaction is endothermic.

(b) K_c will decrease because the concentration of the reactants will decrease and the concentrations of the products will increase when the temperature is increased.

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