Consider the following reaction:
N_{2}O_{4(g | vedclass

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Question

(A) The given reaction is endothermic $(\Delta H^{\circ} > 0)$.
$(a)$ According to Le Chatelier's principle,decreasing the temperature favors

Vedclass · Accepted Answer

$a$. Towards reactant,$b$. No change

Vedclass · Answer

(A) The given reaction is endothermic $(\Delta H^{\circ} > 0)$.
$(a)$ According to Le Chatelier's principle,decreasing the temperature favors the exothermic direction to release heat. Since the forward reaction is endothermic,the reverse reaction is exothermic. Therefore,the equilibrium shifts towards the reactant side.
$(b)$ Adding an inert gas like $N_{2}$ at constant temperature and constant volume does not change the partial pressures of the reacting species. Therefore,there is no effect on the equilibrium position.

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