For the equilibrium 2NO_{2(g)} rightleftharpo | vedclass

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(B) The given reaction is $2NO_{2(g)} \rightleftharpoons N_2O_{4(g)} + 21.9 \ kcal$.
Since the heat is released on the product side,the reaction is e

Vedclass · Accepted Answer

Favor the decomposition of $N_2O_4$

Vedclass · Answer

(B) The given reaction is $2NO_{2(g)} \rightleftharpoons N_2O_{4(g)} + 21.9 \ kcal$.
Since the heat is released on the product side,the reaction is exothermic $(\Delta H < 0)$.
According to Le Chatelier's principle,for an exothermic reaction,an increase in temperature shifts the equilibrium in the backward direction to absorb the excess heat.
Therefore,the backward reaction is favored,which means $N_2O_4$ will decompose into $NO_2$.
Thus,an increase in temperature favors the decomposition of $N_2O_4$.

For the equilibrium $2NO_{2(g)} \rightleftharpoons N_2O_{4(g)} + 21.9 \ kcal$,an increase in temperature will:

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