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

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(B) The given reaction is $2NO_{2(g)} \rightleftharpoons N_2O_{4(g)} + 14.6 \ kcal$. Since heat is released in the forward direction,the forward react

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Favour the decomposition of $N_2O_4$

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(B) The given reaction is $2NO_{2(g)} \rightleftharpoons N_2O_{4(g)} + 14.6 \ kcal$. Since heat is released in the forward direction,the forward reaction is exothermic and the reverse reaction is endothermic. According to Le Chatelier's principle,an increase in temperature shifts the equilibrium in the direction that absorbs heat (endothermic direction). Therefore,an increase in temperature will favour the reverse reaction,which is the decomposition of $N_2O_4$ into $NO_2$.

For the equilibrium $2NO_{2(g)} \rightleftharpoons N_2O_{4(g)} + 14.6 \ kcal$,the increase in temperature would

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