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(A) The reaction $2NO_{2(g)} \rightleftharpoons N_2O_{4(g)}$ is exothermic in the forward direction (formation of $N_2O_4$).According to Le Chatelier'

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The reaction is exothermic and $NO_2$ is darker in colour than $N_2O_4$

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(A) The reaction $2NO_{2(g)} \rightleftharpoons N_2O_{4(g)}$ is exothermic in the forward direction (formation of $N_2O_4$).According to Le Chatelier's principle,increasing the temperature shifts the equilibrium towards the endothermic direction (reverse),which produces more $NO_2$.Since the mixture is darker at high temperatures,$NO_2$ must be the darker-coloured gas compared to $N_2O_4$.Similarly,at low pressure,the equilibrium shifts towards the side with more moles of gas (the reactant side,$NO_2$),which also results in a darker colour.Therefore,the reaction is exothermic and $NO_2$ is darker in colour than $N_2O_4$.

When a sample of $NO_2$ is placed in a container,this equilibrium is rapidly established: $2NO_{2(g)} \rightleftharpoons N_2O_{4(g)}$. If this equilibrium mixture is a darker colour at high temperatures and at low pressure,which of these statements about the reaction is true?

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