The formation of NO_2 in the reaction 2NO + O | vedclass

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(D) According to Le Chatelier's principle,for the reaction $2NO(g) + O_2(g) ightleftharpoons 2NO_2(g) + 	ext{heat}$:$1$. The reaction is exothermic

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Both $(b)$ and $(c)$

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(D) According to Le Chatelier's principle,for the reaction $2NO(g) + O_2(g) ightleftharpoons 2NO_2(g) + 	ext{heat}$:$1$. The reaction is exothermic (releases heat). Therefore,decreasing the temperature shifts the equilibrium to the right to produce more heat,favoring the formation of $NO_2$.$2$. The total number of moles of gaseous reactants is $3$ ($2$ moles of $NO$ and $1$ mole of $O_2$),while the number of moles of gaseous products is $2$ ($2$ moles of $NO_2$). Increasing the pressure shifts the equilibrium towards the side with fewer moles of gas,which is the product side,thus favoring the formation of $NO_2$.Therefore,both high pressure and low temperature favor the formation of $NO_2$.

The formation of $NO_2$ in the reaction $2NO + O_2 \rightleftharpoons 2NO_2 + \text{heat}$ is favoured by

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