Higher yield of NO in the reaction N_{2(g)} + | vedclass

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Question

(A) The given reaction is $N_{2(g)} + O_{2(g)} \rightleftharpoons 2 NO_{(g)}$ with $\Delta H = +180.7 \ kJ \ mol^{-1}$.Since the reaction is endotherm

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Only $A, C, D$

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(A) The given reaction is $N_{2(g)} + O_{2(g)} \rightleftharpoons 2 NO_{(g)}$ with $\Delta H = +180.7 \ kJ \ mol^{-1}$.Since the reaction is endothermic $(\Delta H > 0)$, according to Le Chatelier's principle, an increase in temperature favors the forward reaction, leading to a higher yield of $NO$.Increasing the concentration of reactants ($N_2$ or $O_2$) also shifts the equilibrium in the forward direction to consume the added reactants, thereby increasing the yield of $NO$.Therefore, higher temperature $(A)$, higher concentration of $N_2$ $(C)$, and higher concentration of $O_2$ $(D)$ all favor the formation of $NO$.

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