The formation of nitric oxide by the reaction | vedclass

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Question

(D) According to Le Chatelier's principle:$1$. Since the reaction is endothermic $(\Delta H > 0)$,a high temperature favors the forward reaction.$2$.

Vedclass · Accepted Answer

High temperature and excess reactant concentration

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(D) According to Le Chatelier's principle:$1$. Since the reaction is endothermic $(\Delta H > 0)$,a high temperature favors the forward reaction.$2$. Since the number of moles of gaseous products $(2 \ mol)$ is equal to the number of moles of gaseous reactants $(1+1 = 2 \ mol)$,the pressure has no effect on the equilibrium position.$3$. According to the law of mass action,increasing the concentration of reactants ($N_2$ and $O_2$) shifts the equilibrium in the forward direction.Therefore,the correct conditions are high temperature and excess reactant concentration.

The formation of nitric oxide by the reaction $N_2 + O_2 \rightleftharpoons 2NO$ with $\Delta H = +43.200 \ kcal$ is favoured by:

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