N_2 and O_2 combine to form nitric oxide as f | vedclass

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(B) The given reaction is: ${N_2}_{(g)} + {O_2}_{(g)} ightleftharpoons 2NO - 	ext{heat}$.
This can be rewritten as: ${N_2}_{(g)} + {O_2}_{(g)} + \

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High temperature

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(B) The given reaction is: ${N_2}_{(g)} + {O_2}_{(g)} ightleftharpoons 2NO - 	ext{heat}$.
This can be rewritten as: ${N_2}_{(g)} + {O_2}_{(g)} + 	ext{heat} ightleftharpoons 2NO$.
Since the reaction involves the absorption of heat,it is an endothermic reaction $(\Delta H > 0)$.
According to Le Chatelier's principle,for an endothermic reaction,an increase in temperature shifts the equilibrium in the forward direction to absorb the extra heat.
Therefore,high temperature favors the production of $NO$.

$N_2$ and $O_2$ combine to form nitric oxide as follows: ${N_2}_{(g)} + {O_2}_{(g)} \rightleftharpoons 2NO - \text{heat}$. Which of the following conditions will favor the production of $NO$?

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