In the reaction N_{2(g)} + 3H_{2(g)} rightlef | vedclass

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Question

(B) The given reaction is $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$.
This is an exothermic reaction $(\Delta H < 0)$.
According to Le

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Increasing pressure

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(B) The given reaction is $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$.
This is an exothermic reaction $(\Delta H < 0)$.
According to Le Chatelier's principle,for an exothermic reaction,a decrease in temperature favors the forward reaction.
Since the number of moles of gaseous products $(2)$ is less than the number of moles of gaseous reactants $(1+3=4)$,an increase in pressure shifts the equilibrium towards the side with fewer moles,which is the product side.
Therefore,the yield of $NH_3$ increases with high pressure and low temperature.
Among the given options,increasing pressure is the correct factor for increasing the yield.

In the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the yield of the product increases on:

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