In the manufacture of ammonia by Haber's | vedclass

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Question

(A) The given reaction is $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + 92.3 \ kJ$.
Since the reaction is exothermic $(\Delta H < 0)$,acco

Vedclass · Accepted Answer

Increasing the temperature

Vedclass · Answer

(A) The given reaction is $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + 92.3 \ kJ$.
Since the reaction is exothermic $(\Delta H < 0)$,according to Le Chatelier's principle,a decrease in temperature favors the forward reaction.
Therefore,increasing the temperature is unfavourable for the production of ammonia.
Increasing the pressure favors the side with fewer moles of gas (product side),and removing ammonia also shifts the equilibrium to the right.
Thus,the correct option is $A$.

In the manufacture of ammonia by Haber's process,$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + 92.3 \ kJ$,which of the following conditions is unfavourable?

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