For the reaction N_{2(g)} + 3H_{2(g)} rightle | vedclass

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Question

(C) According to Le Chatelier's principle,when an inert gas is added to a reaction at constant pressure,the volume of the system increases to maintain

Vedclass · Accepted Answer

Towards the left

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(C) According to Le Chatelier's principle,when an inert gas is added to a reaction at constant pressure,the volume of the system increases to maintain the pressure.This leads to a decrease in the partial pressure of the reacting species.The equilibrium shifts in the direction where the total number of moles of gaseous products is greater.For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the number of moles of gaseous reactants is $1 + 3 = 4$,and the number of moles of gaseous products is $2$.Since the number of moles of gaseous reactants $(4)$ is greater than the number of moles of gaseous products $(2)$,the equilibrium will shift towards the side with more moles to compensate for the volume increase.Therefore,the equilibrium shifts towards the left (towards the reactants).

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,in which direction will the equilibrium shift if an inert gas is added at constant pressure?

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