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

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(D) According to Le Chatelier's principle,if a change is applied to a system at equilibrium,the system will shift in a direction that counteracts the

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by increasing pressure and decreasing temperature.

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(D) According to Le Chatelier's principle,if a change is applied to a system at equilibrium,the system will shift in a direction that counteracts the change.$N_{2(g)} + 3H_{2(g)} ightleftharpoons 2NH_{3(g)} + 	ext{Heat}$$(a)$ Increasing the concentration of $NH_{3(g)}$ shifts the equilibrium in the backward direction to consume the added product.$(b)$ Decreasing the pressure shifts the equilibrium toward the side with more moles of gas (the reactant side,$4 	ext{ moles}$ vs $2 	ext{ moles}$),which is the backward direction.$(c)$ Decreasing the concentration of $N_{2(g)}$ and $H_{2(g)}$ shifts the equilibrium in the backward direction to produce more reactants.$(d)$ Increasing pressure shifts the equilibrium toward the side with fewer moles of gas (the product side,$2 	ext{ moles}$ vs $4 	ext{ moles}$),which is the forward direction. Since the reaction is exothermic,decreasing the temperature also favors the forward direction.

For the reversible reaction,
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + \text{heat}$
The equilibrium shifts in the forward direction:

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For the reversible reaction,$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + \text{heat}$The equilibrium shifts in the forward direction: