A container was charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature? 3H₂(g) + N₂(g) ⇄ 2NH₃(g)

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Quizplus · Accepted Answer

According to Le Chatelier's principle, when the volume of a system at equilibrium is increased, the equilibrium will shift in the direction that produces more moles of gas. In this case, the production of hydrogen and nitrogen produces two moles of gas, while the production of ammonia only produces one mole of gas. Therefore, the equilibrium will shift towards hydrogen and nitrogen production at the expense of ammonia.

A Container Was Charged with Hydrogen, Nitrogen, and Ammonia Gases