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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According to Le Chatelier's principle, when the volume of the container is increased at constant temperature, the system will try to counteract the change. Since the reaction produces two moles of gas on the left side and one mole of gas on the right side, decreasing the volume of the container would shift the equilibrium to the left to decrease the number of moles of gas. Therefore, increasing the volume will shift the equilibrium to the right to increase the number of moles of gas. As a result, more hydrogen and nitrogen will be produced at the expense of ammonia in order to increase the number of moles of gas.

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