For the reaction N$_2$(g) + 3H$_2$(g) ⇌ 2NH$_3$(g), an increase in pressure at constant temperature will

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shift the equilibrium to the right, producing more ammonia.. There are 4 moles of gas on the left and 2 on the right. By Le Chatelier's principle, increasing pressure favours the side with fewer gas molecules, so more ammonia forms. Pressure changes do not alter the equilibrium constant, only the position.

Answer

A) shift the equilibrium to the right, producing more ammonia.

Answer

B) increase the value of the equilibrium constant.

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C) have no effect on the position of equilibrium.

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D) shift the equilibrium to the left, producing more nitrogen and hydrogen.

For the reaction N$_2$(g) + 3H$_2$(g) ⇌ 2NH$_3$(g), an increase in pressure at constant temperature will

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