What happens to the position of equilibrium when the pressure is increased in a reaction involving gaseous reactants and products?

According to Le Chatelier's principle, increasing the pressure will shift the equilibrium position towards the side with fewer moles of gas. This occurs because the system attempts to counteract the change by reducing the pressure, leading to a higher concentration of the products if they are on the side with fewer gas moles. This answer is anchored to Equilibrium and Le Chatelier's principle.

According to Le Chatelier's principle, increasing the pressure will shift the equilibrium position towards the side with fewer moles of gas. This occurs because the system attempts to counteract the change by reducing the pressure, leading to a higher concentration of the products if they are on the side with fewer gas moles. is the best answer because it directly supports the AQA A-Level Chemistry objective to use Le Chatelier's principle to predict the effect of pressure changes. This reasoning is anchored to Equilibrium and Le Chatelier's principle in Chemical equilibria, Le Chatelier's principle and Kc, and it separates Le Chatelier from similar A-Level ideas rather than relying on a vague recall statement. Other options are weaker if they use the wrong evidence, calculation, mechanism, observation, unit, or conclusion for this subtopic.