What occurs when there is an increase in pressure in a gaseous system at equilibrium?

What occurs when there is an increase in pressure in a gaseous system at equilibrium?

• A. The system decreases the number of product molecules
• B. The system increases the number of reactant molecules
• C. The system shifts toward the side with fewer moles of gas
• D. The system does not respond to pressure changes

Answer: (C)

In a gaseous system at equilibrium, changes in pressure can affect the position of equilibrium according to Le Chatelier's principle. When pressure is increased, the system will respond by shifting the equilibrium in a direction that reduces the total number of gas molecules. This shift is aimed at opposing the change, which, in this case, is the increase in pressure. When a reaction has more moles of gas on one side than the other, increasing the pressure will favor the side with fewer moles of gas. This is because reducing the number of gas molecules decreases the overall pressure exerted by the gas molecules in the system. By promoting the formation of products or reactants that consist of fewer moles of gas, the system effectively works to decrease the pressure back towards its original state at equilibrium. For instance, consider a hypothetical reaction where 2 moles of gas on the reactants' side are converted into 1 mole of gas on the products' side. If the pressure increases, Le Chatelier's principle predicts that the equilibrium will shift to the products' side, where there is only 1 mole of gas, thereby reducing the pressure. Thus, when analyzing the effect of increased pressure on a gaseous system at equilibrium, the correct understanding is

In a gaseous system at equilibrium, changes in pressure can affect the position of equilibrium according to Le Chatelier's principle. When pressure is increased, the system will respond by shifting the equilibrium in a direction that reduces the total number of gas molecules. This shift is aimed at opposing the change, which, in this case, is the increase in pressure.

When a reaction has more moles of gas on one side than the other, increasing the pressure will favor the side with fewer moles of gas. This is because reducing the number of gas molecules decreases the overall pressure exerted by the gas molecules in the system. By promoting the formation of products or reactants that consist of fewer moles of gas, the system effectively works to decrease the pressure back towards its original state at equilibrium.

For instance, consider a hypothetical reaction where 2 moles of gas on the reactants' side are converted into 1 mole of gas on the products' side. If the pressure increases, Le Chatelier's principle predicts that the equilibrium will shift to the products' side, where there is only 1 mole of gas, thereby reducing the pressure.

Thus, when analyzing the effect of increased pressure on a gaseous system at equilibrium, the correct understanding is