How does the addition of an inert gas at constant volume affect the equilibrium

How does the addition of an inert gas at constant volume affect the equilibrium of a reaction?

How does the addition of an inert gas at constant volume affect the equilibrium of a reaction?

Step 1: Understand what an inert gas is. An inert gas is a gas that does not react with the substances in the reaction.
Step 2: Know that equilibrium in a reaction means the rates of the forward and reverse reactions are equal.
Step 3: Recognize that adding an inert gas at constant volume means the total volume of the system does not change.
Step 4: Realize that the addition of the inert gas increases the total pressure of the system but does not change the amount of reactants or products.
Step 5: Understand that the partial pressures of the reactants and products remain the same because the inert gas does not participate in the reaction.
Step 6: Conclude that since the partial pressures are unchanged, the equilibrium position of the reaction is also unchanged.

Le Chatelier's Principle – The principle that states if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change.
Partial Pressure – The pressure exerted by a single component of a mixture of gases, which is relevant in determining the equilibrium position of reactions involving gases.
Inert Gas Behavior – Inert gases do not react with the components of the reaction and do not affect the equilibrium position when added at constant volume.