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

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

Options:

  1. Shifts equilibrium to the right
  2. Shifts equilibrium to the left
  3. No effect on equilibrium
  4. Increases the reaction rate

Correct Answer: No effect on equilibrium

Solution: 

Adding an inert gas at constant volume does not change the partial pressures of the reactants or products, thus having no effect on the equilibrium position.

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

Practice Questions

Q1
How does the addition of an inert gas at constant volume affect the equilibrium of a reaction?
  1. Shifts equilibrium to the right
  2. Shifts equilibrium to the left
  3. No effect on equilibrium
  4. Increases the reaction rate

Questions & Step-by-Step Solutions

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.
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