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What happens to a reversible reaction at equilibrium when an inert gas is added to the system but pressure remains unchanged?
1. More of the product is formed
2. Less of the product will be formed
3. More of the reactants will be formed
4. It remains unaffected

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Correct Answer - Option 1 : More of the product is formed

Explanation:

Le- Chatelier's principle:

  • Equilibrium is a condition that occurs when a chemical reaction is reversible, and the forward and reverse reactions occur simultaneously, at the same rate.
  • Le Chatelier's Principle- "if a chemical system at equilibrium experiences a change in concentration, temperature or total pressure, the equilibrium will shift in order to minimize that change".
  • ​Effect of change of concentration:
    • According to Le - Chatelier's Principle, when the concentration of one of the reactants in a system at equilibrium is increased so that the system is no longer at equilibrium, instantaneously, then the equilibrium will shift so as to decrease the concentration of the reactant.
    • This means the equation or equilibrium will shift forward.
    • If there is an increase in the concentration of any of the products, then the equilibrium shifts towards the backward direction so as to decrease the concentration of the products.
  • Effect of change of pressure:
    • Change of pressure will have no effect on the state of equilibrium if;
    • The system does not involve gaseous reactants or products.
    • The number of moles of gaseous reactants and products is equal on both sides.
    • According to Le- Chatelier's principle, on increasing the pressure, the rate of reaction will shift to the side where there is a decrease of pressure or a lesser number of moles of gaseous components.
  • Effect of addition of inert gas:
    • When an inert gas is added to an equilibrium system at constant volume, there will be an increase in the total pressure of the system. The concentrations of the products and reactants will not change. There will be no change in the position of the equilibrium.
    • This is because the ratio of the moles of the components to the volume of the container will not change.
    • When a gas is added to the system at equilibrium keeping the pressure constant, the volume increases.
    • This causes a decrease in the number of moles of gases per unit volume.
    • Hence, the equilibrium shifts towards the direction in which there is an increase in the number of moles of gases.


Hence,  when an inert gas is added to the system at equilibrium but pressure remains unchanged, more of the product is formed.

  • When a catalyst is introduced at equilibrium, there will be no change in the rate of the reaction.

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