Le Chatelier’s Principle
Chemistry ⇒ Chemical Kinetics and Equilibrium
Le Chatelier’s Principle starts at 11 and continues till grade 12.
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See sample questions for grade 11
Describe the effect of decreasing the volume of a container on a gaseous equilibrium where the number of moles of gas is greater on the reactant side.
Describe the effect of increasing the concentration of a product in a reversible reaction at equilibrium.
Describe what happens to the equilibrium position if both reactant and product concentrations are increased equally.
Describe what happens to the equilibrium position when an inert gas is added to a reaction mixture at constant volume.
Explain how a catalyst affects the position of equilibrium according to Le Chatelier’s Principle.
Explain why changing the pressure only affects equilibria involving gases.
Explain why increasing the temperature of an endothermic reaction increases the yield of products.
Explain why the addition of an inert gas at constant pressure can affect the equilibrium position in a gaseous system.
For the reaction: 2A(g) ⇌ B(g) + C(g), if the total pressure is increased, what will happen to the equilibrium position?
For the reaction: 2NO(g) + O2(g) ⇌ 2NO2(g), what will happen if the temperature is increased, given that the reaction is exothermic?
For the reaction: 2NO2(g) ⇌ N2O4(g), what will happen if the temperature is decreased, given that the reaction is exothermic?
For the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g), what will happen if more SO2 is added?
For the reaction: CaCO3(s) ⇌ CaO(s) + CO2(g), what will happen if CO2 is removed from the system?
For the reaction: H2(g) + I2(g) ⇌ 2HI(g), what will happen to the equilibrium if the volume of the container is doubled?
For the reaction: H2O(l) ⇌ H2O(g), what will happen to the equilibrium if the pressure is increased?
For the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g), what will happen to the yield of NH3 if the pressure is increased?
In an endothermic reaction at equilibrium, what is the effect of decreasing the temperature?
State Le Chatelier’s Principle.
A reaction at equilibrium is subjected to a sudden increase in pressure by decreasing the volume. The reaction is: PCl5(g) ⇌ PCl3(g) + Cl2(g). Predict the effect on the equilibrium position and justify your answer.
A sealed container contains the equilibrium mixture: 2SO2(g) + O2(g) ⇌ 2SO3(g). Predict and explain the effect on the equilibrium position if the temperature is decreased, given that the forward reaction is exothermic.
