Le Chatelier's Principle Worksheet
Explore Le Chatelier's Principle and its applications in chemical equilibrium with this comprehensive worksheet for Grade 10 Science students.
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Le Chatelier's Principle Worksheet
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Read each question carefully and answer to the best of your ability. Show all your work for calculations.
1. Which of the following statements best describes Le Chatelier's Principle?
When a chemical system at equilibrium is disturbed, it will shift in a direction that relieves the stress.
The rate of the forward reaction is equal to the rate of the reverse reaction at equilibrium.
Catalysts increase the rate of both forward and reverse reactions equally.
Increasing the temperature always increases the yield of products.
2. Consider the following equilibrium reaction: N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + Heat. If the temperature of the system is increased, what will happen?
The equilibrium will shift to the right, favoring product formation.
The equilibrium will shift to the left, favoring reactant formation.
The equilibrium will remain unchanged.
The reaction will stop.
3. According to Le Chatelier's Principle, if the concentration of a reactant is increased in a system at equilibrium, the equilibrium will shift to the to consume the added reactant.
4. Adding a catalyst to a system at equilibrium will the rates of both the forward and reverse reactions, but it will not affect the position of the equilibrium.
5. Increasing the pressure on a gaseous system at equilibrium will always favor the side with fewer moles of gas.
True
False
6. For an endothermic reaction, increasing the temperature will shift the equilibrium to the left.
True
False
7. Explain how changing the volume of a container affects a gaseous equilibrium system. Provide an example.
8. Consider the reaction: CO(g) + Cl₂(g) ⇌ COCl₂(g). If CO is removed from the system, in which direction will the equilibrium shift? Justify your answer.
9. Analyze the provided image of a chemical equilibrium graph. Describe what happens at the point where the concentrations of reactants and products become constant.
