Le Chatelier's Principle Worksheet
Explore Le Chatelier's Principle and its application to chemical equilibrium with various practice problems.
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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. Apply your knowledge of Le Chatelier's Principle to predict the shifts in equilibrium.
1. State Le Chatelier's Principle in your own words.
2. Consider the following equilibrium reaction:
N₂(g) + 3H₂(g) ⇌ 2NH₃(g)
If the concentration of N₂(g) is increased, which way will the equilibrium shift?
To the left (towards reactants)
To the right (towards products)
No shift in equilibrium
The reaction will stop
3. For an exothermic reaction, increasing the temperature will shift the equilibrium to the , favoring the formation of . For an endothermic reaction, increasing the temperature will shift the equilibrium to the , favoring the formation of .
4. Consider the following reaction occurring in a closed container:
2SO₂(g) + O₂(g) ⇌ 2SO₃(g)
a) If the pressure of the system is increased by decreasing the volume, in which direction will the equilibrium shift? Explain your reasoning.
b) If an inert gas like Argon is added to the system, increasing the total pressure but not changing the volume, how will the equilibrium be affected? Explain.
5. A catalyst speeds up both the forward and reverse reactions equally, thus having no effect on the position of equilibrium.
True
False
6. Analyze the provided chemical equilibrium graph. Describe what happens to the concentrations of reactants and products at point 'A' and point 'B'.
