7.2.3 - Effect of Pressure Changes (for Gas‐Phase Equilibria)
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Practice Questions
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What happens to equilibrium when the pressure is increased in a reaction with 4 moles of gas on one side and 2 moles on the other?
💡 Hint: Recall Le Châtelier’s Principle.
Does adding an inert gas change the position of equilibrium?
💡 Hint: Think about partial pressures.
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Interactive Quizzes
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What does increasing pressure do to a gas-phase equilibrium with unequal moles of gas?
💡 Hint: Remember the relationship between pressure and volume.
True or False: Adding an inert gas at constant volume causes the equilibrium position to shift.
💡 Hint: Reflect on how inert gases influence partial pressures.
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Challenge Problems
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You have a sealed container with the following equilibrium: $$4 NH_3(g) \rightleftharpoons 2 N_2(g) + 6 H_2(g)$$. If the volume of the container is suddenly halved, what will happen to the equilibrium position?
💡 Hint: Calculate moles on both sides to see the impact of changing volume.
In a reaction where the moles total to 5 on one side and 3 on another, discuss the implications of suddenly lowering pressure. What will happen and why?
💡 Hint: Relate to Le Châtelier’s Principle for clearer insight.
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