Practice Effect Of Pressure Changes (for Gas‐phase Equilibria) (7.2.3) - Unit 7: Equilibrium

Practice: Effect of Pressure Changes (for Gas‐Phase Equilibria)

Lesson 7.2.3Unit 7: Equilibrium

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9 questions

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6 sample questions

Question 1.
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?
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Recall Le Châtelier’s Principle.
Question 2.
Does adding an inert gas change the position of equilibrium?
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Think about partial pressures.
3Question 3.
What does increasing pressure do to a gas-phase equilibrium with unequal moles of gas?
- It shifts left
- It shifts right
- It has no effect
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Remember the relationship between pressure and volume.
4Question 4.
True or False: Adding an inert gas at constant volume causes the equilibrium position to shift.
- True
- False
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Reflect on how inert gases influence partial pressures.
Question 5.
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?
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Calculate moles on both sides to see the impact of changing volume.
Question 6.
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?
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Relate to Le Châtelier’s Principle for clearer insight.

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