Practice Equilibrium Constant In Terms Of Partial Pressures (kp) (6.2.2)

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6 sample questions

Question 1.
What does Kp stand for?
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Think about what equilibrium means for gases.
Question 2.
Identify the term Δn_gas.
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Consider how the number of gas molecules changes from reactants to products.
3Question 3.
What is Kp used for?
- Calculating solubility
- Equilibrium of gaseous reactions
- Kinetic energy of gases
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Focus on what Kp measures.
4Question 4.
True or False: Kp changes with pressure.
- True
- False
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Consider the definition of equilibrium constants.
Question 5.
For the reaction: 3H₂(g) + N₂(g) ⇌ 2NH₃(g), if Kp = 6.35 at a certain temperature and the partial pressures are P_H2 = 0.5 atm, P_N2 = 0.5 atm, calculate P_NH3 at equilibrium.
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Rearrange the equation to find the unknown pressure.
Question 6.
Explain how decreasing the volume of a reaction container affects Kp for the reaction: A(g) + B(g) ⇌ C(g) + D(g) where Δn_gas = -1.
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Focus on Le Chatelier's principle regarding volume and pressure.

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