Practice Kp: Equilibrium Constant In Terms Of Partial Pressures (7.1.3) - Unit 7: Equilibrium

Practice: Kp: Equilibrium Constant in Terms of Partial Pressures

Lesson 7.1.3Unit 7: Equilibrium

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6 sample questions

Question 1.
What does Kp stand for?
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Think about how gas concentrations are important in equilibrium.
Question 2.
Define partial pressure.
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Consider how gases interact in a mixture.
3Question 3.
What is Kp used for in gas-phase reactions?
- To determine rates
- To determine equilibrium positions
- To measure concentrations
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Think about what Kp represents.
4Question 4.
True or False: Kp and Kc are identical for all reactions.
- True
- False
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Kp is specifically for gases, while Kc involves concentrations.
Question 5.
A gas phase reaction has an initial concentration of reactants with Kc = 0.25 at 350K. Given that Δn = -1, calculate Kp and discuss how the pressures might vary if temperature increases to 400K.
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Pay attention to how Δn influences adjustments in equilibrium.
Question 6.
Given the reaction 2 NO(g) + O₂(g) ⇌ 2 NO₂(g) with Kp at 298K found to be 2.0. If the reaction occurs at higher temperatures, assess expected shifts in Kp and the implications for industrial production.
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Reflect on the role of exothermic reactions in temperature dynamics.

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