7.1.3 - Kp: Equilibrium Constant in Terms of Partial Pressures
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Practice Questions
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What does Kp stand for?
💡 Hint: Think about how gas concentrations are important in equilibrium.
Define partial pressure.
💡 Hint: Consider how gases interact in a mixture.
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Interactive Quizzes
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What is Kp used for in gas-phase reactions?
💡 Hint: Think about what Kp represents.
True or False: Kp and Kc are identical for all reactions.
💡 Hint: Kp is specifically for gases, while Kc involves concentrations.
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Challenge Problems
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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.
💡 Hint: Pay attention to how Δn influences adjustments in equilibrium.
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.
💡 Hint: Reflect on the role of exothermic reactions in temperature dynamics.
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