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2. Use the information below to determine whether a reaction mixture in which the partial pressures of PCI3, Cl2 and PCls are 0.20, 0.40, and 0.60 atm, respectively is at equilibrium at 450 K. PCI3 (g) + Cl2 (g) = PCI5 (g) Kp = 3.8 at 450 K. a) Is the reaction at equilibrium? Show your work. b) If the reaction is not at equilibrium, in which direction does the reaction proceed? Justify your answer. c) If enough PCI3 is injected into the reaction mixture to double its partial pressure, would the mixture be closer to equilibrium? Explain why or why not.

2. Use the information below to determine whether a reaction mixture in which the partial pressures of PCI3, Cl2 and PCls are 0.20, 0.40, and 0.60 atm, respectively is at equilibrium at 450 K. PCI3 (g) + Cl2 (g) = PCI5 (g) Kp = 3.8 at 450 K. a) Is the reaction at equilibrium? Show your work. b) If the reaction is not at equilibrium, in which direction does the reaction proceed? Justify your answer. c) If enough PCI3 is injected into the reaction mixture to double its partial pressure, would the mixture be closer to equilibrium? Explain why or why not.

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.29QE
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2. Use the information below to determine whether a reaction mixture in which the partial pressures of PCI3, Cl2 and PCIs are 0.20, 0.40, and 0.60 atm, respectively is at equilibrium at 450 K. PCI3 (g) + Cl2 (g) = PCI5 (g) Kp = 3.8 at 450 K. a) Is the reaction at equilibrium? Show your work. b) If the reaction is not at equilibrium, in which direction does the reaction proceed? Justify your answer. c) If enough PCI3 is injected into the reaction mixture to double its partial pressure, would the mixture be closer to equilibrium? Explain why or why not.
Transcribed Image Text:2. Use the information below to determine whether a reaction mixture in which the partial pressures of PCI3, Cl2 and PCIs are 0.20, 0.40, and 0.60 atm, respectively is at equilibrium at 450 K. PCI3 (g) + Cl2 (g) = PCI5 (g) Kp = 3.8 at 450 K. a) Is the reaction at equilibrium? Show your work. b) If the reaction is not at equilibrium, in which direction does the reaction proceed? Justify your answer. c) If enough PCI3 is injected into the reaction mixture to double its partial pressure, would the mixture be closer to equilibrium? Explain why or why not.
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