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

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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