Use the information below to determine whether or not a reaction mixture in which the partial pressures of PCl3, Cl2, and PCl5 are 0.21 atm, 0.41 atm, and 0.59 atm, respectively, is at equilibrium at 450 K. Kp = 3.8 at 450 K.PCl3(g) + Cl2(g) -> PCl5(g)Part 1:What is the numerical value for Q for this reaction? Remember to always express your answer to correct number of significant figures.Part 2:If the reaction mixture is not at equilibrium, in which direction does the reaction proceed to achieve equilibrium?

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Answered: Use the information below to determine…

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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Use the information below to determine whether or not a reaction mixture in which the partial pressures of PCl₃, Cl₂, and PCl₅ are 0.21 atm, 0.41 atm, and 0.59 atm, respectively, is at equilibrium at 450 K. K_p = 3.8 at 450 K.
PCl₃(g) + Cl₂(g) -> PCl₅(g)

Part 1:

What is the numerical value for Q for this reaction? Remember to always express your answer to correct number of significant figures.

Part 2:

If the reaction mixture is not at equilibrium, in which direction does the reaction proceed to achieve equilibrium?

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