When 6.00 mol each of 12 (g), Br2 (g), and IBr(g) are placed in a 2.00L vessel at constant temperature, they reach equilibrium according to the following equation: |2 (g) + Br2 (g) = 2 IBr (g) If Keq for this reaction is 0.683: a. Is this system at equilibrium? If not, which way will it shift to reach equilibrium? b. Determine the concentrations of all entities at equilibrium. Show all your steps.

When 6.00 mol each of 12 (g), Br2 (g), and IBr(g) are placed in a 2.00L vessel at constant temperature, they reach equilibrium according to the following equation: |2 (g) + Br2 (g) = 2 IBr (g) If Keq for this reaction is 0.683: a. Is this system at equilibrium? If not, which way will it shift to reach equilibrium? b. Determine the concentrations of all entities at equilibrium. Show all your steps.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 28QAP: For the system PCl5(g)PCl3(g)+Cl2(g)K is 26 at 300C. In a 1.0-L flask at 300C, a gaseous mixture...

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