Consider the following reaction at 373 K: COCl2(g) ⇄ CO(g) + Cl2(g) Kc= 2.9 x 10-10 The concentrations of the gases in a 1.00 L reaction flask are [COCl2] = 3.50 x 10-3 M, [Cl2] = 3.25 x 10-6 M, and [CO] = 1.11 x 10-5 M.
Consider the following reaction at 373 K: COCl2(g) ⇄ CO(g) + Cl2(g) Kc= 2.9 x 10-10 The concentrations of the gases in a 1.00 L reaction flask are [COCl2] = 3.50 x 10-3 M, [Cl2] = 3.25 x 10-6 M, and [CO] = 1.11 x 10-5 M.
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 3PS: Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A...
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Consider the following reaction at 373 K:
COCl2(g) ⇄ CO(g) + Cl2(g) Kc= 2.9 x 10-10
The concentrations of the gases in a 1.00 L reaction flask are [COCl2] = 3.50 x 10-3 M,
[Cl2] = 3.25 x 10-6 M, and [CO] = 1.11 x 10-5 M.
1. Is the mixture of gases at equilibrium? The answer should be supported with
calculations.
2. If not, in which direction will the reaction proceed to reach equilibrium?
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