22. The equilibrium constant for the following reaction is 14.9 2 NO (g) + Cl2(g) 2NOCK(g) Kc = 14.9 A reaction container is found to contain the following concentrations of these three gases: [NO] 0.0500mol/L [Cl₂] 0.100mol/L [NOCI] a. Show that the system is not at equilibrium. 0.100mol/L b. What shift would need to take place in order to establish equilibrium? Justify your answer.

Chemistry: The Molecular Science
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ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
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22. The equilibrium constant for the following reaction is 14.9
2 NO
(g)
+ Cl2(g)
2NOCK(g)
Kc = 14.9
A reaction container is found to contain the following concentrations of these three gases:
[NO]
0.0500mol/L
[Cl₂]
0.100mol/L
[NOCI]
a. Show that the system is not at equilibrium.
0.100mol/L
b. What shift would need to take place in order to establish equilibrium? Justify your answer.
Transcribed Image Text:22. The equilibrium constant for the following reaction is 14.9 2 NO (g) + Cl2(g) 2NOCK(g) Kc = 14.9 A reaction container is found to contain the following concentrations of these three gases: [NO] 0.0500mol/L [Cl₂] 0.100mol/L [NOCI] a. Show that the system is not at equilibrium. 0.100mol/L b. What shift would need to take place in order to establish equilibrium? Justify your answer.
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