The equilibrium constant, K, for the following reaction is 10.5 at 350 K.2CH2Cl2 (g) CH4 (g) + CCl4 (g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.43×10-2 M CH2Cl2, 0.176 M CH4 and 0.176 M CCl4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.143 mol of CH4(g) is added to the flask?
The equilibrium constant, K, for the following reaction is 10.5 at 350 K.2CH2Cl2 (g) CH4 (g) + CCl4 (g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.43×10-2 M CH2Cl2, 0.176 M CH4 and 0.176 M CCl4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.143 mol of CH4(g) is added to the flask?
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 57QRT
Related questions
Question
The equilibrium constant, K, for the following reaction is 10.5 at 350 K.
2CH2Cl2
- (g)
CH4
- (g) +
CCl4
- (g)
An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.43×10-2 M CH2Cl2, 0.176 M CH4 and 0.176 M CCl4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.143 mol of CH4(g) is added to the flask?
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