An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.37×10-2 M CH2Cl2, 0.174 M CH4 and 0.174 M CCl4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.18×10-2 mol of CH2Cl2(g) is added to the flask?
An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.37×10-2 M CH2Cl2, 0.174 M CH4 and 0.174 M CCl4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.18×10-2 mol of CH2Cl2(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 5.37×10-2 M CH2Cl2, 0.174 M CH4 and 0.174 M CCl4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.18×10-2 mol of CH2Cl2(g) is added to the flask?
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