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The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2C12(g) CH4(g) + CC14(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.48×10-2 M CH2C12, 0.178 M CH4 and 0.178 M CC14. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.60×10-2 mol of CH2Cl2(g) is added to the flask? [CH2Cl2] = M [CH4] = M [CC14] = M

The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2C12(g) CH4(g) + CC14(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.48×10-2 M CH2C12, 0.178 M CH4 and 0.178 M CC14. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.60×10-2 mol of CH2Cl2(g) is added to the flask? [CH2Cl2] = M [CH4] = M [CC14] = M

Chemistry: The Molecular Science
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
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The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2C12(g) CH4(g) + CC14(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.48×10-2 M CH2Cl2, 0.178 M CH4 and 0.178 M CC14. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.60×10-2 mol of CH2Cl2(g) is added to the flask? [CH2Cl2] = M [CH4] = M [CC14] = M The equilibrium constant, K, for the following reaction is 1.29×10-2 at 600 K. COC12(g) CO(g) + Cl2(g) An equilibrium mixture of the three gases in a 1.00 L flask at 600 K contains 0.242 M COCI2, 5.59×10- 2 M CO and 5.59×10-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 2.90×10-2 mol of Cl2(g) is added to the flask? [COCI2] = M [CO] = M [C12] = M
Transcribed Image Text:The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2C12(g) CH4(g) + CC14(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.48×10-2 M CH2Cl2, 0.178 M CH4 and 0.178 M CC14. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.60×10-2 mol of CH2Cl2(g) is added to the flask? [CH2Cl2] = M [CH4] = M [CC14] = M The equilibrium constant, K, for the following reaction is 1.29×10-2 at 600 K. COC12(g) CO(g) + Cl2(g) An equilibrium mixture of the three gases in a 1.00 L flask at 600 K contains 0.242 M COCI2, 5.59×10- 2 M CO and 5.59×10-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 2.90×10-2 mol of Cl2(g) is added to the flask? [COCI2] = M [CO] = M [C12] = M
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