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 0.107 mol of CCl4(g) is added to the flask?

The equilibrium constant, K, for the following reaction is 2.02×10-2 at 513 K. PCl5 (g) PCl3 (g) + Cl2 (g) An equilibrium mixture of the three gases in a 7.25 L container at 513 K contains 0.246 M PCl5,   7.04×10-2 M PCl3 and 7.04×10-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 12.7 L? [PCl5] = ?M [PCl3] = ?M [Cl2] = ?M

Consider the following reaction:             2 NO(g) + Br2(g) ⇌ 2 NOBr(g)  At a specific temperature, the equilibrium concentrations were determined to be [NO] = 0.067 M, [Br2] = 0.072 M, and [NOBr] = 0.142 M. Based on the value of the equilibrium constant, describe the position of the equilibrium.      the position of equilibrium lies to the left, hence the reaction will contain a high concentration of NO and Br2.      The position of equilibrium lies to the right, hence the reaction will contain a higher concentration of NOBr.      the position of equilibrium lies to the right, hence the reaction will contain a high concentration of NO and Br2.      The position of equilibrium lies to the left, hence the reaction will contain a high concentration of NOBr.

The equilibrium constant, K, for the following reaction is 3.15×10-2 at 627 K. COCl2 (g)  CO (g) +  Cl2 (g) An equilibrium mixture of the three gases in a 9.27 L container at 627 K contains 0.265 M COCl2,   9.13×10-2 M CO and 9.13×10-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 18.0 L? [COCl2] =  M [CO] =  M [Cl2] =  M