The equilibrium constant, K, for the following reaction is 1.2010-2 at 500 K. PCI5(g) =PCl;(g)+ Cl2(g) An equilibrium mixture of the three gases in a 1.00 L flask at 500 K contains 0.295 M PCI5, 5.9510- M PCI3 and 5.9510 M Cl. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.64x10-2 mol of PCI3(g) is added to the flask? [PCI5] M [PCI3] = M [C2] M