The equilibrium constant, K, for the following reaction is 1.2010-2 at 500 K. PCI5(g) =PCl;(g)+ Cl2(g)...

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The equilibrium constant, K, for the following reaction is 1.20×10-2 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, 5.95×10- M PCI3 and 5.95×10 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 The equilibrium constant, K, for the following reaction is 1.20×10-2 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, 5.95×10- M PCI3 and 5.95×10 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

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Given The equilibrium constant K for the following reaction i... View the full answer