Question

When 1.000 mol of PCl5 is introduced into a 5.000 L container at 500 K, 78.50 % of the PCl5dissociates to give an equilibrium mixture of PCl5, PCl3, and Cl2:
PCl5(g)⇌PCl3(g)+Cl2(g)

Part A

Calculate the values of Kc and Kp.

Part B

K_{P =}

Part C

If the initial concentrations in a particular mixture of reactants and products are  = 0.504  ,  = 0.129  , and  = 0.594  , in which direction does the reaction proceed to reach equilibrium?

In the direction of formation of PCl3 and Cl2.

In the direction of formation of PCl5

Part D

What are the concentrations when the mixture reaches equilibrium?

Enter your answers numerically separated by commas.

Me PCl5, Me PCl3, Me Cl2 =

Answer 1