Could someone help me on this question please...
If phosphorus pentachloride is heated in a sealed tube the following equilibrium is set up:
PCl5(g) ----> PCl3(g) + Cl2(g)
At a given temperature (T) a sample of phosphorus pentachloride is 40.0% dissociated, the total equilibrium pressure being 2.00 atm. Calculate the partial pressures of each of the components of the equilibrium mixture, to three significant figures. Hence calculate the value of Kp under these conditions.
So far I have worked out the mole ratio to be 0.6x (PCl5) and 0.2x each for both PCl3 and Cl2 (but I'm not sure if this is right). I don't know what to do from there.
Any help would be appreciated. Thanks in advance.