My problem is:
1.00 mol of CO and 1.00 mol of Cl2 are introduced into an evacuated 1.75 L flask and the following equilibrium is established at 668 K:
CO (g) + Cl2 (g) ↔ COCl2 (g)
The reaction has a Kp = 22.5. What is the total gas pressure at equilibrium?
I guess I am confused where to start. I've found other problems, but with different information, so I got confused. I know I am going to use the ideal gas law. But do I need to form some sort of ICE chart? I know the temp, R constant, and the moles, but where does the Kp come into play?