1. The problem statement, all variables and given/known data Introduced into a 1.70 −L flask is 0.120 mol of PCl5(g); the flask is held at a temperature of 227∘C until equilibrium is established. PCl5(g)⇌PCl3(g)+Cl2(g) What is the total pressure of the gases in the flask at this point? [Hint: Use data from Appendix D in the textbook and appropriate relationships from this chapter.] 2. Relevant equations From the data tables I got ΔG for the following to be: Cl2 = 0 PCl3 = -267.8 PCl5 = -305 From this I know ΔG to be 37.2. ΔG=-RTln(K) (1) PV=nRT (2) 3. The attempt at a solution Using equation (1) I found K and then found the moles of each substance at equilibrium. I added these together and put them into equation (2) to get P. This isn't working for me. Is there a better way to do it?