1) I just want to check if this one is correct reaction => CCl4(g) <==> C(s) = 2Cl2(g) Kp= .76 find the initial partial pressure of CCl4 that will produce an equilibrium total pressure of 1.20 atm p.total = p.CCl4 + p.Cl2 CCl4 <=> 2Cl2 i. press x 2x change 1.20 - x 1.20 - 2x kp = .76 = (p.Cl2^2)/(p.CCL4) = (1.2-2x)^2/(1.2-x) x= .8557 or x= .1543 .8557 will not work so take x = .1543 p.CCl4 = 1.20- .1543 = 1.05 atm the rub is that if I use x to find p.Cl2 I get .892 atm 1.05 + .892 =/= 1.2 ? Q2. Ok constant temp =25 C constant volume reaction; Nh4HS (g)<==> NH3(g) + H2S(g) step 1; some NH4HS decomposed in an evacuated container to give a total pressure at equililbrium of .659 atm step 2; extra NH3 is added. re-established equilibrium gives a partial pressure for NH3 of .750 atm find Kp I'm stuck on this one. .