wayoftheyetigirl

I've done all the work, I just keep coming up wrong on my math. I'm not sure what I'm missing. The equilibrium constant, Kp, for the following reaction is 0.636 at 600 K: COCl2(g) CO(g) + Cl2(g) Calculate the equilibrium partial pressures of all species when COCl2(g) is introduced into an evacuated flask at a pressure of 1.73 atm at 600 K. PCOCl2= PCO= PCl2= setting up ICE, I know that Kp=x/(1.73-x)=.636 (.636)[1.73-x]^2=x (.636)[1.73^2-2(1.73)x + x^2]=x (.636)x^2-[2(1.73)(.636)+1]x + (.636)(1.73)^2 x^2-[2(1.73)+1/(.636)]x + 1.73^2= 0 a=1 b= -[2(1.73)+1/(.636)]= -5.032 c= (1.73)^2= 2.993 quadratic equation such that: [(-5.032)^2-4(2.993)]^1/2 = [13.349]^1/2= 3.654 x=(-(-5.032)+-3.654)/2 x=4.343 or .689 Go with .689 since the other value of x is greater than the initial pressure of 1.73. PCO=PCL2=(1.73-x)=(1.73-.689)=1.041 PCOCL2=x=.689