What is the apparent molar mass of the gaseous mixture that results when COCl2(g) is allowed to dissociate at 395 ∘C and a total pressure of 3.00 atm?
COCl2(g)⇌CO(g)+Cl2(g)
Kp=4.44×10−2 at 395 ∘C
Think of the apparent molar mass as the molar mass of a hypothetical single gas that is equivalent to the gaseous mixture.

Question

What is the apparent molar mass of the gaseous mixture that results when COCl2(g) is allowed to dissociate at 395 ∘C and a total pressure of 3.00 atm? 
COCl2(g)⇌CO(g)+Cl2(g) 
Kp=4.44×10−2 at 395 ∘C 
Think of the apparent molar mass as the molar mass of a hypothetical single gas that is equivalent to the gaseous mixture.

aaronq · Answer

what have you tried?

anonymous · Answer

I set up the ice table and ending up solving for x using the quadratic formula. once solving for x I calculated 0.323, -0.421. I don't know what to do next

aaronq · Answer

so $[CO]=[Cl_2]=0.323$?

i think ultimately, you have to plug it into PV=nRT -> $PV=\dfrac{m}{M}RT$ and solve for M.