Equilibrium Equation with Partial Pressures PCl3(g) +Cl2(g) <-> PCl5(g)?

Question

An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr, respectively. A quantity of Cl2(g) is injected into the mixture, and the total pressure jumps to 263.0 Torr.

The appropriate chemical equation is
PCl3(g) +Cl2(g) <-> PCl5(g)

What are the new Partial Pressures:

PCl3

Cl2

PCl5

I have an answer of
PCl3= 6.2
PCl5= 224

I can't find the answer for Cl2!
please help. I got an answer of 32.8 torr for Cl2 but it is wrong. Thanks.

Answer 1

You 32.8 torr for Cl2 is pressure Cl2 when the 19.6 torr Cl2 was added. If your value of PCl3 of 6.2 (torr?) is right, the new equilibrium pressure for Cl2 will be 32.8-6.2 = ? Do you know the 6.2 and 224 values are correct?

Answer 2

"Do you know the 6.2 and 224 values are correct?"
-yes these are correct.

I did what u told me and got 20.4 but it marked me wrong? What should I do?

Answer 3

never mind you just subtract them and get 26.6 and that is the right answer! Thank you soo much!

Answer 4

Right. I have 26.6 also.

Answer 5

1.2454 = ((217+x)/(32.8-x).(13.2-x))
324.2-58.5x+1.25x^2=0
Solved for x= 6.42

Pcl5 = 217+x=223.42
PCl3 = 13.2-x = 6.78
Cl2 = 26.38

Answer 6

Ans=
Pressure PCl3= 6.78 Torr
Pressure PCl2= 26.4 Torr
pressure PCl5= 224 Torr

Answer 7

I suck at chem

Answer 8

Ppcl3 6.78 torr
Pcl2 26.4
Ppcl5 224