# CHEMISTRY

posted by Kylie

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

PCl3= 6.2
PCl5= 224

I can't find the answer for Cl2!

1. DrBob222

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?

2. Kylie

"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?

3. Kylie

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

4. DrBob222

Right. I have 26.6 also.

5. Anonymous

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

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

7. alyssa

I suck at chem

8. Kelly

Ppcl3 6.78 torr
Pcl2 26.4
Ppcl5 224

## Similar Questions

1. ### chemistry

Please help me with this question For the system, PCl5 (g) --> PCl3 (g) + Cl2 (g) K= 26 @ 3000C In a 5.0 L flask, the gaseous mixture consists of all three gasses with partial pressures as follows: PCl5 = 0.012 atm PCl3 = 0.90 atm …
2. ### Chemistry

Please help me with this question For the system, PCl5 (g) --> PCl3 (g) + Cl2 (g) In a 5.0 L flask, the gaseous mixture consists of all three gasses with partial pressures as follows: PCl5 = 0.012 atm PCl3 = 0.90 atm Cl2 = 0.45 …
3. ### chemistry

Please help me with this question For the system, (the previous post i forgot to post the Kp) PCl5 (g) --> PCl3 (g) + Cl2 (g) In a 5.0 L flask, the gaseous mixture consists of all three gasses with partial pressures as follows: …
4. ### Chemistry

When a sample of PCl5(g) (0.02087 mol/L) is placed in 83.00 L reaction vessel at 491.0 °C and allowed to come to equilibrium the mixture contains 103.0 grams of PCl3(g). What is the equilibrium concentration (mol/L) of Cl2(g)?
5. ### Chemistry

An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has a partial pressure 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 …
6. ### chemistry

For the reaction below, Kp= 28.63 at 800 K. Calculate the equilibrium partial pressures of the reactants and products if the initial pressures are PpCl5=0.5600 atm and PpCl3= 0.4700 atm PCl5(g) <--> PCl3(g) + Cl2(g) PCl5=?
7. ### chemistry

at an equilibrium mixture of PCl5, PCl3, and Cl2 has partial pressures of 217.0 Torr, 13.2 Torr and 13.2 Torr respectively. a quantity of Cl2 is injected into the mixture, and the total pressure jumps to 263.0 Torr (at the moment of …
8. ### chemistry

at an equilibrium mixture of PCl5, PCl3, and Cl2 has partial pressures of 217.0 Torr, 13.2 Torr and 13.2 Torr respectively. a quantity of Cl2 is injected into the mixture, and the total pressure jumps to 263.0 Torr (at the moment of …
9. ### Chemistry - Answer Check

The two common chlorides of Phosphorus, PCl3 and PCl5, both important in the production of other phosphorous compounds, coexist in equilibrium as shown in the balanced chemical reaction below: PCl3 (g) + Cl2 (g) <-----> PCl5 …
10. ### chemistry

For the exothermic reaction PCl3(g)+Cl2(g)⇌PCl5(g) K = 0.160 at a certain temperature. A flask is charged with 0.507 bar PCl3 , 0.507 bar Cl2, and 0.304 bar PCl5 at this temperature. What are the equilibrium partial pressures of …

More Similar Questions