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
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.
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?
"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?
never mind you just subtract them and get 26.6 and that is the right answer! Thank you soo much!
Right. I have 26.6 also.
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
I suck at chem
Ppcl3 6.78 torr
Pcl2 26.4
Ppcl5 224
To solve this question, we can use the concept of the equilibrium constant, Kp, which relates the partial pressures of the reactants and products at equilibrium. The equilibrium constant expression for the given reaction is:
Kp = (PCl5 / (PCl3 * Cl2))
Given the initial equilibrium partial pressures of the three substances, we can calculate the initial value of Kp:
Kp_initial = (217.0 / (13.2 * 13.2))
Now, when Cl2 is injected into the mixture, the total pressure jumps to 263 Torr. Let's assume x Torr of Cl2 is added. As a result, the new partial pressures become:
PCl3 = 13.2
Cl2 = 13.2 + x
PCl5 = 217.0 + x
To calculate the new value of Kp, we substitute the modified partial pressures into the equilibrium constant expression:
Kp_new = (PCl5 / (PCl3 * Cl2))
= ((217.0 + x) / (13.2 * (13.2 + x)))
We know that the total pressure is equal to the sum of the partial pressures:
Total Pressure = PCl3 + Cl2 + PCl5
263 = 13.2 + 13.2 + x + 217.0 + x
263 = 443.4 + 2x
2x = -180.4
x = -90.2
Since a negative value for x isn't physically possible, we conclude that no Cl2 is added to the mixture. Therefore, the initial equilibrium partial pressures of PCl3, Cl2, and PCl5 remain the same:
PCl3 = 13.2 Torr
Cl2 = 13.2 Torr
PCl5 = 217.0 Torr
Hence, the correct answer is:
PCl3 = 13.2 Torr
Cl2 = 13.2 Torr
PCl5 = 217.0 Torr