Achieve question #4
Hi! I am confused on how to go thorugh the process on question 4, where is states, At a certain temperature, the given reaction has an equilibrium constant of Kp=389. PCL3(g)+Cl2(g) ---> <-- PCL5(g)
PCl5 is placed in a sealed container at an initial pressure of 0.0680 bar. What is the total pressure at equilibrium? Any advice would help!
Achieve question #4
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Hao Tam Tran 3H
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Re: Achieve question #4
Hi!
To start, you should make an ICE chart (it should not matter if you do the reverse reaction, the order is only important for the K formula itself for which one goes on top).
PCl3 + CL2 <> PCL5
I 0 0 0.068
C +x +x -x
E x x 0.068-x
We can then solve Kp = 389 = (0.068-x)/(x^2) by solving for x and then using the quadratic formula. Use this x to find the equilibrium partial pressures of all the reactants and products. To find the total pressure, add all these partial pressures together.
To start, you should make an ICE chart (it should not matter if you do the reverse reaction, the order is only important for the K formula itself for which one goes on top).
PCl3 + CL2 <> PCL5
I 0 0 0.068
C +x +x -x
E x x 0.068-x
We can then solve Kp = 389 = (0.068-x)/(x^2) by solving for x and then using the quadratic formula. Use this x to find the equilibrium partial pressures of all the reactants and products. To find the total pressure, add all these partial pressures together.
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