At a certain temperature, the given reaction has an equilibrium constant of Kp=359 .
PCl3(g)+Cl2(g)↽−−⇀PCl5(g)
PCl5 is placed in a sealed container at an initial pressure of 0.0640 bar . What is the total pressure at equilibrium?
I am still a little bit confused on the steps to solve this if someone can explain it would be great.
Can someone help me understand how to solve this part of the homework from week 1?
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Re: Can someone help me understand how to solve this part of the homework from week 1?
PCl3(g) +Cl2(g) <--> PCl5(g)
Since we are given the initial pressure of PCl5, we find the equilibrium concentrations of the reverse reaction and use the inverse of the given Kp to find the total pressure.
Given
Kp= 359
Initial Partial Pressure of PCl5= 0.0640 bar
We are trying to determine the total pressure at equilibrium. The total pressure equals the sum between all the equilibrium partial pressure. So we need to find the equilibrium partial pressures and add them up.
PCl5 Cl2 PCl3
I 0.0640 0 0
C -x +x. +x
E. 0.0640 -x. x x
Kp= ((X^2)/(0.0640-x)) = 1/359.
From here solve for the value of x.
x= 0.012
Then use x to find the equilibrium pressures of PCl5, Cl2, and PCl3.
P(PCl5)= 0.0640-0.012= 5.2*10^-2
P(Cl2)=P(PCl3)= 0.012
Finally, add up the equilibrium pressures you calculate to determine the total pressure.
So total pressure = 2(0.012) + (5.2*10^-2) = 7.6 * 10^-2.
Since we are given the initial pressure of PCl5, we find the equilibrium concentrations of the reverse reaction and use the inverse of the given Kp to find the total pressure.
Given
Kp= 359
Initial Partial Pressure of PCl5= 0.0640 bar
We are trying to determine the total pressure at equilibrium. The total pressure equals the sum between all the equilibrium partial pressure. So we need to find the equilibrium partial pressures and add them up.
PCl5 Cl2 PCl3
I 0.0640 0 0
C -x +x. +x
E. 0.0640 -x. x x
Kp= ((X^2)/(0.0640-x)) = 1/359.
From here solve for the value of x.
x= 0.012
Then use x to find the equilibrium pressures of PCl5, Cl2, and PCl3.
P(PCl5)= 0.0640-0.012= 5.2*10^-2
P(Cl2)=P(PCl3)= 0.012
Finally, add up the equilibrium pressures you calculate to determine the total pressure.
So total pressure = 2(0.012) + (5.2*10^-2) = 7.6 * 10^-2.
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