At a certain temperature, the given reaction has an equilibrium constant of Kp=349.
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?
question 4
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Re: question 4
You would use the ice chart and find the individual concentrations of the prodcts/reactants using the given k value and the initial value. You cannot assume small x since the k value is not that small. Once you have found the individual molarities of all of them add them up to get the total pressure.
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Re: question 4
use an ICE table:
initial: PCl3=0, Cl2=0, PCl5=0.0680 bar
change: PCl3= +x, Cl2=+x, PCl5= - x
equilibrium: x, x, 0.0680 bar - x
Then use Kp value to find x.
349=(0.0680 - x)/x^2
Find x and plug it back into the equilibrium row of the ice table and sum up the total pressure.
Hope this helps.
initial: PCl3=0, Cl2=0, PCl5=0.0680 bar
change: PCl3= +x, Cl2=+x, PCl5= - x
equilibrium: x, x, 0.0680 bar - x
Then use Kp value to find x.
349=(0.0680 - x)/x^2
Find x and plug it back into the equilibrium row of the ice table and sum up the total pressure.
Hope this helps.
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- Posts: 98
- Joined: Fri Sep 24, 2021 6:07 am
Re: question 4
Just to add onto the previous replies, don't forget that when you make your final equation using the Kp value, you will probably need to rearrange the equation to be a quadratic in order to find the ending value of x!
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