Question
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:
PCl5 = 0.012 atm
PCl3 = 0.90 atm
Cl2 = 0.45 atm
Kp = 26 @300 C degree
Is the system at equilibrium?
If yes, explain. If no, which way will the system shift to establish equilibrium?
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:
PCl5 = 0.012 atm
PCl3 = 0.90 atm
Cl2 = 0.45 atm
Kp = 26 @300 C degree
Is the system at equilibrium?
If yes, explain. If no, which way will the system shift to establish equilibrium?
Answers
It's a good thing you have provided the equilibrium constant Kp for that reaction. I was not able to find it.
If the mixture were at equilibrium, you would have
Pcl3*Pcl2/Ppcl5 = 26
In this case, that ratio is
.9*.45/.012 = 33.8
There are more products than there would be at equilibrum, so the reaction will favor the reverse direction.
If the mixture were at equilibrium, you would have
Pcl3*Pcl2/Ppcl5 = 26
In this case, that ratio is
.9*.45/.012 = 33.8
There are more products than there would be at equilibrum, so the reaction will favor the reverse direction.
28
Related Questions
Look at my previous post....
Can anyone please answer my science question???
well what's the quest...
Is there any way that the postings could be numbered?
The post below this one by TONY obviously re...
Question 5
If you want your Facebook post to be seen by an audience outside of your followers, you...
What kinds of comments should a person post or not post online to maintain safety and etiquette?...