Asked by Jack
Please help me with this question
For the system,
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
Is the system at equilibrium?
If yes, explain. If no, which way will the system shift to establish equilibrium?
For the system,
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
Is the system at equilibrium?
If yes, explain. If no, which way will the system shift to establish equilibrium?
Answers
Answered by
DrBob222
Jack,
Do you have a K<sub>p</sub> listed in your problem? I don't believe it's possible to work it without a K<sub>p</sub>. Of course we could make an educated guess, but even that wouldn't do much good without a temperature to help us. The Kp is what we need.
Do you have a K<sub>p</sub> listed in your problem? I don't believe it's possible to work it without a K<sub>p</sub>. Of course we could make an educated guess, but even that wouldn't do much good without a temperature to help us. The Kp is what we need.