Vatche Kaprielian
New member
Basic info:
When 9.25 of ClF3 was introduced into an empty 2.00 L container at 700.0 K, 19.8% of the ClF3 decomposed to give an equilibrium mixture of ClF3, ClF, and F2. ClF3(g) --> and <--- ClF(g) + F2(g)
Part 1:
What is the value of the equilibrium constant Kc at 700.0K ?
Part 2:
What is the value of the equilibrium constant Kp at 700.0K ?
Part 3:
In a separate experiment, 41.6 g of ClF3 was introduced into an empty 2.00 L container at 700.0 K . What are the concentrations of ClF3, ClF, and F2 when the mixture reaches equilibrium?
No matter what I try, I keep getting the wrong answer, please help!
When 9.25 of ClF3 was introduced into an empty 2.00 L container at 700.0 K, 19.8% of the ClF3 decomposed to give an equilibrium mixture of ClF3, ClF, and F2. ClF3(g) --> and <--- ClF(g) + F2(g)
Part 1:
What is the value of the equilibrium constant Kc at 700.0K ?
Part 2:
What is the value of the equilibrium constant Kp at 700.0K ?
Part 3:
In a separate experiment, 41.6 g of ClF3 was introduced into an empty 2.00 L container at 700.0 K . What are the concentrations of ClF3, ClF, and F2 when the mixture reaches equilibrium?
No matter what I try, I keep getting the wrong answer, please help!