At 25C, an equilibrium mixture of gases con- tains 0.00680 mol/L PCl3, 0.0290 mol/L Cl2, and 0.00500 mol/L PCl5.
PCl5(g) ⇀ ↽ PCl3(g) + Cl2(g)
What is the equilibrium constant for the reaction?
How would I do this? I'm so confused!
There isn't anything here to be confused about.
............PCl5 --> PCl3 + Cl2
E.........0.00500..0.00680..0.0290
What's K.
Kc = (PCl3)(Cl2)/(PCl5)
Plug in the equilibrium numbers and solve for Kc.
So I disregard the temperature?
To determine the equilibrium constant for the given reaction, you need to use the concentrations of the reactants and products at equilibrium. The equilibrium constant is denoted by K and it relates the concentration of the products to the concentration of the reactants.
In this case, you are given the concentrations of PCl3, Cl2, and PCl5 at equilibrium. You will use these values to calculate the equilibrium constant for the reaction.
The equilibrium constant expression for the reaction is given by:
K = [PCl3] * [Cl2] / [PCl5]
Now let's substitute the given concentrations into the equation:
K = (0.00680 mol/L) * (0.0290 mol/L) / (0.00500 mol/L)
K = 0.198 / 0.005
K = 39.6
Therefore, the equilibrium constant (K) for the reaction is 39.6.
Remember, to calculate the equilibrium constant for any reaction, you need to know the concentrations of the reactants and products at equilibrium, and then use those values to calculate K using the equilibrium constant expression.