Phosphorus trichloride and phosphorus pentachloride equilibrate in the presence of molecular chlorine according to the following reaction:
(g) + (g) → (g)
An equilibrium mixture at 450 K contains = 0.124 bar, = 0.157 bar,and = 1.30 bar.
What is the value of K_p at this temperature?

Question

Phosphorus trichloride and phosphorus pentachloride equilibrate in the presence of molecular chlorine according to the following reaction:

(g) +

(g) →

(g)
An equilibrium mixture at 450 K contains Phosphorus trichloride and phosphorus pentachloride equilibrate in the presence of molecular chlorine according to the following reaction: (g) + (g) → (g) An equilibrium mixture at 450 K contains = 0.124 bar, = 0.157 bar,and = 1.30 bar. What is the value of Kp at this temperature? A) 66.8 B) 1.50 × C) 2.53 × 10-2 D) 1.02 E) 4.63

= 0.124 bar, Phosphorus trichloride and phosphorus pentachloride equilibrate in the presence of molecular chlorine according to the following reaction: (g) + (g) → (g) An equilibrium mixture at 450 K contains = 0.124 bar, = 0.157 bar,and = 1.30 bar. What is the value of Kp at this temperature? A) 66.8 B) 1.50 × C) 2.53 × 10-2 D) 1.02 E) 4.63

= 0.157 bar,and Phosphorus trichloride and phosphorus pentachloride equilibrate in the presence of molecular chlorine according to the following reaction: (g) + (g) → (g) An equilibrium mixture at 450 K contains = 0.124 bar, = 0.157 bar,and = 1.30 bar. What is the value of Kp at this temperature? A) 66.8 B) 1.50 × C) 2.53 × 10-2 D) 1.02 E) 4.63

= 1.30 bar.
What is the value of K_p at this temperature?

Quizplus · Accepted Answer

The equilibrium constant (Kp) can be found using the partial pressures of the products and reactants: Kp = (PCl3)^2/((PCl5)(Cl2)^2) Substituting the given values, we get: Kp = (0.124)^2/((0.157)(1.30)^2) = 66.8 The value of K_p is simply the value of Kp at the given temperature, so the answer is A) 66.8.

Phosphorus Trichloride and Phosphorus Pentachloride Equilibrate in the Presence of Molecular