Question

Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reaction: PCl3 (g) + Cl2 (g) → PCl5 (g) An equilibrium mixture at 450 K contains PPCl3 = 0.348 atm, PCl2 = 0.441 atm, and PPCl5 = 10.24 atm. What is the value of Kp at this temperature? Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reaction: (g) + (g) (g) An equilibrium mixture at 450 K contains = 0.348 atm, = 0.441 atm, and = 10.24 atm. What is the value of Kp at this temperature? 66.7 1.50 ⋅ 10−2 12.99 1.57 9.45

Answer 1

Answer : The value of
`K_p` at this temperature is 66.7

Explanation : Given,

Pressure of
`PCl_3` at equilibrium = 0.348 atm

Pressure of
`Cl_2` at equilibrium = 0.441 atm

Pressure of
`PCl_5` at equilibrium = 10.24 atm

The balanced equilibrium reaction is,

`PCl_3(g)+Cl_2(g)\rightleftharpoons PCl_5(g)`

The expression of equilibrium constant
`K_p` for the reaction will be:

`K_p=((p_(PCl_5)))/((p_(PCl_3))(p_(Cl_2)))`

Now put all the values in this expression, we get :

`K_p=((10.24))/((0.348)(0.441))`

`K_p=66.7`

Therefore, the value of
`K_p` at this temperature is 66.7