Question

The partial pressures in an equilibrium mixture of NO, Cl2, and NOCI at 500 K are as follows: PNo = 0.240 atm, Pel2 = 0.608 atm, and PNoci= 1.35 atm. What is Kp at 500 K for the reaction: 2 NO (g) + Cl2(g) + 2NOCI (g)?

Answer 1

Answer : The value of
`K_p` at temperature 500 K is 52.0

Explanation : Given,

Partial pressure of
`NO` at equilibrium = 0.240 atm

Partial pressure of
`Cl_2` at equilibrium = 0.608 atm

Partial pressure of
`NOCl` at equilibrium = 1.35 atm

The balanced equilibrium reaction is,

`2NO(g)+Cl_2(g)\rightleftharpoons 2NOCl(g)`

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

`K_p=((p_(NOCl))^2)/((p_(NO))^2(p_(Cl_2)))`

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

`K_p=((1.35)^2)/((0.240)^2(0.608))`

`K_p=52.0`

Therefore, the value of
`K_p` at temperature 500 K is 52.0