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:

$K_p=\frac{(p_{NOCl})^2}{(p_{NO})^2(p_{Cl_2})}$

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

$K_p=\frac{(1.35)^2}{(0.240)^2(0.608)}$

$K_p=52.0$

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