Question

Consider the reaction between NONO and Cl2Cl2 to form NOClNOCl: 2NO(g)+Cl2(g)⇌2NOCl(g)2NO(g)+Cl2(g)⇌2NOCl(g) A reaction mixture at a certain temperature initially contains only [NO]=[NO]= 0.53 MM and [Cl2]=[Cl2]= 0.64 MM. After the reaction comes to equilibrium, the concentration of NOClNOCl is 0.36 MM. Part A Find the value of the equilibrium constant (Kc)(Kc) at this temperature.

Answer 1

Answer : The value of equilibrium constant (Kc) is, 9.75

Explanation :

Now we have to calculate the value of equilibrium constant (K).

The given chemical reaction is:

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

Initial conc. 0.53 0.64 0

At eqm. (0.53-2x) (0.64-x) 2x

The expression for equilibrium constant is:

`K_c=([NOCl]^2)/([NO]^2[Cl_2])`

As we are given that:

2x = 0.36 M

x = 0.18 M

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

`K_c=((2x)^2)/((0.53-2x)^2* (0.64-x))`

`K_c=((2* 0.18)^2)/((0.53-2* 0.18)^2* (0.64-0.18))`

`K_c=9.75`

Thus, the value of equilibrium constant (Kc) is, 9.75