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 : 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:

Initial conc.     0.53          0.64              0

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

The expression for equilibrium constant is:

As we are given that:

2x = 0.36 M

x = 0.18 M

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

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