Question

2 upper N upper o upper c l double-headed arrow 2 upper N upper O (g) plus upper C l subscript 2 (g).

At equilibrium, the concentrations are as follows.


[NOCl] = 1.4 ´ 10–2 M

[NO] = 1.2 ´ 10–3 M

[Cl2] = 2.2 ´ 10–3 M

Answer 1

Answer: The equilibrium constant for the reaction is 0.000016.

Step-by-step explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric coefficients.

The given balanced equilibrium reaction is,

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

The expression for equilibrium constant for this reaction will be,

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

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

`K_c=((1.2* 10^(-3))^2* (2.2* 10^(-3)))/((1.4* 10^(-2))^2)`

`K_c=0.000016`

Thus the equilibrium constant for the reaction is 0.000016.