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).

Answer 1

Answer: The equilibrium constant for the reaction is 0.000016.

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,

$K_c=\frac{[NO]^2[Cl_2]}{[NOCl]^2}$

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

$K_c=\frac{(1.2\times 10^{-3})^2\times (2.2\times 10^{-3})}{(1.4\times 10^{-2})^2}$

$K_c=0.000016$

Thus the equilibrium constant for the reaction is 0.000016.