The equilibrium between nitrogen dioxide, \({\text{N}}{{\text{O}}_{\text{2}}}\), and dinitrogen tetroxide, \({{\text{N}}_{\text{2}}}{{\text{O}}_{\text{4}}}\), is shown below.

\[\begin{array}{*{20}{l}} {{\text{2N}}{{\text{O}}_{\text{2}}}{\text{(g)}} \rightleftharpoons {{\text{N}}_{\text{2}}}{{\text{O}}_{\text{4}}}{\text{(g)}}}&{{K_{\text{c}}} = 0.01} \end{array}\]

What happens when the volume of a mixture at equilibrium is decreased at a constant temperature?

I.     The value of \({K_{\text{c}}}\) increases

II.     More \({{\text{N}}_{\text{2}}}{{\text{O}}_{\text{4}}}\) is formed

III.     The ratio of \(\frac{{{\text{[N}}{{\text{O}}_{\text{2}}}{\text{]}}}}{{{\text{[}}{{\text{N}}_{\text{2}}}{{\text{O}}_{\text{4}}}{\text{]}}}}\) decreases

A.     I and II only

B.     I and III only

C.     II and III only

D.     I, II and III

C