A mixture of 2.0 mol of \({{\text{H}}_{\text{2}}}\) and 2.0 mol of \({{\text{I}}_{\text{2}}}\) is allowed to reach equilibrium in the gaseous state at a certain temperature in a \({\text{1.0 d}}{{\text{m}}^{\text{3}}}\) flask. At equilibrium, 3.0 mol of HI are present. What is the value of \({K_{\text{c}}}\) for this reaction?

\[{{\text{H}}_{\text{2}}}{\text{(g)}} + {{\text{I}}_{\text{2}}}{\text{(g)}} \rightleftharpoons {\text{2HI(g)}}\]

A.     \({K_{\text{c}}} = \frac{{{{(3.0)}^2}}}{{{{(0.5)}^2}}}\)

B.     \({K_{\text{c}}} = \frac{{3.0}}{{{{(0.5)}^2}}}\)

C.     \({K_{\text{c}}} = \frac{{{{(3.0)}^2}}}{{{{(2.0)}^2}}}\)

D.     \({K_{\text{c}}} = \frac{{{{(0.5)}^2}}}{{{{(3.0)}^2}}}\)

A