What is the equilibrium constant expression, \({K_{\text{c}}}\), for the following reaction?

\[{\text{2NOBr(g)}} \rightleftharpoons {\text{2NO(g)}} + {\text{B}}{{\text{r}}_{\text{2}}}{\text{(g)}}\]

A.     \({K_{\text{c}}} = \frac{{{\text{[NO][B}}{{\text{r}}_{\text{2}}}{\text{]}}}}{{{\text{[NOBr]}}}}\)

B.     \({K_{\text{c}}} = \frac{{{{{\text{[NO]}}}^{\text{2}}}{\text{[B}}{{\text{r}}_{\text{2}}}{\text{]}}}}{{{{{\text{[NOBr]}}}^{\text{2}}}}}\)

C.     \({K_{\text{c}}} = \frac{{{\text{2[NO]}} + {\text{[B}}{{\text{r}}_{\text{2}}}{\text{]}}}}{{{\text{[2NOBr]}}}}\)

D.     \({K_{\text{c}}} = \frac{{{{{\text{[NOBr]}}}^{\text{2}}}}}{{{{{\text{[NO]}}}^{\text{2}}}{\text{[B}}{{\text{r}}_{\text{2}}}{\text{]}}}}\)

B