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