Consider the following reaction.

\[{\text{5B}}{{\text{r}}^ - }{\text{(aq)}} + {\text{BrO}}_3^ - {\text{(aq)}} + {\text{6}}{{\text{H}}^ + }{\text{(aq)}} \to {\text{3B}}{{\text{r}}_2}{\text{(aq)}} + {\text{3}}{{\text{H}}_2}{\text{O(l)}}\]

The rate expression for the reaction is found to be:

\[{\text{rate}} = k{\text{[B}}{{\text{r}}^ - }{\text{][BrO}}_3^ - {\text{][}}{{\text{H}}^ + }{{\text{]}}^2}\]

Which statement is correct?

A.     The overall order is 12.

B.     Doubling the concentration of all of the reactants at the same time would increase the rate of the reaction by a factor of 16.

C.     The units of the rate constant, \(k\), are \({\text{mol}}\,{\text{d}}{{\text{m}}^{ - 3}}{{\text{s}}^{ - 1}}\).

D.     A change in concentration of \({\text{B}}{{\text{r}}^ - }\) or \({\text{BrO}}_3^ - \) does not affect the rate of the reaction.

B