The bromination of acetone that occurs in acid solution is represented by this equation. CH_3 COCH_3( aq )+ Br_2( aq ) → CH_3 COCH_2 Br ( aq ) + H^+(…

The bromination of acetone that occurs in acid solution is represented by this equation. $$\begin{aligned} & \mathrm{CH}_3 \mathrm{COCH}_3(\mathrm{aq})+\mathrm{Br}_2(\mathrm{aq}) \rightarrow \mathrm{CH}_3 \mathrm{COCH}_2 \mathrm{Br}(\mathrm{aq}) \\ & +\mathrm{H}^{+}(\mathrm{aq})+\mathrm{Br}^{-}(\mathrm{aq}) \end{aligned} $$ These kinetic data were obtained for given reaction concentrations. Initial Concentrations, M

$\displaystyle \left[\mathrm{CH}_3 \mathrm{COCH}_3\right]$	$\displaystyle \left[\mathrm{Br}_2\right]$	$\displaystyle \left[\mathrm{H}^{+}\right]$
$\displaystyle 0.30$	$\displaystyle 0.05$	$\displaystyle 0.05$
$\displaystyle 0.30$	$\displaystyle 0.10$	$\displaystyle 0.05$
$\displaystyle 0.30$	$\displaystyle 0.10$	$\displaystyle 0.10$
$\displaystyle 0.40$	$\displaystyle 0.05$	$\displaystyle 0.20$

Initial Rate, disappearance of $\displaystyle \mathrm{Br}_2, \mathrm{M} \mathrm{~s}^{-1}$ $$\begin{aligned} & 5.7 \times 10^{-5} \\ & 5.7 \times 10^{-5} \\ & 1.2 \times 10^{-4} \\ & 3.1 \times 10^{-4} \end{aligned} $$ Based on these data, the rate equation is :