# The bromination of acetone that occurs in acid solution is represented by this equation $CH_3COCH_3(aq)+Br_2(aq) \rightarrow CH_3COCH_2Br(aq) +H^+(aq)+Br^-(aq)$

 Initial Concentrations, M [$CH_3COCH_3$] [$Br_2$] [$H^+$] 0.30 0.05 0.05 0.30 0.10 0.05 0.30 0.10 0.10 0.40 0.05 0.20

Initial rate, disapperance of $Br_2,Ms^{-1}$

$\begin {array} {1 1} (1)\;5.7 \times 10^{-5} & \quad (2)\;5.7 \times 10^{-5} \\ (3)\;1.2 \times 10^{-4} & \quad (4)\;3.1 \times 10^{-4} \end {array}$

Based on these data, the rate equation is :

$\begin {array} {1 1} (1)\;Rate=K[CH_3COCH_3][Br_2][H^+] & \quad (2)\;Rate=K[CH_3COCH_3][H^+] \\ (3)\;Rate=K[CH=COCH_3][Br_2] & \quad (4)\;Rate=K[CH_3COCH_3][Br_2][H^+]^2 \end {array}$

Can you answer this question?