The bromination of acetone that occurs in acid solution is represented by this equation. <br> $CH_3COCH_3(aq.)+Br_2(aq.)\longrightarrow CH_3COCH_2Br(aq)+H^+(aq)+Br^-(aq.)$ <br> These kinetic data were obtained from given reaction concentrations. <br> <br> Initial rate, disappearance of $Br_2, Ms^{-1}$ <br> $5.7 \times 10^{-5}$ <br> $5.7 \times 10^{-5}$ <br> $1.2 \times 10^{-4}$ <br> $3.1 \times 10^{-4}$ <br> Based on these data, the rate equation is :

Question

( A ) Rate =$K[CH_3COCH_3][H^+]$
( B ) Rate = $K[CH_3COCH_3][Br][H^+]^2$
( C ) Rate = $K[CH_3COCH_3][Br_2][H^+]$
( D ) Rate = $K[CH_3COCH_3][Br_2]$