The bromination of acetone is acid catalyzed:H+ catalystCH3COCH3 + Br2 = CH3COCH2Br + H+ + BrβThe rates of reaction were determined by measuring the rates of disappearance of bromine using different concentrations of acetone, bromine, and H+ ions, and the following data were obtained at a certain temperature.Rate of disappearanceExpt# [CH3COCH3] [Br2] [H+] of Br2 (mol Β· Lβ1 Β· sβ1)(M) (M) (M) _1 0.30 0.050 0.050 5.9 x 10β52 0.30 0.10 0.050 5.9 x 10β53 0.30 0.050 0.10 1.2 x 10β44 0.15 0.050 0.050 2.9 x 10β5βββββββββββββββββββββββββββ(a) Determine the rate law for the reaction and calculate the rate constant.(b) The following mechanism has been proposed for the reaction:O OH+β βStep-1: CH3-C-CH3 + H3O+ β CH3-C-CH3 + H2O (fast equilibrium)OHβStep-2: (CH3)2CβOH+ + H2O = CH3-CβCH2 + H3O+ (slow)OH Oβ βStep-3: CH3-CβCH2 + Br2 = CH3-C-CH2Br + HBr (fast)Show that the rate law deduced from the mechanism is consistent with that shown in part (a).(Answer: (a) Rate = k[CH3COCH3][H3O+]; k = 3.9 x 10β3 Mβ1 β sβ1)