The bromination of acetone which occurs in acid solution is represented by the equation: CH_(3)COCH_(3)(aq) + Br_(2)(aq) to CH_(3)COCH_(2)Br(aq) + H^(+)(aq) + Br^(-1)(aq) The following kinetic data was obtained for the given reaction concentration: Initial rates of disappearance of of Br_(2)(Ms^(-1) 5.7 xx 10^(-5), 5.7 xx 10^(-5) 1.2 xx 10^(-4), 3.1 xx 10^(-4) Based on these data, the rate equation is:

The bromination of acetone which occurs in acid solution is represente

1.	The bromination of acetone which occurs in acid solution is represented by the equation: CH_(3)COCH_(3)(aq) + Br_(2)(aq) to CH_(3)COCH_(2)Br(aq) + H^(+)(aq) + Br^(-1)(aq) The following kinetic data was obtained for the given reaction concentration: Initial rates of disappearance of of Br_(2)(Ms^(-1) 5.7 xx 10^(-5), 5.7 xx 10^(-5) 1.2 xx 10^(-4), 3.1 xx 10^(-4) Based on these data, the rate equation is:
Answer» RATE = `k[CH_(3)COCH_(3)][Br_(2)][H^(+)]^(2)` Rate = `k[CH_(3)COCH_(3)][Br_(2)][H^(+)]` Rate = `k[CH_(3)COH_(3)][H^(+)]` Rate = `k[CH_(3)COCH_(3)][Br_(2)]` Solution :c) From the first two experiments, it is clear that when the concentration of `Br_(2)` is doubled, the initial rate of disappearance of `Br_(2)` remains unchanged. This means that order of reaction with RESPECT to `Br_(2)` is zero. The PROBABLY rate LAW for the reaction will be: `k[CH_(3)COCH_(3)][H^(+)]`