The bromination of acetone that occurs in acid solution is represented by this equation.
`CH_(3)COCH_(3) (aq) + Br_(2) (aq) rarr`
`CH_(3)COCH_(2) Br(aq) + H^(+) (aq) + Br(aq)`
These kinetic data were obtained for given reaction concentrations.
Initial concentration, `M`
`{:([CH_(2)COCH_(3)],[Br_(2)],[H^(+)],("Initail rate) (disappearance of "Br_(2)),),(0.30,0.05,0.05,5.7 xx 10^(-5),),(0.30,0.10,0.05,5.7xx10^(-5),),(0.30,0.10,0.10,1.2xx10^(-4),),(0.40,0.5,0.20,3.1xx10^(-4),):}`

Options

A. Rate `=k[CH_(3)COCH_(3)][Br_(2)][H^(+)]^(2)`
B. Rate `=k[CH_(3)COCH_(3)][Br_(2)][H^(+)]`
C. Rate `=k[CH_(3)COCH_(3)][H^(+)]`
D. Rate `=k[CH=COCH_(3)][Br_(2)]`

Answer

C

Explanation

According to the given data, when concentration of `Br_(2)` is doubled, the initial rate of disappearance of `Br_(2)` remains unaffected. So order of reaction with respect to `Br_(2)` is zero. The rate law for the reaction will be :
`k[CH_(3)COCH_(3)][H^(+)]`