The bromination of acetone that occurs in acid solution is represented by `CH_(3)COCH_(3)(aq)+Br_(2)(aq)rarrCH_(3)COCH_(2)Br(aq)+H^(+)(aq)+Br^(-)(aq)`
These kinetic data were obtained for given reaction concentration

Based on these data rate equation is

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_(3)COCH_(3)][Br_(2)]`

Answer

C

Explanation

Rate `k[CH_(3)COCH_(3)]^(alpha)[Br_(2)]^(beta)[H^(+)]^(gamma)`
Dividing eq(i) by eq (ii) `1=[1/2]^(beta) i.e beta=0`
Dividing eq (i) by eq (iv) `(5.7 xx10^(-5))/(3.1xx10(^-4))=[3/4]^(alpha)xx[1/4]^(1)`
`alpha=1` thus rate law will be rate =`k[CH_(3)COCH_(3)]^(1)[H^(+)]^(1)`