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 concentrations :

Based on these data, rate equations 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)]`

Explanation

`"Rate"=k[CH_(3)COCH_(3)]^(alpha)[Br_(2)]^(beta)[H^(+)]^(gamma)`
`5.7xx10^(-5)=k[[0.30]^(alpha)[0.05]^(beta)[0.05]^(gamma)" ".....(i)`
`5.7xx10^(-5)=k[0.30]^(alpha)[0.10]^(beta)[0.05]^(gamma)" ".....(ii)`
`1.2xx10^(-4)=k[0.30]^(alpha)[0.10]^(beta)[0.10]^(gamma)" ".....(iii)`
`3.1xx10^(-4)=k[0.40]^(alpha)[0.05]^(beta)[0.20]^(gamma)" ".....(iv)`
Divinding eq. (i), be eq. (ii)
`1=[(1)/(2)]^(beta),i.e.,beta=0`
Dividing eq. (ii) by eq. (ii),
`1=[(1)/(2)]^(gamma),i.e.,gamma=1`
Dividing eq (i) by eq. (iv)
`(5.7xx10^(-5))/(3.1xx10^(-4))=[(3)/(4)]^(alpha)xx[(1)/(4)]^(1)`
Thus, rate law will be
rate `k=[CH_(3)COCH_(3)]^(1)[H^(+)]^(1)`