The bromination of acetone that occurs in acid solution is represented by this equation.
${\mathrm{CH}}_3{\mathrm{COCH}}_3\left(\mathrm{aq}\right)+{\mathrm{Br}}_2\left(\mathrm{aq}\right)\to$
${\mathrm{CH}}_3{\mathrm{COCH}}_2\mathrm{Br}\left(\mathrm{aq}\right)+{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+{\mathrm{Br}}^{-}\left(\mathrm{aq}\right)$
These kinetic data were obtained for given reaction concentrations. Initial concentrations, M

Based on these data, the rate equation is

Here, Rate of disappearance of ${\mathrm{Br}}_2=$ Rate of reaction.
- On comparing (1) & (2)
On doubling the concentration of ${\mathrm{Br}}_2$, there is no change in the rate of reaction.
$\Rightarrow$order wrt ${\mathrm{H}}_2=1$.
- On comparing (3) & (4)

$$\begin{gathered} \left[{\mathrm{CH}}_3{\mathrm{COCH}}_3\right]\to \frac{4}{3}\left[{\mathrm{CH}}_3{\mathrm{COCH}}_3\right] \\ and \\ \left[{\mathrm{H}}^{+}\right] \to 2\left[{\mathrm{H}}^{+}\right] \\ \text{ the rate became }\frac{8}{3}\text{ times of itself. } \\ \Rightarrow \text{ order wrt }{\mathrm{CH}}_3{\mathrm{COCH}}_3=1\text{. } \\ \therefore \text{ Rate equation }\Rightarrow \text{ rate }=\mathrm{K}\left[{\mathrm{CH}}_3{\mathrm{COCH}}_3\right] \left[{\mathrm{H}}^{+}\right] \end{gathered}$$