The bromination of acetone that occurs in acid solution is represented by this equation. ${CH}_{3} {COCH}_{3} (aq) {+ Br}_{2} (aq)$ $\to {CH}_{3} {COCH}_{2} Br (aq) {+ H}^{+} (aq) {+ H}^{+} (aq) {+ Br}^{-} (aq)$
These kinetic data were obtained for given reaction concentrations. Based on given data, the rate equations is :

see full answer

Your Exam Success, Personally Taken Care Of

1:1 expert mentors customize learning to your strength and weaknesses – so you score higher in school , IIT JEE and NEET entrance exams.

An Intiative by Sri Chaitanya

$Rate = k [{CH}_{3} {COCH}_{3}] [H^{+}]$

$Rate = k [{CH}_{3} {COCH}_{3}] [{Br}_{2}]$

$Rate = k [{CH}_{3} {COCH}_{3}] [Br] [H^{+}]$

$Rate = k [{CH}_{3} {COCH}_{3}] [{Br}_{2}] {[H^{+}]}^{2}$

answer is A.

(Unlock A.I Detailed Solution for FREE)

Best Courses for You

JEE

NEET

Foundation JEE

Foundation NEET

CBSE

Detailed Solution

Rewriting the given data for the reaction

${CH}_{3} {COCH}_{3} (aq) {+ Br}_{2} (aq) \overset{H^{+}}{\to}$ ${CH}_{3} {COCH}_{2} Br (aq) {+ H}^{+} (aq) {+ Br}^{-} (aq)$

S.No	$\begin{array}{l} Initial concentration \\ {of CH}_{3} {COCH}_{3} in M \end{array}$	$\begin{array}{l} Initial concen. \\ {of Br}_{2} in M \end{array}$	$\begin{array}{l} Initial conc. \\ {of H}^{+} in M \end{array}$	$\begin{array}{l} Rate of disappearance of \\ B r_{2} i n M s^{- 1} i . e . - \frac{d}{d t} [B r_{2}] o r \frac{d x}{d t} \end{array}$
1.	0.30	0.05	0.05	$5.7 \times 10^{- 5}$
2.	0.30	0.10	0.05	$5.7 \times 10^{- 5}$
3.	0.30	0.10	0.10	$1.2 \times 10^{- 4}$
4.	0.40	0.05	0.20	$3.1 \times 10^{- 4}$

Actually this reaction is auto catalyzed and involvers complex calculation for concentration terms. We can look at the above results in a simple way to find the dependence of reaction rate (i.e., rate of disappearance of ${Br}_{2}$ ). From data (1) and (2) in which concentration of ${CH}_{3} {COCH}_{3} {and H}^{+}$ remain unchanged and only the concentration of ${Br}_{2}$ is doubled, there is no change in rate of reaction. It means the rate of reaction is independent of concentration of ${Br}_{2}$ .Again form (2) and (3) in which $({CH}_{3} {COCH}_{3}) and ({Br}_{2})$ remain constant but $H^{+}$ increases from 0.05 M to 0.10 i.e. doubled. The rate of reaction changes from ${5.7 × 10}^{-5} {to 1.2 × 10}^{-4}$ , thus it also becomes almost doubled. It shows that rate of reaction is directly proportional to $[H^{+}]$ . From (3) and (4), the rate should have doubled due to increase in conc of $[H^{+}]$ from 0.10