The bromination of acetone that occurs in acid solution is represented by this equation. {CH}₃ {COCH}₃ \; { (aq.) } \; + {Br}₂ \; { (aq.) } \; arrow {CH}₃ {COCH}₂ {Br}({aq.}) + {H}^+ \; {(aq.)} \; + {Br}^- \; {(aq.)} These kinetic data were obtained from given reaction concentrations. Initial concentrations, (M) [{CH}₃ {COCH}₃] [{Br}₂] [{H}^+] 0.30 0.05 0.05 0.30 0.10 0.05 0.30 0.10 0.10 0.40 0.05 0.20 Initial rate, disappearance of {Br}₂, {Ms}^{-1} 5.7 × 10^{-5} 5.7 × 10^{-5} 1.2 × 10^{-4} 3.1 × 10^{-4} Based on these data, the rate equation is :

Question

Examsnet · Accepted Answer

Correct Answer is : Rate =k[CH3COCH3][H+]= k[{CH}₃ {COCH}₃][{H}^+]=k[CH3​COCH3​][H+]

$[\mathrm{CH}_3 \mathrm{COCH}_3]$	$[\mathrm{Br}_2]$	$[\mathrm{H}^+]$
$0.30$	$0.05$	$0.05$
$0.30$	$0.10$	$0.05$
$0.30$	$0.10$	$0.10$
$0.40$	$0.05$	$0.20$

AIPMT 2008 Physics and Chemistry Paper