Rate of Reaction Homework: Bromination of Acetone Order

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The discussion focuses on determining the order of the bromination reaction of acetone, which is catalyzed by acid. The rate of disappearance of bromine was measured across various concentrations of acetone, bromine, and hydronium ion. Initial calculations suggested an order of reaction that was later corrected, indicating a misunderstanding of the data presented in the table. The user ultimately resolved their confusion and successfully worked through the problem. The key takeaway is the importance of accurately interpreting experimental data to deduce reaction orders.
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Homework Statement



The bromination of acetone is catalyzed by acid.

CH3COCH3 + Br2 + H2O ------> CH3COCH2 + Br- + H3O+

The rate disappearance of bromine was measured for several different initial concentration of acetone, bromine and hydronium ion as represented in the following table

Initial concentration
(mol L-1) Initial of rate of change [Br2] (x10-5)
Run [CH3COCH][Br2][H3O+] (mol-s s-1)
1 0.30 0.05 0.05 5.7
2 0.30 0.10 0.05 5.7
3 0.30 0.05 0.10 12.0
4 0.40 0.05 0.20 31.0
5 0.40 0.05 0.05 7.6Deduce the order of the reaction with respect to each reactant and also the overall order of the reaction.

Homework Equations


The Attempt at a Solution

[CH3COCH3]

Rate 4/Rate 3 = 31e10-5/12e10-5=k(0.40)en(0.05)em/k(0.30)en(0.05)en
= 2.58 =1.33en

n=2.08

This is not right. I don't know what I'm doing wrong. someone please help me.
 
Last edited:
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I didn't quite understand the table itself.
 
Yeah the table didn't come out right.

But I figured out how to work the problem.
 

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