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Rate of Reaction

  1. Oct 30, 2012 #1
    1. The problem statement, all variables and given/known data

    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 7.6


    Deduce the order of the reaction with respect to each reactant and also the overall order of the reaction.



    2. Relevant equations



    3. 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: Oct 30, 2012
  2. jcsd
  3. Oct 31, 2012 #2

    AGNuke

    User Avatar
    Gold Member

    I didn't quite understand the table itself.
     
  4. Nov 1, 2012 #3
    Yeah the table didn't come out right.

    But I figured out how to work the problem.
     
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