The Iodination of Acetone lab- Need help with determining the reaction orders

  1. I need to find the variable m in the following equation
    rate=k(acetone)m(I2)n(H+)p

    Here is our expirmental data
    Exp. 1
    10 ml of 4 M acetone + 10 ml of 1 M HCl + 10 ml 0.005 M I2 reacted in 68 sec.
    Exp. 2
    20 ml of 4 M acetone + 10 ml of 1 M HCl + 10 ml 0.005 M I2 reacted in 27.6 sec.


    I calculated the initial concentration of each to be
    Exp. 1 (Acetone)=0.8 M (H+)=0.2M (I2)=0.001M
    Exp. 1 (Acetone)=1.6 M (H+)=0.2M (I2)=0.001M
    I found the rate of reaction to be
    Exp. 1 = 1.47 * 10-5
    Exp. 2 = 3.63 * 10-5

    Then I plugged the data into the equation
    rate=k(acetone)m(I2)n(H+)p
    and solved for "m"
    but i got 1.26

    My question is whether or not this number is even close and if it is should I just round it to 1 or what is the correct answer?
     
  2. jcsd
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