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Chemistry rate reactions

  1. Sep 15, 2010 #1
    1. The problem statement, all variables and given/known data
    Is this first or second order rate? Calculate the rate constant and be certain to give its units.
    A (mM) / Time
    1 / 0
    .5 / 11
    .25 / 20
    .1 / 48
    .05 / 105

    2. Relevant equations
    Well wikipedia has both the first and second order integrated reactions there http://en.wikipedia.org/wiki/Rate_equation

    but I have a feeling that this is some sort of weird rate reaction.

    3. The attempt at a solution

    At first glance it looks like a second order rate but If I plug in in an attempt to find k none of the K values match. I also tried a first order reaction and that didn't work as well. Also due to the fact that the first three concentrations go down by half and the time is not consistent it is most likely not a simple first order exponential decay. You just need to trust me that plugging the times into the regular second order rate equation does not come out with a homogeneous rate constant.

    Well thanks guys in advanced i'm stumped.
    Last edited: Sep 15, 2010
  2. jcsd
  3. Sep 15, 2010 #2
    You can try the method of "half life reaction" it will give a n order (numeric)
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