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Chemical Kinetics: Reaction Mechanism

  1. Feb 20, 2010 #1
    1. The problem statement, all variables and given/known data

    1. According to the mechanism below, what is the correct expression for the rate of consumption of A? In the mechanism, M is a molecule that collides with A and A* is a highly-energized form of A.

    Step 1 (reversible): A + M <---> A* + M rate constants k1 and k-1

    Step 2 (irreversible): A* ---> C rate constant k2

    Select one of the following:

    Rate = k1 [A] [M] / (k-1[M] + k2)
    Rate = [A] / [C]
    Rate = k1k2 [A] [M] / (k-1[M] + k2)
    Rate = k1k2 [A]
    Rate = k1[A]
    Rate = (k1 [A] [M] + k-2[C] ) / (k-1[M] + k2)
    Rate=k1k2 / (k-1+k-2)
    Rate = (k1+k2-k-1-k-2) [A]
    Rate = k1k2 [A] / (k-1+k2[M])
    Rate=k1+k2-k-1-k-2
    Rate = [C] / [A]
    Rate = k1k2 [A] [M] / k-1


    2. Relevant equations



    3. The attempt at a solution

    I tried to assume a steady-state approximation as I'm not sure which is the slow step. I found the overall rate of reaction and assumed it to be equivalent to the consumption of A.
     
  2. jcsd
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