CHEM102 Lecture Notes - Lecture 6: Transition State Theory, Collision Frequency, Elementary Reaction

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24 Sep 2017
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CHEM102 Full Course Notes
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From the diagram, only one out of five collisions is favourable. In reality, only 1 out of 167 collisions would have the correct orientation. The collision frequency factor a, of the arrhenius equation (k = ae-ea/rt) is dependent on the orientation of the molecules (probability of successful collision, p and collision frequency, z) Orientation probability p varies from 1 to 10-6 for most reactions. Z (collision frequency) is dependent on the size of the molecule. For a reaction with rate = k [a] [b] Rate of reaction = pz x e-ea/rt [a] [b] Rate of reaction = orientation factor x energy factor x collision frequency. This theory depicts the potential energy change of molecules during a collision leading to a reaction. It is assumed that in every reaction (or every step in an overall reaction), a transition state is formed. When molecules approach each other, there is strong repulsion between the electron clouds when they get too close.

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