Lec 05 Jan 14 Wed - Complete Handout 1 Summary of Rate...

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1.12 3. Arrhenius Model (14-8) Why are some reactions frst-order and some others reactions second- order? To understand this you have to look at the molecular level. BUT • actually observed rate is smaller than the rate of collisions of molecules with enough energy to form products… • collisions need the proper relative orientation in order to make products. • molecules must collide to react • however, only a small fraction of collisions leads to products • an energy threshold (minimum energy) is needed to obtain a successful chemical reaction • this must mean that some molecules don’t have sufficient energy to form products. From kinetic molecular theory of gases, we know that the average kinetic energy of a gas depends on temperature We will assume: As T is increased, the fraction of molecules with E > E min = E a increases (more successful collisions at higher temperature) (Fig. 14-8) Fraction with enough energy to form product Fraction of molecules with enough energy = e Ea RT
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Lec 05 Jan 14 Wed - Complete Handout 1 Summary of Rate...

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