CHM135H1 Lecture Notes - Lecture 1: Reaction Rate Constant, Reagent, Collision Theory

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13 Feb 2015
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CHM135H1 Full Course Notes
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CHM135H1 Full Course Notes
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It does not explain how a reaction takes place. It does not explain why reactions take place. Where is kinetics useful? atmospheric physics biochemistry archaeology etc. , etc. Kinetics explains how reactions take place: how a reaction occurs how quickly it occurs rate of reaction. Rate of reaction: how long a reaction takes to progress can (and want to!) measure rate: Rate depends upon: concentration of reactants, concentration of reactants, temperature, presence of catalyst, concentration of reactants. For a a + b b c c + d d, Rate law: rate (at any time) = k [a]m [b]n k = rate constant - independent of [ ] Dependent upon t m = order in a n = order in b. D[hcl] dt d[ch3chclch3] dt rate = k [hcl]n [ch3chch2]m where (experimentally determined): therefore also experimentally determined: k = 3. 76 x 10-3 at 25oc s-1 m-3. How is the rate law experimentally determined: the method of initial rates.

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