S10_Student_Lecture_05

S10_Student_Lecture_05 - 1/27/10 Differential Rate Law aA +...

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Differential Rate Law aA + bB products rate = - [A]/ t = k [A] m [B] n Called “differential” because instantaneous rate is equated with the “derivative” of the concentration (or the slope of the tangent of our [A] vs time plot at time t) - [A]/ t ~-d[A]/dt Relates rate as a function of concentration Ex. What is the initial rate when [A] = 1 M and [B] = 2 M? We used initial rates at defined concs. to determine reaction order and rate constant k 1/27/10
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Integrated Rate Law: relates concentration as a function of time Obtained by “integrating” the differential rate law Why do we need it? Why do it? 1. Integrated rate laws can be used to determine long a reaction takes or how much reactant or product is present at a given time 2. The integrated form of the rate law depends on the a new of the reaction. 3. They provide a new way to determine… 4. For simplicity, we will only look at one reactant reactions, [A], where the product does not affect rate
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Integrated Rate Laws First Order = Differential Rate Law t t t t d = [A]/ t = ln [ A ] 0 [ A ] t = kt
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Integrated Rate Laws First Order Zero order n = 0 Second order n = 2 First order n = 1 Ln [A] 0 _________________
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S10_Student_Lecture_05 - 1/27/10 Differential Rate Law aA +...

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