L4_115b08

L4_115b08 - L4: First exam: Chemical Kinetics (Chapter 18...

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L4: First exam: Chemical Kinetics (Chapter 18 only!) - rates of chemical rxns - integrated rate laws - zero-, first, and second order rxns; - pseudo first or second order kinetics - mechanisms - rate expression <-> mechanism <-> molecularity - rate limiting rxn, fast equilibrium, steady state apprx. - Michaelis-Menten kinetics and catalysis - T-dependence of rxn rates, Arrhenius law - activated complex and activation energy Not required: Kinetics and Chemical Equilibrium Reaction Dynamics (section 18.6) You need to know all definitions, in particular rate (R). Equations and constants will be given to you. Lab Orientation Lecture and Review of Exam 1: Thursday, 4:00 pm, SGM 101
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2 2 2 kt e C C = 0 L4: Review kt C C 2 1 1 0 + = Also for A + B when [A] = [B] kt C C = 0
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Pseudo first order reaction: When one reactant, C, is in great excess over another, its concentration does not change during the reaction, even when the second reactant is totally depleted. In this case [C] t = [C] 0 = constant at ANY time Example: C + D A + B; [C] >> [D] [D] is the limiting reagent It is found experimentally that R = k[C][D] At the end of the reaction [C] ~ [C] 0 So R ~ k[C] 0 [D] = k eff [D] where k eff = k[C] 0
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The rate for the reaction O+NO 2 -> NO + O 2 was studied with a large excess of NO 2 : [NO 2 ] 0 =1.0x10 13 molec/cm 3 . The overall rate law is given by: R = k [NO 2 ] [O] n . A plot of ln[O]
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L4_115b08 - L4: First exam: Chemical Kinetics (Chapter 18...

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