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Reaction Rates and Mechanism Notes

by: Erik Roseberry

Reaction Rates and Mechanism Notes CHEM 0970

Marketplace > Engineering and Tech > CHEM 0970 > Reaction Rates and Mechanism Notes
Erik Roseberry
GPA 3.0
Chemistry 2
Dr. Maleckar

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About this Document

Covers almost all of Chapter 14 in detail. Includes all major points with depth to make sure you understand the material.
Chemistry 2
Dr. Maleckar
Class Notes
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This 3 page Class Notes was uploaded by Erik Roseberry on Friday January 23, 2015. The Class Notes belongs to CHEM 0970 at a university taught by Dr. Maleckar in Fall. Since its upload, it has received 239 views.


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Date Created: 01/23/15
Erik Roseberry Dr Maleckar Chemistry 2 Notes Week 012315 Chapter 14 Chemical Kinetics Study of Reaction Rates Fast Reaction Combustion Slow Reaction Iron Rusting Cement Setting Food Cooking Reactant Rate amount of product formedtime Measured in MolaritySeconds As concentration rate goes up reaction rate also increases 0 As temperature goes up reaction rate increases Gases react quicker than Liguids which are faster than Solids Catalysts increase rate of reaction by lowering energy needed to start a reaction activation energy energy needed to start a reaction Gets regenerated in process of reaction Rate Law aAbB l with C as a potential catalyst dDeE Will form rate law kAmB Cp k rate constant varies with temp m n and 0 determined experimentally Necessary to have data on reaction in order to determine rate law Impossible to determine from aA I bBcC alone The following are examples C3H6 I CH2CHCH3 given Rate Law kC3H61 rst order because power of 1 2NO2H2 l N22H20 given Rate Law kNO2H2 second order NO rst order H2 third order overall CH3COCH32 H catalyst CH3COCH2H Rate Law kCH3COCH3H second order reaction rate not dependent on l2 because its not in rate law Will only increase reaction rate if increased catalyst or rst reactant Integrated Rate Law acquired through complex not important integration Or for half life reactions Collision Theory For every successful reaction activation energy must be met through collision of two or more particles Transition State Theory There must be a state of unstable transition in between the reaction of one molecule into another where all elements involved are separated and held together by weak bonds Potential Energy Diagrams 1 Endothermic starts with low energy and must peak over high activation energy to react Ends with higher energy than beginning 2 Exothermic generally lower activation energy this reaction loses energy through the reaction and ends in more stable low energy position Arrhenius Equation relates k and temperature Basic Ea Activation Energy Joules A Frequency factor dif cult to obtain often given R Gas Constant T Temperature Kelvin Rearrangedr or Mechanism details about speci c reaction including steps in between AA l CE often slower reaction EB AD often fast AB l CD nal Strikethrough means they cancelled each other out Molecularity number of molecules on the reactant side of any elementary reaction Elementary Reaction individual reactions in mechanism Unimolecular 1 reactant molecule 0 Rate Equation kA Bimolecular 2 reactant molecules colliding at same time 0 Rate Equation kAB Termolecular 3 reactants very rare 0 Rate Equation kABC In order to graph a reaction order sometimes it is best to use linear A v Time or ogarithmicnA v Time or inverse 1A v Time all depends which graph will give you the most linear relationship for the speci c equation


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