Lecture4 - Thermodynamics and kinetics Thermodynamics...

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1 Physical Chemistry Lecture 4 Introduction to chemical kinetics Thermodynamics and kinetics Thermodynamics Observe relative stability of states Energy differences Static comparisons of states Kinetics Observe changes of state over time Several different topics Empirical description of the rate of reaction Determination of experimental parameters Microscopic theories Rates A chemical reaction is described by an equation of the type Rates: Rate of change of [H 2 O]: d[H 2 O]/dt Rate of change of [H 2 ]: d[H 2 ]/dt Rate of change of [O 2 ]: d[O 2 ]/dt Rates related by the overall equation 1 oxygen molecule disappears for every 2 hydrogen molecules in the above reaction H gas O gas H O liquid 22 2 1 2 () ( )  Reaction velocity The rates of appearance of products and disappearance of reactants are related by stoichiometry of the reaction Define the reaction velocity , v, in terms of “normalized” rates of appearance of products and disappearance of reactants Example of the production of water: v di dt i 1 [] v dH dt dO dt dHO dt  [ ] 2 2 Rate laws Description of how the reaction velocity depends on parameters such as concentrations, temperature, pressure, etc.
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This note was uploaded on 02/02/2012 for the course CHEM 444 taught by Professor Dybowski,c during the Fall '08 term at University of Delaware.

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Lecture4 - Thermodynamics and kinetics Thermodynamics...

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