Lecture 10 - Experiment 10 Click to edit Master text styles...

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• Click to edit Master text styles – Second level • Third level – Fourth level » Fifth level Experiment 10 Chemical Kinetics Discovery Lab CH 204 Fall 2008 Dr. Brian Anderson
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• Click to edit Master text styles – Second level • Third level – Fourth level » Fifth level Last week in lab Titration curves Changing composition of a weak acid solution as strong base is added pH meters, pH standards Witnessed the awesome power of a buffer solution to resist changes in pH
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• Click to edit Master text styles – Second level • Third level – Fourth level » Fifth level Thermo vs Kinetics Thermodynamics is concerned only with where you start and where you finish. Kinetics is all about how you get there: reaction rates and reaction mechanisms (the individual steps of a reaction).
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• Click to edit Master text styles – Second level • Third level – Fourth level » Fifth level Reaction rate How quickly a reactant disappears, or how quickly a product forms. Δ [A] d[A] Δ t dt How fast the reaction goes depends on the concentrations of the reactants. This is expressed in an equation we call a ratelaw. = Rate = - -
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• Click to edit Master text styles – Second level • Third level – Fourth level » Fifth level Rate Laws Rate laws tell you how the rate of a reaction (M/sec) depends on the concentrations. For the reaction A + B C, a typical rate law is Rate = k[A][B] Most rate laws are 1 st or 2 nd order. (Sum of the exponents equals 1 or 2.) This example is 1 st order in A and B, and 2 nd order overall.
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• Click to edit Master text styles – Second level • Third level – Fourth level » Fifth level Reaction Mechanisms
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This note was uploaded on 12/17/2009 for the course CH 310 N taught by Professor Blocknack during the Spring '08 term at University of Texas at Austin.

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Lecture 10 - Experiment 10 Click to edit Master text styles...

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