Section10_Kinetics_1

Section10_Kinetics_1 - KINETICS I Reaction Rates and the...

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KINETICS I Reaction Rates and the Rate Law By the end of this lecture, you will be able to: (1) Understand the difference between kinetics and thermodynamics . (2) Understand rate, average rate, initial rate and instantaneous rate. (3) Write a generic expression for the rate of a chemical reaction. (4) Understand order of reaction. (5) Know what differential and integrated rate laws are and how they differ. (6) Know how to Fnd integrated rate laws from differential ones for 1 st and 2 nd order reactions. Page 1 of 20
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Kinetics vs. Thermodynamics Thermodynamics “Will the reaction proceed, and, if so, to what extent?” ( i.e. , Is it spontaneous under the given conditions, and what will be the Fnal distribution of reactants and products?) Kinetics “How quickly will the reaction proceed, and by what mechanism?” e.g. , C( diamond ) C( graphite ) Spontaneous ( Δ G° = 3 kJ mol -1 ), but very slow (millions of years). Page 2 of 20
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Kinetics is the study of the rates and mechanisms of chemical reactions. We cannot determine rate and mechanism by inspection of chemical equations or from tabulated data. Kinetics are path-dependent . Rate Rate is the change in concentration per unit time (mol L 1 s 1 ) of a reactant or product. Consider the reaction: A B Page 3 of 20
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The rate of loss of A ( i.e. , decrease in [A] over time) is equal to the rate of buildup of B ( i.e. , increase in [B] over time). That is: d [ A ] dt = d [ B ] dt or is the instantaneous rate of the reaction at a given time. Rate is always
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This note was uploaded on 06/20/2008 for the course CHEM 024b taught by Professor Jones during the Winter '07 term at UWO.

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Section10_Kinetics_1 - KINETICS I Reaction Rates and the...

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