Kinetics+Part+5 - 1 Reaction Mechanisms Mechanisms detail...

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Mechanisms detail the steps in an overall reaction and they include all reaction intermediates. These intermediates do not appear in the overall reaction, but they are essential for the reaction to occur. Individual steps of a proposed reaction – elementary reactions A → product Unimolecular Rate = k [A] 2A → product Bimolecular Rate = k [A] 2 A + B product Bimolecular Rate = k [A][B] 2A + B product Termolecular Rate = k [A] 2 [B] The rate law for an elementary reaction, unlike that for an overall reaction, can be deduced from the reaction stoichiometry. An elementary reaction occurs in one step, so its rate must be proportional to the product of the reactant concentrations. The equation coefficients are the reaction orders in the rate law for an elementary step; that is, reaction order equals molecularity. The Rate-Determining Step of a Reaction Mechanism Usually one step in a series of steps is much slower that the others, so it limits how fast the overall reaction proceeds – rate- determining step (RDS). Since the RDS limits the rate of the overall reaction, its rate law represents the rate law for the overall reaction. NO
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This note was uploaded on 09/30/2010 for the course EEE 4306 taught by Professor Eisenstadt during the Spring '08 term at University of Florida.

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Kinetics+Part+5 - 1 Reaction Mechanisms Mechanisms detail...

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