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Rate Determining Step The overall reaction rate cannot exceed the rate of the slowest elementary process. Because this slow step limits the overall reaction rate it is called the rate-determining step. A variety of conditions may cause a particular step to limit the overall reaction rate. These include the step having: complex collision geometry a high activation energy low concentrations of reactants a termolecular collision Text Pages Reaction Mechanisms and Catalysis Reaction Mechanisms
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Reaction MechanismsStudies have shown that most reactions occur by a series of steps called the reaction mechanism. The individual steps in such a series are called elementary processes. These steps are themselves individual balanced chemical reactions that may be added together algebraically to give the overall balanced chemical equation.
Text Page 57
1.5 Reaction Mechanisms and Catalysis
Intermediates and CatalystsIn any multi-step reaction mechanism the first collision, or decomposition of anenergized reactant, always produces some product that is consumed in a later step ofthe mechanism. Such a species is called a reaction intermediate.
CatalystA catalyst functions by “providing an alternate, lower-energy pathway” for a reaction to follow
Text Pages58 - 59
1.5 Reaction Mechanisms and Catalysis
Species Identification
Rate Determining StepThe overall reaction rate cannot exceed the rate of the slowest elementary process. Because this slow step limits the overall reaction rate it is called the rate-determining step. A variety of conditions may cause a particular step to limit the overall reaction rate. These include the step having:
• complex collision geometry• a high activation energy• low concentrations of reactants• a termolecular collision
Text Pages58 - 59
1.5 Reaction Mechanisms and Catalysis
Reaction Mechanisms
Overall Activation Energy
Example: Notice that Figure 1.5.3 has three “peaks” corresponding to the three steps in the catalyzed reaction mechanism. The rate-determining step is the second one. This stepwould also determine Ea for the overall reaction.
Text Pages 59 - 61
1.5 Reaction Mechanisms and Catalysis
Potential Energy Diagrams
Heterogeneous and Homogeneous Catalysts
Heterogeneous catalysts are those in which reactions are limited to their surface area only. The form of catalysis in which the phase of the catalyst differs from that of the reactantsExample: Catalytic Converter
Catalysts which exist in the same phase as the rest of the reaction system, aresometimes called homogeneous catalysts.Example: metalloenzymes
Text Pages 59 - 61
1.5 Reaction Mechanisms and Catalysis
Catalysts