Reaction Mechanisms Chemical Kinetics-5.

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Reaction Mechanisms Chemical Kinetics-5

Reaction Mechanisms Series of elementary steps reactions go through to completion Sum of steps must = overall reaction Mechanism must agree with experimental rate law Molecularity: Unimolecular step: one molecule/atom as reactant Bimolecular step: 2 molecules/species as reactants Termolecular step: very, very, very rare. Rate determining step matches the rate law because reaction cannot proceed faster than its slowest step. Rate law can be written from rate determining step Intermediates cannot be in the rate law.

Example A) Rate determining step, RDS? B) Rate law? C) Overall reaction? D) Intermediates? H2O2  2 OH- slow H2O2 + OH-  H2O + HO2 fast HO2 + OH-  H2O + O2 fast Catalyst: Accelerates reaction by providing an alternate mechanism with lower activation energy.

A + B  C fast A + C  D slow A) Rate determining step, RDS? B) Rate law? C) Overall reaction? D) Intermediates? A + B  C fast A + C  D slow