CHEM 1415 1st EditionLecture 15Unit: Reaction Mechanisms; CatalysisOutline of Current Lecture I. ChlorofluorocarbonsII. CatalystIII. Reaction MechanismsIV. Table 1: SummaryCurrent Lecture Chlorofluorocarbons o So inert they stay together all the way to the upper atmosphere and react with ozoneoCl+O3→ClO +O2oClO +O3→ Cl+2 O2oCl+ClO +2 O3→ 3 O2+ClO+Clo2O3→3 O2oClis a catalyst Catalysto Molecule is present at the beginning of the reaction and is regenerated so that it is present at the end of the reactiono Homogenous catalyst – catalyst is in the same phase at the end as it was in the beginningo Heterogeneous catalyst – catalyst is in a different phase than it was at the beginningo Reactive Intermediate – molecule is generated and then used up so that there is none at the end of the process, i.e. ClO Reaction Mechanismso A collection of one or more molecular steps that account for the way reactants became productso Elementary steps – individual steps in a reaction mechanism Unimolecular – steps with one reactant Bimolecular – steps with two reactants Termolecular – steps with three reactantsThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.Table 1: Summary of rate reactions and molecularityTypes of Elementary Reaction Molecularity Rate LawA →products unimolecular Rate = k[A]A+B→products2A→productsBimolecular Rate = k[A][B]Rate = k[ A ]2A+B+C→products2A+B→productsTermolecular Rate = k[A][B][C]Rate = k[ A ]2[B]A+B+C+D→products Not
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