CHEM 102 1nd Edition Lecture 12 Outline of Last Lecture I. Reaction mechanism and rate law expression II. ExampleIII. Effective temperature Outline of Current Lecture IV. Effects of catalystV. Types of catalysts VI. Most reactions don’t go to completionVII. Kc (conventional concentration): is an equilibrium constant, all aq and g species are unitsof MCurrent Lecture- Effects of catalysto Catalysts are substances that speed up reactionso They can appear in an equation A + B + catalyst C + catalyst A + B Co Catalysts lower the Ea of rate of determining step (slow step) Catalysts lower Ea by getting involved in reaction and changing the mechanism - Types of catalysts o Homogenous catalysts Same phase o Heterogeneous catalysts Solids Provides a surface which the reactions can occur- 2 H2 (g) + O2 (g) 2 H2O (l)o Catalysts vs. intermediates Intermediates are made then destroyed Catalysts are there are the beginning and then there are the end- Most reactions don’t go to completiono Most attention state of chemical equilibrium Reactants products (reversible reactions)These 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.- Kc (conventional concentration): is an equilibrium constant, all aq and g species are unitsof Mo Set solids and liquids equal to 1 M Note: molarity is really “activity”, M at dilute concentrationso Ignore pure solids and pure liquids Only include aq and go A thermodynamic activity o Depends only on To Has no
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