CHEM 102 1nd Edition Lecture 11 Outline of Last Lecture I. Rate of reaction depends on four factorsII. Nature of reactantsIII. Concentration complicatedOutline of Current Lecture II. Reaction mechanism and rate law expression III. ExampleIV. Effective temperature Current Lecture- Reaction mechanism and rate law expression o Series of steps that takes the reactants and turns them into productso Unomolecular decomposition (A B+C)o Bimolecular collision (A + B C) Trimolecular collisions are VERY rareo The slowest step controls the overall reaction Called the rate determining step Step with the highest activation energyo The experimentally derived rate law expression is tightly connected to the slow step of the mechanism- Exampleo 2A + B + C AC + AB Rate law expression=k [A]x [B]y [C]zo After doing experiment, rate = k [A][B][C]o Concentrate on slow step and ignore all steps afterward Rate = k[A]2 where 2 is the number of times A appears as a reactant - Not the mechanismo A2 is an intermediate as it is neither a reactant nor product It was formed and then destroyed- Effective temperature o 1 step reaction A + B C (rate = k[A]1[B]1)- Exothermic, not dependent on temperatureThese 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. As T increases, energy of molecules increases- More molecules have necessary energy to create transition state and ultimately form
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