CHEM 122 11th Edition Lecture 19 Outline of Last LectureI. Activation Energya. Forward and reverseII. Svante Arrheniusa. Arrhenius equationb. Frequency factorc. Straight line equationIII. Fraction of collision EquationOutline of Current Lecture I. Activation EnergyII. Reaction MechanismsIII. Molecularity of Elementary RactionsIV. Determining Rate law from a multistep reaction mechanismCurrent LectureActivation Energy- The activation energy can be determined by measuring the rate constant, k and 2 temperatures.olnk1k2=EaR(1T2−1T1)Reaction Mechanisms: the sequence of events leading from reactants to products.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.- Elementary Reactions: collisions of 2 molecules at a time, requires at least 2 steps.- An overall reaction, broken down into series of simple, elementrary reactions- The elementary steps must always ad together to give the overall reaction.- Reaction Intermediate: species that appears in a reaction mechanism but neither is a reactant or a product.- Molecularity: the number of reactant molecules that participate in a single elementary reaction.MOlecularity of Elementary Reactions:- Unimolecular: a single molecule is involved in the mechanismo A products Rate=k[A]- Bimolecular: A collision between two reacting moleculeso most commono A + B Products Rate= k[A][B]- Termolecular: the simultaneous collision between 3 racting moleculeso very rareo A + B + C Products Rate= k[A][B][C]- Coefficients of the equation determine the exponents in the Rate law.Determining the rate Law From a MultiStep Raction Mechanism:- the rate law for the overall reaction is determined by the slowest elementary step.- Equilibrium: Rate (forward)=
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