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United States (324,192)
Chemistry (249)
CHEM 341 (46)
Lecture

Thermodynamics, kinetics, reaction coordinate diagram, Gibbs free energy change, reaction rate

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Department
Chemistry
Course
CHEM 341
Professor
Debbie Crans
Semester
Fall

Description
7 September π bond is nucleophile + H is electrophile + Double bond “attacks” H “The rich gets richer” H goes to C that already has more H Markovnikov rule Thermodynamics and Kinetics Thermodynamics – relative amounts of Y and Z present when the reaction has reached equilibrium Kinetics – how fast Y is converted to Z Reaction Coordinate Diagram Plot of change in energy as a function of reaction progress Transition state – point on energy surface where progress in either direction leads downhill Equilibrium – Stability – Thermodynamics mA + nB ↔ sC + tD S t [products] [C ][D] Keq [reactants] = [A] [B] n Gibbs Free Energy Change ΔG° = (free energy of products) – (free energy of reactants) An exergonic reaction, ΔG° is negative, K >eq An endergonic reaction, ΔG° is positive,
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