Chapter 13 lecture 3

Chapter 13 lecture 3 - Chapter 13 Lecture 3 Theories of...

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Chapter 13 Lecture 3 Theories of Chemical Kinetics Collision Theory Transition State Theory Temperature Effects Arrhenius equation k = Ae -Ea/RT Rate constant k is a constant, but does change with temperature R is 8.3 Joules/mole-K At higher Temperatures, A changes, A is composed of Zp 1)Collision frequency increases: Z 2) Probability factor increases: p This is the probability that collision will lead to reaction 3)Zp is the number of collisions per second leading to product.
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Alternate form of Arrhenius equation: A RT E k a ln ln + - = If you take two points off the line, ie you measure the rate constant at two different temperatures, then you can use: - = 2 1 1 2 1 1 ln T T R E k k a
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Example Homework Problem 56: The following decomposition is known to be first order: DTBP Acetone + Ethane DTBP stands for di-tert-butyl-peroxide Find the activation energy if t ½ = 100 minutes at 145 o C t ½ = 320 minutes at 135 o C
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Reaction Mechanisms: The basics: For a reaction: aA + bB cC + dD The rate law is: R = [A] n
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