Chapter 13 lecture 3

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

Info iconThis preview shows pages 1–5. Sign up to view the full content.

View Full Document Right Arrow Icon
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.
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
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
Background image of page 2
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
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Reaction Mechanisms: The basics: For a reaction:
Background image of page 4
Image of page 5
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 04/16/2008 for the course CHEM 1123 taught by Professor Paul during the Fall '06 term at Arkansas.

Page1 / 8

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

This preview shows document pages 1 - 5. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online