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For more information, please see full course syllabus of Chemistry
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Lecture Comments (5)

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Post by beatrice vaillant beatrice vaillant on December 2, 2014

any upcoming lectures about supra molecular chemistry?

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Post by Norman Cervantes on January 23, 2013

great anology

0 answers

Post by Eric Burkholder on December 3, 2012

As an American who is way too attached to his antiquated system...
...bravo sir. Good laughs were had.

0 answers

Post by nabeel hamad on December 6, 2011

I am searching for any video that deals with the subject of complexes. Can you please help me find a video that deals with this topic.

0 answers

Post by Patrick Patton on October 25, 2010

I plotted both these graphs and their linearity look very similar to each other. I wouldn't know which one to pick if asked in an exam situation.
Is there a more obvious way to determine the order?

Kinetics, Rate Laws, Reaction Mechanism

  • Define rate of reaction for given reactions in terms of reactants and products

  • Rate law as experimental observation of effects of changing concentrations on rates

  • Order of reaction: exponent in rate law expression for component

  • Overall order = sum of individual orders

  • Integrated rate expressions for first and second order reactions; how to plot them

  • First order: t versus ln[concn]; second order t versus 1/[concn]

  • A reaction mechanism is a hypothesis to explain observed rate laws

  • Elementary reactions are hypothetical; add together to get mechanism and overall rate law

  • Learn to interpret some simple rate laws in terms of elementary reactions, for example RBr reacting with OH- where R = ethyl; and tert-butyl

  • Rate limiting or slowest step limits observed rate of a multi-stage reaction

Kinetics, Rate Laws, Reaction Mechanism

Lecture Slides are screen-captured images of important points in the lecture. Students can download and print out these lecture slide images to do practice problems as well as take notes while watching the lecture.

  • Intro 0:00
  • Reaction Rate 1:30
    • Chemical Reaction Rate
    • Example: Methyl Bromide and Sodium Hydroxide
  • Reaction Rates: Changing Concentrations 10:28
    • Example: Double Initial Concentrations
  • Order of Reaction 17:05
    • Experimental Rate Law
    • Overall Rate
  • Initial Rate Measurement 23:24
    • Example: Methyl Bromide and Sodium Hydroxide
  • Integrated Rate Laws: First Order Reaction 29:54
    • Integrated Rate Equation
    • Example: Transitional Metal Complex
  • Integrated Rate Laws: Second Order Reaction 38:12
    • Integrated Rate Equation
  • Experimental Rate Laws 39:41
    • Example: Transitional Metal Complex
  • Experimental Rate Laws, cont. 42:45
    • Example: Nitramide
  • Reaction Mechanism 46:12
    • Hypothetical Aspect
    • Predict Outcomes
  • Elementary Reactions and Reaction Mechanisms 49:43
    • Example: Methyl Bromide and Hydroxide Ion
  • Rate Limiting Step 54:47
    • Example: Rate Limiting Step
  • Additional Example 1
  • Additional Example 2