CHE 102 Lecture Notes - Lecture 1: Kinetic Theory Of Gases, Rate Equation, Chemical Kinetics

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31 Oct 2017
Department
Course
Professor
Chemistry 102 Winter 2010
Announcements
1. Next midterm exam on Feb. 22, Monday.
Chapter 11.1-11.3 (note these sections are
based on Chapter 6 concepts, e.g. ΔH, and
Chapter 9 concepts, e.g. IMF’s), skip
Clausius-Clapeyron and relative humidity,
Chapter 11.5 (note this section is related to
bonding types and IMF’s),
Chapter 12.1-12.3
Today
1. Determination of rate law by integration.
2. Activation energy.
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Chemistry 102 Winter 2010
2
Review
Chemical kinetics is the study of rates of
chemical processes, including chemical
reactions and physical changes.
reaction rate: the change in concentration of a
reactant or product per unit time.
Reaction rates are always positive.
For a given chemical, a positive sign means
production of that chemical. A negative sign
means consumption of that chemical.
Kinetic Molecular Theory fits the observation of
a reaction rate depending on the concentration of
reactants:
More reactants (higher concentration), faster
rate.
Fewer reactants (lower concentration),
slower rate.
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Chemistry 102 Winter 2010
3
A rate law summarizes the relationship between
reactant concentration and reaction rate.
Cv+(aq) + OH-(aq) CvOH(aq)
rate = k[Cv+]
2 NO2(g) + F2(g) 2 NO2F(g)
rate = k[NO2][F2]
The rate law must be determined experimentally.
The most common experimental methods:
1. Initial rates
2. Integrated rate laws
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