Physical chemistry course study guide
The Elements of Physical Chemistry
, Peter Atkins (5th edition), Freeman (2009)
Course Prefix & Number: CHEM3050
Course Title: Physical Chemistry
Credit Hours: 3-0-3
Prerequisites:
“C” or better g
rade in PHYS 2212 (or concurrent enrollment), MATH2202,
CHEM2800, CHEM2800L
Course Description: This one semester course in physical chemistry provides a survey of
thermodynamics, chemical equilibria, and kinetics. It also includes an introduction to the quantum
mechanical principles important in understanding molecular spectroscopy and molecular
modeling.
Chapter 0 Introduction
1.
All terms in boldface.
2.
Review Appendices 1 and 2
3.
Interconvert measurements within the set of SI units
4.
Interconvert the following units of pressure: Pa, bar, atm, torr, "mm Hg"
5.
Calculation of the hydrostatic pressure in a liquid as a function of depth
6.
Kelvin and Celsius (centigrade) temperature scales
7.
Relationships between Avogadro's number (N
A
), Boltzmann's constant (k
B
) and the ideal
gas constant (R)
8.
Identify intensive and extensive properties
Chapter 1: The Properties of Gases
Sections 1 4-1.8 relevant to Kinetics and Reaction Rates
1.
Assumptions of the kinetic molecular theory of gases and its use in the derivation of the
ideal gas law
2.
General form of the Maxwell distribution of molecular speeds and how this distribution is
affected by temperature changes and by changes in the mass of the gas
3.
The terms mean free path, collision frequency, time of flight, collision cross-section,
means speed, mean square speed, root mean square speed
4.
Calculation of values for the mean free path and the collision frequency and be able to
describe how they are affected by changes in pressure, temperature and molar mass of
the gas
5.
Differentiating between the terms
diffusion
and
effusion
6.
Graham's Law of Effusion: effusion rate dependence on molar mass
Chapter 10 The Rates of Reactions
1.
All terms in boldface
2.
Description of the reaction rate in terms of the rates of concentration changes of
reactants and products, given the overall chemical reaction
3.
Experimental rate law and the names of the parameters appearing in this empirical
equation
4. The 1
st
and 2
nd
order reaction in one component in terms of the defining rate expressions,
the integrated rate laws and the half-lives of the reactions
5.
Experimental methods for obtaining rate laws: graphing Log(rate) against
Log(concentration), initial rate method, excess reagent (flooding) method,

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