Physical Chemistry I (PHS 701)
Instructor: Michalakis
Savva, Ph.D. Fall 2009
Contact
Information: Office: HS 610
Telephone: 488-1471
e-mail: msavva@liu.edu
Website: http://myweb.brooklyn.liu.edu/msavva/
Course description
The
fundamentals of Physical Chemistry are studied with emphasis upon the
application of these on pharmaceutical sciences. The main elements that are
covered in this course are: Thermodynamics, Kinetics and electrochemistry.
Prerequesites
General
and Organic Chemistry and working knowledge with differential calculus.
Calculus
II, differential equations I (MAT 100 and MAT610, respectively) are highly
recommended.
Grades
will be based on a midterm exam (40 % of the final grade) and a 2.5-hour final
exam (60% of the final grade), which will include new cumulative material.
Exams will require calculation, and derivation/manipulations, similar to
problems and exercises given in the text. No
test grades will be dropped. The grading scale will be determined at the
end of the course and may not follow a linear scale.
No make-up exams will be given for the
midterm exam. If the midterm exam is
missed, the final grade will be calculated from the average of the quizzes and
the final exam. If the final exam is missed, a grade of Incomplete will be
submitted to the registrar and a makeup final will be given at a time and day
determined by the instructor. The material for the exams
will be extracted from the assigned text books, lectures and other
handouts/scientific articles.
Required Text
Lionel
M. Raff, Principles of Physical
Chemistry, Prentice Hall, 2001.
Objectives
1.
Understand the
behavior of gases and liquids under certain conditions and be able to calculate
changes in Energy, Enthalpy and Entropy of Ideal and non-ideal gases.
2.
Use of Hess’ law
to compute heats of reaction.
3.
Determine
conditions under which processes become spontaneous.
4.
Understand the
criteria for chemical reaction equilibria.
5.
Understand the criteria
for phase equilibrium for a pure substance.
6.
Learn to express
the thermodynamics of liquids and solids in terms of their equilibrium vapors.
7.
Understand
thermodynamic properties of pure solids.
8.
Understand the
variation of the heat capacity of solids with temperature.
9.
Understand
assumptions and limitations of Raoult’s law.
10. Calculate properties for non-electrolytic and
electrolytic solutions.
Chapter 1 Properties of Gases
1.1
Equation of State: General Considerations
1.2
Ideal-gas Equation of State
1.3
Nonideal Gases
HW problems: 1.1, 1.2, 1.6, 1.7-1.11, 1,13, 1,14, 1.16, 1.19, 1.23-1.29, 1.31, 1.32, 1.34-1.36
Chapter 2 The 1st Law of
Thermodynamics
2.1
Mathematics of Change
2.2
Work and Heat
2.3 The
First Law of Thermodynamics
2.4
Heat Capacity
2.5
The Joule-Thomson Experiment
2.6
Joule’s Experiment
2.8
Adiabatic Processes
HW problems: 2.1, 2.2, 2.4-2.12, 2.14-2.17, 2.19, 2.20, 2.22, 2.23, 2.25, 2.26
Chapter 3 Thermochemistry
3.1
Heats of Reaction
3.2
Measurement of Heats of Reaction
3.3
Bond Enthalpies
HW problems: 3.1-1.14
Chapter 4 The 2nd Law of
Thermodynamics
4.1
Spontaneity
4.2
Carnot Heat Engines
4.3
Refrigerators and Heat Pumps
4.4
The Second Law of Thermodynamics
4.5
Entropy
4.6
Reversible, Spontaneous and Nonspontaneous processes
4.7
Molecular Interpretation of Entropy
4.8
Internal Energy and Enthalpy Differentials in terms of Entropy
4.9
Temperature, Pressure and Volume Dependence of the Entropy
4.10
Computation of (∂U/∂V)T and (∂H/∂P)T
from the Equation of State
4.11
The Third Law of Thermodynamics
HW problems: 4.1-4.5, 4.9, 4.13, 4.15, 4.17, 4.19, 4.21, 4.23, 4.25-4.28.
Chapter 5 Chemical Equilibria
5.1
Reversible and Irreversible Processes Revisited
5.2 Total
Differentials of G and A
5.3
Maxwell’s Relationships
5.4
Open Systems: The Chemical Potential
5.5
Standard Chemical Potentials: The Equilibrium Constant
5.6
The Gibbs-Helmholtz Equations
5.7
The Temperature Dependence of Kp
5.8
Le Chatelier’s Principle
HW problems: 5.1-5.14
Chapter 6 Phase Equilibrium
6.1
Qualitative Description of Phase Transitions
6.2
General Condition for Phase Equilibrium
6.3
The Clapeyron and Clausius-Clapeyron Equations
6.4
The Triple Point: Phase Diagrams
6.5
Effect of Total Pressure on the Equilibrium Vapor Pressure
HW problems: 6.1, 6.2, 6.5-6.7, 6.9, 6.11-6.13
Chapter 8 Thermodynamics of
Nonelectrolytic Solutions
8.1
Ideal Solutions
8.2
Nonideal Solutions
HW problems: 8.1-8.9, 8.13-8.18, 8.21
Chapter 9 Thermodynamics of
Electrolytic Solutions (if time permits)
9.1
The Chemical Potential of Electrolytic Solutions
9.2
The Calculation of Ionic Activity Coefficients: Debye-Huckel Theory
9.3
Measurement of Ionic Activity Coefficients
9.4
Ionic Equilibria
9.5 Conductivity
of Solutions
9.6
Electrochemistry