Fall 2000
Syllabus for CHEM-382 Physical Chemistry I
Four hours credit:
Three 50 minute lecture - discussion periods and one three hour laboratory period each week.
Instructor: Prof. Sondra Dittmer
Office Phone: 928-5477
Office: Reed 210
E-mail: dittmer@olivet.edu
Textbook: Physical Chemistry (6th ed.) By P.W. Atkins. W.H. Freeman Company
References: HTTP://WWW.WHFREEMAN.COM/PCHEM/INDEX.HTM
Physical Chemistry is a subject that discovers and applies basic physical principles to the various areas of chemistry. The students in Physical Chemistry I class should demonstrate knowledge and understanding at an advanced level in the following areas:
1. Knowledge and principles
properties of gases Ch. 1
temperature, pressure
perfect gases
mixtures of gases
imperfect gases
The first law of thermodynamics - concepts Ch. 2
heat, work, energy
expansion work
thermochemistry
internal energy
enthalpy
heat capacity
The first law - machinery Ch. 3
state functions, differentials
temperature dependence of U, H
adiabatic expansion
The second law of thermodynamics - concepts Ch. 4
entropy
natural events
entropy changes
phase transitions
irreversible change
Carnot cycle
refrigeration
Gibbs, Helmholtz functions
maximum work
the third law
The second law - machinery Ch. 5
combining the first and second laws
T, P dependence of G
chemical potential
properties of real gases
open systems
Changes of state - pure materials Ch. 6
phase equilibria
phase diagrams
real systems:
CO2, H2O, C, He
Changes of state - mixtures Ch. 7
partial molar quantities
thermodynamics of mixing
chemical potential
colligative properties
mixtures of volatile liquids
real solutions, activities
Changes of state - the phase rule Ch. 8
the phase rule
one-component systems
two-component systems
three-component systems
Changes of state - chemical reactions Ch. 9
Gibbs function minimum
perfect gas equilibria
equilibrium constants
response of equilibrium to T, P changes
applications
Equilibrium electrochemistry - ions and electrodes Ch. 10
activities of ions in solution
Debye-Huckel theory
electrodes
electrochemical cells
standard electrode potentials
thermodynamic data from EMF's
applications of EMF measurements
2. Development of skills in the process of science.
Problem solving skills to perform numerical calculations and mathematical derivations related to physico-chemical principles
Laboratory skills to design and carry out experiments involving precise physico-chemical measurements
Logical skills to relate factual knowledge to scientific theory
Reading and critical evaluation of scientific literature
3. Understanding the investigative nature of science
Recognizing the importance of experiment in the development of science, especially the generalizations of thermodynamics
Developing theoretical models from mathematics, chemistry, and physics
Exploring relationships between experiment and theory
4. Attitudes about science
Appreciating Nature as God's handiwork
Viewing science as a worthy human endeavor
Applying scientific principles to problems of everyday living
Understanding science as an unfinished enterprise, with much to be discovered
Specific objectives for each learning unit will be given in behavioral terms, and will be evaluated by student performance on problem assignments, unit tests, a final examination, and laboratory reports.
Test 1 The First Law Sept. 18
Test 2 The Second Law Oct. 16
Test 3 Phase Equilibria, Changes of State Nov. 20
FINAL EXAM 10:30-12:20 p.m., Monday Dec. 18
Grading Procedure:
Problems from Text 10%
Laboratory reports 20%
Unit Tests 40%
Final Exam 20%
Term Paper 10%
Each one of these areas will be graded separately and the grades averaged using the above percentages.
Attendance Policy:
A record of attendance in class and laboratory will be kept. Experience indicates that excessive absence has detrimental effect on performance in chemistry classes. It is highly unlikely that a student missing 25% or more of the class sessions could receive a passing grade. It is especially difficult to make up laboratory work that has been missed. Absence from laboratory affects the students with whom you work, also.
Directions for Laboratory Work:
The completed reports are due two weeks after finishing the experiment. I will read the draft version of the first lab report and make comments. You can turn in the final version and the grade will be given to the final version. The rest of the lab report will be graded upon the first version.
Homework:
It is important to complete your homework assignments on you own because they will help you to understand the concepts that seem abstract during lecture, to enhance your problem-solving skills and prepare you for the tests (the problems in each test are similar to those in your homework). homework will be collected for completeness, not correctness. The answers to the problems are reserved in the library. I suggest that you work on the problem on your own first. If you have trouble with any of the problem, come and see me or, check out the answers. If you still don’t understand, come and see me.
Term Paper:
You are required to write a term paper for Physical Chemistry I. It has to be typed, double spaced, at least 8 pages longs (including diagrams, equation derivations). The suggested topics are : 1) reviews of the physical chemistry as a discipline; 2) derivation of certain equation(s), 3) application of thermodynamic laws in industries, social science, astronomy,..... You can choose your own topic. Please let me know before you start. Each person should work on a different topic.
The goal of the paper is to develop good library, literature review and WWW search skills as well as to have an in-depth understanding of a specific topic in physical chemistry. Deadlines
Oct. 5
Final approval of topic after consultation with facultyOct. 19 Bibliography due, based on library texts, computer search, WWW sites
Nov. 2 Outline of the paper due
Nov. 23 Final paper due
Dec.11 Oral presentation (15 minutes each)
CHEM 382
Laboratory Schedule Fall 1999
Sept. 4 Gas Density and Molecular Weight Hand-out
Sept. 11 Bomb Calorimetry I Exp. 3
Sept. 18 Test #1
Sept. 25 Revival
Sept. 27 Solution Calorimetry Hand-out
Oct. 2 Vapor pressure of a pure liquid Exp. 5
Oct. 9 Fall Break
Oct. 16 Test #2
Oct. 23 Liquid-vapor equilibrium: mixture Exp. 6
Oct. 30 Solid-liquid equilibrium Exp. 7
Nov. 6 Review for Test 3
Nov. 13 Test #3
Nov. 23 Electrochemical cells and the Nernst Equation Labworks
Nov. 30 Entropy and Enthalpy Labworks
Dec. 4 Reviews
Exp. = Physical Chemistry--Methods, Techniques and Experiments by SIME
Labworks = Computer Experiments in Chemistry
You are encouraged to choose your own experiments from the materials mentioned above or other sources. Please let me know in advance so we can get the materials ready.
Lab report should include PURPOSE, THEORY, METHODS, RESULTS (INCLUDING ALL CALCULATIONS, AND LAB NOTES), AND CONCLUSION (WHAT DID YOU LEARN FROM THIS LAB, WHAT SCIENTIFIC PRINCIPLE DID YOU PROOF OR DISPROOF, EVALUATION OF THE EXPERIMENT). Lab report is due ONE week after the experiment is conducted.
CHEM 382
Physical Chemistry I
Fall, 1999
Study Guide, Unit I
The student will:
1. Define the following terms:
Ch. 0 perfect gas
gas constant
real gas
extensive property
intensive property
molar property
energy
kinetic energy
potential energy
Coulomb potential energy
Ch. 1 state
system
equation of state
pressure
limiting law
temperature
kinetic theory
r.m.s. speed
Maxwell distribution
mean free path
compression factor
virial equation of state
van der Waals equation
critical constants
principle of corresponding states
Ch. 2 system
surroundings
heat
work
internal energy
exothermic
endothermic
state function
expansion work
reversible expansion
heat capacity
calorimetry
enthalpy
standard state
standard enthalpy change
enthalpy of phase transition
of solution
of ionization
of dissociation
Hess's law
thermochemical equations
thermodynamic cycle
Born-Haber cycle
lattice enthalpy
standard reaction enthalpies
standard enthalpies of formation
Kirchoff's law
2. State the Zeroth law of thermodynamics
3. State the first law of thermodynamics, verbally and by means of an equation.
4. Derivations, and related mathematical operations:
a. Solve the van der Waals equation for P and for V.
b. Derive the expression for work in the isothermal reversible expansion of an ideal gas.
c. Apply Hess's law to the determinations of standard reaction, enthalpies from tabulated thermochemical data.
d. Using a Born-Haber cycle, estimate lattice enthalpies for ionic compounds.
Chem. 382
Phys. Chem. I
Fall 1999
Study Guide, Unit II
The student will:
1. Define the following terms:
Ch. 3 exact differential
Joule experiment
Joule-Thomson experiment
π
Tα
κ
Tμ
JTadiabatic process
Ch. 4 spontaneous process
entropy (stat.)
entropy (thermo)
Carnot cycle
Clausius inequality
Nernst heat theorem
efficiency
coefficient of performance
adiabatic demagnetization
Helmholtz function (A)
Gibbs function (G)
maximum work
Ch. 5 fundamental equation
Maxwell relations
Gibbs-Helmholtz equation
chemical potential
fugacity
2. Calculate changes in various thermodynamic properties resulting from adiabatic processes.
3. State the Second law of thermodynamics, verbally and by means of an equation.
4. State the Third law of thermodynamics.
5. List criteria for spontaneous change in terms of entropy, internal energy, enthalpy, and the Gibbs function.
6. Derivations, and related mathematical operations:
dU = π
TdV + CVdTChem 382
Phys. Chem. I
Fall 1999
Study Guide, Unit III
The student will:
1. Define the following terms:
Ch. 6 phase
phase diagram
phase boundaries
triple point
Clapeyron equation
Clauisius - Clapeyron equation
first order transition
second order transition
Ch. 7 partial molar quantity
Gibbs-Duhem equation
mixing functions
excess functions
ideal solution
ideal dilute solution
Raoult's law
Henry's law
colligative properties
osmosis
azeotropes
real solution
activity
activity coefficient
2. Interpret phase diagrams for one component systems (pure substances).
3. Apply the Clapeyron equation to discussion of phase boundaries.
4. Apply the Clausius-Clapeyron equation to the description of solid/vapor and liquid/vapor equilibria.
5. Compare first order and second order phase transitions with regard to the temperature dependency of V,H, μ, S, and C
p.6. Interpret phase diagrams for binary systems having at least one volatile component. Identify Raoult's law and Henry's law behavior, and deviations from these laws observed for real solutions.
7. Compare the colligative properties with regard to their characteristics and their applications for study of solutions.
8. Derivations and related mathematical operations.
Clausius - Clapeyron equation in integrated form.
CHEM 382
Physical Chemistry I
Fall 1999
Study Guide, Unit IV
The student will:
1. Define the following terms:
Ch. 8 phase
phase diagram
component
thermal analysis
azeotropes
partial miscibility
critical temperature
variance
eutectic
reaction quotient
incongruent melting
tie line
lever rule
Ch. 9 reaction Gibbs function
exergonic
endergonic
equilibrium constant
Le Chatelier's principle
autoprotolyses (of water)
buffer
Biological standard state
Ch. 10 mean (ionic) activity coefficient
ionic strength
Debye-Huckel limiting law
half-reaction
electrodes
electrochemical cells
Nernst equation
standard potential
2. Derivations, etc.
Ch. 8 (a) The Gibbs Phase Rule
Ch. 9 (b) Relationships between ΔG and K
p© Van't Hoff equation
Ch. 10 (a) The relationship between the zero-current cell potential and the reaction Gibbs function.
3. Other activities
Ch. 8 (a) Apply the Gibbs phase rule to phase diagrams of 1, 2, and 3 component systems.
(b) Interpret phase diagrams by identifying points, lines, and areas as to their physical state, composition, and equilibrium conditions.
Ch. 9 (a) Calculate Kp
and ΔG, given equilibrium pressure or concentration data.(b) Treat gaseous equilibria in terms of a dissociation factor, α.
Ch. 10 (a) Obtain ΔG, ΔH, and ΔS data from temperature dependence of cell potentials.