FALL 1999: Chemistry 160

Physical Chemistry;

Instructor: J. V. Acrivos-DH16;
One Semester (3 units)-Tel. 408-924-4971,2; FAX:..4945; e-mail: acrivos@chemibr1.sjsu.edu

OFFICE HOUR PRIVELEGES FOR STUDENTS WHO ATTEND CLASS: determined by students' schedule for best attendance. e-mail question answered in 24 hours.

Green Sheet:

I. Problem Solving Texts: P.W.Atkins, "The Elements of Physical Chemistry" W.H. Freeman (1992)

Reference: "Physical Chemistry", W.H. Freeman, 5th Edition (1994b).
Additional Reference: W.J.Moore, "Physical Chemistry", Prentice-Hall, 4th ed.

Reminder: October 11 MT1, Closed Book Examination, one question from homework, one from quiz and two others. MT1Grades: 160_MT1.html

See lecture notes, and www MS browser only if you have adobe reader and mathematica fonts in your PC.

For current news, grades and announcements during the semester please look here. Students will be assigned a number the first day of classes. This number must appear in all homework, quiz and tests. Otherwise no credit is given.

II. Prerequisites indicated in Catalog are strictly enforced. Students will be required to present copies of the official transcript the second day of classes. Students that do not present the official transcripts will be dropped during the first week.

Course contents: Modules (mod#) are timely posted in the www which can be accessed through the Computer Laboratory at One Washington Square:

http://www.sjsu.edu/testupdates/faculty/Acrivos/front.html

"click" on Teaching Philosophy and there click on 160"
5.1. Thermodynamics mod1, or mod_1.PDF but note that you will you need the proper fonts: mathematica and abobe reader in your PC. Textbook Ch. 1-3
5.2. Chemical Equilibrium, Electrochemistry: mod2 or mod_2.PDF mod3: but note that you will you need the proper fonts: mathematica and abobe reader in your PC. Textbook Ch. 3-5
5.3. Theory: Quantum, Spectroscopy, Kinetics, mod4 mod5 mod0: Ch. 7-11

III. Course Grade:

  1. Homework, Attendance/Open Book Quiz*: 10%/10%
    The homework consists of the first four problems of every chapter assigned above plus others assigned in class. Grading is done according to the required format for lectures, homework and quiz as described in (C). Homework is due the second Monday after assignment with 50% off for every day late; attendance is taken and is required for office hours.
  2. Three types of exams: A. Closed Book Problems: in class; B. Open Book Take Home and C. ACS Multiple Choice in class.
    October 11: 15%
    November 12: 15%
    December 8: 15%
  3. Final examination: (ACS Standardized Test): 35% of grade

IV. Study Time: For two hours of study per unit per week an average student gets an average course, i.e., at least six hours of study per week are required to obtain an average grade in an average course.

V. The departmental policy on cheating is sanctioned.

VI. EMERGENCIES AND EVACUATIONS: If you hear a continuously sounding alarm, or are told to evacuate by Emergency Coordinators (colored badge identities), walk quickly to the nearest stairway (end of each hall). Take your personal belongings as you may not be immediately allowed to return. Follow instructions of Emergency Coordinators. Be quiet so you can hear. Once outside, move away from the building. Do not return to the building unless the Police or Emergency Coordinators announce that it is permissible.

VII. REQUIRED PROCEDURE FOR SOLVING PROBLEMS, (% GRADE)

  1. (15%) Statement of:
    1. The system under study:
    2. The data available:
    3. The objective to be achieved:
  2. (25%) Statement of the pertinent relations with text reference.
  3. (40%) Carry out numerical analysis including all units used. Underline the correct answer. Block diagrams, computer output and graphs are allowed.
  4. (20%) State the physical significance of results, i.e., what do the results mean?

VIII CHEM160 SYLLABUS: The lecture topics are given according to the above format and they may take more than one 50 minute period.

I. THERMODYNAMICS LECTURES (T)

One: Two equations of state are presented, the ideal gas and the van der Waals correction: isotherms, isobars and isometrics for the two type gases are discussed. The CO2 isotherms near the critical region are used. The new synthesis in supercritical fluids is discussed.

Two: The critical region for a van der Waals gas is discussed.

Three: The concept of internal energy is introduced using the definitions for heat transferred and work done on the system. The enthalpy function is introduced. The 1st Law of Thermodynamics is discussed.

Four: The relation between heat capacity at constant volume and constant pressure is obtained and the ratio Cp/Cv for an ideal gas is discussed.

Five: Basic thermodynamic processes are defined. The experiments of Joule and Joule-Thomson are described.

Six: The Joule-Thomson coefficient is used to show concepts of refrigeration.

Seven & Eight: Heats of reaction at any temperature are discussed using the 1st Law. Examples on heats of formation, bond enthalpies and heats of solution are discussed. Isothermal reversible, adiabatic reversible and adiabatic irreversible processes are discussed using a numerical example. The Second Law of Thermodynamics is introduced in reference to example worked in Lecture nine. Third Law of Thermodynamics is presented.

II.THERMODYNAMICS:EQUILIBRIA (CE), ELECTROCHEMISTRY (EL)

One and Two: Phase equilibrium are discussed; definitions of composition, treatment of data, physical significance. Applications of the Calusius-Clapeyron Relation

Three to Six: Gibbs Phase Rule. Phase diagrams for one, two and three component systems are discussed. Concepts of first, second, etc., phase transitions are presented .Concept of equilibrium constant is presented for gaseous reactions. The concept of activity is presented together with activity coefficients. Numerical examples are used to illustrate the Law of Braun-Le Chatelier.

Seven to Eight: Laws of Faraday are presented together with the Laws of Kohlrausch and Arrhenius theory; the ionic mobility and transport are discussed. The concept of electrostatic/elcetrochemical potential is presented. Debye-Huckel Theory. The electrical potential difference is a galvanic cell is introduced.

Nine to Ten: The different types of reversible cells are discussed. The comparison of free energy and the emf of the reversible cell is discussed. Standard electrode potentials and calculation of equilibrium constants from emf data. Temperature dependence of the emf and calculation of thermodynamic constants for cell reaction.

III. THEORY: QUANTUM, SPECTROSCOPY AND CHEMICAL KINETICS

One to Five: Quantum Chemistry: Atomic and Molecular Wave Functions.

Six to Ten: Spectroscopy, NMR, ESR, IR, UV, X-Ray Regions.

Eleven to Fourteen: Chemical Reaction Kinetics, experiment and theory.

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