CHEM 337 PHYSICAL CHEMISTRY I (3 credits)

Syllabus, Fall, 2008

Instructor:

Dr. Norman Shank Office: Jordan 358 Phone: 2590 nshank@messiah.edu

Text: Ball, David W. Physical Chemistry, Brooks/Cole, 2003.

Prerequisites: CHEM 106 and MATH 108 or 111.

Description: In Physical Chemistry I we will study the thermodynamics and kinetics of systems of chemical interest. After analyzing a macroscopic system, we will build physical and mathematical models to increase our understanding of that system, and to learn new things about it. The general approach will usually consist of one or more of the following steps:

1. Describe and analyze the macroscopic physical system.

2. Construct a microscopic physical model. (This is not required for

thermodynamic studies.)

3. Construct a mathematical model. This is usually a differential equation.

4. Integrate the differential equation.

5. Use the integrated equation to learn more about the physical system.

Objectives:

1. To learn a few basic principles about the structure of matter, the laws of thermodynamics, and the time dependent behavior of reacting chemical systems. Then to show how these few principles can be applied, through logical argument, to describe many aspects of chemical changes and chemical equilibria.

• Describe structure and composition of matter.
• Apply principles from thermodynamics and kinetics to the study of chemical systems, employing both qualitative and quantitative approaches.
• Use the theories of microscopic properties to explain macroscopic behavior.
• Explain the role of energy in determining the reactivity of molecules.
• Use and understand various methods of molecular modeling for understanding structure and reactivity.

2. To develop skill in calculating properties of chemical systems, using mathematical models for the principles mentioned above.

3. To make connections between science and the Christian faith.

• Understand the goals and limitations of the scientific process.
• Recognize that the physical world is created and sustained by God, and that science is our tool to understand this physical world.

Topics Sections in Text

1. Introduction; systems, state variables . . 1.1 – 1.4

2. Partial derivatives, nonideal gases . . . 1.5 – 1.6, 1.8 – 1.9

3. Work, heat, First Law of Thermodynamics . 2.1 – 2.4

4. Enthalpy, heat capacity . . . . . 2.5 – 2.8

5. Phase changes . . . . . . . 2.9

6. Chemical changes . . . . . . 2.10 – 2.13

7. Entropy, Second Law of Thermodynamics . 3.1 – 3.4

8. Entropy calculations, Third law of Thermo. . 3.5 – 3.8

9. Spontaneity conditions, Gibbs free energy . 4.1 – 4.3

10. Thermodynamic equations of state . . . 4.4 – 4.6

11. Using Gibbs energy; fugacity . . . . 4.7 – 4.10

12. Chemical equilibrium, equilibrium constant . 5.1 – 5.3

13. Chemical equilibrium in condensed phases . 5.4

14. Changes in equilibrium constants . . . 5.5 – 5.7

15. Electrochemical potentials . . . . 8.1 – 8.3

16. Relating electrochemistry to thermodynamics 8.4 – 8.5

17. Ionic solutions . . . . . . . 8.6 – 8.7

18. Conductance . . . . . . . 8.8 – 8.9

19. Kinetic-molecular theory . . . . . 19.1 – 19.2

20. Maxwell-Boltzmann distribution . . . 19.3

21. Collision of gas particles . . . . . 19.4 – 19.6

22. Observed rate laws . . . . . . 20.1 – 20.3

23. Temperature dependence of rates . . . 20.6

24. Kinetic mechanisms . . . . . . 20.7 – 20.8

25. Chain and oscillating reactions . . . . 20.9

26. Transition State Theory . . . . . 20.10 – 20.11