Physical Chemistry for the Chemical and Biological Sciences

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Chemistry 223H1 Fall Term 2009 Instructor: Dr. D.F. McIntosh Email: [email protected] Office hours: Fridays 4:00 – 5:00 pm Rm 223 in Lash Miller Lectures: T : LM 159 2:00 – 3:30 pm F : LM 159 2:00 – 3:30 pm Textbook: Physical Chemistry for the Biological Sciences by Raymond Chang. (in the Bookstore) Midterm: Wednesday, October 28, 2009: 2:30 – 4:30 pm
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Other Suggested Reading …… ….these additional texts also provide very useful discussions of topics covered in this course …. . 1. Physical Chemistry 7 th Edition Atkins P., de Paula J. 2. The Elements of Physical Chemistry with Applications in Biology Atkins P. *** Please note that if not specified the figures within the slides are taken from the Chang Text. *** The majority of the problems are also taken from the Chang Text.
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Problem Sets & Tutorials Problems Recommended problems will be assigned for each chapter. They will not be graded. Full solutions will be covered in detail at the TUTORIALs. TUTORIALS: Thursdays 2:00-3:00 pm (A–Li) MS 2172 Alon Eisenstein (Liang–Z) TZ 6 Shell Ip A teaching assistant will go over solutions to problems and answer any specific questions.
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Course Evaluation 45 % Midterm Wednesday, October 28, 2009 2:30 to 4:30 pm 55 % Final Exam To Be Scheduled
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Outline of the Course 1) Review and Definitions 2) Molecules and their Energies 3) 1 st Law of Thermodynamics 4) 2 nd Law of Thermodynamics 5) Gibbs Free Energy 6) Phase Diagrams and REAL Phenomena 7) Non-Electrolyte Solutions & Simple Mixtures 8) Chemical Equilibrium 9) Kinetics
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SECTION 1.0. Review and Definitions Relevant Sections in Text …….Chapter 2 (sections 2.1 – 2.8)
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SECTION 1.0. Review and Definitions GOALS: 1) to review some basic definitions 2) to review the gas laws (i.e. Boyle’s law, Charles’ law, Avogadro’s law) and the “ideal” gas equation 3) to understand difference between an ideal gas and a real gas (i.e. Z, van der Waals equation) Why is this important: we need these basic concepts to understand molecules and their energies…….
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1.1. Review and Definitions A) Define System: OPEN : mass and energy exchange CLOSED : only energy exchange ISOLATED : no mass nor energy exchange SYSTEM S u r o n d i gs Surroundings g s OPEN CLOSED ISOLATED
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B) Define Properties of Matter Extensive Properties ……properties whose values are directly proportional to amount of material in system e.g. mass, area, volume, energy Intensive Properties …….properties whose values are not dependent on amount of material in system e.g. temperature, pressure, density …. Intensive properties are usually defined as ratio of two Extensive properties…… Pressure = Force/Area Density = Mass/Volume
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C) Temperature How do we define temperature ? ….. hot or cold Need more precise “scientific” definition……. . - temperature is a variable - consider closed systems A & B (no mass exchange) “ An ISOTHERM” P A V A P B V B A B P A ’V A ’P B ’V B A B heat exchange
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1.2. Review of GAS Laws A) Boyle’s Law …relationship between Pressure (P) and Volume (V) V 1 / P …….PV = constant so P 1 V 1 = P 2 V 2 (constant n and T) B) Charles’ Law …relationship between V and T V T so V 1 /T 1 = V 2 /T 2
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1 - Chemistry 223H1 Fall Term 2009 Instructor Dr D.F...

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