RelativeResourceManager4 - Physical chemistry course study...

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Physical chemistry course study guide The Elements of Physical Chemistry , Peter Atkins (5th edition), Freeman (2009) Course Prefix & Number: CHEM3050 Course Title: Physical Chemistry Credit Hours: 3-0-3 Prerequisites: “C” or better grade in PHYS 2212 (or concurrent enrollment), MATH2202, CHEM2800, CHEM2800L Course Description: This one semester course in physical chemistry provides a survey of thermodynamics, chemical equilibria, and kinetics. It also includes an introduction to the quantum mechanical principles important in understanding molecular spectroscopy and molecular modeling. Chapter 0 Introduction 1. All terms in boldface. 2. Review Appendices 1 and 2 3. Interconvert measurements within the set of SI units 4. Interconvert the following units of pressure: Pa, bar, atm, torr, "mm Hg" 5. Calculation of the hydrostatic pressure in a liquid as a function of depth 6. Kelvin and Celsius (centigrade) temperature scales 7. Relationships between Avogadro's number (N A ), Boltzmann's constant (k B ) and the ideal gas constant (R) 8. Identify intensive and extensive properties Chapter 1: The Properties of Gases Sections 1 4-1.8 relevant to Kinetics and Reaction Rates 1. Assumptions of the kinetic molecular theory of gases and its use in the derivation of the ideal gas law 2. General form of the Maxwell distribution of molecular speeds and how this distribution is affected by temperature changes and by changes in the mass of the gas 3. The terms mean free path, collision frequency, time of flight, collision cross-section, means speed, mean square speed, root mean square speed 4. Calculation of values for the mean free path and the collision frequency and be able to describe how they are affected by changes in pressure, temperature and molar mass of the gas 5. Differentiating between the terms diffusion and effusion 6. Graham's Law of Effusion: effusion rate dependence on molar mass Chapter 10 The Rates of Reactions 1. All terms in boldface 2. Description of the reaction rate in terms of the rates of concentration changes of reactants and products, given the overall chemical reaction 3. Experimental rate law and the names of the parameters appearing in this empirical equation 4. The 1 st and 2 nd order reaction in one component in terms of the defining rate expressions, the integrated rate laws and the half-lives of the reactions 5. Experimental methods for obtaining rate laws: graphing Log(rate) against Log(concentration), initial rate method, excess reagent (flooding) method,
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6. Arrhenius expression for the empirical description of the temperature dependence of the experimental rate constant 7. Reaction mechanisms are described by a sequence of elementary reactions 8. Writing rate expressions for elementary reactions 9. Approach of the collision theory in expressing the rate constant in terms of collision rates, steric factor and energy factor 10. Activated complex theory and its explanation of the Arrhenius expression for the
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This note was uploaded on 03/01/2011 for the course CHEM 3050 taught by Professor Staff during the Spring '08 term at Kennesaw.

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RelativeResourceManager4 - Physical chemistry course study...

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