Lect+19+08 - Lecture Goals You will have a plain language...

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Lecture Goals You will have a plain language understwanding of Thermodynamic equilibrium in Ideal Gases You will have a plain language understanding of Thermodynamic equilibrium in Ideal Solutions Equilibrium involving multiple phases You will have a plain language understanding of the equilibrium constant You will be able to use the equilibrium constant and associated chemical reaction to calculate pressures (concentrations) You will be able to use the reaction quotient to analyze equilibrium problems You will have a plain language understanding of the effect of changes in reactant/product pressure, reactor volume, and temperature on equilibria
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Announcements I will hold office hours Monday from 1-2 and on Wednesday 12-1 Exam 2 is the Tuesday after break (March 4) There will be reviews for the exam on Monday during class and on Monday evening March 3 No class this Friday (as indicated in the syllabus). I will not be available for this Friday’s office hours.
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Announcements Exam 2 will be composed of between 25 and 35 multiple choice problems valued at 2 and 4 pts. Numerical problems, conceptual problems, and concept identification problem will make up the majority of the exam. The practice exam 2 emphasizes conceptual problems more heavily than the exam will. The new material includes 11.5, 11.6; 12.1- 12.6; 13.1, 13.5-13.7; 14.1-14.6
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Thermodynamic Description of Equilibrium Ideal Gas reactions How does G change with changing pressure for ideal gas in isothermal situation? 2200 G = H - T S, ideal gas dT = 0, so H = 0 2200 S = nR lnV f /V i = nR lnP i /P f So G = - T S = -nRT lnP i /P f = nRT lnP f /P i 1.00 atm is taken as the reference state for a gas at any pressure so 2200 G = nRT lnP i
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This note was uploaded on 04/01/2008 for the course CHEM 230 taught by Professor Sharp during the Winter '08 term at University of Michigan.

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Lect+19+08 - Lecture Goals You will have a plain language...

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