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Unformatted text preview: 1 Property of Gases Chapter 1 and 21 of the textbook The perfect gas States of gases Gas law Kinetic model of gases Real gases Molecular interactions Van der Waals equation Principle of corresponding states Based on Rob Schurkos note In this course, most assigned problems are from list A of the textbook! Homework 2 has been updated!! Redownload! Some problems are from the Numerical or Theoretical problems which is proceed with P, such as P1.1 Perfect Gas Individual Gas EOS Gas laws & example Mixtures of Gases Partial pressure Mole fraction Example Molecular interpretation Deriving EOS Maxwell distribution Molecular speeds & meaning to everyday life Collision theory & Chemical kinetics 2 Chapter 1.2 Chapter 21.121.3 3 Prefect Gas Equation of State (EOS) ( , , ) p f T V n = pV nRT = We can vary p, V, n, T, but they always have following relation (Several equivalent form) R= 8.31451 J K1 mol1 : gas constant nRT nRT pV p V T V p nR = = = 1 1 2 2 1 1 2 2 pV p V n T n T = In a industrial process, a gas goes from p 1 ,V 1 ,T 1 ,n 1 to p 2 ,V 2 ,T 2 ,n 2 , then 4 R is related to the Boltzmann constant, k: R = k x N A , where k = 1.3806 x 1023 J K1 N A = 6.022 x 10 23 mol1 5 In an industrial Process, nitrogen enters the vessel at 100 atm and 300K, and is then heated to 500K at constant volume. What is the final pressure if it behaved as a perfect gas? Black board example 6 Prefect Gas Equation of State (EOS) Boyles Law: When n and T are constant: pV=const, p 1/V , V 1/p. Charles Law: If n and V are held constant: p T If n and p are held constant: V T Avogadros Principle: When T and p are constant : V n, p n . 1 1 2 2 1 1 2 2 pV p V n T n T = 1 1 2 2 pV pV = 1 2 1 2 p p T T = 1 2 1 2 V V T T = 1 2 1 2 V V n n = 1 2 1 2 p p n n = 7 Graph the Laws Isotherm lines Isobar lines Isochor lines http://hyperphysics.phyastr.gsu.edu/Hbase/kinetic/idegas.html#c6 8 Visualize the laws Boyles Law Charles Law To see the movie, display in slide show mode. 9 P V T surface 10 Standard Condition standard ambient pressure and temperature (SATP): T = 298.15 K, p = 1 bar, molar volume of gas V m = 24.790 L mol1 (This is the default condition) standard temperature and pressure (STP) T = 0 o C, p = 1 atm, molar volume of gas V m = 22.414 L mol1 11 Mixture of Gases The partial pressure of a gas is the pressure it would exert if all the other gases in the mixture were absent. .........
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 Fall '08
 Raineri,F
 Physical chemistry, Mole, pH

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