Chem 161-2011 Lecture 23

Chem 161-2011 Lecture 23 - CHEMISTRY 161-2011 LECTURE 23...

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Chem 161-2011 Lecture 19 1 CHEMISTRY 161-2011 LECTURE 23 – DEC. 2ND CHAPTER 11 – GASES CHAPTER 12 -- INTERMOLECULAR FORCES ANNOUNCEMENTS ATTENDANCE MISCELLANEOUS Tue, 11/29 review for exam III in place of lecture Wed, 11/30 Exam III, 9:40 – 11:00 PM, Ch 8.4-10.8. Fri, 12/2 Lecture 23 – Finish Ch. 11; begin Ch. 12 Tue, 12/6 Lecture 24 – Ch. 12 Fri, 12/9 Lecture 25 (last lecture) – Ch. 12 Tue, 12/13 Review for final exam Fri, 12/16 Final exam; noon – 3 PM ( L e c 2 2 ) R e v E x I I I L e c 2 3 27 28 29 30 1 2 3 L e c 2 4 L e c 2 5 4 5 6 7 8 9 10 R e v F n l e x 11 12 13 14 15 16
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Chem 161-2011 Lecture 19 2 Chapter 11 (cont.) The Gas Laws The Combined Gas Law: The Pressure-Temperature-Amount-Volume Relationship Real Gases Factors that Cause Deviation from Ideal Behavior The van der Waals Equation van der Waals Constants Gas Mixtures Dalton’s Law of Partial Pressures Reactions with Gaseous Reactants and Products Calculating the Required Volume of a Gaseous Reactant Determining the Amount of Reactant Consumed Using Change in Pressure Using Partial Pressures to Solve Problems Chaper 12 - Intermolecular Forces and the Physical Properties of Liquids and Solids Intermolecular Forces Dipole-dipole interactions Hydrogen bonding Dispersion forces Ion-dipole interactions Properties of liquids Surface tension Viscosity Vapor pressure
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Chem 161-2011 Lecture 19 3 CHAPTER 11 - GASES IMPORTANT GAS FORMULAS (KE) avg = (3/2)RT Use SI units: KE = J; R = 8.314J/(Kmol); T = K Root mean square velocity = μ RMS = (3RT/MW) Use SI units: R = 8.314J/(Kmol); MW = kg/mol Effusion rate: Rate 1 /Rate 2 = (MW 2 /MW 1 ) Effusion time: Time 1 /Time 2 = (MW 1 /MW 2 ) Avogadro’s Law: n 1 /n 2 = V 1 /V 2 (P and T are constant) Boyle’s Law: P 2 /P 1 = V 1 /V 2 (n and T are constant) Charles’s Law: T 1 /T 2 = V 1 /V 2 (n and P are constant) Pressure: Pressure = force/area Pressure = gravity x density x height 1 mm = 1 Torr 1 atm = 760 mm = 14.696 lb/in 2 Ideal Gas Law: PV = nRT PV = (g/MW)RT P = (g/VMW)RT D = g/L = g/V P = (D/MW)RT Combination Gas Law : P 1 V 1 /n 1 T 1 = P 2 V 2 /n 2 T 2 Also, (P 1 V 1 MW 1 )/(g 1 T 1 ) = (P 2 V 2 MW 2 )/(g 2 T 2 ) Also, (P 1 MW 1 )/(D 1 T 1 ) = (P 2 MW 2 )/(D 2 T 2 ) If any variables are constant, a new equation is derived. e.g., at constant P and T P 1 V 1 /n 1 T 1 = P 2 V 2 /n 2 T 2 V 1 /n 1 = V 2 /n 2 , which is Avogadro’s law e.g., at constant T and V P 1 V 1 /n 1 T 1 = P 2 V 2 /n 2 T 2 P 1 /n 1 = P 2 /n 2 ; n 1 /n 2 = P 1 /P 2 ; n 1 /n T = P 1 /P T , which is Dalton’s law Dalton’s Law of Partial Pressures : P 1 + P 2 + P 3 + . . . = P T
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Chem 161-2011 Lecture 19 4 The Combination Gas Law is used when the conditions DO change. P 1 V 1 /n 1 T 1 = R P 2 V 2 /n 2 T 2 = R Therefore, P 1 V 1 /n 1 T 1 = P 2 V 2 /n 2 T 2 If any variables are constant, a new equation is derived. e.g., at constant P and T P 1 V 1 /n 1 T 1 = P 2 V 2 /n 2 T 2 V 1 /n 1 = V 2 /n 2 , which is Avogadro’s law e.g., at constant T and V P 1 V 1 /n 1 T 1 = P 2 V 2 /n 2 T 2 P 1 /n 1 = P 2 /n 2 ; n 1 /n 2 = P 1 /P 2 ; n 1 /n T = P 1 /P T , which is Dalton’s law Correspondingly, Boyle’s law, Charle’s law, and several other laws can be derived from the Combination Gas Law.
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Chem 161-2011 Lecture 19 5 ZUMDAHL 6 TH EDITION CHEM 161-2009 RECITATION 5 TH WEEK CHAPTER 5 - GASES GAS LAWS 45 An ideal gas is contained in a cylinder with a volume of 5.0 x 10
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Chem 161-2011 Lecture 23 - CHEMISTRY 161-2011 LECTURE 23...

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