Oct_05 - Vapourization escaping molecules are bumped out by...

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Van der Waals Constants a – is a measure of the intermolecular forces between gas molecules b – is a measure of the size of the gas molecules
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Pressure of 0.50 mole of He or CO 2 in a 1.00 L container at 25ºC. Ideal gas: Helium: a = .03412, b=.0237 P = 12.23 atm Carbon Dioxide: a = 3.592, b=.04267 P VdW = 11.59 atm P VdW = 12.37 atm Examples
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Chapter 9 – Liquids and Solutions Phase Diagrams and Phase Equilibria Physical properties of Solutions Chapter 9: 7, 11, 13, 25, 35, 37, 47, 67, 89
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States of Pure Substances Solids high density, not very compressible intermolecular attractions >> kinetic energy Liquids high density, not very compressible intermolecular attractions > kinetic energy Gases low density, compressible intermolecular attractions < kinetic energy
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Unformatted text preview: Vapourization escaping molecules are bumped out by collisions requires heat energy from surroundings Liquid-Vapour Equilibrium dynamic equilibrium the partial pressure of the gas is called the vapour pressure of the gas (depends on T) Vapour Pressure Curves normal boiling point (b.p.) is the temperature where equilibrium vapour pressure equals 1 atm (760 torr) the curves are exponentials: ln (P) T 1-Component Phase Diagrams Heating Curve 12 2 1 Phase Diagram of Carbon Dioxide Water solid-liquid equilibrium line has a negative slope which is uncommon supercooled water movie Phases of Water Ice Water...
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This note was uploaded on 01/20/2011 for the course CHEM 154 CHEM 154 taught by Professor Yang during the Spring '10 term at The University of British Columbia.

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Oct_05 - Vapourization escaping molecules are bumped out by...

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