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Oct_05 - Vapourization ● escaping molecules are...

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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 1→2 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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