Chapter 10_Liquids & Solids_post

Chapter 10_Liquids & Solids_post - CHM 11200 Spring...

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CHM 11200 Spring 11 Chapter 10 Liquids & Solids
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Properties of Gases, Liquids & Solids Gas: Free particles with kinetic energy of motion much greater than intermolecular energies of attraction Liquid: Particles in contact with kinetic energy of motion comparable to intermolecular energies of attraction
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Solid: Particles in fixed positions with kinetic energy of motion much smaller than intermolecular energies of attraction Properties of Gases, Liquids & Solids
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States of Matter (p 13 & 14) Gas Solid Liquid 4
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States of Matter Gases – CO 2 (g) , H 2 O (g) 5 Solids – CO 2 (s) , H 2 O (s) Liquids – H 2 O ( l ) , Fe ( l ) We denote the states of matter symbolically:
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Physical (Phase) Changes
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Phase changes are physical changes they do not change the identity of the substance melting Solid Gas Liquid Liquid Solid Gas Physical (Phase) Changes freezing condensation evaporation sublimation deposition
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When we place a liquid in a closed container, some of the liquid evaporates (and some of this evaporated liquid will re-condense). This evaporation continues until the rate of liquid molecules evaporating equals the rate of gas molecules condensing. At this point an equilibrium is reached. The net number of gas molecules will remain constant. Liquid in Closed Container
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The partial pressure of gas in equilibrium with a liquid (in a closed container) is called its vapor pressure . Vapor Pressure
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The boiling point of a liquid is the temperature at which the vapor pressure of the liquid equals atmospheric pressure. Vapor Pressure and Boiling Point
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Example 1 (Practice Problem 10.1, p 380) 11
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Example 2 (Practice Problem 10.2, p 382) 12
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Cooling and Heating Curves
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Energy Changes Remember in Chapter 6 we talked about the heat absorbed or released by a substance when it changes temperature: q = C x m x ∆T heat change specific heat mass temperature change
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Energy Changes in Phase Changes During phase changes, we must consider each step on the heating curve individually:
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