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1
Chapter 15.1 – 15.8
• Partial Pressure– (Whiteboard)
• Liquids vs. Gases• Liquid Properties
– Vapor Pressure, Heat of Vaporization, Boiling Point
– Viscosity, Surface Tension
• Intermolecular Forces• Selected Properties of Solids• NOTE: Be sure to prepare for tomorrow – it’s
somewhat tough…
2
Partial Pressure
• (Whiteboard)
3
Liquids vs. Gases
Property Gases Liquids
Compress?
Container?
Density?
Mixing?
4
Properties of Liquids
• Vapor Pressure• Heat of Vaporization• Boiling Point
• Viscosity• Surface Tension
5
Liquids – Physical Properties
Substance Vapor Pressure (20°C)
Boiling Point (°C)
Heat of Vaporization(kJ/mol)
MercuryWaterBenzeneEtherEthane
0.001217.575
44227,000
357100
8035
-89
5941312615
6
Liquid Properties (Hvap, BP, VP)
Hvap
BP
(boi
ling
poin
t)VP(vapor pressure)
Low
H
igh
High High
High Low
Hig
h
Low
Low LowLow
Low
7
Vapor Pressure of Water
• Look at Figure 15.12, pg 411.– H2O VP @20.0 °C
______________ mmHg
– H2O VP @ 36.7 °C ______________ mmHg
• About a 30 mmHg difference, about 4% extra gas volume…
O2 Gas&
H2O Vapor!
8
Intermolecular Forces
• Recall:– Bond Polarity is bases on the electronegativity
difference: H-F H H O
– Molecular Polarity• Net effect of bond dipoles, “swimming”
• The picture is an atomic force micrograph of the sintered surface of apolycrystalline aluminum oxide ceramic. The dark lines separate individualcrystals. The contrast within each crystal is due to surface facets.