Chapter 11 lecture 2

# Chapter 11 lecture 2 - Let both Temperature and Pressure...

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Time or Heat added T Cooling curve At some constant pressure BP MP 1 2 3 4 5

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Look at What you See: What phases are present? 1 2 3 4 5 A DP tid-bit Water vapor above 100 o C a.k.a “Steam” is invisible
Use Heat of Fusion and Vaporization ( H X moles) for phase changes On the angles use specific heat (q=ms T). 1. Mark BP and MP at the pressure given (usually assumed 1 atm) For MethanolMP = -97.7 o C; BP = 64.7 o C 2. Look up specific heats of gas, liquid and solid as needed. How many kJ of heat must be removed to change 1.25 moles of Methanol gas @ 25 o C to a liquid at 15.5 o C

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Put it all together: Evaporation – Condensation Melting – Fusion (Freezing) Sublimation – Deposition IMF Part KE Part H fus + H vap = H sub q= ms T When KE overcomes IMF the liquid will boil
Phase Diagrams

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Unformatted text preview: Let both Temperature and Pressure Vary (Containers) CO 2 H 2 O Words: Triple Point Critical Pressure Critical Temperature Super critical fluid “Normal” means at 1 Atmos Cutting Ice with a wire Explanations for BP, Surface Tension, Viscosity (Cohesive) and Wetting (Adhesive) Types of Intermolecular Forces (IMF) Van der Waals 1. Dispersion Forces Instantaneous and Induced Dipoles 1. Permanent dipole-dipole (Special Case Hydrogen bonding Dipoles: Electronegativity, separation, Induced and Temporary Dipoles Look for big electron “floppy” molecues Predicting Boiling Points Molar Mass IMF Homologous Series Halide Gases Pentanol vs Dimethylpentane X X X Molar Mass BP (K) H 2 Te H 2 Se H 2 S 200 400 100...
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## This note was uploaded on 04/16/2008 for the course CHEM 1123 taught by Professor Paul during the Fall '06 term at Arkansas.

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Chapter 11 lecture 2 - Let both Temperature and Pressure...

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