Lecture_4

Lecture_4 - Lecture 4 A. Awesome, aced it B. Probably...

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Unformatted text preview: Lecture 4 A. Awesome, aced it B. Probably managed a B C. Didnt really grasp it too well D. Where am I? Boiling Point and Vapor Pressure Experiment 2 Review of Acid/Base Chemistry Extraction Techniques Drying Organic Liquids Recrystallization Experiment 3 Should be reading for Week 3: Chapter 4- Glassware Chapter 13-13.4, 13.8 Distillation Should be reading for Week 4: Chapter 11- Extraction Chapter 12- Drying Organic Liquids Chapter 15- Recrystallization Properties of solutions that depend upon the number of particles, not the mass of the particles. Freezing (Melting) point depression Freezing Point total = Freezing Point solvent T f Boiling point elevation Boiling Point total = Boiling Point solvent + T b Osmotic Pressure Vapor Pressure Liquid Vapor Vapor Pressure: pressure a liquid exerts on environment Boiling Point: when vapor pressure equals atmospheric pressure What chemical features influence boiling point? A. Size of the molecule B. Hydrogen bonding C. Van der Walls forces D. Surface Area E. All of the above A. ethylbenzene B. tert-butyl benzene C. benzene D. methylbenzene Mohrig, page 128 Raults Law ( P = PX) P = partial vapor pressure P = vapor pressure of pure substance X = mol fraction of pure substance in solution X A = mol A / total number of moles solution Question: What is the partial pressure of ethanol (P=45.00kPa, FW=46.07g/mol) if 3.00 grams of it is mixed with 3.00 grams of something unknown (FW=32.04)? But doesnt that unknown substance also have a partial pressure that contributes? P total =P A + P B (Sum of the partial pressures) Question: Assuming the unknown is methanol (P=81.00kPa) what is the total vapor pressure above the solution? Lets say we have an equal number of moles of ethanol and methanol in solution. What is the fraction of ethanol in the vapor? the fraction of ethanol in the vapor?...
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Lecture_4 - Lecture 4 A. Awesome, aced it B. Probably...

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