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Chem1212K, Week 4 Notes

by: Bethany B.

Chem1212K, Week 4 Notes CHEM 1212K

Marketplace > Georgia Gwinnett College > Chemistry > CHEM 1212K > Chem1212K Week 4 Notes
Bethany B.


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These notes cover the last material that will be on the first test. The properties of liquids, vapor pressures, and phase change diagrams are all from chapter 11 in the textbook.
Principles Chemistry II w/Lab
Omar Villanueva
Class Notes
General Chemistry, vapor pressure, Heat of Vaporization, phase change, Exam 1
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This 2 page Class Notes was uploaded by Bethany B. on Friday September 9, 2016. The Class Notes belongs to CHEM 1212K at Georgia Gwinnett College taught by Omar Villanueva in Fall 2016. Since its upload, it has received 5 views. For similar materials see Principles Chemistry II w/Lab in Chemistry at Georgia Gwinnett College.


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Date Created: 09/09/16
9.10.16 Chemistry 1212KNotes[Week 4] Chapter 11 Lecture Cont. (Intermolecular Forces) Whichhas a higher boilingpoint? C H O Ethanol or C H O Dimethyl Ether 2 6 2 6 Why? Properties of Liquids  Low compressibility,lack of rigidity,andhigh density comparedwithgases.  Surface tension—resistance of aliquidto an increase inits surface area: o Liquids withlarge intermolecular forcestendto have highsurface tensions  Capillary action—spontaneous risingof aliquidin a narrow tube: o Cohesiveforces—intermolecular forcesamongthe molecules of the liquid  For the meniscus of mercury,the cohesive forcesdominate. o Adhesive forces—forces betweenthe liquidmolecules andtheir container  For water,the adhesive forceswin. Vapor pressure  Inaclosedcontainer,some of the H O ch2n(l) to H O 2 (g)but the vapor is containedwithin the container. o Endothermic H vap=(+)  At “Dynamic Equilibrium”—the evaporationrate is beingmet witha condensationrate (some of the molecules are evaporatingandothers are condensing) o Vapor Pressure—the pressure of the vapor presentatequilibriumthatkeeps the liquid fromall becoming vapor o The systemis at equilibrium whenno netchange occurs inthe amount of liquid or vapor because the two opposite processes exactly balance eachother.  Whatis the vapor pressure of waterat100C? 1 atm Whatdoes Vapor PressureDependon? 1. Intermolecular forces—The strongerthe forces inthe liquid, the lower the vapor pressure. CH 4(l) H 2 (l)  Dispersion  H-bonding High Vapor Pressure  Dispersion  Dipole-Dipole Lower VaporPressure 2. Temperature—Athigher temperatures,more particles will have enoughenergy to overcome the intermolecular forcesof liquidand vaporize (chapter 5? -gases). Clausius—ClapeyronEquation −Δ???? ln( ) = ????????????(1 − 1 ) ????1 ???? 2 ????1 Pvap= vapor pressure H vap enthalpy of vaporization R= 8.3145 J/Kmol T= temperature (in kelvin) Phase Change Diagrams  A convenientway of representingthe phases of a substance as afunctionof temperature and pressure.Every Phase Diagramis differentfor differentcompounds/elements.  Critical point—themaximum temp/pressure asubstance canexistinthe liquid phase  Triple point—atacertaintemperatureandpressure, the solid/liquid/gas phases canexistatthe same time for that element  The “equilibriumlines” show all of the points of phase changes. So the line betweensolidand liquid is the melting point, the line betweenliquid and gas is the boiling line, the line between solidand gas is the sublimation line.  The phase withthe largestarea (or whicheveris atthe lowestpressure/temp.) is denser. Exam 1 Content:Chapters 9-11.9 2


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