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UGA CHEM 1211 - Chemistry - Chapter 12 - 1

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Slide 1Slide 2Slide 3Comparison of Solids, Liquids, and GasesSlide 5PressureSlide 7Slide 8Slide 9Slide 10Boyle’s Law: The Volume-Pressure RelationshipSlide 12Charles’ Law: The Volume-Temperature RelationshipCharles’ Law: The Volume-Temperature RelationshipCharles’ Law: The Volume-Temperature RelationshipSlide 16Slide 17Standard Temperature and PressureThe Combined Gas Law EquationThe Combined Gas Law EquationSlide 21Slide 22Avogadro’s Law and the Standard Molar VolumeAvogadro’s Law and the Standard Molar VolumeSlide 25Summary of Gas Laws: The Ideal Gas LawSlide 27Summary of Gas Laws: The Ideal Gas LawSlide 29Slide 30Slide 31Slide 32Slide 33Dalton’s Law of Partial PressuresDalton’s Law of Partial PressuresDalton’s Law of Partial PressuresDalton’s Law of Partial PressuresDalton’s Law of Partial PressuresMass-Volume Relationships in Reactions Involving GasesMass-Volume Relationships in Reactions Involving GasesGeneral formulaE grp E geo Hybridizaton and bond angle mol geo/shapeAB22 Linear Sp 180 LinearAB33 Trigonal planar Sp2 120 Trigonal planarAB2U 3 Trigonal planar Sp2 120 Bent/angularAB44 Tetrahedral Sp3 109.5 TetrahedralAB3U 4 Tetrahedral Sp3 109.5 Trigonal pyramidalAB2U24 Tetrahedral Sp3 109.5 Angular/bentSigma bonds?Pi bonds?Clicker Q: How many σ bonds are in this molecule? 11Clicker Q: How many π bonds? 1Ch. 12 Gases and the kinetic-molecular theoryEnd of chapter problems (partial list): 5,6, 12, 14-18, 20, 23, 25-29, 31-45, 48-51, 58-66, 67, 68, 72, 74-804Comparison of Solids, Liquids, and Gases•The density of gases is much less than that of solids or liquids.Densities (g/mL)Solid Liquid GasH2O 0.917 0.998 0.000588CCl41.70 1.59 0.00503 Gas molecules must be very far apart compared to liquids and solids.5Composition of the Atmosphere and Some Common Properties of GasesGas % by VolumeN278.09O220.94Ar 0.93CO20.03He, Ne, Kr, Xe 0.002CH40.00015H20.00005Composition of Dry Air6Pressure•Pressure is force per unit area.–lb/in2–N/m2•Atmospheric pressure is measured using a barometer.•Definitions of standard pressure (KNOW not on resources)–76 cm Hg–760 mm Hg–760 torr–1 atmosphere–101.3 kPaHg density = 13.6 g/mLConversions:Boyle’s Law: The Volume-Pressure Relationship At a given T, the product of the pressure and volume of a definite mass of gas is constant.PV = k (constant n, T) T always in Kelvinhttp://www.grc.nasa.gov/WWW/k-12/airplane/aboyle.html good example9•http://www.youtube.com/watch?v=t8wFIMbMJvs&feature=related scuba dive example•http://www.rkm.com.au/animations/GAS-volume-pressure.html ok example10At 25oC a sample of He has a volume of 4.00 x 102 mL under a pressure of 7.60 x 102 torr. What volume would it occupy under a pressure of 2.00 atm at the same T? Think what it should be first.V1 = 400 mLP1= 760 torr (1 atm / 760 torr) = 1 atmP2 = 2.00 atmV2 = T = constant11Boyle’s Law: The Volume-Pressure Relationship•Notice that in Boyle’s law we can use any pressure or volume units as long as we consistently use the same units for both P1 and P2 or V1 and V2.•Use your intuition to help you decide if the volume will go up or down as the pressure is changed and vice versa.Clicker Q: What volume will 2.50 l of a gas occupy if the pressure is changed from 760. mm Hg to 630. mm Hg?250 L ( 760 mm) = 630 mm ( x) x = 3.02 L13Charles’ Law: The Volume-Temperature Relationship•Charles’s law states that the volume of a gas is directly proportional to the absolute temperature at constant pressure.•http://www.grc.nasa.gov/WWW/k-12/airplane/aglussac.html good one•http://group.chem.iastate.edu/Greenbowe/sections/projectfolder/flashfiles/gaslaw/boyles_law_graph.html cool one can change volume•http://www.nclark.net/GasLaws good website with lots of examples–Gas laws must use the Kelvin scale to be correct.V = kt V/T = kV1/T1 = V2/T2•Relationship between Kelvin and centigrade.273 + C= K o14Charles’ Law: The Volume-Temperature Relationshipabsolute zero = -273.15 0C15Charles’ Law: The Volume-Temperature RelationshipA sample of hydrogen, H2, occupies 1.00 x 102 mL at 25.0oC and 1.00 atm. What volume would it occupy at 50.0oC under the same pressure? 108 mLV1 = 1.00 x 102 mLT1 = 298 KP = 1 atmV2 = T2 = 323 K(1.00 X 102 mL)/(298 K) = V2/(323K)V2 = 108 mLTemperature increase = expect volume to increaseIf 20.0 l of oxygen are cooled from 100.°C to 0.°C, what is the new volume?(20.0L)/(373K)= (273K)/(V2)V2= 14.6 LClicker Q: 3.00 l of hydrogen at -20.°C are allowed to warm to a room temperature of 27°C. What is the volume at RT if the P remains constant?3.00 L / 253 K = V2 / 300V2 = 3.56 L18Standard Temperature and Pressure•Standard temperature and pressure is given the symbol STP.–It is a reference point for some gas calculations. •Standard P = 1.00000 atm or 101.3 kPa•Standard T = 273.15 K or 0.00oCKNOW19The Combined Gas Law Equation•Boyle’s and Charles’ Laws combined into one statement is called the combined gas law equation.–Useful when the V, T, and P of a gas are changing. http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/gasesv6.swf awesome site for all gas laws22211122112211TV PTV P k TV P:is law gas combined The :gas of samplegiven aFor TVTV VPVPLaw Charles' Law sBoyle'20The Combined Gas Law EquationA sample of nitrogen gas, N2, occupies 7.50 x 102 mL at 75.00C under a pressure of 8.10 x 102 torr. What volume would it occupy at STP?V1 = 750 mLT1 = 348 KP = 810 torrV2 = T2 = 273 KP2 = 760 torr(810 torr (750 mL))/348 = (760x)/273V2 = 627 mL21A sample of methane, CH4, occupies 2.60 x 102 mL at 32oC under a pressure of 0.500 atm. At what temperature would it occupy 5.00 x 102 mL under a pressure of 1.20 x 103 torr?V1 = 260 mLT1 = 305 KP1 = 380 torrV2 = 500 mLT2 = P2 = 1200 torr380torr(260mL)/305K = 1200 torr(500mL)/xX=1.85 x 103 KClicker Q: Given 20.0 l of ammonia gas at 5°C and 730. torr, calculate the volume at 50.°C and 800. torr.V1 = 20 LT1 = 278 KP1 = 730 torrV2 = xT2 = 323 KP2 = 800 torr730 (20) / 278 = 800 (x)/323V2 = 21.2 L23Avogadro’s Law and theStandard Molar Volumehttp://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/gasesv6.swf awesome site for all gas laws24Avogadro’s Law and theStandard Molar Volume•Avogadro’s Law states that at the same temperature and pressure, equal volumes of two gases contain the same number of molecules (or moles) of gas.•If we set the temperature and pressure for any gas to


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