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Test Chapter 12 Gas Laws

Test Chapter 12 Gas Laws. Conversion Factors 1 atm = 101.32 kPa = 760 mm Hg = 760 torr = 14.6 psi. Gas Constant R = .0821 L atm mol K or 8.314 L kPa mol K. Volume 1L = 1000ml =1 dm 3 1cm 3 = 1ml. Temperature C + 273 = K. Guy- Lussac’s P 1 = P 2 T 1 T 2 direct

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Test Chapter 12 Gas Laws

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  1. Test Chapter 12 Gas Laws Conversion Factors 1 atm = 101.32 kPa = 760 mm Hg = 760 torr = 14.6 psi Gas Constant R = .0821 L atm mol K or 8.314 L kPa mol K Volume 1L = 1000ml =1 dm3 1cm3 = 1ml Temperature C + 273 = K

  2. Guy-Lussac’s P1 = P2 T1 T2 direct proportion Boyle’s Law P1V1 = P2V2 inverse proportion Charles’ Law V1 = V2 T1 T2 direct proportion Ideal PV=nRT Avogadro V1 = V2 n1 n2 Combined Law P1V1= P2V2 T1 T2 Density =P Molar Mass RT Graham’s Law of Effusion rate of effusion for gas 1 = M2 rate of effusion for gas 2  M1 Dalton’s law of Partial Pressures: Ptotal = pa+pb+pc P dry gas = P barometer – P water vapor

  3. Kinetic Molecular Theory • Gases consist of tiny particles • atoms or molecules whose size is small compared to the great distances between them • Gas molecules are in constant, random motion. • Molecular collisions are elastic - do not lose kinetic energy from collisions • Temperature measures average kinetic energy of the gas molecules.

  4. Pressure = Force Area Barometer measure atmospheric pressure Higher pressure reads higher on the barometer Manometer compares gas to atmospheric pressure h is difference between inside and outside pressure. Atmospheric pressure ± h = inside pressure.

  5. Properties of the Atmosphere Layers include: thermosphere mesosphere stratosphere troposphere Air is N2 78% O2 21% Ar .93% CO2 .033% trace amounts of Ne, NH3, He, CH4,Kr As altitude increases: P TMoles

  6. Images from http://csep10.phys.utk.edu/astr161/lect/earth/atmosphere.html

  7. Consider separate 1.0 L gaseous samples of H2, SO2, Cl2, and O2 at STP. • Rank the gases in order of increasing average kinetic energy. • Rank the gases in order of increasing average velocity. • Rank the gases in order of increasing density. • If the kelvin temperature is doubled and the volume and amount are constant what will change? • If the pressure is reduced by 1/3, and the temperature and amount are constant, what will change? • How will reducing the volume at constant pressure affect the temperature if the amount is constant?

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