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The Gas Laws

The Gas Laws. Pressure. Force per unit area. Gas molecules fill container. Molecules move around and hit sides. Collisions are the force. Container has the area. Measured with a barometer. Vacuum. Barometer.

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The Gas Laws

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  1. The Gas Laws

  2. Pressure • Force per unit area. • Gas molecules fill container. • Molecules move around and hit sides. • Collisions are the force. • Container has the area. • Measured with a barometer.

  3. Vacuum Barometer • The pressure of the atmosphere at sea level will hold a column of mercury 760 mm Hg. • 1 atm = 760 mm Hg 760 mm Hg 1 atm Pressure

  4. Units of pressure • 1 atmosphere = 760 mm Hg • 1 mm Hg = 1 torr • 1 atm = 101,235 Pascals = 101.325 kPa • Can make conversion factors from these.

  5. What is 724 mm Hg in torr? • 724 torr • 96.5 torr • 0.953 torr • 73,359 torr

  6. What is 724 mm Hg in kPa? • 724 kPa • 96.5 kPa • 0.953 kPa • 73,359 kPa

  7. What is 724 mm Hg in atm? • 724 atm • 96.5 atm • 0.953 atm • 73,359 atm

  8. The Gas Laws • Boyle’s Law • Pressure and volume are inversely related at constant temperature. • PV= k • As one goes up, the other goes down. • P1V1 = P2 V2 • Graphically

  9. V P (at constant T)

  10. Slope = k V 1/P (at constant T)

  11. Examples • 20.5 L of nitrogen at 25ºC and 742 torr are compressed to 9.8 atm at constant T. What is the new volume? • 2.04 L • .264 L • .467 L

  12. 30.6 mL of carbon dioxide at 740 torr is expanded at constant temperature to 750 mL. What is the final pressure in kPa? • 30.2 kPa • .0397 kPa • 4.025 kPa • 169843 kPa

  13. Charles' Law • Volume of a gas varies directly with the absolute temperature at constant pressure. • V = kT (if T is in Kelvin) • V1 = V2 T1 = T2 • Graphically

  14. He CH4 H2O V (L) H2 -273.15ºC T (ºC)

  15. Examples • What would the final volume be if 247 mL of gas at 22ºC is heated to 98ºC , if the pressure is held constant? • 1100 mL • 196 mL • 311 mL

  16. At what temperature would 40.5 L of gas at 23.4ºC have a volume of 81.0 L at constant pressure? • 592.8 K • 592.8 0C • 319.8 K

  17. Avogadro's Law • At constant temperature and pressure, the volume of gas is directly related to the number of moles. • V = k n (n is the number of moles) • V1 = V2 n1 = n2

  18. Gay- Lussac Law • At constant volume, pressure and absolute temperature are directly related. • P = k T • P1 = P2 T1 = T2

  19. Combined Gas Law • If the moles of gas remains constant, use this formula and cancel out the other things that don’t change. • P1 V1 = P2 V2. T1 T2

  20. Ideal Gas Law • PV = nRT • V = 22.41 L at 1 atm, 0ºC, n = 1 mole, what is R? • R is the ideal gas constant. • R = 0.08306 L atm/ mol K • Tells you about a gas is NOW. • The other laws tell you about a gas when it changes.

  21. Ideal Gas Law • A hypothetical substance - the ideal gas • Think of it as a limit. • Gases only approach ideal behavior at low pressure (< 1 atm) and high temperature. • Use the laws anyway, unless told to do otherwise. • They give good estimates.

  22. Example • A 47.3 L container containing 1.62 mol of He is heated until the pressure reaches 1.85 atm. What is the temperature? • 316 K • 658 K • 27.1 K

  23. Gas Density and Molar Mass • D = mass/Volume • Let MMstand for molar mass • MM = mass/n • n= PV/RT • PV = mass RT MM

  24. Example • What is the density of ammonia at 23ºC and 735 torr? • 0.676 g/L • 0.987 g/L • 1.20 g/L

  25. Gases and Stoichiometry • Reactions happen in moles • At Standard Temperature and Pressure (STP, 0ºC and 1 atm) 1 mole of gas occupies 22.42 L. • If not at STP, use the ideal gas law to calculate moles of reactant or volume of product.

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