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CHAPTER 6-A The Ideal Gas Law

CHAPTER 6-A The Ideal Gas Law. Gas Pressure. Gas Pressure. Units of pressure: atmosphere (atm) mm Hg (760 mm Hg = 1 atm) Pressure is force exerted per unit area Pa (kg/ms 2 , 101,325 Pa = 1 atm). Pressure–Volume Law (Boyle’s Law): . Boyle’s Law. Boyle’s Law.

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CHAPTER 6-A The Ideal Gas Law

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  1. CHAPTER 6-A The Ideal Gas Law © 2012 by W. W. Norton & Company

  2. Gas Pressure

  3. Gas Pressure • Units of pressure: atmosphere (atm) • mm Hg (760 mm Hg = 1 atm) • Pressure is force exerted per • unit area • Pa (kg/ms2, 101,325 Pa = 1 atm)

  4. Pressure–Volume Law (Boyle’s Law): Boyle’s Law

  5. Boyle’s Law • Pressure–Volume Law (Boyle’s Law):

  6. Boyle’s Law • Pressure–Volume Law (Boyle’s Law): V  1/P

  7. Charles’ Law • Temperature–Volume Law (Charles’ Law):

  8. Charles’ Law • Temperature–Volume Law (Charles’ Law): V  T

  9. Avogadro’s Law • The Volume–Amount Law (Avogadro’s Law):

  10. Avogadro’s Law • The Volume–Amount Law (Avogadro’s Law): V  n

  11. The Ideal Gas Law • Ideal gases obey an equation incorporating the laws of Charles, Boyle, and Avogadro. P V = n R T Where R is the combined proportionality constant. The gas constant, R = 0.08206 L·atm·K–1·mol–1

  12. Ideal Gas Law • What volume does 1 mole of methane gas (CH4) occupy at standard temperature and pressure (1.00 atm and 273.15 K)? • What volume does 1 mole of carbon dioxide gas occupy under the same conditions? • What is the volume occupied by 7.40 g of CO2 at STP?

  13. Ideal Gas Law • Oxygen gas is normally sold in 49.0 L steel containers at a pressure of 150.0 atm. How many moles (n) of oxygen does one container hold at 20oC? • What volume would the gas occupy if the pressure was reduced to 1.02 atm and the temperature raised from 20oC to 35oC?

  14. Ideal Gas Law • An inflated balloon with a volume of 0.55 L at sea level, where the pressure is 1.0 atm, is allowed to rise to a height of 6.5 km, where the pressure is about 0.40 atm. Assuming that the temperature remains constant, what is the final volume of the balloon?

  15. The Ideal Gas Law • Sulfur hexafluoride (SF6) is a colorless, odorless, very unreactive gas. Calculate the pressure (in atm) exerted by 1.82 moles of the gas in a steel vessel of volume 5.43 L at 69.5°C.

  16. Dalton’s Law of Partial Pressures Flash Animation - Click to Continue

  17. Dalton’s Law of Partial Pressures • The Partial Pressure (Px) of gas X in a mixture of gases is the pressure that gas X would exert if it alone occupied the container. • When calculating partial pressure, use the ideal gas law and ignore other gases in the container.

  18. Dalton’s Law of Partial Pressures • In a mixture of gases the total pressure, Ptot, is the sum of the partial pressures, Px, of the gases: • Dalton’s law allows us to work with mixtures of gases.

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