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Chapter 13 Outline

Chapter 13 Outline. Gases and their properties. Gases and their properties. Standard #4 The kinetic molecular theory describes the motion of atoms and molecules and explains the properties of gases. A. Air composed of several kinds of colorless gases. Relative Composition of air:.

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Chapter 13 Outline

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  1. Chapter 13 Outline Gases and their properties

  2. Gases and their properties Standard #4 The kinetic molecular theory describes the motion of atoms and molecules and explains the properties of gases.

  3. A. Air composed of several kinds of colorless gases Relative Composition of air: * Nitrogen: 78% * Oxygen: 21% * Carbon Dioxide: * Noble Gases trace amounts * Water Vapor (the amount varies) 1%

  4. B. Some gases have color Nitrogen Dioxide is SMOG! Chlorine • C. Any 1 mole of a gas occupies • 22.4 L

  5. Nature of Gases 1. Gases have Mass

  6. 2. Gases are easy to Compress

  7. 3. Gases fill their container

  8. Molecules travel from a high concentration to a low concentration 4. Gases Diffuse

  9. I smell something weird!

  10. 5. Gases Effuse The escape of gas molecules through a tiny hole into an evacuated space.

  11. 5. Gases Effuse Gases Effuse:

  12. 6. Exerts Pressure on Wall of container The pressure of the gas depends on the temperature! What do you think will happen to the gas and the amount of pressure if this balloon is placed near a heat source/light?

  13. Volume of balloon at room temperature Volume of balloon at 0°C

  14. The Characteristics of Gases Video

  15. The Kinetic Molecular Theory 1. Gases consist of small particles • Gases are separated by large distances • Gases are in constant Rapid Motion • Collisions are elastic No loss of energy with collisions. Energy is conserved There is a loss of energy with collisions.

  16. Kinetic Molecular Theory Video clip

  17. Measuring Pressure: • Pressure: Force • Area • 1. Pressure is high…area is small • 2. Pressure is low…area is LARGE

  18. Units for measuring PRESSURE 1atm 760.mmHg 101.3kPa 14.7lb/in2 or psi = = = End of day 1

  19. D. Instrument that measures: B. Temperature: A. Pressure: Barometer Thermometer

  20. Converting pressure and Temperature on overhead projector! Get calculators ready!!!!!!!!!! Stop Day 1

  21. Boyle’s Law: P and V Robert Boyle States that the volume of a gas is inversely proportional to the pressure at constant temperature 25 January 1627 – 30 December 1691

  22. Low pressure= High Volume High pressure= Low Volume Constant temperature and Constant Number of gas particles

  23. Boyle’s law animation

  24. Jacues Charles Nov. 1746 - Apr. 1823 States that the volume of a gas is directly related to its temperature at constant pressure.

  25. Charles’ Law Visuals

  26. Dalton's law of partial pressures was stated by in 1801: John Dalton

  27. The total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual component gases.  The partial pressure is the pressure that each gas would exert if it alone occupied the volume of the mixture at the same temperature

  28. Video clip on the gas laws 4 mins

  29. Ideal Gas Law

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