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Chapter 6
Gases
 
 
 
Movie
Title
 Movie
Caption
 Animation illustrating Boyle's law
Notes
 Animation: P-V Relationships (**) As the pressure of a gas is increased at constant temperature its volume decreases in a nonlinear fashion. A plot of volume as a function of 1/P is linear. This is consistent with Boyle's law which states that the pressure and volume of a gas are inversely proportional.
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 Movie
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 The decomposition of water to form hydrogen and oxygen.
Notes
 Animation: Electrolysis of Water (*) When a direct current is passed through water it decomposes to form oxygen and hydrogen. The volume of hydrogen gas produced at the negative electrode is twice the volume of the oxygen gas formed at the positive electrode. This indicates that water contains twice as many hydrogen atoms as oxygen atoms, which is an illustration of the law of constant composition.
Movie
Title
 Movie
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 Effect of temperature and molecular mass on the average kinetic energy of gaseous molecules
Notes
 Animation: Kinetic Energy in a Gas (**) The average kinetic energy of a gas is depends on its temperature and its mass. A graph of the distribution of molecular speeds of a gas at two temperatures shows that the average speed of the molecules of a gas is greater at the higher temperature. Species with different molecular masses have the same average kinetic energies at any given temperature, but the smaller molecules have a greater average speed.
Movie
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 Movie
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 The decomposition of sodium azide causes an airbag in an automobile to inflate.
Notes
 Animation: Airbags (**) A decomposition reaction involving NaN3 is used to inflate airbags in automobiles. When a collision occurs a hot piece of metal causes an explosive reaction which forms N2 gas. The N2 gas formed causes the rapid inflation of the airbag. As the airbag cools, the N2 gas contracts, causing the airbag to shrink, releasing the passenger. This animation also illustrates Charles' law and the stoichiometry of gases.
6.1
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 p 244-1a
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Notes
 liquid bromine with brown bromine vapor above
6.3
Title
 06.03
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 The concept of liquid pressure. All the interconnected vessels fill to the same height. As a result the liquid pressures are the same, despite the different shapes and volumes of the containers
Notes
  
6.4
Title
 06.04
Caption
 Measurement of atmospheric pressure with a mercury barometer
Notes
  
6.5
Title
 06.05
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 Measurement of gas pressure with an open-end manometer
Notes
  
6.
Title
 06.06
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 Relationship between gas volume and pressure-Boyle’s law. When the temperature and amount of gas are held constant, gas volume is inversely proportional to the pressure: a doubling of the pressure causes the volume to decrease to one-half its original value.
Notes
  
6.7
Title
 06.07
Caption
 An application of Boyle’s law-Example 6-3 illustrated. The final volume is the volume of the cylinder plus the volume of the tank. The amount of gas and its temperature remain constant when the cylinder is connected to the tank, but the pressure drops from 21.5 atm (the initial pressure) to 1.55 atm.
Notes
  
6.81
Title
 06.08
Caption
 Two containers with pistons
Notes
  
6.10.1UN
Title
 06.10.01
Caption
 Applying the Ideal Gas Equation
Notes
  
6.141
Title
 06.14
Caption
 Dalton’s law of partial pressures illustrated. The pressure of each gas is proportional to the number of moles of gas. The total pressure is the sum of the partial pressures of the individual gases
Notes
  
6.15
Title
 06.15
Caption
 Collecting a gas over water
Notes
  
6.16
Title
 06.16
Caption
 Visualizing molecular motion
Notes
  
6.17
Title
 06.17
Caption
 Distribution of molecular speeds-hydrogen gas at 0 °C. The percentages of molecules with a certain speed are plotted as a function of the speed. Three different speeds are noted on the graph and discussed in the text.
Notes
  
6.18
Title
 06.18
Caption
 Distribution of molecular speeds: effects of molar mass and temperature
Notes
  
6.21a
Title
 06.21a
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 H2 & N2 molecules separated by barrier, barrier removed, gases mixed
Notes
  
6.21b
Title
 06.21b
Caption
 H2 & N2 molecules separated from a vacuum by a barrier, pinhole opened in barrier, molecules pulled through pinhole
Notes
  
6.22
Title
 06.22
Caption
 The behavior of real gases-compressibility factor as a function of pressure at 0 °C. Values of the compressibility factor less than 1 signify that intermolecular forces of attraction are largely responsible for deviations from ideal gas behavior. Values greater than 1 are found when the volume of the gas molecules themselves is a significant fraction of the total gas volume.
Notes
  
6.23
Title
 06.23
Caption
 Intermolecular forces of attraction. Attractive forces of the red molecules for the green molecule cause the green molecule to exert less force when it collides with the wall than if these attractions did not exist.
Notes
  
6.23.3UN
Title
 06.23.03
Caption
 Charles's law: A dramatic illustration
Notes
  
6.23.7UN
Title
 06.23.07
Caption
 beaker with small toy diver, hand holding beaker and diver sinks
Notes
  
Table 6.1
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 Table 6.1
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Notes
  
Table 6.1.1
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 Table 6.1.1
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Notes
 Table of Vapor Pressures in margin of p198