Chapter 9: The Gaseous State

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dante01
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312037
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Chapter 9: The Gaseous State
Updated:
2015-11-25 06:31:07
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chem
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  1. All gases have relatively _________densities
    low
  2. Properties of gases
    • -low densities
    • -move rapidly
    • -high velocities and kinetic energies
  3. Why do all gases expand when heated?
    -the temperature increase causes an increase in the kinetic energy of the gas molecules, making them move faster, collide harder and spread out
  4. Warm or Cool gas has the greater density?
    Cool
  5. Why does a hot air balloon rise in the atmosphere?
    • -hot air rises quickly and displaces the cooler air
    • -most trips are in the morning or evening when air is cooler
  6. What causes the balloon to inflate?
    The air that you are blowing into a balloon causes pressure. If this pressure is larger than atmospheric pressure then the balloon will expand
  7. Atmospheric Pressure
    total pressure exerted by gases in the atmosphere
  8. Pressure (P) =
    force of gas particles/ area of the container
  9. 1 atm = ____mmHg
    760
  10. 1 atm = ____torr
    760
  11. 1 atm = ____Pa
    101,325
  12. Conversation factor: Pa to atm
    1 atm/ 101,325 Pa
  13. Conversation factor: atm to mmHg
    760 torr/ 1 atm
  14. Pressure is directly proportional to
    • 1) Number of molcules (n)
    • -more molecules = more collisions with walls =pressure
    • 2) constant Temperature (T)
    • 3) constant volume (V)
  15. K =
    C + 273.15
  16. Pressure and volume relation
    • -Inversely proportional
    • -Boyle's law
    • -as pressure increases, volume decreases
    • -When the volume of a gas shrinks, the gas molecules have less space to move around and so they hit their
    • container more often. The more frequently the gas impacts the container walls, the higher the pressure.
    • So, as volume decreases, the pressure increases. If the container expands, the impacts are less frequent
    • and the pressure decreases.
  17. Volume and temperature relation
    • As temperature increases, volume increases
    • -charles law
  18. Boyle's Law
    • -as gas pressure increases, gas volume decreases
    • -(T and n are held constant)
    • P1V1=P2V2
  19. Charle's law
    • -As gas temperature increases, gas volume increases
    • -(P and n are held constant)
    • V1/T1=V2/T2
  20. Avogadro's Law
    • -As thee number of moles of gas increases, gas volume increases
    • -(P and T are held constant)
    • -V1/n1=V2/n2
  21. Combined Gas Law
    • -Combining Boyle and Charles law
    • -(n is held constant)
    • P1V1/T1=P2V2/T2
  22. Ideal gas law
    PV= nRT
  23. R=
    0.0821 Latm/mol K
  24. Mass =
    mol x MM
  25. d =
    P x MM/ RT
  26. Calculate the density of ___at STP
    = molar mass / 22.4 L
  27. n =
    mass in grams (g) / molar mass (M)
  28. What is the molar mass of the gas?
    PV =
    gRT/M
  29. Conditions where real gases deviate from ideal gases
    1) At high pressure (small volumes)

    2) at low temperature
  30. Partial Pressure =
    Patm - PH2O

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