CH 11 Gas Laws

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Author:
Anonymous
ID:
50091
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CH 11 Gas Laws
Updated:
2010-11-16 22:41:06
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Chemistry
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Description:
Review of CH 11 in Timberlake text. Gases
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  1. What is the kinetic molecular theory?
    It is a theory that explains the behaivor of gases by examining individual molecules. Below is the theory.

    • 1. Gases consist of individual molecules or atoms in constant random motion
    • 2. Particles are widely spaced
    • 3. Particles do not attract or repel each other
    • 4. Particles collide with each other and with the sides of it's container.
    • 5. Temperature is expressed in Kelvin (degrees celcius + 273) which indicates kinetic energy in particles.

    REVIEW THIS DIAGRAM

  2. For gas law problems what units do you use for pressure, volume, mass, and temperature.
    • Pressure = atm
    • Volume = L
    • Mass = mol
    • temperature = Kelvin (degrees celcius + 273)
  3. Boyle's Law
    P1V1=P2V2
  4. Charle's Law
    • V1 / T1 = V2 / T2
  5. Gay-Lussac's Law
    P1 / T1 = P2 / T2
  6. Combined Gas Law
    P1V1 / T1 = P2V2 / T2
  7. Avogadro's Law
    V1 / n1 = V2 / n2

    • Avagadro's Law also states that 1 mole of any gas has a volume of 22.4L This is called the molar gas volume.
  8. What is STP and what are the values?
    Standard Temperature (273 K) and Pressure (1 atm).
  9. Ideal Gas Law
    PV= nRT
  10. Dalton's Law of Partial Pressures
    Ptotal = P1 + P2 + P3 +...

    In essence the total pressure is the sum of all the pressures of all gases in a container.
  11. Gas Laws in Chemical Reactions
    • 1. Convert given mass to moles.
    • 2. Use mole to mole ratio to convert unknown to moles.
    • 3. Use the other givens and the unknown in mole and plug them into the Ideal Gas Law (PV=nRT) to solve for unknown.

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