Gases, Kinetics, and Chemical Equilibrium

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Gases, Kinetics, and Chemical Equilibrium
2010-10-27 06:01:38
chem pt2

Gases, Kinetics, Chemical Equilibrium
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  1. Mean free path is:
    The distance traveled by a gas molecule between collisions.
  2. Four ideal gas characteristics
    • gas molecules of zero volume
    • gas molecules exert no forces on other repulsive forces due to collisions
    • gas molecules make completely elastic collisions
    • the average kinetic energy of gas molecules is directly proportional to the temperature of the gas
  3. The ideal gas law is:
    PV = nRT

    R = 0.08206 L atm K-1 mol-1
  4. Charle's law says that:
    volume is proportional to temperature at constant pressure
  5. Boyle's law says that:
    volume is inversely proportional to pressure at constant temperature
  6. Avogadro's law states that:
    volume is proportional to the number of moles at constant temperature and pressure
  7. Solving for the partial pressure of a particular gas:
    χa * Ptotal = Pa
  8. Dalton's law of partial pressures states that:
    the total pressure is equal to the sum of the partial pressures

    Ptotal = Pa + Pb + Pc + ... + Pn
  9. Relationship between velocity and mass of two gases
    v1 / v2 = √m2 / √m1
  10. Real gases differ from ideal gases because they exhibit these behaviors
    • Vreal > Videal
    • Preal < Pideal
  11. For a new molecule to be formed according to the collision theory 2 requirements must be met:
    • molecules collide with enough kinetic energy (to overcome activation energy)
    • molecules collide in the correct orientation
  12. What is the relationship between temperature and rate of reaction
    Temperature and rate of reaction is proportional. As the temperature increases so does the rate of the reaction.