Chem.ch11.exam3

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xiongav
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114529
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Chem.ch11.exam3
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2011-11-04 23:21:55
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Gases chemical reactions
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Chem.ch11.exam3
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  1. KMT: Kinetic Moleculer Theory (main points)
    1) Gas particles/atoms are in constant motion.

    2) Gas particles don't interact.

    3) Particle volume is tiny compared to the container volume in a gas.

    4) The kinetic energy of the gas particles is proportional to the temperature (in units of K, kelvin).
  2. Pressure & Units. Formulas.

    PSI

    1 atmosphere
    P = force/area; P = nRT / V

    PSI: pounds/in2

    1 atmosphere = 760 mm Hg = 760 torr = 14.7 psi
  3. Ideal Gas Law.
    Developed over time between P and T and V.

    PV = nRT

    • P=pressure (units of atmospheres)
    • V=volume (of liters, L)
    • n=# of moles of gas (can be CO2, Ar, etc.)
    • *You can predict the r'ship between PVT, as long as it's a gas
    • R=gas constant (always this value: .0821 L x atm / mol x K
    • T=temperature (units of K, kelvin)
  4. What is Boyle's Law?
    The pressure and the volume of a gas are inversly proportional to each other, temperature kept constant.
  5. What's Charle's Law?
    The temperature and the volume of a gas are directly proportional, assuming pressure is kept constant.

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