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Kinetic Theory Of Gas
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Kinetic Theory Of Gas

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Transcript

  • 1. Gas Law
    Kinetic Theory of Gases
  • 2. Gas in closed container
    Number of molecules is constant
    Mass of gas is constant
    Behavior of the gas depends on properties of gas
  • 3. Properties of Gas
    Volume
    Molecules move freely and fill the whole space
    Gas volume = container volume
    Temperature
    Average kinetic energy of molecules is proportional to the temperature
  • 4. Properties of Gas (cont)
    Pressure
    When the molecules collide and bounce back, there is a change in momentum
    Force is exerted on the wall
    Force per unit area is the pressure of the gas
  • 5. Relationship Between Pressure and Volume
    When the volume decrease, the number of molecules per unit volume increases.
    Same number of molecules will move in a smaller space
    Molecules collide more frequently with the walls of container.
    Thus, pressure will increase
  • 6. Boyle’s Law
    For a fixed mass of gas, the pressure of the gas is inversely proportional to its volume when the temperature is kept constant.
    P α 1/V
    PV = constant
    P1V1 = P2V2
  • 7. Example
    The air in a syringe has an initial volume of 12.0 cm3 and pressure of 100 kPa. The nozzle of the syringe is closed and the piston is pushed inwards until the volume of the air becomes 7.5 cm3. What is the pressure of the compressed air in the syringe?
  • 8. Solution
    P1 = 100 kPa
    V1 = 12.0 cm3
    P2 = final pressure
    V2 = 7.5 cm3
    Using Boyle’s law,
    P1V1 = P2V2
    P2 = P1V1/ V2
    P2 = (100 × 12.0) / 7.5
    P2 = 160 kPa