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Understanding Ideal Gas Law

  1. Sep 29, 2010 #1
    I'm curious from a lab sort of perspective, how does one keep a gas at a constant temperature yet decrease both pressure and density? Like how could I reduce the pressure of argon gas with the gas kept at room temperature? Put it in a vacuum larger than the space it normally occupies or something? How is that constructed?
  2. jcsd
  3. Sep 30, 2010 #2
    Yes, you have to change the volume (or the amount of argon). Then you may have to wait for thermal equilibrium.
    What about a cylinder with a moving piston?
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