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    juggalo_89's Avatar
    juggalo_89 Posts: 1, Reputation: 1
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    #1

    Apr 17, 2012, 10:37 PM
    Chemistry
    What happens to the original pressure of a sample of a gas with each of the following changes. Triple the volume and half the kelvin temperature. Half the volume and double the kelvin temperature
    Chic_Bowdrie's Avatar
    Chic_Bowdrie Posts: 54, Reputation: 8
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    #2

    Jul 28, 2012, 10:10 AM
    School's probably out on this one, but here's practicing an answer:

    Assuming the sample behaves as an ideal gas, PV = nRT enables predicting what happens under the change in conditions specified. Using subsripts to describe the before (b) and after (a) conditions: Pa/Pb = TaVb/TbVa. In the first case, the pressure would be 1/6 after and four times more in the second case.
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