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24 May, 17:24

A weather balloon is filled with helium that occupies a volume of 5.27 10^4 L at 0.995 atm and 32.0°C. After it is released, it rises to a location where the pressure is 0.720 atm and the temperature is - 12.7°C. What is the volume of the balloon at that new location?

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  1. 24 May, 18:36
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    Ideal gas law:

    pv = nrt

    nr is mole times the ideal gas constant, these are both held constant (do not change value)

    pv/t = nr

    Then you can set the conditions before = after

    pv/t = PV/T

    before: (convert to Kelvin)

    (0.995) (5.27x10^4) / 305

    After: (convert to Kelvin)

    (0.720) V / 206.3

    solve for V, volume after.

    (0.995) (5.27x10^4) / 305 = (0.720) V / 206.3

    4.926 x 10^4 L = V
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