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Why is it not possible to cool a gas to...

Why is it not possible to cool a gas to a temperature of absolute `(0 K)` ?

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It is not possible to cool a gas to a temperature of absolute zero because the gas liquefies before attaining this temperature.
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Knowledge Check

  • The absolute temperature of a gas

    A
    is a measure of number of molecules of the gas
    B
    indicates nature of the gas
    C
    is a measure of volume of the gas
    D
    none of these

  • A gas is undergoing an adiabatic process. At a certain stage, the volume and absolute temperature of the gas are V_(0), T_(0) and the magnitude of the slope of the V-T curve is m. molar specific heat of the gas at constant pressure is [Assume the volume of the gas is taken on the y-axis and absolute temperature of the gas taken on x-axis]

    A
    `(mRT_(0))/(V_(0))`
    B
    `(MRT_(0))/( 2V_(0))`
    C
    `((V_(0)+mT_(0))R)/(V_(0))`
    D
    `((V_(0)+mT_(0))R)/(2V_(0))`

  • If the temperature of the body theta and time of cooling 't' and room temperature of the surrounding theta_(0) . The cooling curve is

    A
    B
    C
    D

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    If it were possible for a gas in a container to reach the temperature 0K, its pressure would be zero. Would the molecules not collide with the walls? Would they not transfer momentum to the walls?

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