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Why do the gases at low temperature and ...

Why do the gases at low temperature and high pressure show large deviations from ideal behaviour ?

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When temperature is low and pressure is high the intermolecular forces become appreciable thus the volume occupied by the molecular is not negligibly small as composed to volume of gas.
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Knowledge Check

  • Real gases show deviations from, ideal behaviour when

    A
    temperature is low and pressure is high
    B
    temperature si high and Pressure is low
    C
    both temperature and pressure are low
    D
    both temperature and pressure are high

  • Any gas shows maximum deviation from ideal gas behaviour at

    A
    ` 0^(@)C` and 1 atmospheric pressure
    B
    `100^(@)C` and 2 atmospheric pressure
    C
    ` –100^(@)C` and 5 atmospheric pressure
    D
    `500^(@)C` and 1 atmospheric pressure

  • For a gas deviation from ideal behaviour is maximum at :

    A
    `0^(@)C` and 1.0 atm
    B
    `100^(@)C` and 2.0 atm
    C
    `-13^(@)C` and 1.0 atm
    D
    `-13^(@)C` and 2.0 atm

    • Similar Questions

    Explore conceptually related problems

    Write the conditions of temperature and pressure when gases deviate most from the ideal behaviour? Write real gas equation for n moles of a gas.

    For ideal gases, Z = 1 at all temperature and pressure.

    Write the conditions in terms of temperature and pressure under which gases deviate from ideal behaviour.

    At which one of the following temperature and pressure conditions the deviation of a gas from ideal behaviour is expected to be minium ?

    The negative deviation from an ideal behaviour stands for

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