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For an ideal gas, the isothermal free ex...

For an ideal gas, the isothermal free expansion and adiabatic free expansion are basically the same processes- explain.

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According to the first law of thermodynamics, `DeltaU=q+w`. In free expansion of a gas, w=0. again, in an adiabatic process, q=0
Hence, in an adiabatic free expansion of an ideal gas, the change in internal energy `DeltaU=0+0=0`. Also, in an isothermal process, the change in internal energy of an ideal gas is zero. again for free expansion of an ideal gas, w=0. so, in an isothermal free expansion of an ideal gas, `DeltaU=q+w or, 0=q+0 or q=0`. therefore, it can be concluded that both processes are basically the same.
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Knowledge Check

  • In the isothermal expansion of an ideal gas

    A
    there is no change in the temperature of the gas
    B
    there is no change in the internal energy of the gas
    C
    the work done by the gas is equal to the heat supplied to the gas
    D
    the work done by the gas is equal to the chang in its internal energy

  • For isothermal free expansion of an ideal gas-

    A
    `DeltaU=0`
    B
    `DeltaS lt0`
    C
    `DeltaS gt0`
    D
    `DeltaH gt0`

  • In the thermal expansion of an ideal gas

    A
    there is no change in the temperature of the gas
    B
    there is no change in the internal energy of the gas
    C
    the work done by the gas is equal to the heat supplied to the gas
    D
    the work done by the gas is equal to the change in its internal energy

    • Similar Questions

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    What is the source of work done by the gas in the adiabatic expansion?

    Adiabatic process is essentially a very fast process. Explain.

    How will the temperature of an ideal gas change in an adiabatic expansion?

    The temperature of a gas decreases in an adiabatic expansion. Explain.

    Sign of DeltaU in adiabatic expansion of a gas is _____.

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