Calculate the internal energy change of one m | vedclass

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(D) For an adiabatic process,the heat exchange $q = 0$. In a free expansion process,the gas expands against zero external pressure,so the work done $w

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Zero

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(D) For an adiabatic process,the heat exchange $q = 0$. In a free expansion process,the gas expands against zero external pressure,so the work done $w = 0$. According to the first law of thermodynamics,$\Delta U = q + w$. Since both $q = 0$ and $w = 0$,the change in internal energy $\Delta U = 0 + 0 = 0$. Therefore,the internal energy change for an ideal gas during adiabatic free expansion is zero.

Calculate the internal energy change of one mole of an ideal gas during an adiabatic free expansion process from a volume of $2 \ L$ to $5 \ L$.

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