Adiabatic free expansion of an ideal gas must | vedclass

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(C) According to the first law of thermodynamics, $Q = \Delta U + W$. In an adiabatic process, $Q = 0$. In free expansion, the external pressure $P_{e

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Isothermal

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(C) According to the first law of thermodynamics, $Q = \Delta U + W$. In an adiabatic process, $Q = 0$. In free expansion, the external pressure $P_{ext} = 0$, so the work done $W = P_{ext} \Delta V = 0$. Substituting these values into the first law: $0 = \Delta U + 0$, which implies $\Delta U = 0$. For an ideal gas, internal energy $U$ is a function of temperature only $(U = f(T))$. Since $\Delta U = 0$, the change in temperature $\Delta T = 0$, meaning the temperature remains constant. Therefore, the process is isothermal.

Adiabatic free expansion of an ideal gas must be

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