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(C) For an ideal gas, the internal energy $U$ is a function of temperature $T$ only, i.e., $U = f(T)$.$1$. In isothermal processes, $\Delta T = 0$, so

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Adiabatic expansion of an ideal gas.

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(C) For an ideal gas, the internal energy $U$ is a function of temperature $T$ only, i.e., $U = f(T)$.$1$. In isothermal processes, $\Delta T = 0$, so $\Delta U = 0$.$2$. In adiabatic processes, the first law of thermodynamics is $\Delta U = q + w$. Since $q = 0$, $\Delta U = w$.$3$. For adiabatic expansion, the gas does work on the surroundings, so $w $4$. For adiabatic compression, work is done on the gas, so $w > 0$. Thus, $\Delta U > 0$, which means internal energy increases.Therefore, adiabatic expansion leads to a decrease in internal energy.

Which of the following processes exhibits a decrease in the internal energy of a system?

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