When a gas undergoes adiabatic expansion,it c | vedclass

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(D) In an adiabatic process,there is no heat exchange with the surroundings,so $q = 0$. According to the first law of thermodynamics,$\Delta U = q + w

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Its internal energy is used to perform work.

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(D) In an adiabatic process,there is no heat exchange with the surroundings,so $q = 0$. According to the first law of thermodynamics,$\Delta U = q + w$. Since $q = 0$,we have $\Delta U = w$. During expansion,the gas does work on the surroundings,so $w Consequently,the change in internal energy $\Delta U$ is negative,meaning the internal energy of the gas decreases. Since the internal energy of an ideal gas depends only on temperature $(U \propto T)$,a decrease in internal energy leads to a decrease in temperature,causing the gas to cool down.

When a gas undergoes adiabatic expansion,it cools down because:

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