In an adiabatic expansion of a gas,

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(B) In an adiabatic process,there is no exchange of heat with the surroundings,so $dQ = 0$.According to the first law of thermodynamics,$dQ = dU + dW$

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Its temperature falls

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(B) In an adiabatic process,there is no exchange of heat with the surroundings,so $dQ = 0$.According to the first law of thermodynamics,$dQ = dU + dW$,where $dU$ is the change in internal energy and $dW$ is the work done by the gas.Since $dQ = 0$,we have $dU = -dW$.In an expansion,the gas does work on the surroundings,so $dW > 0$.This implies $dU Since the internal energy of an ideal gas is directly proportional to its temperature $(U \propto T)$,a decrease in internal energy leads to a decrease in temperature.Therefore,in an adiabatic expansion,the temperature of the gas falls.

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