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(C) In an adiabatic process, there is no exchange of heat with the surroundings, i.e.,$dQ = 0$.According to the first law of thermodynamics, $dQ = dU

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increases.

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(C) In an adiabatic process, there is no exchange of heat with the surroundings, i.e.,$dQ = 0$.According to the first law of thermodynamics, $dQ = dU + dW$.Since $dQ = 0$, we have $dU = -dW$.When a system is compressed, work is done on the system, so $dW Therefore, $dU = -dW > 0$, which means the internal energy of the system increases.Since the internal energy of an ideal gas is directly proportional to its temperature $(U \propto T)$, an increase in internal energy leads to an increase in the temperature of the system.

$A$ thermodynamic system is compressed adiabatically, then its temperature

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