This question tests the understanding of thermodynamics, specifically adiabatic processes, internal energy, and the relationship between work, heat, and temperature. * **Core concepts:** Adiabatic process, work, internal energy, temperature, first law of thermodynamics. * **Solution:** In an adiabatic process, no heat is exchanged with the surroundings. When a gas is rapidly compressed, work is done *on* the gas. Because there's no heat transfer, this work must be converted into an increase in the gas's internal energy. The internal energy of an ideal gas is directly related to its temperature. Thus, both internal energy and temperature will increase during compression. * **Option A analysis (Incorrect):** The temperature increase is correct; however, the internal energy increases because the work done goes into increasing the internal energy of the gas. This is a confusion on how to apply the first law. * **Option B analysis (Incorrect):** In an adiabatic process of compression, the temperature increases, not decreases, because work is done on the gas, increasing the internal energy and thus temperature. This reverses cause and effect. * **Option C analysis (Correct):** This is the correct description of an adiabatic compression. Both the temperature and the internal energy increase, because the work is converted directly to internal energy. * **Option D analysis (Incorrect):** The temperature does not remain the same, it increases since the internal energy increases. While it’s true that no heat exchange, that is not the only thing to consider. This fails to make the connection between internal energy and temperature.