Final answer:
When a gas is compressed, the frequent and energetic collisions of gas particles result in an increased temperature. This is in accordance with the kinetic theory of gases and the ideal gas law.
Step-by-step explanation:
As a gas is compressed, its particles are forced closer together, resulting in more frequent and energetic collisions with the walls of the container. According to the kinetic theory of gases, these collisions transfer energy to the walls, which is interpreted as an increase in temperature. Hence, when a gas is compressed, assuming no heat is lost to the surroundings, its temperature increases.
This behavior can be understood through the ideal gas law, where the product of pressure (P) and volume (V) is proportional to the amount of substance (n) and temperature (T). Quickly compressing a gas increases its pressure, which, with the quantity of gas remaining constant, leads to an increase in temperature to maintain the equation balance. This also aligns with the principle that the average kinetic energy of gas particles, which is proportional to temperature, increases as the particles are squeezed closer and move faster.
The answer to the student's question is: As a gas is compressed, its temperature increases.