Kaplan Nursing Entrance Practice Exam

What is the relationship between the average kinetic energy of gas particles and temperature according to the kinetic molecular theory?

1. It is proportional to the absolute temperature of the gas

2. It remains constant regardless of temperature

3. It decreases as pressure increases

4. It increases at lower temperatures

The correct answer is: It is proportional to the absolute temperature of the gas

The average kinetic energy of gas particles is indeed proportional to the absolute temperature of the gas, as outlined by the kinetic molecular theory. This theory posits that gas particles are in constant motion and that their movement generates kinetic energy. As the temperature of the gas increases, the average energy of its particles also rises, reflecting the conversion of thermal energy into kinetic energy. This relationship is crucial in understanding gas behavior, as higher temperatures lead to increased particle speed and energy. For instance, when gas is heated, its molecules move faster, consequently raising the average kinetic energy. This direct relationship helps explain various gas laws and phenomena, like how increasing temperature can increase the pressure of a gas in a rigid container, since the same number of molecules moving faster will collide more often and with greater force against the walls of the container. Other options do not accurately represent the relationship defined by kinetic molecular theory. The constancy of average kinetic energy across temperatures would contradict the established principles of thermodynamics. The notion that kinetic energy decreases with increased pressure is not supported, as pressure in a gas is more a function of temperature and volume than a direct effect on kinetic energy at constant volume. Lastly, the statement about increased kinetic energy at lower temperatures misaligns with the foundational principles of