Kaplan Nursing Entrance Exam Practice 2025 – Comprehensive Prep

The kinetic molecular theory of gases provides a framework for understanding the behavior of gas particles. This theory is built on several key principles, which include the concepts in the first three options.

Gas molecules are considered to have no intermolecular forces, meaning they do not exert forces on one another as they move. This is fundamental to the behavior of gases, as it allows them to expand and fill their containers without significant resistance. Additionally, gas particles are in constant random motion, which means they move in all directions and at varying speeds, contributing to the pressure exerted by the gas on the walls of its container.

The third principle highlights that gas particles have negligible volume compared to the size of their container. This means that the volume occupied by the individual gas molecules themselves is so small that it can be ignored when calculating the overall volume of the gas.

On the other hand, while temperature does relate to the average kinetic energy of gas particles, the use of Celsius temperature in this context is not appropriate for expressing the relationship within the framework of the kinetic molecular theory. The average kinetic energy of gas particles is proportional to temperature, but it must be measured in Kelvin for the direct relationship to hold true. Therefore, stating that it is proportional to the temperature in Celsius