What principle does the kinetic molecular theory assert about gas particles?

The kinetic molecular theory articulates that gas particles are in constant, random motion. This principle is foundational to understanding the behavior of gases and is based on a few key tenets. First, gas particles are far apart compared to their size, which allows them to move freely without significant interactions with one another. As they collide with each other and with the walls of their container, these particles exhibit random motion in various directions at varying speeds.

This constant motion leads to the assertion that the average kinetic energy of the gas particles is directly proportional to the temperature of the gas, which explains why heating a gas increases its temperature and the energy of the particles. Additionally, since the motion is random, the direction and speed of gas particles are unpredictable, contributing to the distribution of velocities observed in a sample of gas.

By contrast, the other options present understandings that do not align with the principles of kinetic molecular theory. Gas particles, for example, are not stationary at any temperature, as this would contradict the natural behaviors observed in gases. Also, gas particles do not only exist at low pressures; they can exist and function over a wide range of pressures. Lastly, while gases may emit light under certain conditions (such as during excitation or combustion), this is not