The kinetic molecular theory is a collection of several rules that describe the behavior of gases. The nature of gas molecules was examined by scientists, such as Robert Boyle and Jacques Charles, who outlined their observations in several laws that eventually became the Kinetic Molecular Theory. Volume, temperature and pressure are all taken into account when observing and understanding the behavior of gases.
The kinetic molecular theory is composed of five postulates, one of which states that gas particles are in constant random motion and, according to Newton’s laws, remain in random motion unless acted upon by an outside force. Another rule is that the volume gas molecules occupy is negligible when compared to the volume of the container in which they exist. A third rule posits that when gas molecules collide, there is no loss or gain of energy. Another rule states that there is no notable force of attraction between gas particles. The last rule explains that kinetic energy can be determined by using the equation 3kT/2, in which k is a constant and T is the temperature.
Other properties of gases can be inferred from these rules. For example, if the temperature of a gas remains constant, then the kinetic energy of a sample of molecules does not change, no matter how much time passes. Furthermore, the shape and mass of gas particles doesn't determine their kinetic energy; only temperature does this.