KMT Introduction

Basic Assumptions of the Kinetic Molecular Theory

By the late 19th century, scientists began accepting the atomic theory of matter started relating it to individual molecules. The Kinetic Molecular Theory of Gases is a theory that developed  from observations that scientists made about gases to explain their macroscopic properties. In other words it explains the different states of matter (solid, liquid, gas) and why they exist. The following are the basic assumptions of the Kinetic Molecular Theory:

1. Gases consist of very large numbers of tiny spherical particles that are far apart from one another compared to their size. The particles of a gas may be either atoms or molecules. The distance between the particles of a gas is much, much greater than the distances between the particles of a liquid or a solid.  Most of the volume of a gas, therefore, is composed of the empty space between the particles. In fact, the volume of the particles themselves is considered to be insignificant compared to the volume of the empty space.
2. Gas particles are in constant rapid motion in random directions. The fast motion of gas particles gives them a relatively large amount of kinetic energy.  Kinetic energy is the energy that an object possesses because of its motion. The particles of a gas move in straight-line motion until they collide with another particle or with one of the walls of its container.
3. Collisions between gas particles and between particles and the container walls are elastic collisions.  An elastic collision is one in which there is no overall loss of kinetic energy.  Kinetic energy may be transferred from one particle to another during an elastic collision, but there is no change in the total energy of the colliding particles.
4. There are no forces of attraction or repulsion between gas particles. Attractive forces are responsible for particles of a real gas condensing together to form a liquid.  It is assumed that the particles of an ideal gas have no such attractive forces. The motion of each particle is completely independent of the motion of all other particles.
5. The average kinetic energy  of gas particles is dependent upon the temperature of the gas. As the temperature of a sample of gas is increased, the speeds of the particles are increased. This results in an increase in the kinetic energy of the particles. Not all particles of gas in a sample have the same speed and so they do not have the same kinetic energy. The temperature of a gas is proportional to the average kinetic energy of the gas particles.

The Kinetic Molecular Theory (KMT)  applies specifically to a model of a gas called an ideal gas.  An ideal gas is an imaginary gas whose behavior perfectly fits all the assumptions of the kinetic-molecular theory. In reality, gases are not ideal, but are very close to being so under most everyday conditions.

 

Example of assumption #3 of KMT:   Gas particles are in random straight-line motion according to the kinetic-molecular theory. The space between particles is very large compared to the particle size.