The kinetic molecular theory states that gas particles: Have strong intermolecular forces Are significantly affected by gravity. Vibrate around fixed points. Move in random straight-line motions.

## Step 1<br />The kinetic molecular theory is a fundamental concept in the study of gases. It provides a microscopic explanation for the macroscopic properties of gases. The theory assumes that gases consist of a large number of particles (atoms or molecules) that are in constant, random motion. <br /><br />## Step 2<br />The theory also assumes that the volume of the individual gas particles is negligible compared to the total volume of the gas. This means that the particles are not fixed in place but can move freely.<br /><br />## Step 3<br />The theory also assumes that there are no attractive or repulsive forces between the particles, except during collisions. This means that the particles do not have strong intermolecular forces.<br /><br />## Step 4<br />The theory also assumes that the collisions between the particles are perfectly elastic, meaning that there is no net loss of kinetic energy. This means that the particles do not lose energy during collisions.<br /><br />## Step 5<br />The theory also assumes that the average kinetic energy of the particles is proportional to the temperature of the gas. This means that the particles move faster at higher temperatures.<br /><br />## Step 6<br />Based on these assumptions, the statement that "move in random straight-line motions" is the most accurate description of the behavior of gas particles according to the kinetic molecular theory.