The kinetic molecular theory is a model that explains the behavior of gases based on the motion and interactions of their individual particles. Consider the following statements: A. Gas particles are in constant, random motion. B. The average kinetic energy of a gas is proportional to the pressure exerted by the gas. C. The volume of the individual gas particles is negligible compared to the volume of the container. Which statements are true according to the kinetic molecular theory? Choose 1 answer: A A only D Aand B C Aand C D A, B, and C

The correct answer is C: A and C.<br /><br />According to the kinetic molecular theory:<br /><br />A. Gas particles are in constant, random motion. - This statement is true. The theory states that gas particles move continuously and randomly.<br /><br />B. The average kinetic energy of a gas is proportional to the pressure exerted by the gas. - This statement is not true according to the kinetic molecular theory. The average kinetic energy of a gas is proportional to the temperature of the gas, not the pressure.<br /><br />C. The volume of the individual gas particles is negligible compared to the volume of the container. - This statement is true. The theory assumes that the size of the gas particles is so small compared to the distances between them that their volume can be considered negligible.