Test: Kinetic Molecular Theory of Gases - MCAT MCQ

According to the Kinetic Molecular Theory, gas molecules are in constant motion, moving in random directions and colliding with each other and the walls of the container.

The Kinetic Molecular Theory assumes that gas molecules do not have strong attractive forces between them. Instead, they only interact through collisions.

The average kinetic energy of gas molecules is directly proportional to the temperature of the gas, according to the Kinetic Molecular Theory.

According to the Kinetic Molecular Theory, the average speed of gas molecules is directly proportional to the temperature. Therefore, as the temperature decreases, the speed of gas molecules also decreases.

The pressure exerted by a gas is a result of the collisions between gas molecules and the walls of the container. According to the Kinetic Molecular Theory, the average kinetic energy of the gas molecules determines the magnitude of these collisions and thus the pressure.

According to the Kinetic Molecular Theory, increasing the temperature of a gas sample at constant volume will result in an increase in the average kinetic energy of the gas molecules, leading to more frequent and energetic collisions with the container walls, thus increasing the pressure.

According to the Kinetic Molecular Theory, gas molecules are assumed to have a negligible volume compared to the volume of the container. This assumption allows us to treat gases as point particles.

According to the Kinetic Molecular Theory, the average kinetic energy of gas molecules is directly proportional to the temperature. Therefore, doubling the temperature will result in quadrupling the average kinetic energy.

According to the Kinetic Molecular Theory, a gas behaves most ideally under conditions of low pressure and high temperature. At low pressures, gas molecules are far apart and experience fewer intermolecular forces. At high temperatures, gas molecules have higher kinetic energy and move more rapidly, reducing the effect of intermolecular forces.

According to the Kinetic Molecular Theory, at the same temperature, gas molecules with higher molar masses will have lower average velocities. This is because the kinetic energy is the same for all gas molecules at a given temperature, but lighter molecules will have higher speeds to compensate for their lower mass, while heavier molecules will have lower speeds.