Which assumptions of the kinetic–molecular theory explain the behavior of gases described by Charles's law? Explain your answer.

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1. Charles's law states that the volume of a gas is directly proportional to its temperature when pressure is held constant. This can be expressed as V \propto T.
2. The kinetic-molecular theory of gases provides a framework to understand this behavior by making several key assumptions about gas particles.
3. One assumption is that gas particles are in constant, random motion. As temperature increases, the kinetic energy of the particles increases, causing them to move more rapidly.
4. Another assumption is that the volume of the gas particles themselves is negligible compared to the volume of the container. This means that the space between particles increases as they move faster, leading to an increase in volume.
5. Finally, the theory assumes that there are no intermolecular forces between gas particles. This allows the particles to expand freely and fill the container as temperature increases, consistent with Charles's law.

Key Concepts

Kinetic-Molecular Theory

The kinetic-molecular theory explains the behavior of gases based on the idea that gas particles are in constant, random motion. It posits that these particles collide elastically with each other and the walls of their container, leading to pressure. The theory also assumes that the volume of the gas particles themselves is negligible compared to the volume of the container, allowing for the simplification of gas behavior.

Charles's Law

Charles's law states that the volume of a gas is directly proportional to its temperature when pressure is held constant. This means that as the temperature of a gas increases, its volume also increases, provided the pressure does not change. This relationship is crucial for understanding how temperature affects gas behavior and is derived from the kinetic-molecular theory.

Temperature and Kinetic Energy

In the context of gases, temperature is a measure of the average kinetic energy of the gas particles. As temperature increases, the kinetic energy of the particles also increases, leading to more vigorous motion and greater collisions with the walls of the container. This increase in motion is what causes the volume of the gas to expand, as described by Charles's law.