KINETIC THEORY OF MATTER AND GAS LAWS (PART 2)
The Kinetic Theory of Matter explains the behavior of matter in different states—solid, liquid, and gas—by considering the motion of its particles. According to this theory, matter is composed of tiny particles (atoms, molecules, or ions) that are in constant motion. In solids, particles vibrate in fixed positions, while in liquids, they move more freely, and in gases, the particles are widely spaced and move rapidly in all directions. This movement is influenced by factors such as temperature and pressure. The theory helps explain key properties of gases, such as pressure, volume, and temperature, and forms the foundation for the Gas Laws. The ideal gas laws, including Boyle’s Law (pressure inversely proportional to volume at constant temperature), Charles’s Law (volume directly proportional to temperature at constant pressure), and Avogadro’s Law (volume directly proportional to the number of molecules at constant temperature and pressure), describe how gases behave under varying conditions. These principles are fundamental in understanding gas behavior in both everyday life and scientific applications.