Ideal Gas Laws

The kinetic theory explains gas behavior using particle motion. Gas particles are in constant rapid, random motion, colliding with each other and the container walls. These collisions create pressure.

An ideal gas is a theoretical model where particles occupy negligible volume, have perfectly elastic collisions, and experience no intermolecular forces. Real gases deviate from this at high pressures and low temperatures.

Boyle's Law states that pressure is inversely proportional to volume when temperature is constant. If you compress a gas (decrease volume), the pressure increases because particles hit the walls more frequently.

Charles's Law states that volume is directly proportional to absolute temperature when pressure is constant. Heating a gas makes particles move faster, so the gas expands to maintain constant pressure.

The combined gas law relates pressure, volume, and temperature when all three can change. Applications include understanding why car tire pressure increases on hot days (constant volume, higher temperature = higher pressure) and why weather balloons expand as they rise (lower atmospheric pressure = larger volume).