The Gas State
In a gas, particles move fast and far apart, colliding elastically and exerting pressure on their container; Boyle's law and the ideal gas law (PV=nRT) describe how pressure, volume, temperature, and amount relate, from absolute zero upward.
At zero Kelvin, motion nearly stops completely Add heat, and every particle starts to jostle Warm it further, kinetic energy climbs higher Faster particles hit the walls with more force More force on the walls means more pressure inside Squeeze the same gas into a smaller space Boyle's law, pressure and volume trade evenly Double the pressure, the volume drops by half Particles fly straight until they strike something Elastic collisions, no energy lost in the bounce Room between particles stretches wide and thin A gas fills every corner of its container No fixed shape, no fixed volume, particles roam free PV equals nRT, the ideal gas law ties it together Pressure, volume, moles, and temperature, four numbers linked Helium, oxygen, steam, every gas obeys the same rules Cool it back down, the particles slow again One state, countless gases, one set of laws
Key Concepts: Gas particles move fast, far apart, and collide elastically, exerting pressure on their container | Boyle's law (pressure and volume trade inversely at constant temperature) and the ideal gas law (PV=nRT) describe real, testable relationships | Kinetic energy rises with temperature, starting from absolute zero (0 Kelvin) | No fixed shape or volume; a gas fills its container | Companion to "I'm Aiery"
Key Words: kinetic energy, elastic collision, pressure, Boyle's law, ideal gas law, absolute zero