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KMT: Kinetic Moleculer Theory (main points)
1) Gas particles/atoms are in constant motion.
2) Gas particles don't interact.
3) Particle volume is tiny compared to the container volume in a gas.
4) The kinetic energy of the gas particles is proportional to the temperature (in units of K, kelvin).

Pressure & Units. Formulas.
PSI
1 atmosphere
P = force/area; P = nRT / V
PSI: pounds/in2
1 atmosphere = 760 mm Hg = 760 torr = 14.7 psi

Ideal Gas Law.
Developed over time between P and T and V.
PV = nRT
 P=pressure (units of atmospheres)
 V=volume (of liters, L)
 n=# of moles of gas (can be CO2, Ar, etc.)
 *You can predict the r'ship between PVT, as long as it's a gas
 R=gas constant (always this value: .0821 L x atm / mol x K
 T=temperature (units of K, kelvin)

What is Boyle's Law?
The pressure and the volume of a gas are inversly proportional to each other, temperature kept constant.

What's Charle's Law?
The temperature and the volume of a gas are directly proportional, assuming pressure is kept constant.

