Home > Preview
The flashcards below were created by user
on FreezingBlue Flashcards.
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.
P = force/area; P = nRT / V
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.
What would you like to do?
Home > Flashcards > Print Preview