# Chem.ch11.exam3

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1. 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).
2. 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
3. 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)
4. What is Boyle's Law?
The pressure and the volume of a gas are inversly proportional to each other, temperature kept constant.
5. What's Charle's Law?
The temperature and the volume of a gas are directly proportional, assuming pressure is kept constant.
 Author: xiongav ID: 114529 Card Set: Chem.ch11.exam3 Updated: 2011-11-05T03:21:55Z Folders: Description: Chem.ch11.exam3 Show Answers: