Chem.ch11.exam3

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).

P = force/area; P = nRT / V

PSI: pounds/in2

1 atmosphere = 760 mm Hg = 760 torr = 14.7 psi

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)

The pressure and the volume of a gas are inversly proportional to each other, temperature kept constant.

The temperature and the volume of a gas are directly proportional, assuming pressure is kept constant.