the gas phase

pressure volume relationship (inversely related)

PV=K; boyles law

v/t = b (directly related)

Charles law

v/n= a (directly related)

avogadro’s law

PV=nRT

ideal gas law

van der waals equation is useful for non-ideal gasses at

low temperatures and high pressures

absolute zero

the temperature at which all movement of all particles stop; 0 K/ -273 C

STP

1 mole of any ideal gas take up 22L of space

The universal gas constant (R)

8 LKPa/ Kmol

kinetic molecular energy of gases

KE = .5mv²

Average kinetic energy of gases

KE avg = 1.5 RT

Ideal gas rules

gas particles have no volume, no attractive or repulsive forces; high temperature and high volume, low pressure are ideal conditions for an ideal gas to behave ideally

graham’s law

when gas escapes, smaller particles escape first and faster

Under normal conditions like STP, real gases have

a slightly smaller but almost same pressure when compared to an ideal gas

Under extreme pressure or low temperature, real gasses have

a higher pressure when compared to an ideal gas at extreme pressures & lower pressure (compared to ideal gases) at low temperatures

PV/RT ratio = 1 with one mole of gas but if > 1

the system is in extreme conditions and results in higher pressures due to more elastic collisions against the container walls