Ideal Gas Law
PV=nRT
P
Pressure
V
Volume
n
Moles
R
Constant
T
Temperature
Boyle's Law
The volume of a fixed mass of gas varies inversely with the pressure at constant temperature PV=K P1V1 = P2V2
STP
0 degrees C and 1 atm
Charles's Law
The volume of a fixed mass of gas at constant pressure varies directly with Kelvin temperature V=kT V1 / T1 = V2 / T2
Gay-Lussac's Law
The pressure of a fixed mass of gas at constant volume varies directly with the Kelvin temperature P=kT P1 / T1 = P2 / T2
Combined Gas Law
expresses the relationship between pressure, volume, and temperature of a fixed amount of gas PV / T = k P1V1T2 = P2T2T1
Gay-Lussac's Law of Combining Volumes
at constant temperature and pressure, the volumes of gaseous reactants and products can be expressed as ratios of small whole numbers
Avogadro's Law
equal volumes of gases at the same temperature and pressure contain equal numbers of molecules V = kn V-volume k-constant n-amount of gas in moles
Standard Molar Volume of a Gas
the volume occupied by one mole of a gas at STP =22.414 L
Grahm's Law of Effusion
the rates of effustion of gases at the same temperature and pressure are inversely proportional to the square roots of their molar masses Rate of effusion of A / B = ?Mb / ?Ma
Kinetic-Molecular Theory
particles of matter are always in motion
Ideal Gas
a hypothetical gas that perfectly fits all the assumptions of the kinetic-molecular theory
Elastic Collision
a collision in which there is no net loss of total kinetic energy
diffusion
spontaneous mixing of the particles of two substances caused by their random motion
effusion
a process by which gas particles pass though a tiny opening
Real Gas
a gas that does not behave completely according to the assumptions of the kinetic-molecular theory
Millimeters of Mercury
mmHg 760 mmHg
atmosphere pressure
1 atm
Kilopascal
101.325kPa
Dalton's law of partial pressures
the total pressure of a gas mixture is the sum of the partial pressures of the component gases
partial pressure
the pressure of each gas in a mixture