Introduction to Gases
Refers to a gas that exactly obeys the assumptions of the kinetic theory
ideal gas
The pressure of a gas at STP
100 kPa
The name for the process of mixing molecules of one substance through another substance by random molecular motion
diffusion
P1V1 = P2V2
Boyle's Law
SI unit of pressure
pascal
This has a value of 8.314 L x kPa / (K x mol)
gas constant R
A relation in which the value of one variable depends on the reciprocal of another variable
inverse proportion
V1/n1 = V2/n2
Avogadro's Law
A compact and rugged instrument that senses pressure using a flexible, airtight metal box
aneroid barometer
PV = nRT
ideal gas law
This law states that the rate of diffusion is inversely proportional to the square root of molar mass
Graham's law of diffusion
V1/T1 = V2/T2
Charles's Law
The assumption that the kinetic energy of gas molecules is directly related to temperature best explains why the volume of a gas is affected by temperature is used with this theory
kinetic theory of matter
Gives relationship between volume and pressure at constant temperature
Boyle's Law
This equals the average atmospheric pressure at sea level
standard atmosphere (atm)
Ptotal = P1 + P2 + P3 ...
Dalton's law of partial pressures
A relation in which the value of one variable depends directly upon the value of another variable
direct proportion
Gives relationship between volume and temperature at constant pressure
Charles's Law
This law can be used to convert gas volume to moles and vice versa
ideal gas law
rate1/rate2 = (square root) M2/M1
Graham's law of diffusion