Note: k = a constant
Boyle’s Law: the pressure of a fixed mass of gas is inversely proportional the volume provided the temperature is constant.
p µ 1/V
p = k / V
pV = constant
Charle’s Law: the volume of a fixed mass of gas is directly proportional to its temperature in Kelvin, provided the pressure remains constant.
V µ T
V = kT
Pressure Law: the pressure of a fixed mass of gas is directly proportional to the temperature in Kelvin, provided the volume remains constant.
P µ T
p = kT
Ideal Gas equation: combining the above laws gives this equation.
pV=nRT
p=pressure in Nm-3 or Pascals; V=volume in m3; n= number of moles of gas; R= gas constant, 8.314 J K-1 mol-1; T=temperature in Kelvin.
Assumptions made when using the Ideal Gas Equation:
- Pressure is the result of molecules colliding with the walls of the container.
- Collisions between molecules are perfectly elastic (kinetic energy remains constant).
- Intermolecular forces are negligible.
- The actual volume of gas molecules is negligible compared to the volume of the container.
- The average kinetic energy of the gas molecules is proportional to the temperature in Kelvin. (K.E.=G kT)
Boltzmann constant: Basically, the gas constant for 1 molecule of gas
L = R/NA
L= Boltzmann constant, R=gas constant, NA=Avogadro constant.
