Kinetic theory of gases

• The kinetic theory of gases?states that molecules in gases are constantly moving
• The theory makes the following assumptions:
  • The gas molecules are moving very fast and randomly
  • The molecules hardly have any volume
  • The gas molecules do not attract or repel each other (no?intermolecular forces)
  • No kinetic energy is lost when the gas molecules collide with each other (elastic collisions)
  • The temperature of the gas is related to the average kinetic energy of the molecules
• Gases that follow the kinetic theory of gases are called?ideal gases
• However, in reality gases do not fit this description exactly?but?may come very close and are called?real gases

Ideal gases

• The volume that an ideal gas occupies depends on:
  • Its pressure
  • Its temperature
  • See section?Changing gas volume?of page?Gas Pressure

• When a gas is?heated?(at constant pressure) the particles gain more?kinetic energy?and undergo more?frequent collisions?with the container wall
• To keep the?pressure constant, the molecules must get further apart and therefore the?volume increases
• The?volume?is therefore?directly proportional?to the?temperature?(at constant pressure)

The volume of a gas increases upon heating to keep a constant pressure (a); volume is directly proportional to the pressure (b)

Limitations of the ideal gas law

• At very?high pressures?and?low temperatures?real gases do not obey the kinetic theory as under these conditions:
  • Molecules are close to each other
  • There are instantaneous dipole- induced dipole or permanent dipole- permanent dipole forces between the molecules
  • These attractive forces pull the molecules away from the container wall
  • The volume of the molecules is not negligible
• Real gases therefore do not obey the following kinetic theory?assumptions?at high temperatures and pressures:
  • There is zero attraction between molecules (due to attractive forces, the?pressure?is?lower?than expected for an ideal gas)
  • The volume of the gas molecules can be ignored (volume?of the gas is?smaller?than expected for an ideal gas)

Ideal gas equation

• The?ideal gas equation?shows the relationship between pressure, volume, temperature and number of moles of gas of an ideal gas:

pV = nRT

p = pressure (pascals, Pa)

V = volume (m³)

n = number of moles of gas (mol)

R = gas constant (8.31 J K^-1?mol^-1)

T = temperature (kelvin, K)

• The ideal gas equation can also be used to calculate the?molar?mass?(Mr) of a gas

Worked example: Calculating the volume of a gas

Answer

• Step 1:?Rearrange the ideal gas equation to find volume of gas

• Step 2:?Calculate the volume the oxygen gas occupies

p = 220 kPa = 220 000 Pa

n = 0.781 mol

R = 8.31 J K^-1?mol^-1

T = 21^oC = 294 K

= 0.00867 m³

= 8.67 dm³

Worked example: Calculating the molar mass of a gas

Answer

• Step 1:?Rearrange the ideal gas equation to find the number of moles of gas

• Step 2:?Calculate the number of moles of gas

p = 300 kPa = 300 000 Pa

V = 1000 cm³?= 0.001 m³

R = 8.31 J K-1?mol^-1

T = 23?^oC = 296 K

• Step 3:?Calculate the molar mass using the number of moles of gas