gas laws

• Real gases


  Deviate from ideal gases at low temperatures and at high pressure
• Explanation for real gases deviating from ideal gases at low temperatures

  1. Decrease in kinetic energy of molecules, particles move more slowly

  2. Particles are closer together (not so close that they repel)

  3. Attractive forces increase and could become so strong that the substance condenses
• Explanation for real gases deviating from ideal gases at high pressure

  1. Gas particles' own volume contributes to the total volume of the gas, therefore volume is larger

  2. Larger particles have stronger intermolecular forces and will show a smaller volume because the forces pull the particles closer to each other
• Liquefaction takes place when the gas experiences high pressure under critical temperature, which does not include all circumstances
• properties of Ideal gas

  • Particles are identical in every way
  • Ideal gas only occupies volume due to the movement of the gas particles, the particles themselves have no volume
  • No forces of attraction or repulsion between the particles
  • Collisions between particles are perfectly elastic
• Real gases


  Do not have the properties of an ideal gas
• At low pressure, gases with a large molecular mass (N2 and CO2)


  Have lower pV value, stronger intermolecular forces (London forces), causing molecules to be closer together, smaller volume than expected
• At high pressures, N2 and CO2


  Volume of the particles contributes to the total volume, volume is larger than expected
• At high pressures, H2 and He


  Small particles, therefore the attractive forces (London forces) are negligibly small, gas molecules move closer together, repulsive forces exist, volume is larger than expected
• At high pressure and low temperatures, real gases deviate from ideal gases
• Boyle's law


  The pressure of an enclosed mass of gas is inversely proportional to the volume of the gas provided the temperature remains constant
• The higher the temperature, the greater the volume for the same pressure
• The pressure exerted by Earth's atmosphere is known as atmospheric pressure, an increase in height causes air pressure to decrease
• ideal gas


  Hypothetical gas that obeys all the gas laws under all circumstances of temperature and pressure