Gas Laws

• 1. Gases consist of large number of particles that are far apart relative to their sizes. That means that gases have volume based on their movement...not their particle size.
  2. Collisons between gas particles and between particles and container walls are elastic collisions

  3. gas particles are in continuous, rapid, and random motion
  4. there are no forces of attraction or repulsion between gas particles
  5. the average kinetic energy of gas particles depends on the temperature of gases
• • elastic collisions there is no net loss of kinetic energy
  • energy is just transferred between the particles but is not converted to other type of energy
• Ideal gases have

  • no intermolecular forces
  • have elastic collisions
  • no volume so are infinitely compressible
• Gases will act Ideal if they are:

  • non polar (no attractive/repulsive forces)
  • high temps low pressure
• Standard pressure

  1.0 atm = 101.3 kPa = 760 mmHg = 760 torr
• more collisions = more pressure

  less collisions = less pressure
• Boyle: pressure and volume are inversely related and temperature remains constant

  P1 V1 = P2 V2
• Charles: Volume and temperature are directly related and pressure remains constant

  V1 = V2

  T1 = T2
• Gay Lussac: Presure and temperature are directly related and volume remains constant

  P1 = P2

  T1 = T2