GASES

• Kinetic energy is measured in joules (J)
• Assumptions of the kinetic molecular theorem:

  • The molecules of gases are far apart from one another.
  • The molecules of a gas are always in constant random motion, frequently colliding with one another. These collisions are perfectly elastic
  • The particles of an ideal gas exert no attractive forces on one another or on their surroundings
  • The average kinetic energy of gas molecule depends on the absolute temperature of the gas
• Volume is the space occupied by matter
• Temperature is the amount of kinetic energy the particle have
• 1 atm = 760 mmHg = 760 torr = 101.325 kPa
• Pressure is the amount of force applied per unit area
• The Kinetic Molecular Theory explains how gases behave at a molecular level
• It is one in which intermolecular forces are negligible and gas molecules occupy a negligible volume.

  Ideal gas
• It behaves almost as an ideal gases at ordinary temperatures and pressures.

  Real gases