Kinetic Molecular Theory

• Gas particles move in random and straight line motion.
• Gas has greater kinetic energy due to gases existing at higher temperatures
• As temperature increases, particles move faster and, thus, have greater kinetic energy
• Gases are composed of molecules


  The distance of molecules is far greater than its dimension
• Molecules collide elastically with container walls and one another


  Energy may transfer from one molecule to another as the result of collision, but the total energy in the system remains the same
• There are no attractive or repulsive forces between gas molecules
• The average kinetic of the molecules is directly related to the Kelvin temperature of gas
• Volume


  space occupied by the gases

  occupy all the spaces of the container that they are confined

  1 L = 1000 mL
• Pressure


  average effect of the forces of the colliding molecules

  1 atm = 760 mmHg = 101325 Pa
• Temperature

  measure of the hotness or coldness of an object

  proportional to the average kinetic energy of its molecules

  + 273 K

  1.8 * (C) + 32