B3

• pressure


  the force applied per unit area
• 3 assumptions of ideal gas

  • there is a very large number of particle, which allows statistical averages to be taken
  • the volume of each particle is negligible (small enough to be ignored) compared to the volume of the container
  • there are no intermolecular forces between the particles
• 4 assumptions of ideal gas

  • the particles move randomly in all directions at high speeds
  • collisions between particles and between particles and the walls of the container are perfectly elastic – kinetic energy is conserved
  • the duration of a collision is negligible compared to the time between collisions
  • the potential energy between particles is zero.
• an ideal gas is good approximations of real gases when the real gas:

  is at a high temperaure, a low pressure and low density
• avogadro's constant


  the number of particles in one mole of a substance
• Molar mass


  a total of the atomic masses of all atoms that are present in a given compound
• Avogadro’s constant


  the number of atoms or molecules in one mole of a substance, equal to 6.023 × 10^23
• atomic number



  number of protons
• mass number, atomic mass


  sum of protons and neutrons
• a mole


  One mole of a substance contains the same number of fundamental units as there are atoms in exactly 12.00 g of 12C
• Charles's law


  pressure is constant
• boyle's law


  temperature is constant
• Gay-Lussac's law


  volume is constant
• avogadro's law


  V1/n1 = V2/n2
• What is the main difference between real gases and ideal gases?

  Real gases have molecules with volume, intermolecular forces, and non-elastic collisions, whereas ideal gases do not.
• potential energy in the ideal gas is zero because there is no intermolecular forces between particles -- no intermolecular potential energy