Molar Volume - PowerPoint

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					Molar Volume
• Gas pressure is a result of gas particles colliding
  with the walls of a container
• The unit for pressure is the pascal (Pa) and is
  equal to 1N/m2
• Normally pressure is reported in kilopascals
  (kPa) which is 1000Pa
• A non-rigid container (i.e. balloon) will change
  volume so that the atmospheric pressure outside
  the container is the same as the pressure inside
  the container
              Charles’s Law
• Explains the
  relationship between
  volume and
  temperature (if         V1 V2
  pressure is held
• States that the ratio   T1 T2
  between volume and
  temperature will be
                Boyle’s Law
• Explains the
  relationship between
  volume and pressure
  (if temperature is held
                            p1V1  p2V2
• States that the
  product of pressure
  and volume will be
              Ideal Gas Law
• Combines Charles’s
  and Boyle’s Law
  along with the mole
  concept to explain an
  ideal gas                pV  nRT
• Involves the ideal gas
  constant (R =
  8.314472 JK-1mol-1)
    Standard Temperature and
  Pressure and Standard Ambient
    Temperature and Pressure
• There are two standards that have been
  established for temperature and pressure:
  – STP – 273K and 101.3kPa
  – SATP – 298K and 100kPa
• These will be crucial when dealing with the
  concept of Molar Volume
            Molar Volume
• For each of the gases on the periodic table
  look up:
  – Their density (g/L)
  – Their molar mass (remember some are
    diatomic) (g/mol)
• Then calculate:
  – The volume one mole of gas would occupy
             Molar Volume
• The two commonly used values for Molar
  Volume are:
              VSTP  22.4L / mol
              VSATP  24.8L / mol
• The equation we will use to employ Molar
  Volume is:
         Practice Problems
• Page 73
  – Questions 38-43

• Section Review
  – Questions 1-6, Page 74

• Chapter Review
  – Page 75-77