Unit 5  Part 7    Moles  Grams And  Liters
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Unit 5 Part 7 Moles Grams And Liters

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Unit 5  Part 7    Moles  Grams And  Liters Unit 5 Part 7 Moles Grams And Liters Presentation Transcript

  • Part 7 – Moles into Grams and Liters
  • WEIGHING (MASSING) IN CHEMISTRY
    • Chemists use mass, and normally small masses such as grams.
    • However they must relate the mass of chemical back to the counting of individual atoms.
  • The Gram Atomic Mass (GAM)
    • gram atomic mass- the mass of one mole of an element.
    • The gram atomic mass numerically equals the atomic mass of the element in grams.
  • Example:
    • Find the gram atomic mass of the following elements:
      • Na, Hg, Fe, S
  • Gram Formula Mass (GFM)
    • gram formula mass- the mass of one mole of a compound.
    • For gram formula mass we add together the gram atomic masses of the elements which make up the compound.
  • Example
    • Find the gram formula mass of the following compounds:
      • CoCl 2 , H 2 O, H 2 S0 4
    • Name these compounds.
  • Converting between moles and grams of a substance.
    • Conversions between moles and the mass of a substance uses the gram atomic mass or gram formula mass.
  • To convert from moles to grams
    • 1. Find the gram formula mass of the compound or element your looking for.
    • 2. Determine the number of moles you were given.
    • 3. Multiply the number of moles by the gram formula mass.
  • Example
    • Find the mass of 0.160 mol H 2 O 2 .
    • Find the mass of 6.0 X 10 26 atoms of Be.
  • To convert from grams to moles
    • 1. Find the gram formula mass of the compound you are looking for.
    • 2. Determine the number of grams you were given.
    • 3. Divide the number of grams you were given by the gram formula mass.
  • Example
    • Find the number of moles in each of the following:
      • 333g SnF 2 .
      • 5.0 X 10 24 molecules of SnF 2 .
  • Try these on you own...
    • Find the mass in each of the quantities below
      • 10.0 mol Cr
      • 3.32 mol K
      • 2.4 mol N 2
    • Find the number of moles in each of the quantities below
      • 10g H 2 O 2
      • 15g Ca(NO 3 ) 2
      • 50g C 20 H 42
  • FINDING VOLUME IN CHEMISTRY
  • The Volume of a mole of gas
    • Although the volumes of 1 mol of a liquid or solid can vary greatly between different substances, the volume of 1 mol of the gas of any substance has the same volume, at equal temperature and pressure.
    • 1 mole of a gas of any substance occupies a volume of 22.4L at STP (standard temperature and pressure).
  • Standard Temperature and Pressure (STP)
    • Temperature and pressure can affect the volume of a gas.
    • In order to “standardize” experiments between scientist, we use a standard set of values to work with gases.
    • Standard Temperature = 0°C
    • Standard Pressure = 1 atm (air pressure at sea level)
  • Examples
    • Determine the volume, in liters, of 0.600 mol of SO 2 gas at STP.
  • Your turn…
    • What is the volume at STP of 0.960 mol CH4?
    • Assuming STP, how many moles are in 89.6 L SO 2 ?
  • Converting between units with moles
    • The mole is the most useful way for chemists to express the amount of matter.
  • Try these...
    • Determine the volume in liters of 50g of SO 2 gas at STP.