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The Mole!
The Mole!
The Mole!
The Mole!
The Mole!
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The Mole!

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Presented by Sharon Williams in the ACT2strand at CAST 2010 in Houston, Texas.

Presented by Sharon Williams in the ACT2strand at CAST 2010 in Houston, Texas.

Published in: Education, Technology
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Transcript

  • 1.  
  • 2. Relating Mass to Numbers of Atoms
    • The Mole!
      • the amount of a substance that contains as many particles as there are atoms in exactly 12 g of carbon-12
      • or
      • the amount of a substance that contains Avogadro’s number of particles
  • 3. Avogadro’s Number
    • The number of particles in exactly one mole of a pure substance.
      • experimentally determined by Avogadro
      • 1 mole = 6.022 136 7 x 10 23 particles
      • analogous to 1 dozen of something
  • 4. Molar Mass
    • The mass of one mole of a pure substance.
      • Units are g/mol
      • Molar mass of an element is equal to the atomic mass of the element in amu.
        • Example:
          • 1 atom of carbon has a mass of 12.01 amu.
          • 1 mole of carbon atoms have a mass of 12.01 g/mol
      • Molar mass of a compound is calculated by adding the masses of all elements in the compound.
  • 5. Mole Conversions
    • If it’s the number of things you wonder, it’s time to use Avogadro’s number!
      • 1 mole = 6.022 x 10 23 things
      • (“things” can be atoms, molecules, ions, formulas units, etc.)
    • When you go from moles to mass, use the formula mass to pass!
      • 1 mole = formula mass in g
      • (find it on the periodic table or add it up)

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