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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
• The number of particles in exactly one mole of a pure substance.
• 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)