1. The Mole

2. (We may buy a dozen eggs. A chemist may use a mole of carbon)
The Mole is...
A SI unit
A counting unit (like a dozen)
(We may buy a dozen eggs. A chemist may use a mole of carbon)
The amount of substance that contains as many particles as there are atoms in 12 g of carbon-12

3. Avogadro’s Number is… The number of particles (atoms) in a mole
6.022 x 1023
If everyone living worked to count the atoms in one mole, it would take 4 million years!
The mole can also be said to be the amount of substance that contains Avogadro’s number of particles.

4. Molar Mass is…
The mass of one mole of a substance
Written in g/mol
٭Molar mass is the same as the atomic mass number and is used as a conversion factor

5. Molar Mass Calculations
Divide by x 1023
molecules/mol
atoms/mol
particles/mol
Multiply by molar mass
g/mol
Atoms, molecules, or particles
Mass
grams
Moles
Multiply by x 1023
molecules/mol
atoms/mol
particles/mol
Divide by molar mass
g/mol

6. Got Mole Problems?
Call Avagadro!

7. Example # 1
What is the mass in g of 3.50 mol of Copper?

8. Example #2
A chemist produces 11.9 g of Al. How many moles of Al are produced?

9. Example #3
How many moles of Ag are in 3.01 x 1023 atoms of Ag?

10. Example #4
What is the mass in grams of 1.20 x 108 atoms of Cu?

11. In-class Practice Problems
What is the mass in g of 2.25 mol of Fe?
How many moles of Ca are in 5.00 g of Ca?
How many moles of Pb are in 1.50 x 1012 atoms Pb?
What is the mass in grams of 7.5 x 1015 atoms of Ni?