1. Review: Molar Mass of Compounds
Ex. Molar mass of CaCl2
Avg. Atomic mass of Calcium = 40.08g
Avg. Atomic mass of Chlorine = 35.45g
Molar Mass of calcium chloride = (2) = _110.98______ g/mol CaCl2 20
Ca 
17 Cl 35.45

2. Practice Calculate the Molar Mass of calcium phosphate Formula =
Ca3(PO4)2
Masses elements:
Ca = 40.08g/mole
P = g/mole
O = g/mole
Molar Mass =
(40.08 g/mole)(3) + (30.97 g/mole)(2) + (16 g/mole)(8)
= g/mole

3. Mole Conversions Learning Target:
Understand how molar mass relates to the number of moles and particles of a substance.

4. Particles (atoms, Formula units, molecules)
Divide by 6.02 X 1023
Multiply by 6.02 X 1023
Moles
Multiply by molar mass from periodic table
Divide by molar mass from periodic table
Mass (grams)

5. 3.5 dozen roses = ?? Roses
2.5 mol roses = ?? Roses (use Avogadro's #)

6. Problem Type #1 – Moles to Mass
Find the mass of mol of magnesium bromide..
Find the molar mass of the compound:
Make the conversion:

7. Problem Type # 2– Mass to Moles
A bottle of copper (II) nitrate contains g of compound. How many moles of copper (II) nitrate are in the bottle?

8. Problem Type #3 – Moles to Particles
Determine the number of atoms that are in 0.78 mol of mercury.

9. Problem Type #4 – Particles to Moles
How many moles of zinc sulfate contain 5.40 x 1024 formula units?

10. Multi-step Mole Conversions
2.5 g Roses = ?? atoms of roses
Atomic mass of 1 Rose is 3.0 g/mol

11. Multi-step Practice
How many molecules are in 7.4 g of potassium phosphate?

12. Multi-step Practice
How many grams of sodium bicarbonate are in 1.8 x 1023 formula units?

13. Molar Volume
Definition: The volume of one mole of an ideal gas at standard conditions (STP) equal to 22.4 L.
STP = standard temperature and pressure which is 0ºC and 1 atmospheric pressure (760 mmHg)
1 mole gas at STP = 22.4 L

14. Particles (atoms, Formula units, molecules)
Divide by 6.02 X 1023
Multiply by 6.02 X 1023
Moles
Multiply by 22.4 L
Divide by 22.4 L
Volume (L)

15. Practice
A container with a volume of 563L contains how many moles of air at STP?
How many molecules of air?

16. Practice
A chemical reaction produced 0.78 mol of H2 gas. What volume will the gas occupy at STP?
How many molecules of H2?
How many atoms of hydrogen?