1. Mole-Mass and Mole-Volume Relationships

2. The Mole-Mass Relationship
To convert the mass of a substance to the number of moles of the substance you have to use the molar mass of an element or compound.
Mass = # of moles x (mass/1mole)

3. The Mole-Mass Relationship
EX: the molar mass of NaCl is 58.5 g/mol, so the mass of 3.00 mol NaCl is calculated:
Mass of NaCl = 3 mol x (58.5 g/1 mol)
= 176 g
When you measure 176 g of NaCl on a balance, you are measuring 3.00 moles of NaCl.

4. The Mole-Mass Relationship Practice
What is the mass of 9.45 mol of aluminum oxide (Al2O3)?
First add up all the masses
Al = 27g x 2 = 54g
O = 16g x 3 = 48g
Al2O3 = 102 g
Then convert from moles to grams:
9.45 mol Al2O3 x (102g/1 mol Al2O3) = 963.9g

5. The Mole-Mass Relationship Practice
16. Find the mass, in grams, of 4.52 x 10-3 mol C20H42.

6. The Mole-Mass Relationship Practice
17. calculate the mass, in grams, of 2.50 mol of iron(II) hydroxide Fe(OH)2.

7. The Mole-Mass Relationship Practice
You can calculate the number of moles using the same relationship you use to find the mass of moles by inverting the conversion factor.
Moles = mass x (1mole/mass)

8. The Mole-Mass Relationship Practice
How many moles of iron(III) oxide are contained in 92.2 g of pure Fe2O3?
Fe2O3 = g = 1 mol
92.2 g Fe2O3 x (1 mol/159.6 g Fe2O3) = mol Fe2O3

9. The Mole-Mass Relationship Practice
18. Find the number of moles in 3.70 x 10-1 g boron.

10. The Mole-Mass Relationship Practice
19. Calculate the number of moles in 75.0 g of dinitrogen trioxide (N2O3)

11. The Mole-Volume Relationship
Avogadro’s hypothesis states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles.
Because of variations due to temperature and pressure, the volume of a gas is usually measured at a standard temperature and pressure.

12. The Mole-Volume Relationship
Standard temperature and pressure (STP) means a temperature of 0C and a pressure of kPa, or 1 atmosphere (atm).

13. The Mole-Volume Relationship
At STP, 1 mol or 6.02 x 1023 representative particles, of any gas occupies a volume of 22.4 L.
The quantity, 22.4 L, is called the molar volume of a gas.

14. The Mole-Volume Relationship
The molar volume is used to convert a known number of moles of gas to the volume of the gas at STP.
Volume of gas = moles of gas x (22.4L/1mol)

15. The Mole-Volume Relationship
Determine the volume, in liters, of 0.60 mol SO2 gas at STP.
1 mol SO2 = 22.4 L SO2
Volume = 0.60 mol SO2 x (22.4L/1mol)
= 13 L SO2

16. The Mole-Volume Relationship - Practice
20. What is the volume of these gases at STP?
A x 10-3 mol CO2
B mol N2

17. The Mole-Volume Relationship - Practice
21. at STP, what volume do these gases occupy?
A mol He
B mol C2H6

18. Calculating Molar Mass from Density
Different gases have different densities. Density of a gas is measured in grams per liter (g/L) and at a specific temperature.
Molar mass = (grams/L) x (22.4 L/1 mole)

19. Calculating Molar Mass from Density
The density of a gaseous compound containing carbon and oxygen is found to be g/L at STP. What is the molar mass of the compound?
Molar mass = (1.964 g/L) x (22.4 L/1 mol)
= 44 g/mol

20. Calculating Molar Mass from Density - Practice
22. a gaseous compound has a density of 3.58 g/L at STP. What is the molar mass of this gas?

21. Calculating Molar Mass from Density
23. What is the density of krypton gas at STP?