1. The Mole Concept

2. Avogadro’s Number
Avogadro’s Number (symbol N) is the number of atoms in grams of carbon.
Its numerical value is 6.02 × 1023.
Therefore, a g sample of carbon contains 6.02 × 1023 carbon atoms.

3. 1 mol = Avogadro’s Number = 6.02 × 1023 units
The Mole
The mole (mol) is a unit of measure for an amount of a chemical substance.
A mole is Avogadro’s number of particles, that is 6.02 × 1023 particles.
1 mol = Avogadro’s Number = 6.02 × 1023 units
We can use the mole relationship to convert between the number of particles and the mass of a substance.

4. How Big Is a Mole?
The volume occupied by one mole of softballs would be about the size of the Earth.
One mole of Olympic shot put balls has about the same mass as the Earth.

5. Mole Calculations We will be using the Unit Analysis Method. Steps:
First we write down the unit asked for
Second we write down the given value
Third we apply unit factor(s) to convert the given units to the desired units

6. Mole Calculations I How many sodium atoms are in 0.120 mol Na?
Step 1: we want atoms of Na
Step 2: we have mol Na
Step 3: 1 mole Na = 6.02 × 1023 atoms Na
= 7.22 × 1022 atoms Na
0.120 mol Na ×
1 mol Na
6.02 × 1023 atoms Na

7. Mole Calculations I
How many moles of potassium are in 1.25 × 1021 atoms K?
Step 1: we want moles K
Step 2: we have 1.25 × 1021 atoms K
Step 3: 1 mole K = 6.02 × 1023 atoms K
= 2.08 × 10-3 mol K
1.25 × 1021 atoms K ×
1 mol K
6.02 × 1023 atoms K

8. Molar Mass
The atomic mass of any substance expressed in grams is the molar mass (MM) of that substance.
The atomic mass of iron is amu.
Therefore, the molar mass of iron is g/mol.
Since oxygen occurs naturally as a diatomic, O2, the molar mass of oxygen gas is 2 times g or g/mol.

9. Calculating Molar Mass
The molar mass of a substance is the sum of the molar masses of each element.
What is the molar mass of magnesium nitrate, Mg(NO3)2?
The sum of the atomic masses is:
( ) =
(62.01) = amu
The molar mass for Mg(NO3)2 is g/mol.

10. 6.02 × 1023 particles = 1 mol = molar mass
Mole Calculations II
Now we will use the molar mass of a compound to convert between grams of a substance and moles or particles of a substance.
6.02 × 1023 particles = 1 mol = molar mass
If we want to convert particles to mass, we must first convert particles to moles and than we can convert moles to mass.

11. Mass-Mole Calculations
What is the mass of 1.33 moles of titanium, Ti?
We want grams, we have 1.33 moles of titanium.
Use the molar mass of Ti: 1 mol Ti = g Ti
= 63.7 g Ti
1.33 mole Ti ×
47.88 g Ti
1 mole Ti

12. Mole Calculations II What is the mass of 2.55 × 1023 atoms of lead?
We want grams, we have atoms of lead.
Use Avogadro’s number and the molar mass of Pb
2.55 × 1023 atoms Pb ×
1 mol Pb
6.02×1023 atoms Pb
207.2 g Pb
1 mole Pb ×
= 87.8 g Pb

13. Mole Calculations II
How many O2 molecules are present in g of oxygen gas?
We want molecules O2, we have grams O2.
Use Avogadro’s number and the molar mass of O2
0.470 g O2 ×
1 mol O2
32.00 g O2
6.02×1023 molecules O2
1 mole O2 ×
8.84 × 1021 molecules O2

14. Gas Density The density of gases is much less than that of liquids.
We can calculate the density of any gas at STP easily.
The formula for gas density at STP is:
= density, g/L
molar mass in grams
molar volume in liters

15. Calculating Gas Density
What is the density of ammonia gas, NH3, at STP?
First we need the molar mass for ammonia;
(1.01) = g/mol
The molar volume NH3 at STP is 22.4 L/mol.
Density is mass/volume:
= g/L
17.04 g/mol
22.4 L/mol

16. Molar Mass of a Gas
We can also use molar volume to calculate the molar mass of an unknown gas.
1.96 g of an unknown gas occupies 1.00L at STP. What is the molar mass?
We want g/mol, we have g/L.
1.96 g
1.00 L
22.4 L
1 mole ×
= g/mol

17. Mole Unit Factors We now have three interpretations for the mole:
1 mol = 6.02 × 1023 particles
1 mol = molar mass
1 mol = 22.4 L at STP for a gas
This gives us 3 unit factors to use to convert between moles, particles, mass, and volume.

18. Mole-Volume Calculation
A sample of methane, CH4, occupies 4.50 L at STP. How many moles of methane are present?
We want moles, we have volume.
Use molar volume of a gas: 1 mol = 22.4 L
4.50 L CH4 ×
= mol CH4
1 mol CH4
22.4 L CH4

19. Mass-Volume Calculation
What is the mass of 3.36 L of ozone gas, O3, at STP?
We want mass O3, we have 3.36 L O3.
Convert volume to moles then moles to mass:
3.36 L O3 × ×
22.4 L O3
1 mol O3
48.00 g O3
= 7.20 g O3

20. Molecule-Volume Calculation
How many molecules of hydrogen gas, H2, occupy L at STP?
We want molecules H2, we have L H2.
Convert volume to moles and then moles to molecules:
0.500 L H2 ×
1 mol H2
22.4 L H2
6.02×1023 molecules H2
1 mole H2 ×
= 1.34 × 1022 molecules H2