1. The Mole
Chemistry

2. What is a Mole?
A mole is a specified number of particles X 1023 particles, to be exact This number is Avogadro’s number.

3. How Large is this Number?
A mole of paper clips (3 cm long) chained together would wrap around the equator 450 trillion times.

4. How Large is this Number?
A mole of cantaloupes (6 inches in diameter) has the same volume as Earth (1.1 x 1012 km3).

5. How Large is this Number?
A mole of pennies distributed evenly to everyone in the world (7 billion people) would enable each person to spend $1.6 million per minute for an entire year.

6. How Large is this Number?
A mole of coffee stirrers (3 cm x 6 mm) would cover the contiguous U.S. coast to coast, border to border, and pile about 40 miles high.

7. A Mole is the Number of Particles. 1 mole of C has 6
****A Mole is the Number of Particles**** 1 mole of C has 6.02 X 1023 particles 1 mole of CO has 6.02 X 1023 particles 1 mole of C02 has 6.02 X 1023 particles So when we write: 2 CO, we mean 2 moles of carbon monoxide 2 CO2, we mean 2 moles of carbon dioxide

8. How many moles of each product/reactant?
2Mg + O2 → 2MgO
Ca(OH)2 + 2HCl → CaCl2 + 2H2O
N2 + 3H2 → 2NH3
2Li + Br2 → 2LiBr

9. Conversions with Moles
So for equations (and dimensional analysis), you can ALWAYS make the conversion factor of: 1 mole of element or compound 6.02 X 1023 atoms or molecules Or

10. Example: How many atoms are in 2.12 mol of C3H8? Knowns: 2.12 mol C3H8
1 mol C3H8 = 6.02 X 1023 molecules C3H8
11 atoms X 1023 molecules C3H mol C3H8 =
1 molecule C3H8 1 mol C3H8
= 1.40 X 1025 atoms

11. Mass of a Mole of a Compound
The molar mass of any compound is the mass in grams of 1 mol of that compound. So you can read the periodic table as the atomic mass = mass in g/mol. What is the molar mass of N? O? So what is the molar mass of N2O?