1. Chapter 8: The Mole – Part 1

2. What is Avogadro’s favorite saying from American History?

4. The thickness of one page in your chemistry textbook is about 0.0065 cm. How many meters is this?

5. What is the thickness of one page in your chemistry book in meters? 0.0065 cm cm 0.01 m = 0.000065 m

6. How many meters high would a stack of one mole of pages be?

7. 6.02 x 10 23 pages page 0.000065 m = 3.9 x 10 19 m

8. The distance to the moon is 380,000,000m. If you took your stack of papers from problem 6 and broke it down into smaller stacks, how many stacks of papers could you make from the earth to the moon?

9. 3.9 x 10 19 m The distance to the moon is 380,000,000m. If you took the 3.9 x 10 19 m stack of papers, how many stacks of papers could be made from the earth to the moon? 3.9 x 10 19 m 380,000,000 m stack = 1.0 x 10 11 stacks 1.0 x 10 11 stacks = 100,000,000,000 stacks

10. 1 mole of pages would be enough to build 100 billion stacks of paper to the moon.

11. The Mole A mole is Avogadro’s number of particles, that is 6.02 × 10 23 particles. 1 mol = Avogadro’s Number = 6.02 × 10 23 units

12. How Big is a Mole? Where would you need to go to see 1 mole of rice grains?

13. How Big is a Mole? 1 mole of rice grains is more than the number of rice grown since the beginning of time?

14. How Big is a Mole? The worlds fastest supercomputer can count the world’s population in ¼ second. How long would it take this computer to count to 1 mole?

15. How Big is a Mole? The worlds fastest supercomputer can count the world’s population in ¼ second. It would take this computer 1.9 million years to count to 1 mole?

16. How Big is a Mole? One mole of marbles would cover the entire Earth (oceans included) for a depth of three miles. One mole of $100 bills stacked one on top of another would reach from the Sun to Pluto and back 7.5 million times. It would take light 9500 years to travel from the bottom to the top of a stack of 1 mole of $100 bills.

17. How Big is a Mole? Where would you need to go to see 1 mole of water.

18. World’s Fastest Super Computer vs. Super Teacher

19. The Marble Contest

20. What is the mass in grams of 1 mole of water? 1.6606 x 10 -24 g/amu 1 mol H 2 O

21. What is the mass in grams of 1 mole of water? 1.6606 x 10 -24 g/amu 1 mol H 2 O mol H 2 O 6.02 x 10 23 H 2 O molecules

22. What is the mass in grams of 1 mole of water? 1.6606 x 10 -24 g/amu 1 mol H 2 O mol H 2 O 6.02 x 10 23 H 2 O molecules molecule H 2 O 18.0 amu

23. What is the mass in grams of 1 mole of water? 1.6606 x 10 -24 g/amu 1 mol H 2 O mol H 2 O 6.02 x 10 23 H 2 O molecules molecule H 2 O 18.0 amu amu 1.6606 x 10 -24 g

24. What is the mass in grams of 1 mole of water? 1.6606 x 10 -24 g/amu 1 mol H 2 O mol H 2 O 6.02 x 10 23 H 2 O molecules molecule H 2 O 18.0 amu amu 1.6606 x 10 -24 g = 18.0 g

26. 1 mol H 2 O = 18.0g This is the gram formula mass of water. This is the molar mass of water. The gram formula mass (molar mass) is the molecular mass of the substance in grams.

27. What is the mass of 1 mol sucrose (C 12 H 22 O 11 )

28. 1 mol sucrose (C 12 H 22 O 11 ) = 342.0g 12 x 12.0 = 144.0 22 x 1.0 = 22.0 11 x 16.0 = 176.0 gfm = 342.0 g

29. Why 6.02 x 10 23 Take the gram formula mass of any substance. Use the conversion factor 1.66 x 10 -24 g/amu. Determine the number of particles in 1 mole.

30. Why 6.02 x 10 23 Take the gram formula mass of any substance (example C = 12.0g/mol and H 2 O = 18.0g/mol). Use the conversion factor 1.66 x 10 -24 g/amu. Determine the number of particles in 1 mole. 12.0 g C1 amu C atom mol 1.66 x 10 -24 g12.0 amu = 6.02 x 10 23 C atoms/mol

31. Why 6.02 x 10 23 Take the gram formula mass of any substance (example C = 12.0g/mol and H 2 O = 18.0g/mol). Use the conversion factor 1.66 x 10 -24 g/amu. Determine the number of particles in 1 mole. 12.0 g C1 amu C atom mol 1.66 x 10 -24 g12.0 amu = 6.02 x 10 23 C atoms/mol 18.0 g H 2 O1 amu H 2 O molecules mol 1.66 x 10 -24 g 18.0 amu = 6.02 x 10 23 H 2 O molecules/mol

32. Why 6.02 x 10 23 Take the gram formula mass of any substance (example C = 12.0g/mol and H 2 O = 18.0g/mol). Use the conversion factor 1.66 x 10 -24 g/amu. Determine the number of particles in 1 mole. 12.0 g C1 amu C atom mol 1.66 x 10 -24 g12.0 amu = 6.02 x 10 23 C atoms/mol 18.0 g H 2 O1 amu H 2 O molecules mol 1.66 x 10 -24 g 18.0 amu = 6.02 x 10 23 H 2 O molecules/mol

33. Why 6.02 x 10 23 It turns out that whenever we take an amount of a substance equal to it’s formula mass in grams we will have 6.02 x 10 23 particles of that substance. This number was named Avogadro’s number and is called a mole. 12.0 g C1 amu C atom mol 1.66 x 10 -24 g12.0 amu = 6.02 x 10 23 C atoms/mol 18.0 g H 2 O1 amu H 2 O molecules mol 1.66 x 10 -24 g 18.0 amu = 6.02 x 10 23 H 2 O molecules/mol