1. © Copyright Pearson Prentice Hall Slide 1 of 43 The Mole: A Measurement of Matter You could measure the amount of sand in a sand sculpture by counting each grain of sand, but it would be much easier to weigh the sand. You’ll discover how chemists measure the amount of a substance using a unit called a mole, which relates the number of particles to the mass. 10.1

2. © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > Slide 2 of 43 Measuring Matter What are three methods for measuring the amount of something? 10.1

3. Slide 3 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > Measuring Matter You often measure the amount of something by one of three different methods—by count, by mass, and by volume. 10.1

4. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 4 of 43 10.1

5. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 5 of 43 10.1

6. © Copyright Pearson Prentice Hall Slide 6 of 43 Practice Problems for Sample Problem 10.1 Problem Solving 10.1 Solve Problem 1 with the help of an interactive guided tutorial.

7. © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > Slide 7 of 43 What is a Mole? What Is a Mole? How is Avogadro’s number related to a mole of any substance? 10.1

8. Slide 8 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > What is a Mole? A mole of any substance contains Avogadro’s number of representative particles, or 6.02  10 23 representative particles. The term representative particle refers to the species present in a substance: usually atoms, molecules, or formula units. 10.1

9. Slide 9 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > What is a Mole? Converting Number of Particles to Moles One mole (mol) of a substance is 6.02  10 23 representative particles of that substance and is the SI unit for measuring the amount of a substance. The number of representative particles in a mole, 6.02  10 23, is called Avogadro’s number. 10.1

10. Slide 10 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > What is a Mole? 10.1

11. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 11 of 43 10.2

12. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 12 of 43 10.2

13. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 13 of 43 10.2

14. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 14 of 43 10.2

15. © Copyright Pearson Prentice Hall Slide 15 of 43 Practice Problems for Sample Problem 10.2 Problem Solving 10.4 Solve Problem 4 with the help of an interactive guided tutorial.

16. Slide 16 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > What is a Mole? Converting Moles to Number of Particles 10.1

17. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 17 of 43 10.3

18. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 18 of 43 10.3

19. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 19 of 43 10.3

20. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 20 of 43 10.3

21. © Copyright Pearson Prentice Hall Slide 21 of 43 Practice Problems for Sample Problem 10.3 Problem Solving 10.5 Solve Problem 5 with the help of an interactive guided tutorial.

22. © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > Slide 22 of 43 The Mass of a Mole of an Element How is the atomic mass of an element related to the molar mass of an element? 10.1

23. Slide 23 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > The Mass of a Mole of an Element The atomic mass of an element expressed in grams is the mass of a mole of the element. The mass of a mole of an element is its molar mass. 10.1

24. Slide 24 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > The Mass of a Mole of an Element One molar mass of carbon, sulfur, mercury, and iron are shown. 10.1

25. Slide 25 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > The Mass of a Mole of an Element 10.1

26. © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > Slide 26 of 43 The Mass of a Mole of a Compound How is the mass of a mole of a compound calculated? 10.1

27. © Copyright Pearson Prentice Hall Slide 27 of 43 The Mole: A Measurement of Matter > The Mass of a Mole of a Compound To calculate the molar mass of a compound, find the number of grams of each element in one mole of the compound. Then add the masses of the elements in the compound. 10.1

28. Slide 28 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > The Mass of a Mole of a Compound Substitute the unit grams for atomic mass units. Thus 1 mol of SO 3 has a mass of 80.1 g. 10.1

29. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 29 of 43 10.4

30. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 30 of 43 10.4

31. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 31 of 43 10.4

32. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 32 of 43 10.4

33. © Copyright Pearson Prentice Hall Slide 33 of 43 Practice Problems for Sample Problem 10.4 Problem Solving 10.7 Solve Problem 7 with the help of an interactive guided tutorial.

34. © Copyright Pearson Prentice Hall Slide 34 of 43 10.1 Section Quiz. 1. Three common ways of measuring the amount of something are by count, by mass, and a.by temperature. b.by volume. c.by area. d.by density.

35. © Copyright Pearson Prentice Hall Slide 35 of 43 10.1 Section Quiz. 2. A mole of hydrogen gas, H 2 (g), contains 6.02 x 10 23 a.molecules. b.atoms. c.amu. d.grams.

36. © Copyright Pearson Prentice Hall Slide 36 of 43 10.1 Section Quiz. 3. The atomic mass of fluorine is 19.0 amu, so the molar mass is a.19.0 amu. b.19.0 g. c.6.02 x 10 23 amu. d.6.02 x 10 23 g.

37. © Copyright Pearson Prentice Hall Slide 37 of 43 10.1 Section Quiz. 4. Calculate the molar mass of ammonium nitrate. a.45.02 g b.80.05 g c.60.06 g d.48.05 g