1. 10.1
Measuring Matter
Measuring Matter
What are three methods for measuring the amount of something?

2. 10.1
Measuring Matter
You often measure the amount of something by one of three different methods—by count, by mass, and by volume.
You can buy items by different types of measurements, such as a count, a weight or mass, or a volume. Classifying Which of these common items are being sold by weight? By volume? By count?

3. 10.1

4. for Sample Problem 10.1

5. 10.1
What is a Mole?
What Is a Mole?
How is Avogadro’s number related to a mole of any substance?

6. 10.1
What is a Mole?
A mole of any substance contains Avogadro’s number of representative particles, or 6.02  1023 representative particles.
The term representative particle refers to the species present in a substance: usually atoms, molecules, or formula units.

7. Converting Number of Particles to Moles
10.1
What is a Mole?
Converting Number of Particles to Moles
One mole (mol) of a substance is 6.02  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  1023, is called Avogadro’s number.

8. 10.1
What is a Mole?

9. 10.2

10. for Sample Problem 10.2
Sample problem 10.2

11. Converting Moles to Number of Particles
10.1
What is a Mole?
Converting Moles to Number of Particles

12. 10.3

13. for Sample Problem 10.3
Sample problem 10.3

14. The Mass of a Mole of an Element
10.1
The Mass of a Mole of an Element
The Mass of a Mole of an Element
How is the atomic mass of an element related to the molar mass of an element?

15. The Mass of a Mole of an Element
10.1
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.

16. The Mass of a Mole of an Element
10.1
The Mass of a Mole of an Element
One molar mass of carbon, sulfur, mercury, and iron are shown.
One molar mass of carbon, sulfur, mercury, and iron are shown. Each of the quantities contains one mole of the element. Applying Concepts How many atoms of each element are shown?

17. The Mass of a Mole of a Compound
10.1
The Mass of a Mole of a Compound
The Mass of a Mole of a Compound
How is the mass of a mole of a compound calculated?

18. The Mass of a Mole of a Compound
10.1
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.

19. The Mass of a Mole of a Compound
10.1
The Mass of a Mole of a Compound
Substitute the unit grams for atomic mass units. Thus 1 mol of SO3 has a mass of 80.1 g.

20. The Mass of a Mole of a Compound
10.1
The Mass of a Mole of a Compound
Molar Masses of Glucose, Water, and Paradichlorobenzene
One molar mass is shown for each of three molecular compounds. Inferring How can you know that each sample contains Avogadro’s number of molecules?

21. 10.4

22. 10.4

23. for Sample Problem 10.4

24. 10.1 Section Quiz.
1. Three common ways of measuring the amount of something are by count, by mass, and
by temperature.
by volume.
by area.
by density.

25. 10.1 Section Quiz.
2. A mole of hydrogen gas, H2(g), contains x 1023
molecules.
atoms.
amu.
grams.

26. 10.1 Section Quiz.
3. The atomic mass of fluorine is 19.0 amu, so the molar mass is
19.0 amu.
19.0 g.
6.02 x 1023 amu.
6.02 x 1023 g.

27. 10.1 Section Quiz.
4. Calculate the molar mass of ammonium nitrate.
45.02 g
80.05 g
60.06 g
48.05 g

28. END OF SHOW