1. Chapter 10: Chemical Quantities (Topic pre-viewed in lab)
Activities
In-class workshops calculation of molar mass (gram-formula mass)
Open-notes evaluations
Quizes and tests
Homework
Lab activities
Mole ratios lab – Qualitative Lab 5
Mole labs – Quantitative Labs 6 , 8, 9
Na2CO3 + CaCl2 yields CaCO3 and 2 NaCl
NaHCO3 and HCl yields CO2 + H2O + NaCl
Percent composition of water in a hydrate
The mole: A measurement of matter TB section 10.1 Mole-Mass and Mole-Volume relationships: TB section 10.2 Percent Composition and Chemical Formula TB section10.3

2. 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 term representative particle refers to the species present in a substance: usually atoms, molecules, or formula units.
The number of representative particles in a mole,  1023, is called Avogadro’s number.

3. 10.1
What is a Mole?

4. 10.2

5. 10.2

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

7. 10.3 Read the question CAREFULLY. What do you need to find? Hints:
How many molecules of propane are in one mole of propane?
How many atoms are there in one molecule of propane?

8. 10.3

9. 10.3

10. 10.3

11. for Sample Problem 10.3
Sample problem 10.3

12. 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 (use Periodic Table)
How is the atomic mass of an element related to the molar mass 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 (gram-formula mass).

13. 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?

14. 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?
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.

15. The Mass of a Mole of a Compound
10.1
The Mass of a Mole of a Compound
One SO3 molecule has a mass of 80.1 amu. Substitute the unit grams for atomic mass units. Thus 1 mol of SO3 has a mass of 80.1 g. One mole of SO3 molecules has a mass of 80.1 grams

16. 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?

17. 10.4

18. 10.1 Section Quiz.
10.1.

19. 10.1 Section Quiz.
2. A mole of hydrogen gas, H2(g), contains x 1023
molecules.
atoms.
amu.
grams.

20. 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.

21. 10.1 Section Quiz.
4. Calculate the molar mass of ammonium nitrate.
45.02 g
80.05 g
60.06 g
48.05 g