1. Chapter 10 “Chemical Quantities”
Yes, you will need a calculator for this chapter!

2. Section 10.1 Da Mole: A Measurement of Matter

3. How do we measure items?
Measure mass in grams.
Measure volume in liters.
Measure amount in MOLES.

4. We’re not talking about this kind of mole!
What is the mole?
We’re not talking about this kind of mole!

5. Moles (mol) It is an amount.
Defined as the number of carbon atoms in exactly 12 grams of carbon-12.
1 mole = 6.02 x of representative particles.
6.02 x 1023 is called: Avogadro’s number.
1 mole = 6.02 x 1023 = Avogadro’s number

6. Similar Words for amount
Dozen:
Mole:
1 dozen muffins = 12 muffins
1 mol muffins = x 1023 muffins
2 dozen puppies = 24 puppies
2 mol puppies = 1.2 x 1024 puppies
36 m&m stuffed donuts = 3 dozen donuts
2.4 x 1024 m&m stuffed donuts = 4 mol donuts

7. What are Representative Particles?
The smallest pieces of a substance:
Changes based on what we’re looking at
For a molecular compound: it is the molecule.
For an ionic compound: it is the formula unit (ex: NaCl, MgS).
For an element: it is the atom.
1 mol of CO2 molecules, 1 mol of NaCl formula units, and 1 mol of H atoms all equal 6.02 x 1023 of that thing.
Remember the 7 diatomic elements? (made of molecules)

8. Measuring Moles
The atomic mass on the PT is also the molar mass (g/mol) – mass (in grams) of 1 mole of that atom
= 16.0 g/mol
Since the mole is the number of atoms in 12 grams of carbon-12,
Gram atomic mass (GAM)- Equals the mass of 1 mole of an element in grams (from periodic table)
12.01 grams of C has the same number of pieces as 1.01 grams of H and grams of Fe.
We can write this as:
12.01 g C = 1 mole C
(this is also the molar mass)
(**Remember we can count things by weighing them.)

9. Find the Molar Mass (g/mol) of the following:
Nitrogen
Aluminum
Zinc
14.01 g/mol
26.98 g/mol
65.39 g/mol

10. What about compound mass?
In 1 mole of H2O, there are 2 moles of H atoms and 1 mole of O atoms
To find the mass of a compound:
Determine number of each element present
Multiply the number times their mass (from the periodic table)
Add them up for the total mass

11. Calculating Compound Mass
Calculate the mass of magnesium carbonate, MgCO3.
24.31 g/mol g/mol x (16.00 g/mol) =
84.32 g/mol MgCO3

12. Practice Problem: What is the mass of one mole of CH4?
1 mole of C = g/mol
4 mole of H x 1.01 g = 4.04g/mol
1 mole CH4 = = g/mol 12

13. Mole Practice 1 mol = particles 2.5 mol MgCl2 = ? particles MgCl2 =
x 1024 Fe particles = ? mol Fe
2.5 mol
6.02 x 1023 particles
1.5 x 1024 particles of MgCl2
1 mol
7.2 x 1024 particles
1 mol
12 mol Fe
6.02 x particles

14. Molar Mass Practice 47 g/mol 180 g/mol 4. Molar mass of BeF2 =
5. Molar mass of C6H12O6 =
Be = 9.0 g/mol
(19.0) =
47 g/mol
F = 19.0 g/mol
C = 12.0 g/mol
6(12.0) + 12(1.0) + 6(16.0) =
H = 1.0 g/mol
180 g/mol
O= 16.0 g/mol

15. Section 10.2 Mole-Mass and Mole-Volume Relationships

16. Use to make conversion factors from these.
Since Molar Mass is…
Number of grams in 1 mole.
grams per mole (g/mol)
Use to make conversion factors from these.
- Use molar mass to convert to grams or mols of a substance.

17. For example How many moles is 5.69 g of NaOH? =
How many grams in .53 mol of NaOH?
.142 mol NaOH 1
mol NaOH
5.69 g NaOH
40.0
g NaOH
40.0
g NaOH
21.2 g NaOH
.53 mol NaOH 1
mol NaOH 17

18. 28.1 grams C 1.000 mol Mg Practice Problems:
How much would 2.34 moles of carbon weigh?
How many moles of magnesium is g of Mg?
28.1 grams C
1.000 mol Mg

19. The Mole-Volume Relationship
Under different circumstances, gases can change.
Two things effect the volume of a gas:
a) Temperature and b) Pressure
**We need to compare all gases at the same temperature and pressure.

20. Standard Temperature and Pressure
abbreviated STP
0ºC (273K) and 1.0 atm pressure
At STP 1 mole of gas occupies L= molar volume
22.4 L/mol of any gas at STP 20

21. Practice Problems: = 0.253 mol O2
What is the volume of 4.59 mole of CO2 gas at STP?
How many moles is L of O2 at STP?
4.59 mol CO2
22.4 L CO2
= 103 L CO2
1 mol CO2
5.67 L O2
1 mol O2
= mol O2
22.4 L O2

22. 12.3 L CH4 22.4 L CH4 8.8 g CH4 1 mol CH4 16.0 g CH4 1 mol CH4
What is the volume of 8.8 g of CH4 gas at STP? =
22.4 L CH4
8.8 g CH4
1 mol CH4
16.0 g CH4
1 mol CH4
12.3 L CH4

23. Summary: These four items are all equal: a) 1 mole
b) molar mass (in grams/mol)
c) 6.02 x 1023 particles (atoms, molecules, or formula units)
d) 22.4 L of a gas at STP
**Thus, we can make conversion factors from them.

24. Avog. # Practice problems:
How many molecules of CO2 are in 4.6 moles of CO2?
How many moles of water is in 5.87 x molecules?
How many atoms of carbon are in moles of Carbon?
How many moles is 7.78 x 1024 formula units of MgCl2?
2.8 x 1024 molecules of CO2
mol H2O (or 9.75 x 10-2)
7.405 x 1023 atoms C
12.9 moles MgCl2

25. Mixed Practice Problems:
How many atoms of lithium is 1.0 g of Li?
How much would 3.45 x 1022 atoms of U weigh?
What is the volume of 10.0 g of CH4 gas at STP?
8.7 x 1022 atoms Li
13.6 g U
14.0 L CH4

26. Section 10.3 Percent Composition and Chemical Formulas

27. Percentage Composition
Percentage by mass of each element in a compound

28. Calculating Percent Composition of a Compound
Like all percent problems:
part whole
Find mass of each element (from the periodic table)
Next, divide by total mass of compound; then x 100
x 100 % = percent

29. Percentage Composition
Find the % composition of Cu2S.
g Cu
g Cu2S
%Cu =
 100 =
79.85% Cu
32.07 g S
g Cu2S
%S =
 100 =
20.15% S

30. Percentage Composition
Find the mass percentage of water in calcium chloride dihydrate, CaCl2•2H2O?
36.04 g g
%H2O =
 100 =
24.51%
H2O

31. Empirical Formula (EF)
Lowest whole number ratio of atoms in a compound
C2H6
simplify subscripts
CH3

32. Empirical Formula (EF)
Just find lowest whole number ratio
C6H12O6
CH4N
Formula is not just ratio of atoms, it is also ratio of moles.
In 1 mole of CO2 there is 1 mole of carbon and 2 moles of oxygen.
In one molecule of CO2 there is 1 atom of C and 2 atoms of O.
= CH2O
= this is already the lowest ratio.

33. Formulas (continued)
Formulas for ionic compounds are ALWAYS empirical (the lowest whole number ratio = cannot be reduced).
*Remember, we simplify beforehand
Examples:
NaCl
MgCl2
Al2(SO4)3
K2CO3

34. Formulas (continued)
Formulas for molecular compounds MIGHT be empirical (lowest whole number ratio).
Molecular:
H2O
C6H12O6
C12H22O11
(Correct formula)
Empirical:
H2O
CH2O
C12H22O11
(Lowest whole number ratio)

35. Formulas
Empirical Formula (EF) = lowest whole number ratio of elements in a compound.
Molecular Formula (MF) = the actual ratio of elements in a compound.
The two can be the same.
CH2 = C2H4 =
C3H6 = H2O =
H2O is also MF EF MF MF EF 35

36. Last extra practice slide
How many O atoms are in 5 mol of Al2O3?
How many Al atoms are in 5 mol of Al2O3?
mol O
6.02e23
atoms O
5 mol Al2O3 3 1
mol Al2O3 1
mol O
9.03e24 atoms O
5 mol Al2O3
2 mol Al
6.02e23 atoms Al
1 mol Al2O3
1 mol Al
6.02e24 atoms Al