1. Mass Relationships in Chemical Reactions
Chapter 3

2. Average atomic mass of lithium:
Natural lithium is:
7.42% 6Li (6.015 amu)
92.58% 7Li (7.016 amu)
Average atomic mass of lithium:
100
= _______ amu
3.1

3. Dozen = 12 Pair = 2 The mole (mol) is the amount of a substance that
contains as many elementary entities as there
are atoms in exactly ______ grams of 12C
1 mol = NA =____________________
___________________ number (NA)
3.2

4. Molar mass is the mass of 1 mole of in grams marbles atoms
eggs
shoes
Molar mass is the mass of 1 mole of in grams
marbles
atoms
1 mole 12C atoms = ____________ atoms = ______ g
1 12C atom = amu
1 mole 12C atoms = ___________ g 12C
1 mole lithium atoms = ___________ g of Li
For any element
___________ (amu) = __________ (grams)
3.2

5. One Mole of: S C Hg Cu Fe
3.2

6. _____ g = ________________ amu
1 amu = ______________ g M
= molar mass in g/mol
NA = Avogadro’s number
3.2

7. Do You Understand Molar Mass?
How many atoms are in g of potassium (K) ?
3.2

8. Molecular mass (or molecular weight) is the sum of
the atomic masses (in amu) in a molecule.
SO2 1S
amu 2O
amu
SO2
amu
For any molecule
________ mass (amu) = ______ (grams)
1 molecule SO2 = _________ amu
1 mole SO2 = ________ g SO2
3.3

9. Do You Understand Molecular Mass?
How many H atoms are in 72.5 g of C3H8O ?
3.3

10. Percent composition of an element in a compound =
n x molar mass of element
molar mass of compound
x 100%
n is the number of moles of the element in 1 mole of the compound
C2H6O
3.5

11. Types of Formulas ____________ Formula
The formula of a compound that expresses the _________________ ratio of the atoms present.
Ionic formula are always ____________ formula
_______ Formula
The formula that states the _____ number of each kind of atom found in _________ of the compound.

12. To obtain an Empirical Formula
1. Determine the _______________ of each element present, if necessary.
Calculate the number of _________ of each element.
Divide each by the smallest number of moles to obtain the_______________.
If _____numbers are not obtained* in step 3), multiply through by the _____ number that will give all whole numbers
* Be careful! Do not round off numbers prematurely

13. A sample of a brown gas, a major air pollutant, is found to contain 2
A sample of a brown gas, a major air pollutant, is found to contain 2.34 g N and 5.34g O. Determine a formula for this substance.
require mole ratios so convert grams to moles

14. Calculation of the Molecular Formula
A compound has an empirical formula of NO2. The colourless liquid, used in rocket engines has a molar mass of 92.0 g/mole. What is the molecular formula of this substance?

15. Empirical Formula from % Composition
A substance has the following composition by mass: % Na ; % B ; % H
What is the empirical formula of the substance?
Consider a sample size of _____ grams
This will contain: _____ grams of Na, ______ grams of B, and _____ grams H
Determine the number of ______ of each
Determine the ________ number ratio

16. g of O = g of sample – (g of C + g of H) 4.0 g O = 0.25 mol O
Combust 11.5 g ethanol
Collect 22.0 g CO2 and 13.5 g H2O
g CO2
mol CO2
mol C
g C
6.0 g C = 0.5 mol C
g H2O
mol H2O
mol H
g H
1.5 g H = 1.5 mol H
g of O = g of sample – (g of C + g of H)
4.0 g O = 0.25 mol O
Empirical formula C0.5H1.5O0.25
Divide by smallest subscript (0.25)
Empirical formula C2H6O
3.6

17. Mass Changes in Chemical Reactions
Write balanced chemical equation
Convert quantities of known substances into moles
Use coefficients in balanced equation to calculate the number of moles of the sought quantity
Convert moles of sought quantity into desired units
3.8

18. Other units Molarity Gases Moles solute / L solution
22.4 L = 1 mole of ANY GAS at STP

19. Methanol burns in air according to the equation
2CH3OH + 3O CO2 + 4H2O
If 209 g of methanol are used up in the combustion,
what mass of water is produced?
3.8

20. Limiting Reagents
6 red left over
6 green used up
3.9

21. Method 1
Pick A Product
?????
The ____ answer will be the correct answer
The _____that gives the _____answer will be the _______ reactant

22. Limiting Reactant: Method 1
10.0g of aluminum reacts with 35.0 grams of chlorine gas to produce aluminum chloride. Which reactant is limiting, which is in excess, and how much product is produced?
2 Al + 3 Cl2  2 AlCl3
Start with Al:
Now Cl2:

23. Method 2 Convert one of the reactants to the _____
See if there is enough _______ to use up the other ______
If there is less than the ______amount, it is the ______ reactant
Then, you can find the desired species

24. Do You Understand Limiting Reagents?
In one process, 124 g of Al are reacted with 601 g of Fe2O3
2Al + Fe2O Al2O3 + 2Fe
Calculate the mass of Al2O3 formed.
3.9

25. Use limiting reagent (Al) to calculate amount of product that
can be formed.
g Al
mol Al
mol Al2O3
g Al2O3
3.9

26. Finding Excess Practice
10.0g of aluminum reacts with 35.0 grams of chlorine gas 2 Al + 3 Cl2  2 AlCl3
We found that _______ is the limiting reactant, and _______ of aluminum chloride are produced.
Given amount of excess reactant
Amount of excess reactant actually used
Note that we started with the limiting reactant! Once you determine the LR, you should only start with it!

27. ___________ is the amount of product that would
result if all the limiting reagent reacted.
_________ is the amount of product actually obtained
from a reaction.
% Yield =
_________Yield
x 100
3.10