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1. The Basics of Stoichiometry and
Mole Calculations
References and Resources
•Our TB: Ch. 3 of Chemistry: The central Science AP version (10th edition)
•Powerpoint *and in-class work
•POGIL activities
•Online resources for our TB (in particular: Practice Quiz and e-book)
•Concept map for Stoichiometry and problem solving (handout)
•Video lectures from chem guy (see next page)
•Chem tours from ch. 3 of the W.W. Norton online book by Gilbert:
•http://www.wwnorton.com/college/chemistry/gilbert2/contents/ch03/studyplan.asp
•*Some figures and examples in this PPT file have been taken from Melissa Brophy’s presentation
at http://teacherweb.com/TX/McNeilHS/brophy/photo2.aspx

2. Resources: Video lectures for Chemistry
• Chemguy videos (google AP chemistry and chemguy videos; use in sequence)
(good, short, video lectures that are appropriate for regular, honors, or AP chemistry)
• chem Guy video for mole 1
http://www.youtube.com/watch?v=xiVweBpjXJo&playnext=1&videos=kHh8a0fILuY&feature=mfu_i
n_order
• Mole 2 chem guy:
http://www.youtube.com/watch?v=xqw2BWdKl1Q&feature=PlayList&p=C09489B20AE215DF&play
next=1&playnext_from=PL&index=19
• Mole 3 (Junior) :
• http://www.youtube.com/watch?v=O7qjYRYxkso&feature=PlayList&p=C09489B20AE215DF&playne
xt=1&playnext_from=PL&index=20
• Stoichiometry video with worked example for predicting amount of product from 2.6 mol of one of
reactant: see http://www.youtube.com/watch?v=-W9-sNfM5Xo&feature=related
• Empirical formula for AP chem with chem. Guy:
http://www.youtube.com/watch?v=fFXtX_8NgsQ&feature=related

3. The Basics of Stoichiometry and
Mole Calculations
Topics (review and new)
• Reading and writing
chemical equations
• Balancing Equations
• Types of reactions
• Formula Weights
• Formula Weights and Molar
Masses
• Percent composition
• Avagadro’s Number
(continued)
• Mole calculations
• Solving problems using
dimensional analysis using
(1) Avagadro’s number, (2)
GFM, or (3) mole ratios
from coefficients of
balanced equations
• Determining Empirical
formulas and Molecular
formulas
• Limiting reagents(reactants)

4. Chemical Equations
• Symbolic representations or
descriptions of chemical
reactions
• Meaning of the symbols,
subscripts, parenthesis, +
signs, arrows, co-efficients,
states of matter, etc. Vocab.
terms: reactants, products,
catalyst, reaction conditions ,
etc.
• Use of particle diagrams (to
represent)
• Conservation of Mass
• Resources: POGIL activity
“Chemical Reaction Equations”
(To Do)
2 H2 (g) + O2 (g) 2 H2O (l)

5. Reading Balanced Chemical Equations
Molecules
Particle diagrams
Mass (amu)
Amount (mol)
Mass (g)
2 H2 (g) + O2 (g) 2 H2O (l)

6. Balancing Equations
Objective: find the smallest whole number ratio of coefficients
for reactants and products that respects the law of
conservation of mass.
How?
• Trial and error to some extent
• Can Not change subscripts in chemical formulas
but you Can change co-efficients in front of the formulas
• Start by balancing those elements that occur in the fewest
chemical formulas
• Move back and forth checking the atom count each time a
co-efficient is changed
_____NaN3 (s) _____ Na (s) + _____N2 (g)

7. Practice Balancing Equations
• (example of a decomposition reaction that is
used in air bags in cars)
_____NaN3 (s) _____ Na (s) + _____N2 (g)

8. Practice Balancing Equations
(Index card activity – to hand in)
• (example of a combustion reaction)
• (Hint: Start with the element that occurs in
the fewest chemical formulas)
___C3H8(g)+___O2(g) ___CO2(g) + ___H2O(g)

9. Formula Weights
• Atomic masses of
atoms, molecules
and formula unit
• Atoms:
• Ex: Au (gold)
• One atom of Au
has a mass of
__________amu
• Calculating formula weights in amu
using chemical formula and the
atomic masses from the periodic
table
• Ex: NaCl
• One formula unit of NaCl has a
mass of ______amu
• Ex: C6H12O6 (glucose)
• One molecule of glucose has a
mass of ______amu

10. What is the percent carbon in C5H8NO4 (the
glutamic acid used to make MSG
monosodium glutamate), a compound used
to flavor foods and tenderize meats?
Percent Composition

11. What is the percent carbon in C5H8NO4?
Step 1: First calculate the Formula weight for
the compound (FW for C5H8NO4 is ________amu)
Step 2: % composition = (mass of part ÷mass of whole) X 100
or
% element = (# atoms of that element)(atomic weight of the element) x 100
Formula weight of the compound
Percent Composition

12. What is the % carbon in MSG?
Step 1: FW for C5H8NO4 is ________amu
C
H
N
O

13. Step 2 % C = (mass of part ÷mass of whole) X 100
or
% element = (# atoms of element)(atomic weight of the element) x 100
Formula weight of the compound
Answer?
% Composition of Carbon in C5H8NO4

14. What is the percent carbon in C5H8NO4 (the
glutamic acid used to make MSG
monosodium glutamate), a compound used
to flavor foods and tenderize meats?
a) 8.22 %C
b) 24.3 %C
c) 41.1 %C
Percent Composition

15. Avagadro’s number and The
Mole
6.02 x 1023
602,000,000,000,000,000,000,000

16. The Mole
• A counting unit
• Similar to a dozen, except instead
of 12, it’s 602 billion trillion
602,000,000,000,000,000,000,000
• 6.02 X 1023 (in scientific notation)
• This number is named in honor of
Amedeo _________ (1776 – 1856),
who studied quantities of gases
and discovered that no matter what
the gas was, there were the same
number of molecules present

17. How big of a unit is a mole?
• If you had Avogadro's number of
unpopped popcorn kernels, and spread
them across the United States of
America, the country would be covered
in popcorn to a depth of over 9 miles.

18. The Mole (abbreviated as mol)
• 1 dozen cookies = 12 cookies
• 1 mole of cookies = 6.02 X 1023 cookies
• 1 dozen cars = 12 cars
• 1 mole of cars = 6.02 X 1023 cars
• 1 dozen Al atoms = 12 Al atoms
• 1 mole of Al atoms = 6.02 X 1023 atoms
Note that the NUMBER is always the same,
but the MASS is very different!

19. = 6.02 x 1023 C atoms
= 6.02 x 1023 H2O molecules
= 6.02 x 1023 NaCl “formula units”
(technically, ionic compounds are not
molecules so they are called formula units)
6.02 x 1023 Na+ ions and
6.02 x 1023 Cl– ions
A Mole of Particles
Contains 6.02 x 1023 particles
1 mole C
1 mole H2O
1 mole NaCl

20. 6.02 x 1023 particles
1 mole
or
1 mole
6.02 x 1023 particles
Note that a particle could be an atom OR a molecule!
Avogadro’s Number as
Conversion Factor

21. 1. Number of atoms in 0.500 mole of Al
a) 500 Al atoms
b) 6.02 x 1023 Al atoms
c) 3.01 x 1023 Al atoms
2.Number of moles of S in 1.8 x 1024 S atoms
a) 1.0 mole S atoms
b) 3.0 mole S atoms
c) 1.1 x 1048 mole S atoms
Learning Check

22. Practice Problems – with /without
using your calculator
• How many hydrogen atoms are in 2.5 moles of
water? (Analyze, plan, solve, check)

23. • The Mass of 1 mole (in grams)
• Equal to the numerical value of the average
atomic mass (get from periodic table)
1 mole of C atoms = 12.0 g
1 mole of Mg atoms = 24.3 g
1 mole of Cu atoms = 63.5 g
Molar Mass or Gram-Formula
Mass (GFM)

24. Other Names Related to Molar Mass or
Gram-Formula Mass (GFM)
• Molecular Mass/Molecular Weight: If you have a single
molecule, mass is measured in amu’s instead of grams. But,
the molecular mass/weight is the same numerical value as 1
mole of molecules. Only the units are different. (This is the
beauty of Avogadro’s Number!)
• Formula Mass/Formula Weight: Same goes for
compounds. But again, the numerical value is the same.
Only the units are different.
• THE POINT: You may hear all of these terms
which mean the SAME NUMBER… just different units

25. Find the molar mass or gram-formula mass
(usually we round to the tenths place)
Learning Check!
A.1 mole of Br atoms
B.1 mole of Sn atoms
= 79.9 g/mole
= 118.7 g/mole

26. Practice Problems – use mole road
map or concept map to help you solve
• How many atoms of copper are there in a 3
gram sample of copper?
(Interconverting mass and numbers of particles)

27. Problems involving Empirical Formulas
and Molecular Formulas
• Resources:
• PPT
• POGIL
• Practice problems (in-class, chapter problem
set, online practice quiz questions)

28. Chemical Formulas of Compounds
• Formulas give the relative numbers of atoms or moles
of each element in a formula unit - always a whole
number ratio (the law of definite proportions).
NO2 2 atoms of O for every 1 atom of N
1 mole of NO2 2 mol of O atoms to every 1 mol of N atoms
• If we know, or can determine, the relative number of
moles of each element in a compound, we can
determine a formula for the compound.

29. Types of Formulas
• Empirical Formula
The formula of a compound that
expresses the smallest whole number
ratio of the atoms present.
Ionic formula are always empirical formula
• Molecular Formula
The formula that states the actual
number of each kind of atom found in one
molecule of the compound.

30. To obtain an Empirical Formula
1. Determine the mass in grams of each
element present, if necessary.
2. Calculate the number of moles of each
element.
3. Divide each by the smallest number of moles
to obtain the simplest whole number ratio.
4. If whole numbers are not obtained* in step 3),
multiply through by the smallest number that
will give all whole numbers
* Be careful! Do not round off numbers prematurely

31. 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
moles of N = 2.34g of N = 0.167 moles of N
14.01 g/mole
moles of O = 5.34 g = 0.334 moles of O
16.00 g/mole
Empirical Formula:
0.334
0.167O
N 0.167 0.334 2
0.167 0.167
N O NO


32. 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?

33. Empirical Formula from % Composition
A substance has the following composition by mass: 60.80 %
Na ; 28.60 % B ; 10.60 % H
What is the empirical formula of the substance?
• Consider a sample size of 100 grams
•This will contain 28.60 grams of B and 10.60 grams H
•Determine the number of moles of each element
•Determine the simplest whole number ratio of each element

34. Determination of Empirical Formulas using
combustion analysis data for organic
compounds
• Experimental method that uses the mass of
starting materials and masses of water and
carbon dioxide produced to solve for the emp.
Formula of organic compounds.
• Steps?

35. Predicting Quantities of Products
Based on Quantities of Reactants Use
(use concept/road map)
Grams of
reactant
(Given)
Moles of
reactant
Moles of
product
Grams of
product
(To Find_

36. How do we do this?
• Predicting Quantities of Products Based on
Quantities of Reactants
• Start from a balanced equation
• Use concept/road map
• Use dimensional analysis with (a) molar mass/
GFM and (b) mole ratios as the basis of
conversion factors

37. Practice Problem (Practice ex. P. 103).
The decomposition of potassium chlorate is commonly used to prepare small
amounts of oxygen gas in the laboratory. How many grams of oxygen gas
can be prepared from 4.50 g of potassium chlorate?

38. Limiting reagents(reactants) problems
(Start with POGIL “Limiting reactants”)
• Start with the balanced chemical equation
• Determine moles of reactants
• Setup tables [(initial, change and end (final)]
or ICE charts
• Identify the limiting reagent/reactant
• Finish the problem using dimensional analysis

40. Activities and Problem set X
TB ch. 3 – all sections required for
regents, SAT II and AP exams
POGIL activities on chemical
reaction equations, limiting
reactants, etc
Lab activities:
• Determination CuxOy formula
• Percent composition of water in a
hydrate
• Others - TBD
Road/Concept map (provided)
Online practice quiz due by ______
• Ch 3 Problems TO DO: write out
questions and answers & show work
• all GIST, sample & practice exercises,
Visualizing concepts,
• end of chapter 3 exercises: 10, 11
(b,e,g), 12 (d,g), 14, 15, 17, 19, 23
(b,d), 26d, 27, 29, 33, 35, 37, 41, 43,
47, 53, 59, 63, 67, 68, 71, 73, 75, 80,
105