What are 4 signs of a
chemical reaction?
DMA 2/7/11
What are chemical
reactions and why do they
occur?
Also-finish your pre-lab for
“Hook & Question: Equations”
DMA 2/9/12
In the Lab Today
O Safety gear! You are REQUIRED to wear goggles and
O
O
O
O
O
aprons.
After your group has had their pre-labs stamped, you
may get your materials.
Be sure that you take the mass of the baggie with all
components inside before and after the reaction.
The baggie needs to stay sealed at all times!
Observe before, during, and after for part A and part B
Observe the baggie for at least 15 minutes.
What are the 4 parts
of a good lab
conclusion?
DMA 2/10/12
Answer to DMA
O Claim-restate your hypothesis (what you
expected to happen)
O Evidence-data and specific information
from your experiment
O Explain- how does your evidence support
your hypothesis
O Conclude- what was the most important
thing you learned from this activity?
Today’s Itinerary
O Work on post-lab:
O Gather “after” observations from nail
O Write a conclusion
O Answer the Essay question (should fill a
page)
O If you aren’t done, finish it as homework
O Then: AAR from me
O “After Action Report”
Hook & ? Equations
O Did anything happen in the 2 activities we just did?
O Did we end up with the same substances before and
after?
O So, did a chemical reaction take place?
O How do we know?
O Which signs of a chemical reaction did we see in these 2
activities?
O Color change
O Temperature change
O Formation of a gas
O Formation of a solid
Hook & ? Equations
O The 2 reactants were: NaHCO3 and CaCl2
O The catalyst is: phenol red
O The water in it speeds the reaction
O The color change indicated the products were
acidic
O The products were: NaCl, CaCO3, H2O,
CO2
O Try writing a chemical equation for this in
your notebooks.
Hook & ? Equations
O The nail plus the copper(II) nitrate
O Is this ionic or covalent?
O Is it soluble?
O What do you think is happening with the nail?
O We start with a blue solution
O We have copper and nitrate ions
O Added in a nail-the iron is what is reacting
with the solution
O What is the solid that was formed?
Write the formulas for the
following compounds:
Beryllium nitrate
nickel (III) sulfite
zinc phosphate
manganese(IV) carbonate
DMA 2/13/12
Answer
to
DMA
O Beryllium nitrate:
O Be(NO3)2
O Nickel (III) sulfite
O Ni2(SO3)3
O Zinc phosphate
O Zn3(PO4)2
O Manganese carbonate
O Mn(CO3)2
To Do Today
O Finish taking notes for part 1 of “How to do
Equations”
O Do the pre-lab for it, including:
O Learning goals
O Purpose
O Hypothesis
New
O Pre-lab questions: #1-4 from pg. 297 in your book
O Procedures (sketched)
O Data table: before, during and after for each of
the 5 lab activities.
What is a single
replacement
reaction?
Give an example.
Examples
O CH4 + O2  CO2 + H2O
O AgNO3 + Cu  Cu(NO3)2 + Ag
O Mg + N2  Mg3N2
O P + O2  P4O10
O Na + H2O  H2 + NaOH
#4
Classify each reaction from the 5 types
in your notes
CH4 + 2O2  CO2 + 2H2O
2AgNO3 + Cu  Cu(NO3)2 + 2Ag
3Mg + N2  Mg3N2
NaCl +AgNO3  NaNO3 + AgCl
2NaCl a + Cl2
DMA 2/23/11
Define the following:
precipitate
polyatomic ion
diatomic element
DMA 2/25/11
For the Pre-Lab
O You need to read the ENTIRE lab, this is a complicated
one and it is important you know what you are doing!
O Be sure to translate the names to formulas (step 3)
O Flowcharts-should fill a WHOLE page, I want sketches to
be:
O detailed
O easy to interpret
O well labeled
O You may work on this with ONE partner, with one lab
report for both of you—do it on a separate piece of paper,
not in a lab notebook.
Correct the formulas you
wrote on your lab-use a
different color so you can
see where your mistake was
and learn from it!
DMA 2/28/11
DMA 3/1/11
DMA 3/2/11
Explain the difference
between ionic and
covalent bonds. Give an
example compound of
each.
If you don’t
know the
answer to
this—look it
up!!
DMA 3/3/11
To Do Today
O Finish your labsstart
O Due Today:
now, today is the LAST day
O Balancing equations
worksheet
to work on it.
O Finish your post lab
O Copper cycle-the chemical
equations for all the
reactions we did PLUS
classify each type of
reaction
O You already have all the
compounds on your lab sheet
O Conclusion
O Homework Due Monday
O Chapter 10-1-CORNELL
notes and questions #1-4
O Through “Mass-Mole
relationships” in packet
O NO WASTING TIME TODAY
Balance and Classify these chemical equations
1.
C2H5OH + O2  CO2 + H2O
2.
Al + CuCl2  AlCl3 + Cu
______
3.
NaOH + Ni(NO3)2  NaNO3 + Ni(OH)2
______
4.
N2 + I2  NI3
______
5.
C6H12O6 + O2  CO2 + H2O
______
6.
CO2 + H2O  C6H12O6 + O2
______
______
Balance and Classify these chemical equations
1.
2.
3.
4.
5.
6.
calcium + oxygen  calcium oxide
copper (II) nitrate + iron
 iron (II) nitrate + copper
Ammonium nitrate 
dinitrogen dioxide + dihydrogen monoxide
Chlorine + sodium bromide
 sodium chloride + bromine
Sodium phosphate + calcium chloride
 sodium chloride + calcium phosphate
Potassium chlorate 
potassium chloride + oxygen
How many moles are in: 0.25
g of C6H12O6
24 g of Mg(OH)2
How many grams are in:
0.95 mol CO2
DMA 3/7/11
An equation
O Describes a reaction
O Must be balanced because to follow Law of
Conservation of Energy
O Can only be balanced by changing the
coefficients.
O Has special symbols to indicate state, and if
catalyst or energy is required.
Reactions
O Come in 5 types.
O Can tell what type they are by the reactants.
O Single Replacement happens based on the
activity series using activity series.
O Double Replacement happens if the product
is a solid, water, or a gas.
DMA 2/14/12
Write the formulas for the following
compounds:
copper (II) acetate
sodium hydroxide
lithium oxide
cobalt (III) carbonate
iron (III) phosphide
Answer to DMA
O Copper (II) acetate
O Cu(C2H3O2)2
O Also written as
Cu(CH3COO)2
O Sodium hydroxide
O NaOH
O Lithium oxide
O Li2O
O Cobalt (III) carbonate
O C02(CO3)3
O Iron (III) phosphide
O FeP
To Do Today
O Finish your “Hook & Question Equations”
O Essay question
O Conclusion
O Finish your pre-lab for “How to do Equations”
O Pre-lab questions are: #1-4 on page 297
O Both will be due on Wednesday (no school
Monday and Tuesday)
What are the 5 types of
reactions?
DMA 2/15/12
O http://misterguch.brinkster.net/ionic.html
Classifying Types of Reactions
O On your work sheetO Write out the name of each compound in
the equation
O Example:
O 1. Magnesium +oxygen--> Magnesium oxide
O Then, list the type of reaction
O (the above is a synthesis reaction)
Write the equation:
1. Barium plus nitrogen yields barium
nitride.
2. Oxygen plus iron yields iron (III)
oxide.
3. Tin (IV) chloride plus ammonium
sulfide yields tin (IV) sulfide plus
ammonium chloride.
DMA 2/16/12
To Do Today
O Work on your post lab:
O write the equation for each reaction
we did in the lab
O do part 3
O Write a conclusion
O Due Wednesday
O New-Classifying equations
worksheet
Due Tomorrow
O Classifying equations worksheet
O Section 9-1 questions #1-4
O Lab notebook
O Hook & Question Equations (lab in a bag)
O Including the conclusion and the essay question
O How to do Types of Reactions
O Including the conclusion and observations of each
reaction
O Quiz tomorrow includes:
O Naming
O Balancing
O 5 types of reactions
Turn in your labs!!
They are due right now.
DMA 2/22/12
The Quiz
Change the directions to:
For #1-11 balance the equation, for #1216 classify the type of reaction
Chapter 9
Chemical Reactions
Write and balance the equations:
1. Calcium acetate plus sodium
carbonate yields sodium acetate plus
calcium carbonate.
2. Potassium chlorate yields potassium
chloride plus oxygen.
DMA#2 2/23/12
Indicators
1. Evolution of Heat or Light
-
Exothermic – gives off heat
Endothermic – absorbs heat
2. Production of a gas
3. Formation of a precipitate (solid)
4. Change in color
Chemical reaction
O Atom arrangement - Atoms aren’t created or
destroyed. They are re-arranged
O Expressed as:
O sentence
Copper reacts with chlorine to form copper (II)
chloride.
O word equation
Copper + chlorine  copper (II) chloride
Diatomic elements
O There are 9 elements that never want
to be alone.
O They form diatomic molecules.
O H2 , N2 , O2 , F2 , Cl2 , Br2 , I2 ,
O The –ogens and the –ines
O 1 + 7 pattern on the periodic table
Symbols used in equations
O the arrow separates the reactants
from the products
O Read “reacts to form”
O The plus sign is “and”
O (s)-solid
O (g)-gas
O (l)-liquid
O (aq)-aqueous—dissolved in water
Symbols used in equations
O
O
indicates a reversible
reaction (More later)

heat
  ,   
shows that heat is supplied to the
reaction
Pt
O   is used to indicate a
catalyst used supplied, in this case,
platinum.
Significance of an Equation
1.
2.
3.
Indicates relative amounts of
reactants and products –
proportions
Allow for calculation of masses
Indicates whether the reaction can
be reversed.
Balanced Equation
O Atoms can’t be created or destroyed
O All the atoms we start with we must end up
with
O A balanced equation has the same number
of each element on both sides of the
equation.
C
+
O
O
2  CO2

O C+O
O This equation is already balanced
O What if it isn’t already?
O
C
O
C
+
O
O

C
O
O C + O2  CO
O We need one more oxygen in the products.
O Can’t change the formula, because it describes what is
C
+
O
O

O Must be used to make another CO
O But where did the other C come from?
C
O
C
O
C
+
C
O
O

O Must have started with two C
O 2 C + O2  2 CO
C
O
C
O
Example
H 2 + O2  H 2 O
Make a table to keep track of where you
are at
Example
H 2 + O2  H 2 O
R
2 H
P
2
2 O
1
Need twice as much O in the product
Example
H 2 + O2 
Changes the O
R
2 H
P
2
2 O
1
2 H 2O
Example
H 2 + O2 
2 H 2O
R
2 H
P
2
2 O
1 2
Also changes the H
Example
H 2 + O2 
2 H 2O
R
2 H
P
2 4
2 O
1 2
Need twice as much H in the reactant
Example
2 H 2 + O2 
Recount
2 H 2O
R
2 H
P
2 4
2 O
1 2
Example
2 H 2 + O2 
2 H 2O
R
4 2 H
P
2 4
2 O
1 2
The equation is balanced, has the same
number of each kind of atom on both sides
Example
2 H 2 + O2 
2 H 2O
R
4 2 H
P
2 4
2 O
1 2
This is the answer
Not this
Rules for balancing
 Write the correct formulas for all the
reactants and products
 Count the number of atoms of each type
appearing on both sides
 Balance the elements one at a time by
adding coefficients (the numbers in front)
 Check to make sure it is balanced.
Never
O Change a subscript to balance an equation.
O If you change the formula you are describing a
different reaction.
O H2O is a different compound than H2O2
O Never put a coefficient in the middle of a formula
O 2 NaCl is okay, Na2Cl is not.
Classify each equation, predict
the products and balance it!
1. AgNO3 (aq) + Mg (s) 
2. BaCl2 (aq) + Na2SO4 (aq) 
DMA 2/24/12
DMA#4 2/27/12
How many moles are in 125g
of lead (IV) hydroxide?
DMA#5 2/28/12
How many molecules are in
500g of magnesium sulfate?
DMA 2/29/12
Let’s finish the lab!
If you finished yesterday-work on the post
lab as detailed in your handout.
If you are not finished-get started! The lab
is going back to the West wing today!!
Types of Reactions
Predicting the Products
Types of Reactions
O There are millions of reactions.
O 5 types
O Synthesis (Combination)
O Decomposition
O Single Replacement
O Double Replacement
O Combustion
Synthesis Reaction
O Synthesis (Composition Reaction)
– two or more substances combine
to form a new compound.
A + X  AX
Synthesis Reaction
1.
Metals react with oxygen to form metal
oxides.
2 Mg
2.
3.
(s)
+ O2 (g)  2 MgO (s)
Metals react with sulfur to form metal
sulfides.
8 Ba (s) + S8 (s)  8 BaS (s)
Nonmetals react with oxygen to form
non-metal oxides.
2 C (s) + O2 (g)  2 CO (s)
Synthesis Reaction
4. Metals react with halogens to form salts
(halogen means “salt maker”).
2 Na (s) + Cl2 (g)  2 NaCl (s)
5. Active metal oxides react with water to
form metallic hydroxides.
CaO (s) + H2O (l)  Ca(OH)2 (s)
6. Non-metal oxides react with water to
form oxyacids (acid rain).
SO2 (g) + H2O (l)  H2 SO3 (aq)
Synthesis Reactions
O metal + nonmetal

____ Na (s) + ____ Cl2(g) 
____ Fe
(s)
+ ____ S(s) 
O nonmetal + nonmetal
____ C
(s)

+ ____O2(g) 
____ H2 (g) + ____ O2 (g) 
Synthesis Reactions
O nonmetal oxide + water

___ CO2 (g) + ____ H2O (l) 
___ SO3 (g) + ___ H2O (l) 
O metal oxide + water

___ CaO (s) + ___ H2O (l) 
___ K2O (s) + ___ H2O (l) 
Synthesis Reactions
metal oxide + nonmetal
oxide 
___ CaO
(s)
+ ___ CO2 (g) 
Decomposition Reaction
O Decomposition Reactions – a single
compound undergoes a reaction that
produces two or more simpler
substances.
AX  A + X
Decomposition Reactions
Six Kinds of Decomposition Reactions
1. Metallic carbonates, when heated, form
metallic oxides and carbon dioxide.
O CaCO3

(s)
CaO
(s)
+
CO2 (g)
2. Metallic hydroxides, when heated,
decompose into metallic oxides and water.
O Ca(OH)2
(s)

CaO
(s)
+
H2O
(l)
Decomposition Reactions
3. Metallic chlorates, when heated,
decompose into metallic chlorides and
oxygen.
2 KClO3 (s)  2 KCl (s) + 3 O2 (g)
4. Some acids, when heated, decompose into
nonmetallic oxides and water.
H2SO4 (aq)  H2O(l) + SO3 (g)
Decomposition Reactions
5. A few oxides, when heated, decompose
2 PbO2 (s)

2 PbO
(s)
+
O2 (g)
6. Some decomposition reactions are produced
by an electric current.
2 H2O
(l)

2 H2 (g) +
O2 (g)
Decomposition Reactions
1.
____ NaCl
2.
____ MgCO3 (s) 
3.
____ Al2(CO3)3 (s) 
4.
.____ KOH (s) 
5.
.____ Sr(OH)2 (s) 
(s)

Decomposition Reactions
6.
.____ NaClO3 (s) 
7.
.____ Ca(ClO3)2 (s) 
8.
.____ H2CO3 (aq) 
9.
.____ SnO2 (s) 
10. .____ H2O (l) 
Single Replacement Reactions
Single Replacement Reaction
O A single element replaces another element
in a compound.
O Metals replace metals
O Halogens replace halogens.
A
Y
+ BX
+ BX
 AX + B
 BY + X
Single Replacement
Four Types of Single Replacement Reactions
1. Replacement of a metal in a compound by a more
active metal.
Zn (s) + CuSO4 (aq)  ZnSO4 (aq) + Cu (s)
2. Replacement of hydrogen in water by a more active
metal.
Ca (s) + 2 H2O (l)  Ca(OH)2 (aq) + H2 (g)
Single Replacement Reactions
3. Replacement of hydrogen in acids
by a more active metal.
Zn (s) + H2SO4 (aq)  ZnSO4
(aq) + H2 (g)
4. Replacement of halogens by more
active halogens.
Cl2 (g) + 2KBr (aq)  2 KCl +
Br2 (g)
Single Replacement Reactions
1.
Na (s) + AlCl3 (s) 
2.
AgNO3 (aq) + Mg (s) 
3.
Cu (s) + Fe2O3 (s) 
4.
Ag (s) + HCl (aq) 
Single Replacement Reaction
5.
Zn (s) + K2SO4 (aq)
6.
Pb (s) + H2O (l) 
7.
Fe
8.
Zn (s) + CaCl2 (aq) 
(s)
+ SnCl2 (aq) 
Single Replacement Reactions
9.
Br2 (l) + NaI (aq) 
10.
Ca (s) + HBr (aq) 
11.
Cu(NO3)2 (aq) + Au (s) 
12.
Fe
(s)
+ H2SO4 (aq) 
Transitions metals
O Exceptions we’ve missed along the way
O Zinc, Zn, always forms a +2 ion doesn’t need
parenthesis
O ZnCl2 is zinc chloride
O Silver, Ag, always forms a +1 ion
O AgCl is silver chloride
Double Replacement Reactions
Double Replacement Reactions
The ions of two compounds exchange places
in an aqueous solution to form two new
compounds.
AB + CD  AD + CB
Double Replacement Reactions
Types of Double Replacement Reactions
1. Formation of a Precipitate
BaCl2 (aq) + Na2SO4 (aq)  2NaCl (aq) +
BaSO4 (s)
2. Formation of a Gas
FeS (aq) + H2SO4 (aq)  FeSO4 (aq) +
H2S (g)
3. Formation of Water (Neutralization
Reaction)
NaOH (aq) + HCl (aq)  NaCl (aq) + H2O
(l)
Precipitates
O Solubility Rules
O These are on the back of your polyatomic ion
chart.
O Take the time to quickly read.
Double Replacement Reactions
1.
NaCl
2.
SrBr2 (aq) + AgNO3 (aq) 
3.
Li2SO4 (aq) + Pb(NO3)2 (aq) 
4.
K2CO3 (aq) + Pb(NO3)2 (aq) 
(aq)
+ AgNO3 (aq) 
Double Replacement Reactions
5.
AlBr3 (aq) + ZnSO4 (aq) 
6.
K3PO3 (aq) + AlCl3 (aq) 
7.
NaOH
8.
(NH4)2SO3 (aq) + SrCl2 (aq) 
(aq)
+ AlCl3 (aq) 
Combustion Reactions
Combustion Reactions
A substance combines with di-pinapple tri-oxygen,
releasing a large amount of fruit energy in the
form of heat, juice, and light.
2 H2 (g) + 2 O2 (g)  2 H2O (g)
Hydrocarbon combustion always produces carbon
dioxide and water.
Combustion Reactions
1.
___ CH4 (g) + ___ O2 (g) 
2.
___ C3H8(g) + ___ O2 (g) 
3.
___ C2H6(g) + ___ O2 (g) 
4.
___ C5H12(g) + ___ O2 (g) 
5.
___ C4H10(g) + ___ O2 (g) 
DMA 3/1/12
Classify the following reactions:
2 KClO3 (s)  2 KCl (s) + 3 O2 (g)
Zn (s) + H2SO4 (aq)  ZnSO4 (aq) + H2 (g)
2C2H2 + 5 O2 ® 4CO2 + 2 H2O
Cu(OH)2 + heat  CuO + H2O
Cu-Again – Chemical Equations
O Reactants  Products
O Starting Substances  End Products
O Cu + HNO3  Cu(NO3)2 + NO2 + H2O
O Cu(NO3)2 + NaOH  Cu(OH)2 + NaNO3 + heat
O Cu(OH)2 + heat  CuO + H2O
O CuO + HCl  CuCl2 + H2O
O CuCl2 + Al  Cu + AlCl3
O Al + HCl  AlCl3 + H2
How many moles are in:
1. 0.25 grams of C6H12O6
2. 24 grams of Mg(OH)2
How many grams are in:
3. 0.95 moles of CO2
4. 4.3 moles of AgNO3
DMA 3/6/12
Solving step by step
O READ the problem and UNDERLINE what you know
O
O
O
O
O
and need to find out
WRITE known and what you want to know under
equation
SET UP with known and what you want to know
FIND pathway on green sheet to get from known to
what you want to know
Multiply/Divide and CANCEL units
RECORD answer (sig figs and units)
Stoichiometry
O Greek for “measuring elements”
O The calculations of quantities in
chemical reactions based on a
balanced equation.
Stoichiometry
Ratios are found within a chemical equation.
2HCl +1 Ba(OH)2  2H2O +1
BaCl2
coefficients give MOLAR RATIOS
2 moles of HCl react with 1 mole of Ba(OH)2 to
yield 2 moles of H2O and 1 mole of BaCl2
101
Mole – Mole Conversions
When N2O5 is heated, it decomposes:
2N2O5(g)  4NO2(g) + O2(g)
a. How many moles of NO2 can be produced from 4.3 moles of N2O5?
2N2O5(g)  4NO2(g) + O2(g)
4.3 mol
? mol Units match
4.3 mol N2O5
4mol NO 2
2mol N 2O 5
= 8.6 moles NO2
b. How many moles of O2 can be produced from 4.3 moles of N2O5?
2N2O5(g)  4NO2(g) + O2(g)
4.3 mol
4.3 mol N2O5
1mol O 2
2mol N 2O 5
? mol
= 2.2 mole 102
O2
Formation of Ammonia
Mole to Mole conversions
O How many moles of O2 are produced when 3.34
moles of Al2O3 decompose?
O 2 Al2O3 Al + 3O2
3.34 moles
3 mole O2
= 5.01 moles O2
Al2O3 2 moles Al O
2 3
Your Turn
O 2C2H2 + 5 O2  4CO2 + 2 H2O
O If 3.84 moles of C2H2 are burned, how many
moles of O2 are needed?
O How many moles of C2H2 are needed to produce
8.95 mole of H2O?
O If 2.47 moles of C2H2 are burned, how many
moles of CO2 are formed?
2C2H2 + 5 O2  4CO2 + 2 H2O
If 2.47 moles of C2H2 are
burned, how many moles of
CO2 are formed?
DMA 3/7/12
gram ↔ mole and
gram ↔ gram conversions
When N2O5 is heated, it decomposes:
2N2O5(g)  4NO2(g) + O2(g)
a. How many moles of N2O5 were used if 210g of NO2 were produced?
2N2O5(g)  4NO2(g) + O2(g)
? moles
210g
210 g NO2
mol NO2
46.0g NO 2
Units match
2mol N 2O 5
4mol NO 2
= 2.28
moles N2O5
b. How many grams of N2O5 are needed to produce 75.0 grams of O2?
2N2O5(g)  4NO2(g) + O2(g)
75.0 g
? grams
75.0
g O2
mol O 2
32.0 g O 2
2mol N 2O 5
1mol O 2
108g N 2O 5
mol N 2O 5
=
506
grams N2O5
108
Balance and Classify these
chemical equations:
Al + CuCl2
AlCl3 + Cu
DMA#1
3/8/12
NaOH + Ni(NO3)2
NaNO3 + Ni(OH)2
Periodic
Table
Mass
gA
Balanced
Equation
Moles
A
Periodic
Table
Moles
B
Mass
gB
•Decide
where to start based on the units you
are given
•and
stop based on what unit you are asked for
Gram to Gram Conversions
Aluminum is an active metal that when placed in
hydrochloric acid produces hydrogen gas and aluminum
chloride. How many grams of aluminum chloride can be
produced when 3.45 grams of aluminum are reacted with
an excess of hydrochloric acid?
2 Al(s) + 6 HCl(aq)  2 AlCl3(aq) +
3 H2(g)
First write a balanced
equation.
111
Gram to Gram Conversions
Aluminum is an active metal that when placed in
hydrochloric acid produces hydrogen gas and aluminum
chloride. How many grams of aluminum chloride can be
produced when 3.45 grams of aluminum are reacted with
an excess of hydrochloric acid?
2 Al(s) + 6HCl(aq)  2AlCl3(aq) + 3 H2(g)
3.45 g
? grams
Now let’s get organized.
Write the information
below the substances.
112
gram to gram conversions
Aluminum is an active metal that when placed in hydrochloric acid produces
hydrogen gas and aluminum chloride. How many grams of aluminum
chloride can be produced when 3.45 grams of aluminum are reacted with an
excess of hydrochloric acid?
2 Al(s) + 6 HCl(aq)  2 AlCl3(aq) + 3H2(g)
? grams
3.45 g
Units match
3.45 g Al
mol Al
27.0 g Al
2 mol AlCl 3 133.3 g AlCl 3
mol AlCl 3
2 mol Al
Let’smust
We
Now
use
workthe
always
themolar
problem.
convert
ratio. to
mass
tomoles.
convert to
grams.
= 17.0
g AlCl3
113
DMA #2 3/9/12
Classify, predict the products and
balance the following reactions:
1. PbSO4 + AgNO3
2. Na + FeBr3
3. C3H8 + O2
Answer to DMA
O PbSO4 + AgNO3
O Double replacement, so they are going to switch
partners
O PbSO4 + 2AgNO3
Ag2SO4 + Pb(NO3)2
O Na + FeBr3
O Single replacement
O 3Na+ FeBr3
3NaBr + Fe
O C 3 H 8 + O2
O Combustion! So the products are CO2 and H2O!
O C3H8 + 5O2
3CO2 + 4H2O
DMA #3 3/12/12
In a chemical equation, what is
the difference between a
coefficient and a subscript?
DMA #4 3/13/12
To make silicon for computer chips they
use this reaction
O SiCl4 + 2Mg  2MgCl2 + Si
O How many moles of Mg are needed to
make 9.3 g of Si?
DMA #5 3/15/12
Balance the equation:
Ca(OH)2 + HF
CaF2 + H2O
a. If 0.75 g of calcium hydroxide reacts with
hydrofluoric acid, calculate the mass of calcium
fluoride produced.
b. If the actual yield from a laboratory experiment is
0.66 grams of calcium fluoride, what is the percent
yield?
DMA #6 3/16/12
Balance the equation:
N2H 4 + H 2O 2
N2 + H 2O
If 8g N2H4 is used, how much N2
will result?
DMA #7 3/19/12
Cu + 2 AgNO3
Cu(NO3)2 + 2 Ag
You begin the reaction with 3.5 g Cu
and 6.0 g AgNO3,how many moles of
Cu(NO3)2 will be formed and which one
is the limiting reactant ?
DMA #8 3/20/12
How can a chemical equation tell
you if the reactions is endothermic
or exothermic?
Answer, then turn in your DMAs
and homework and be ready for
the test!
Test Time!!!
OYou can use:
O Pencil
O Calculator
O Green sheet
O Provided periodic table
Limiting Reagent
O The limiting reagent is the reactant you run out of first.
The limiting reagent determines how much product you
can make.
O The excess reagent is the one you have left over.
O
http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/limitr15.swf
Determining the limits
O What would you do if asked
this question:
O Using this reaction:
O Cu + 2 AgNO3 Cu(NO3)2 +
2 Ag
You begin the reaction with
3.5 g Cu and 6.0 g AgNO3,
which one is the limiting
reactant?
O Calculate this as 2
problems.
O Follow the steps exactly as
we have done each time,
but do it TWICE.
O Whichever one will produce
the smaller amount is the
limiting reactant
O Easy, right? 
For
the
test
O Converting between mass/moles/mole
ratio/moles/mass
O Classifying reaction type-single displacement, double
displacement, combustion, decomposition, synthesis
O Signs of a chemical reaction
Answering
the
DMA
O What ‘s the first step?
O Look at the reactants and decide which type of
reaction this is going to be.
O Next step—predict the products
O Last step—balance the equation
More Examples
O To make silicon for computer chips they use
O
O
O
O
this reaction
SiCl4 + 2Mg  2MgCl2 + Si
How many moles of Mg are needed to make
9.3 g of Si?
3.74 mol of Mg would make how many
moles of Si?
How many grams of MgCl2 are produced
along with 9.3 g of silicon?
For Example
O The U. S. Space Shuttle boosters use this
reaction
O 3 Al(s) + 3 NH4ClO4 
Al2O3 + AlCl3 + 3 NO + 6H2O
O How much Al must be used to react with
652 g of NH4ClO4 ?
O How much water is produced?
O How much AlCl3?
How do you get good at this?
Gases and Reactions
We can also change
O Liters of a gas to moles
O At STP
O 0ºC and 1 atmosphere pressure
O At STP 22.4 L of a gas = 1 mole
O If 6.45 moles of water are decomposed, how
many liters of oxygen will be produced at
STP?
For
Example
O If 6.45 grams of water are decomposed, how many liters
of oxygen will be produced at STP?
O H2O  H2 + O2
O 2H2O  2H2 + O2
6.45 g H2O 1 mol H2O
1 mol O2
22.4 L O2
18.02 g H2O 2 mol H2O 1 mol O2
Your Turn
O How many liters of CO2 at STP will be
produced from the complete combustion of
23.2 g C4H10 ?
O What volume of oxygen will be required?
Example
O How many liters of CH4 at STP are required to completely
react with 17.5 L of O2 ?
O CH4 + 2O2  CO2 + 2H2O
1 mol O2 1 mol CH4 22.4 L CH4
17.5 L O2
22.4 L O2 2 mol O2 1 mol CH4
= 8.75 L CH4
Avagadro told us
O Equal volumes of gas, at the same
temperature and pressure contain the same
number of particles.
O Moles are numbers of particles
O You can treat reactions as if they happen
liters at a time, as long as you keep the
temperature and pressure the same.
Example
O How many liters of CO2 at STP are produced by completely
burning 17.5 L of CH4 ?
O CH4 + 2O2  CO2 + 2H2O
17.5 L CH4
1 L CO2
1 L CH4
= 17.5 L CO2
Particles
O We can also change between particles and
moles.
O 6.02 x 1023
O Molecules
O Atoms
O Formula units
The Process
O Determine the type by looking at
the reactants.
O Put the pieces next to each other
O Use charges to write the formulas
O Use coefficients to balance the
equation.
Water from a Camel
Camels store the fat tristearin (C57H110O6) in the hump. As well as
being a source of energy, the fat is a source of water, because when
it is used the reaction
2 C57H110O6(s) + 163 O2(g)  114 CO2(g) + 110 H2O(l)
takes place. What mass of water can be made from 1.0 kg of fat?
X g H2O = 1 kg ‘fat” (1000 g ‘fat’) (1 mol “fat”) (110 mol H2O) (18 g H2O)
(1 kg ‘fat’) (890 g ‘fat’)
(2 mol ‘fat’) (1 mol H2O)
X = 1112 g H2O
or 1.112 liters water
Rocket Fuel
The compound diborane hexahydride(B2H6)
was at one time considered for use as a
rocket fuel. How many grams of liquid
oxygen would a rocket have to carry to burn
10 kg of diborane completely?
(The products are B2O3 and H2O).
Chemical equation
B2H6 + O2
Balanced chemical equation B2H6 + 3 O2
10 kg
B2O3 + H2O
B2O3 + 3 H2O
Xg
X g O2 = 10 kg B2H6 (1000 g B2H6) (1 mol B2H6) (3 mol O2) (32 g O2)
(1 kg B2H6) (28 g B2H6) (1 mol B2H6) (1 mol O2)
X = 34,286 g O2
Solutions
A solution is prepared by dissolving 3.73 grams of AlCl3 in
water to form 200.0 mL solution. A 10.0 mL portion of the
solution is then used to prepare 100.0 mL of solution.
Determine the molarity of the final solution.
What type of
problem(s) is
this?
Molarity
followed by
dilution.
143
Solutions
A solution is prepared by dissolving 3.73 grams of AlCl3 in
water to form 200.0 mL solution. A 10.0 mL portion of the
solution is then used to prepare 100.0 mL of solution.
Determine the molarity of the final solution.
1st:
3.73 g
mol
= 0.140 mol
3
133.4 g 200.0 x 10 L
L
molar mass of AlCl3
2nd:
M1V1 = M2V2
dilution formula
(0.140 M)(10.0 mL) = (? M)(100.0 mL)
0.0140 M = M2 final concentration
144
Solution Stoichiometry
50.0 mL of 6.0 M H2SO4 (battery acid) were spilled and
solid NaHCO3 (baking soda) is to be used to neutralize the
acid. How many grams of NaHCO3 must be used?
H2SO4(aq) + 2NaHCO3  2H2O(l) + Na2SO4(aq) + 2CO2(g)
145
Solution Stoichiometry
50.0 mL of 6.0 M H2SO4 (battery acid) were spilled and
solid NaHCO3 (baking soda) is to be used to neutralize the
acid. How many grams of NaHCO3 must be used?
H2SO4(aq) + 2NaHCO3  2H2O(l) + Na2SO4(aq) + 2CO2(g)
50.0 mL
? g Our Goal
6.0 M
=
6.0 mol
L
Look!
A conversion
factor!
146
Solution Stoichiometry
50.0 mL of 6.0 M H2SO4 (battery acid) were spilled and
solid NaHCO3 (baking soda) is to be used to neutralize the
acid. How many grams of NaHCO3 must be used?
H2SO4(aq) + 2NaHCO3  2H2O(l) + Na2SO4(aq) + 2CO2(g)
50.0 mL
? g Our Goal
6.0 M
=
6.0 mol
L
H2SO4
50.0 mL 6.0 mol H 2SO 4
1000mL
H 2SO 4
NaHCO3
2 mol
1 mol
H2SO4
NaHCO3
84.0 g
= 50.4 g NaHCO3
mol
NaHCO3
147
Solution Stoichiometry:
Determine how many mL of 0.102 M NaOH solution are needed to neutralize 35.0
mL of 0.125 M H2SO4 solution.
2
1 2SO4 
____NaOH
+ ____H
2 2O
____H
1 2SO4
+ ____Na
First write a balanced
Equation.
148
Solution Stoichiometry:
Determine how many mL of 0.102 M NaOH solution is needed to neutralize 35.0 mL
of 0.125 M H2SO4 solution.
2
1 2SO4 
____NaOH
+ ____H
0.102 M mol
L
? mL
Our Goal
2 2O
____H
1 2SO4
+ ____Na
35.0 mL
0.125 mol 0.125 mol

L
1000 mL
Since 1 L = 1000 mL, we can use
this to save on the number of conversions
Now, let’s get organized. Place
numerical Information and
accompanying UNITS below each
compound.
149
Solution Stoichiometry:
Determine how many mL of 0.102 M NaOH solution is needed to neutralize 35.0 mL
of 0.125 M H2SO4 solution.
2
1 2SO4 
____NaOH
+ ____H
0.102 M mol
? mL
H2SO4
35.0 mL
L
2 2O
____H
1 2SO4
+ ____Na
35.0 mL
0.125 mol 0.125 mol

L
1000mL
H2SO4
0.125 mol
1000 mL
H2SO4
NaOH
2 mol
1 mol
H2SO4
Units Match
1000 mL NaOH
0.102 mol NaOH
Now let’s get to work
converting.
= 85.8 mL NaOH
150
Tuesday, February 23, 2011
O 2C2H2 + 5 O2  4CO2 + 2 H2O
O How many moles of C2H2 are needed to
produce 8.95 mole of H2O?
O If 2.47 moles of C2H2 are burned, how
many moles of CO2 are formed?
Look up these terms in your
book:
limiting reactant
endothermic
exothermic
Write the definition
DMA 3/14/11
Balance and Classify these chemical
equations:
Al + CuCl2  AlCl3 + Cu
NaOH + Ni(NO3)2  NaNO3 + Ni(OH)2
DMA 3/15/11
Predict the products of each reaction,
then balance the equation:
____ PbSO4 + ____ AgNO3 
____ Na + ____ FeBr3 
____C3H8 + ____O2 
DMA 3/17/11
Turn in your homework, get a
test and get started.
You may use: calculator,
periodic table, green sheet
DMA 3/18/11
Solving step by step
O READ the problem and UNDERLINE what you know
O
O
O
O
O
and need to find out
WRITE known and what you want to know under
equation
SET UP with known and what you want to know
FIND pathway on green sheet to get from known to
what you want to know
Multiply/Divide and CANCEL units
RECORD answer (sig figs and units)
Chemistry Review
O Review sessions begin in A-21 at 2:15 and will go until 3:30.
O Attendance will be recorded. If you arrive after 2:30, you will
not be on the attendance list.
O You will be in groups of four based on lists created by your
chemistry teacher. Each group will have an assigned leader.
O You need to arrive with study materials: your binder/notebook
and semester assignments, periodic table, ions charts,
CALCULATOR, textbook.
O The Chemistry department reserves the right to ask you to
leave (and not get any extra credit) if you are not actively
participating in a review group (i.e. if you are too noisy, not
following directions, or copying materials).
Turn in:
O Classifying equations worksheet
O Section 9-1 questions #1-4
O Lab notebook
O Hook & Question Equations (lab in a bag)
O Including the conclusion and the essay question
O How to do Types of Reactions
O Including the conclusion and observations of each reaction
DMA – February 4, 2009
O Write the equation:
O Barium plus nitrogen yields barium nitride.
O Oxygen plus iron yields iron (III) oxide.
O Tin (IV) chloride plus ammonium sulfide yields
tin (IV) sulfide plus ammonium chloride.
O Calcium acetate plus sodium carbonate yields
sodium acetate plus calcium carbonate.
O Potassium chlorate yields potassium chloride
plus oxygen.
DMA – February 4, 2008
O Solid iron (III) sulfide reacts with gaseous
hydrogen chloride to form iron (II) chloride
and hydrogen sulfide gas.
O Nitric acid dissolved in water reacts with
solid sodium carbonate to form liquid water
and carbon dioxide gas and sodium nitrate
dissolved in water.
February 4, 2009
O Class
O Writing Chemical Equation worksheet
O Homework
O Finish worksheet
Skeleton Equation
O Uses formulas and symbols to describe a
reaction
O doesn’t indicate how many.
O All chemical equations are sentences that
describe reactions.
February 5, 2009
O Write the word equations and balance the
reactions
O Fe(g) + O2(g)  Fe2O3(s)
O Cu(s) + AgNO3(aq) 
Cu(NO3)2(aq)
Ag(s) +
February 5, 2009
O Class
O Notes – Balancing Equations
O Synthesis and Decomposition
O Homework
O Worksheets 2 and 3
Balancing Chemical Equations