Chemistry and Chemical Reactivity
6th Edition
1
John C. Kotz
Paul M. Treichel
Gabriela C. Weaver
CHAPTER 4
Chemical Equations and Stoichiometry
Lectures written by John Kotz
©2006
2006
Brooks/Cole
Thomson
©
Brooks/Cole
- Thomson
2
CHEMICAL REACTIONS
Chapter 4
Reactants: Zn + I2
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Product: Zn I2
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Chemical Equations
Depict the kind of reactants and
products and their relative amounts
in a reaction.
4 Al(s) + 3 O2(g) ---> 2 Al2O3(s)
The numbers in the front are called
stoichiometric coefficients
The letters (s), (g), and (l) are the
physical states of compounds.
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Reaction of Phosphorus with Cl2
Notice the stoichiometric coefficients and the
physical states of the reactants and products.
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Reaction of Iron with Cl2
Notice the stoichiometric coefficients and the
physical states of the reactants and products.
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Chemical Equations
4 Al(s) + 3 O2(g)
---> 2 Al2O3(s)
This equation means
4 Al atoms + 3 O2 molecules
---give--->
2 “molecules” of Al2O3
4 moles of Al + 3 moles of O2
---give--->
2 moles of Al2O3
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Chemical Equations
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• Because the same
atoms are present in a
reaction at the
beginning and at the
end, the amount of
matter in a system
does not change.
• The Law of the
Demo of conservation of matter, See
Screen 4.3.
Conservation of
2HgO(s) ---> 2 Hg(liq) + O2(g)
Matter
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Chemical Equations
Because of the principle of the
conservation of matter,
an equation
must be
balanced.
It must have the same
number of atoms of the
same kind on both sides.
Lavoisier, 1788
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Balancing
Equations
___ Al(s) + ___ Br2(liq) ---> ___ Al2Br6(s)
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Balancing
Equations
____C3H8(g) + _____ O2(g) ---->
_____CO2(g) + _____ H2O(g)
____B4H10(g) + _____ O2(g) ---->
___ B2O3(g) + _____ H2O(g)
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STOICHIOMETRY
- the study of the
quantitative
aspects of
chemical
reactions.
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STOICHIOMETRY
It rests on the principle of the conservation of
matter.
2 Al(s) + 3 Br2(liq) ------> Al2Br6(s)
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PROBLEM: If 454 g of NH4NO3
decomposes, how much N2O and H2O are
formed? What is the theoretical yield of
products?
STEP 1
Write the balanced
chemical equation
NH4NO3 --->
N2O + 2 H2O
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454 g of NH4NO3 --> N2O + 2 H2O
STEP 2 Convert mass reactant
(454 g) --> moles
1 mol
454 g •
= 5.68 mol NH4NO3
80.04 g
STEP 3 Convert moles reactant
(5.68 mol) --> moles product
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454 g of NH4NO3 --> N2O + 2 H2O
STEP 3 Convert moles reactant -->
moles product
Relate moles NH4NO3 to moles
product expected.
1 mol NH4NO3 --> 2 mol H2O
Express this relation as the
STOICHIOMETRIC
2 mol .H2 O produced
FACTOR
1 mol NH 4NO 3 used
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454 g of NH4NO3 --> N2O + 2 H2O
STEP 3 Convert moles reactant (5.68
mol) --> moles product
2 mol H 2O produced
5.68 mol NH 4NO 3 •
1 mol NH 4NO 3 used
= 11.4 mol H2O produced
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454 g of NH4NO3 --> N2O + 2 H2O
STEP 4 Convert moles product
(11.4 mol) --> mass product
Called the THEORETICAL YIELD
18.02 g
11.4 mol H2O •
= 204 g H2O
1 mol
ALWAYS FOLLOW THESE STEPS IN
SOLVING STOICHIOMETRY PROBLEMS!
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GENERAL PLAN FOR
STOICHIOMETRY
CALCULATIONS
Mass
product
Mass
reactant
Moles
reactant
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Stoichiometric
factor
Moles
product
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454 g of NH4NO3 --> N2O + 2 H2O
STEP 5 How much N2O is formed?
Total mass of reactants =
total mass of products
454 g NH4NO3 = ___ g N2O + 204 g H2O
mass of N2O = 250. g
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454 g of NH4NO3 --> N2O + 2 H2O
Amounts Table (page 125)
• Compound
NH4NO3
N2O
H2O
• Initial (g)
• Initial (mol)
• Change (mol)
• Final (mol)
• Final (g)
Note that matter is conserved!
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454 g of NH4NO3 --> N2O + 2 H2O
Amounts Table (page 125)
• Compound
• Initial (g)
• Initial (mol)
• Change (mol)
• Final (mol)
NH4NO3
N2O
H2O
454 g
0
0
5.68 mol
0
0
-5.68
0
+5.68 +2(5.68)
5.68
11.4
• Final (g)
0
250
204
Note that matter is conserved!
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454 g of NH4NO3 --> N2O + 2 H2O
STEP 6 Calculate the percent yield
If you isolated only 131 g of N2O, what is
the percent yield?
This compares the theoretical (250. g)
and actual (131 g) yields.
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454 g of NH4NO3 --> N2O + 2
H2O
STEP 6 Calculate the percent yield
actual yield
% yield =
• 100%
theoretical yield
131 g
% yield =
• 100% = 52.4%
250. g
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PROBLEM: Using 5.00 g of H2O2,
what mass of O2 and of H2O can
be obtained?
2 H2O2(liq) ---> 2 H2O(g) + O2(g)
Reaction is catalyzed by MnO2
Step 1: moles of H2O2
Step 2: use STOICHIOMETRIC FACTOR
to calculate moles of O2
Step 3: mass of O2
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Reactions Involving a
LIMITING REACTANT
• In a given reaction, there is not
enough of one reagent to use up the
other reagent completely.
• The reagent in short supply
LIMITS the quantity of product
that can be formed.
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LIMITING REACTANTS
Reactants
2 NO(g) + O2 (g)
Products
2 NO2(g)
Limiting reactant = ___________
Excess reactant = ____________
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LIMITING REACTANTS
Demo of limiting reactants on Screen 4.7
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LIMITING REACTANTS
(See CD Screen 4.8)
React solid Zn with 0.100
mol HCl (aq)
Zn + 2 HCl ---> ZnCl2 + H2
1
2
3
Rxn 1: Balloon inflates fully, some Zn left
* More than enough Zn to use up the 0.100 mol HCl
Rxn 2: Balloon inflates fully, no Zn left
* Right amount of each (HCl and Zn)
Rxn 3: Balloon does not inflate fully, no Zn left.
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LIMITING REACTANTS
React solid Zn with 0.100 mol
HCl (aq)
Zn + 2 HCl ---> ZnCl2 + H2
0.10 mol HCl [1 mol Zn/2 mol HCl]
= 0.050 mol Zn
mass Zn (g)
mol Zn
mol HCl
mol HCl/mol Zn
Lim Reactant
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Rxn 1
7.00
0.107
0.100
0.93/1
LR = HCl
Rxn 2
3.27
0.050
0.100
2.00/1
no LR
Rxn 3
1.31
0.020
0.100
5.00/1
LR = Zn
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Reaction to be Studied
2 Al + 3 Cl2 --->
Al2Cl6
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PROBLEM: Mix 5.40 g of Al with
8.10 g of Cl2. What mass of Al2Cl6 can
form?
Mass
product
Mass
reactant
Moles
reactant
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Stoichiometric
factor
Moles
product
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Step 1 of LR problem:
compare actual mole ratio
of reactants to
theoretical mole ratio.
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Step 1 of LR problem:
compare actual mole ratio of
reactants to theoretical
mole ratio.
2 Al + 3 Cl2 --->
Al2Cl6
Reactants must be in the mole ratio
mol Cl2
3
=
mol Al
2
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Deciding on the Limiting
Reactant
2 Al + 3 Cl2 ---> Al2Cl6
If
mol Cl2
3
>
mol Al
2
There is not enough Al to use up all
the Cl2
Lim reag = Al
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Deciding on the Limiting
Reactant
2 Al + 3 Cl2 ---> Al2Cl6
mol Cl2
3
<
mol Al
2
If
There is not enough Cl2 to use
up all the Al
Lim reag = Cl2
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Step 2 of LR problem:
Calculate moles of each
reactant
We have 5.40 g of Al and 8.10 g of Cl2
1 mol
5.40 g Al •
= 0.200 mol Al
27.0 g
1 mol
8.10 g Cl2 •
= 0.114 mol Cl2
70.9 g
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Find mole ratio of reactants
2 Al + 3 Cl2 ---> Al2Cl6
mol Cl2
0.114 mol
=
mol Al
0.200 mol
= 0.57
This
should be 3/2 or 1.5/1 if
reactants are present in the
exact stoichiometric ratio.
Limiting reactant is
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Cl2
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Mix 5.40 g of Al with 8.10 g of Cl2.
What mass of Al2Cl6 can form?
2 Al + 3 Cl2 ---> Al2Cl6
Limiting reactant = Cl2
Base all calcs. on Cl2
mass
Cl2
moles
Cl2
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mass
Al2Cl6
1 mol Al2Cl6
3 mol Cl2
moles
Al2Cl6
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CALCULATIONS: calculate mass of
Al2Cl6 expected.
Step 1: Calculate moles of Al2Cl6
expected based on LR.
1 mol Al2Cl6
0.114 mol Cl2 •
= 0.0380 mol Al2Cl6
3 mol Cl2
Step 2: Calculate mass of Al2Cl6 expected
based on LR.
0.0380 mol Al2Cl6 •
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266.4 g Al2Cl6
= 10.1 g Al2Cl6
mol
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How much of which reactant will
remain when reaction is complete?
• Cl2 was the limiting reactant.
Therefore, Al was present in
excess. But how much?
• First find how much Al was required.
• Then find how much Al is in excess.
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Calculating Excess Al
2 Al + 3 Cl2
0.200 mol
products
0.114 mol = LR
2 mol Al
0.114 mol Cl2 •
= 0.0760 mol Al req'd
3 mol Cl2
Excess Al = Al available - Al required
= 0.200 mol - 0.0760 mol
= 0.124 mol Al in excess
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Chemical Analysis
Active Figure 4.8
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Chemical Analysis
• An impure sample of the mineral thenardite
contains Na2SO4.
• Mass of mineral sample = 0.123 g
• The Na2SO4 in the sample is converted to
insoluble BaSO4.
• The mass of BaSO4 is 0.177 g
• What is the mass percent of Na2SO4 in the
mineral?
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Chemical Analysis
• Na2SO4(aq) + BaCl2(aq)
--> 2 NaCl(aq) + BaSO4(s)
• 0.177 g BaSO4 (1 mol/233.4 g)
= 7.58 x 10-4 mol BaSO4
• 7.58 x 10-4 mol BaSO4 (1 mol Na2SO4/1 mol BaSO4)
= 7.58 x 10-4 mol Na2SO4
• 7.58 x 10-4 mol Na2SO4 (142.0 g/1 mol)
= 0.108 g Na2SO4
• (0.108 g Na2SO4/0.123 g sample)100%
= 87.6% Na2SO4
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Chemical Analysis
• An impure sample of the mineral thenardite
contains Na2SO4.
• Sample mass = 0.123 g
• The Na2SO4 is converted to insoluble BaSO4.
• The mass of BaSO4 is 0.177 g
• What is the mass percent of Na2SO4 in the
mineral?
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Determining the Formula of a
Hydrocarbon by Combustion
Active Figure 4.9
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Using Stoichiometry to
Determine a Formula
Burn 0.115 g of a hydrocarbon, CxHy, and
produce 0.379 g of CO2 and 0.1035 g of
H2O.
CxHy + some oxygen --->
0.379 g CO2 + 0.1035 g H2O
What is the empirical formula of CxHy?
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Using Stoichiometry to
Determine a Formula
CxHy + some oxygen --->
0.379 g CO2 + 0.1035 g H2O
First, recognize that all C in CO2 and all H
in H2O is from CxHy.
0.379 g CO2
+O2
1 CO2 molecule forms for
each C atom in CxHy
Puddle of CxHy
0.115 g
+O2
0.1035 g H2O
1 H2O molecule forms for
each 2 H atoms in CxHy
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Using Stoichiometry to
Determine a Formula
CxHy + some oxygen --->
0.379 g CO2 + 0.1035 g H2O
First, recognize that all C in CO2 and all H in H2O
is from CxHy.
1. Calculate amount of C in CO2
8.61 x 10-3 mol CO2 --> 8.61 x 10-3 mol C
2. Calculate amount of H in H2O
5.744 x 10-3 mol H2O -- >1.149 x 10-2 mol H
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Using Stoichiometry to
Determine a Formula
CxHy + some oxygen --->
0.379 g CO2 + 0.1035 g H2O
Now find ratio of mol H/mol C to find
values of x and y in CxHy.
1.149 x 10 -2 mol H/ 8.61 x 10-3 mol C
= 1.33 mol H / 1.00 mol C
= 4 mol H / 3 mol C
Empirical formula = C3H4
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