Download - Unit 6 Chemical Reactions
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LecturePLUS Timberlake 1
Unit 6Chemical Reactions
By the end of this PPT You should be able to…
* Compare/Contrast a Chemical & Physical Change.
* Identify the parts of a Chemical Reaction
* Describe the Relationship between a Reactant & Product
*Apply the steps of solving a chemical equation
*State the Law of Conservation of Matter
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LecturePLUS Timberlake 2
Physical Properties
color
melting point
boiling point
electrical conductivity
specific heat
density
state (solid, liquid, or gas)
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LecturePLUS Timberlake 3
Physical Change
Changes in physical properties Melting Boiling Condensation
No change occurs in the identity of the substance
Examples:
Ice , Rain, and Snow are all water
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LecturePLUS Timberlake 4
Chemical Change
Atoms in the reactants are rearranged to form one or more different substances
Old bonds are broken; new bonds form
Examples:
Fe and O2 form rust (Fe2O3)
Ag and S form tarnish (Ag2S)
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A Burning Candle…..
LecturePLUS Timberlake 5
1. Physical Change
2. Chemical Change
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Melting Ice…..
LecturePLUS Timberlake 6
1. Physical Change
2. Chemical Change
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Toasting a marshmallow….
LecturePLUS Timberlake 7
1. Physical Change
2. Chemical Change
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Cutting a pizza…..
LecturePLUS Timberlake 8
1. Physical Change
2. Chemical Change
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A nail rusting…..
LecturePLUS Timberlake 9
1. Physical Change
2. Chemical Change
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LecturePLUS Timberlake 10
Solution E1
Classify each of the following as a
1) physical change or 2) chemical change
A. __2__ a burning candle
B. __1_ melting ice
C. __2__ toasting a marshmallow
D. __1__ cutting a pizza
E. __2__ polishing silver
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Chemical Reaction
A process in which at least one new substance is produced as a result of chemical change.
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LecturePLUS Timberlake 12
A Chemical Reaction
Reactants Products
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LecturePLUS Timberlake 13
Learning Check E2
A. How does an equation indicate a change in
the identity of the reacting substances?
B. How did the yellow and green reactants
combine?
C. Did all the reactants form product? Why or
why not?
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LecturePLUS Timberlake 14
Learning Check E2
A. How does an equation indicate a change in the identity of the reacting substances? The formulas of the reactants are different than the formulas of the products.
B. How did the yellow and green reactants combine? 1 yellow combined with 1 green.C. Did all the reactants form product? Why or why not? No. There were more yellow reactants than green.
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LecturePLUS Timberlake 15
Writing a Chemical Equation
Chemical symbols give a “before-and-after” picture of a chemical reaction
Reactants Products
MgO + C CO + Mg
magnesium oxide to form carbon monoxide
reacts with carbon and magnesium
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LecturePLUS Timberlake 16
Learning Check E3
12 oz of dough, 4 oz mushrooms, 12 slices pepperoni, 8 oz cheese and 5 oz tomato sauce are used to make a pizza. Write a recipe in words for putting together a pizza.
How would you write the recipe as an equation?
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LecturePLUS Timberlake 17
Solution E3
Example: Combine 12 oz dough + 4 oz mushrooms + 12 slices pepperoni + 8 oz cheese + 5 oz tomato sauce and heat 30 minutes at 350°C to produce 1 pizza
12 oz dough + 4 oz mshrm + 12 pep + 8 oz chse 1 pizza+ 5 oz tom sauce
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LecturePLUS Timberlake 18
Reading A Chemical Equation
4 NH3 + 5 O2 4 NO + 6 H2O
Four molecules of NH3 react with five molecules O2 to produce four molecules NO and six molecules of H2O
or
Four moles NH3 react with 5 moles O2 to produce
four moles NO and six moles H2O
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LecturePLUS Timberlake 19
A Balanced Chemical Equation
Same numbers of each type of atom on each side of the equation
Al + S Al2S3 Not
Balanced
2Al + 3S Al2S3 Balanced
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LecturePLUS Timberlake 20
Matter Is Conserved
H2 + Cl2 2 HCl
+ +Total atoms = Total atoms
2 H, 2 Cl 2H, 2 Cl
Total Mass = Total Mass
2(1.0) + 2(35.5) 2(36.5)
73.0 g = 73.0 g
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Law of Conservation of Mass
In any ordinary chemical reaction, matter is not created nor destroyed
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Balance Equations with Coefficients
Coefficients in front of formulas balance each type of atom
4NH3 + 5O2 4NO + 6H2O
4 N = 4 N
12 H = 12 H
10 O = 10 O
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LecturePLUS Timberlake 23
Steps in Balancing An Equation
Fe3O4 + H2 Fe + H2O
Fe: Fe3O4 + H2 3 Fe + H2O
O: Fe3O4 + H2 3 Fe + 4 H2O
H: Fe3O4 + 4 H2 3 Fe + 4 H2O
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LecturePLUS Timberlake 24
Learning Check E4
Fe3O4 + 4 H2 3 Fe + 4 H2O
A. Number of H atoms in 4 H2O
1) 2 2) 4 3) 8
B. Number of O atoms in 4 H2O
1) 2 2) 4 3) 8
C. Number of Fe atoms in Fe3O4
1) 1 2) 3 3) 4
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LecturePLUS Timberlake 25
Solution E4
Fe3O4 + 4 H2 3 Fe + 4 H2O
A. Number of H atoms in 4 H2O
3) 8
B. Number of O atoms in 4 H2O
2) 4
C. Number of Fe atoms in Fe3O4
2) 3
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Learning Check E5
Balance each equation. The coefficients for each equation are read from left to right
A. Mg + N2 Mg3N2
1) 1, 3, 2 2) 3, 1, 2 3) 3, 1, 1
B. Al + Cl2 AlCl3
1) 3, 3, 2 2) 1, 3, 1 3) 2, 3, 2
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LecturePLUS Timberlake 27
Learning Check E5
C. Fe2O3 + C Fe + CO2
1) 2, 3, 2,3 2) 2, 3, 4, 3 3) 1, 1, 2, 3
D. Al + FeO Fe + Al2O3
1) 2, 3, 3, 1 2) 2, 1, 1, 1 3) 3, 3, 3, 1
E. Al + H2SO4 Al2(SO4)3 + H2
1) 3, 2, 1, 2 2) 2, 3, 1, 3 3) 2, 3, 2, 3
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LecturePLUS Timberlake 28
Solution E5
A. 3 Mg + N2 Mg3N2
B. 2 Al + 3 Cl2 2 AlCl3
C. 2 Fe2O3 + 3 C 4 Fe + 3 CO2
D. 2 Al + 3 FeO 3 Fe + Al2O3
E. 2 Al + 3 H2SO4 Al2(SO4)3 + 3 H2