Chapter 5 Chemical Reactions -...
Transcript of Chapter 5 Chemical Reactions -...
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Chapter 5 Chemical Reactions
1. Physical and Chemical Changes
2. Understanding Chemical Changes
3. Chemical Equations
4. Balancing Chemical Equations
5. Types of Chemical Reactions
Table of Contents
Chapter 5
• List down some changes around you and identify them as physical and chemical.
Warm up
• Which changes in your list are reversible and which are irreversible?
• Which changes in your list produce new substances?
1. Physical and Chemical Changes
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Chapter 5 1. Physical and Chemical Changes
• Physical changes are changes in which the identity of a substance does not change. Chemical composition of substances remain unchanged. Breaking of a glass, cutting of a sheet of paper, dissolving of salt in water, freezing of water…etc are physical changes.
• No new substance is formed.• Some physical changes are reversible.
Chapter 5 1. Physical and Chemical Changes
• Changes that cause to produce new substances are
called chemical changes. The rusting of iron, boiling
of an egg, spoiling fruits, burning of coal…etc. are
chemical changes. Chemical changes usually
irreversible.
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Chapter 5 1. Physical and Chemical Changes
Chapter 5 1. Physical and Chemical Changes
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Chapter 5 1. Physical and Chemical Changes
Chapter 5
Section Review1. Identify the following changes as physical or chemical.
Burning of wood, evaporation of alcohol, freezing of
cement, frying of egg, souring of milk, digging of soil,
painting of a wall, cleaning of dishes.
1. Physical and Chemical Changes
1. Chemical changes: Burning of wood, frying of egg,
souring of milk, cleaning of dishes.
Physical changes: Evaporation of alcohol, digging of
soil, painting of a wall
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Chapter 5
Section Review
2. Which of the following changes is different?
A. Raining
B. Sublimation of iodine
C. Combustion of gasoline
D. Distillation of petroleum
1. Physical and Chemical Changes
Chapter 5
Section Review
2. Which of the following changes is different?
A. Raining
B. Sublimation of iodine
C. Combustion of gasoline
D. Distillation of petroleum
1. Physical and Chemical Changes
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Chapter 5
Section Review
3. Wood that has burned and formed carbon dioxide and
water vapor has gone through a
A. chemical change
B. physical change
C. change in state
D. change in color.
1. Physical and Chemical Changes
Chapter 5
Section Review
3. Wood that has burned and formed carbon dioxide and
water vapor has gone through a
A. chemical change
B. physical change
C. change in state
D. change in color.
1. Physical and Chemical Changes
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Chapter 5
• List some evidences that suggest that a chemical reaction has occurred and decide which of them might be indicator for the following changes.
Cooking of cake, photosynthesis, burning of paper, spoiling of fruits, cleaning of a cloth.
Warm up
2. Understanding Chemical Changes
Chapter 5 2. Understanding Chemical Changes
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Chapter 5 2. Understanding Chemical Changes
Chapter 5 2. Understanding Chemical Changes
Evidence of a Chemical Reaction, continued
2. Color ChangePb(NO3)2 + 2KI PbI2 + 2KNO3
yellow ppt
1. Solid Formation (precipitation)3NaOH + AlCl3 Al(OH)3 + 3NaCl
white ppt
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Chapter 5 2. Understanding Chemical Changes
Evidence of a Chemical Reaction, continued
Chapter 5 2. Understanding Chemical Changes
Evidence of a Chemical Reaction, continued
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Chapter 5 2. Understanding Chemical Changes
Evidence of a Chemical Reaction, continued
3. Gas ReleaseCaCO3 + 2HCl CaCl2 + CO2 + H2O
4. Heat Exchange2Al + Fe2O3 2Fe + Al2O3 + Energy
Chapter 5 2. Understanding Chemical Changes
Evidence of a Chemical Reaction, continued
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Chapter 5 2. Understanding Chemical Changes
Evidence of a Chemical Reaction, continued
Chapter 5 2. Understanding Chemical Changes
Section Review
1. What are the indicators for the chemical reaction of
combustion of gasoline in engines?
1. Gas formation, heat exchange, color change
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Chapter 5 2. Understanding Chemical Changes
Section Review
2. Which observation does NOT indicate that a chemical
reaction has occurred?
A. formation of a precipitate
B. production of a gas
C. evolution of energy
D. change in total mass of substances
Chapter 5 2. Understanding Chemical Changes
Section Review
2. Which observation does NOT indicate that a chemical
reaction has occurred?
A. formation of a precipitate
B. production of a gas
C. evolution of energy
D. change in total mass of substances
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Chapter 5 2. Understanding Chemical Changes
Section Review
3. A solid produced by a chemical reaction that then
separates from the solution is called a(n) _________ .
3. A solid produced by a chemical reaction that then
separates from the solution is called a(n) precipitate.
Chapter 5
• Write some word equations that represent the chemical changes given below.
Baking a cake, souring milk, burning a piece of paper, rusting iron
Warm up
3. Chemical Equations
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Chapter 5 3. Chemical Equations
• A chemical equation shows the chemical formulas
and relative amounts of all reactants and products.
• A substance that undergoes a reaction is called a
reactant.
• When reactants undergo a chemical change, each
new substance formed is called a product.
methane + oxygen carbon dioxide + water
CH4 + O2 CO2 + H2O
Chapter 5 3. Chemical Equations
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Chapter 5 3. Chemical Equations
Chapter 5 3. Chemical Equations
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Chapter 5 3. Chemical Equations
• In chemical reactions following properties remain constant.
• Types and number of reacting atoms,
• Total mass of substances.
• Total number of protons, neutrons, and electrons.
• In chemical reactions following properties may change.
• Number of electrons and electronic configurations of
atoms.
• Total number of moles, molecules and volumes.
• Physical properties like color, odor, taste and states.
Chapter 5 3. Chemical Equations
Section Review
1. Knowledge about what products are produced in a
chemical reaction is obtained by
A. inspecting the chemical equation.
B. balancing the chemical equation.
C. laboratory analysis.
D. writing a word equation.
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Chapter 5 3. Chemical Equations
Section Review
1. Knowledge about what products are produced in a
chemical reaction is obtained by
A. inspecting the chemical equation.
B. balancing the chemical equation.
C. laboratory analysis.
D. writing a word equation.
Chapter 5 3. Chemical Equations
Section Review
2. A chemical reaction has NOT occurred if the
products have
A. the same mass as the reactants.
B. less total bond energy than the reactants.
C. more total bond energy than the reactants.
D. the same chemical properties as the reactants.
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Chapter 5 3. Chemical Equations
Section Review
2. A chemical reaction has NOT occurred if the
products have
A. the same mass as the reactants.
B. less total bond energy than the reactants.
C. more total bond energy than the reactants.
D. the same chemical properties as the reactants.
Chapter 5 3. Chemical Equations
Section Review
3. Which word equation represents the reaction that
produces water from hydrogen and oxygen?
A. Water is produced from hydrogen and oxygen.
B. Hydrogen plus oxygen yields water.
C. H2 + O2 water.
D. Water can be separated into hydrogen and oxygen.
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Chapter 5 3. Chemical Equations
Section Review
3. Which word equation represents the reaction that
produces water from hydrogen and oxygen?
A. Water is produced from hydrogen and oxygen.
B. Hydrogen plus oxygen yields water.
C. H2 + O2 water.
D. Water can be separated into hydrogen and oxygen.
Chapter 5 3. Chemical Equations
Section Review
4. How would oxygen be represented in the formula
equation for the reaction of methane and oxygen to
yield carbon dioxide and water?
A. oxygen
B. O2
C. O
D. O3
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Chapter 5 3. Chemical Equations
Section Review
4. How would oxygen be represented in the formula
equation for the reaction of methane and oxygen to
yield carbon dioxide and water?
A. oxygen
B. O2
C. O
D. O3
Chapter 5 3. Chemical Equations
Section Review
5. In an equation, the symbol for a substance in water
solution is followed by
A. (l).
B. (g).
C. (aq).
D. (s).
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Chapter 5 3. Chemical Equations
Section Review
5. In an equation, the symbol for a substance in water
solution is followed by
A. (l).
B. (g).
C. (aq).
D. (s).
Chapter 5 3. Chemical Equations
Section Review
6. Photosynthesis is the process plants use to make
glucose and oxygen gas from carbon dioxide and
water only in the presence of light. Write a word
equation for the reaction.
6. carbon dioxide + water glucose + oxygensunlight
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Chapter 5 3. Chemical Equations
Section Review
7. Solid CuO and gaseous CH4 are combined and
heated. The products are solid copper, carbon
dioxide gas, and water vapor.
7. Consider the reaction;
4CuO(s) + CH4(g) 4Cu(s) + CO2(g) + 2H2O(g).
Describe this reaction in terms of states of matter and
the conditions required for the reaction to happen.
Chapter 5
• Describe the mass change in the burning of a wood.
• Think a way that proves mass does not change in
chemical reactions.
Warm up
4. Balancing Chemical Equations
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Chapter 5 4. Balancing Chemical Equations
Chapter 5
• The law of conservation of mass states that mass is
neither created nor destroyed during chemical reactions.
Total mass is constant in a chemical reaction. This is
known as Lavoisier’s Law.
Conservation of Mass
4. Balancing Chemical Equations
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Chapter 5
Conservation of Mass, continued
4. Balancing Chemical Equations
Chapter 5
• The number of atoms for each element must be the same
on the reactants’ side and on the products’ side.
• A coefficient multiplies the number of atoms of each
element in the formula that follows.
4. Balancing Chemical Equations
• H2O: 2 hydrogen atoms, 1 oxygen atom
• 2H2O: 4 hydrogen atoms, 2 oxygen atoms
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Chapter 5 4. Balancing Chemical Equations
Chapter 5
• Below are some tips for balancing equations:
• Take the coefficients of the most complex compound
as one.
• Balance the elements found in this most complex
compound first.
• Balance the elements last that is free in reactants or
products.
• Balance oxygen and hydrogen atoms at the end.
• Never change the subscripts.
4. Balancing Chemical Equations
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Chapter 5 4. Balancing Chemical Equations
Sample Problem ABalance the equation for the reaction of iron(III) oxide with hydrogen to form iron and water.
Sample Problem A Solution
Fe2O3 + H2 Fe + H2O1 3 32
Chapter 5 4. Balancing Chemical Equations
Sample Problem BBalance the equation below with integer numbers.
Na + H2O NaOH + H2
Sample Problem B Solution
Na + H2O NaOH + H21 1 ½ 1
Then,2Na + 2H2O 2NaOH + 1H2
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Chapter 5 4. Balancing Chemical Equations
Sample Problem CAluminum reacts with arsenic acid, HAsO3, to form H2
and aluminum arsenate. Write a balanced equation for this reaction.
Sample Problem C
Al + HAsO3 H2 + Al(AsO3)3 132
31
Then,2Al + 6HAsO3 3H2 + 2Al(AsO3)3
Chapter 5 4. Balancing Chemical Equations
Sample Problem DFind the unknown substance represented by X in the following balanced equation.
4FeS2 + 11O2 2Fe2O3 + 8X
Sample Problem D
4FeS2 + 11O2 2Fe2O3 + 8SO2
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Chapter 5 4. Balancing Chemical Equations
Chapter 5
Section Review
1. What is the small whole number that appears in front
of a formula in a chemical equation?
A. a subscript
B. a superscript
C. a ratio
D. a coefficient
4. Balancing Chemical Equations
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Chapter 5
Section Review
1. What is the small whole number that appears in front
of a formula in a chemical equation?
A. a subscript
B. a superscript
C. a ratio
D. a coefficient
4. Balancing Chemical Equations
Chapter 5
Section Review
2. According to the law of conservation of mass, the
total mass of the reacting substances is
A. always more than the total mass of the products.
B. always less than the total mass of the products.
C. sometimes more and sometimes less than the total
mass of the products.
D. always equal to the total mass of the products.
4. Balancing Chemical Equations
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Chapter 5
Section Review
2. According to the law of conservation of mass, the
total mass of the reacting substances is
A. always more than the total mass of the products.
B. always less than the total mass of the products.
C. sometimes more and sometimes less than the total
mass of the products.
D. always equal to the total mass of the products.
4. Balancing Chemical Equations
Chapter 5
Section Review
3. A chemical equation is balanced when the
A. coefficients of the reactants equal the coefficients of
the products.
B. same number of each kind of atom appears in the
reactants and in the products.
C. products and reactants are the same chemicals.
D. subscripts of the reactants equal the subscripts of the
products.
4. Balancing Chemical Equations
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Chapter 5
Section Review
3. A chemical equation is balanced when the
A. coefficients of the reactants equal the coefficients of
the products.
B. same number of each kind of atom appears in the
reactants and in the products.
C. products and reactants are the same chemicals.
D. subscripts of the reactants equal the subscripts of
the products.
4. Balancing Chemical Equations
Chapter 5
Section Review
4. When the equation Fe3O4 + Al Al2O3 + Fe is
correctly balanced, what is the coefficient of Fe?
A. 3 B. 4 C. 6 D. 9
4. Balancing Chemical Equations
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Chapter 5
Section Review
4. When the equation Fe3O4 + Al Al2O3 + Fe is
correctly balanced, what is the coefficient of Fe?
A. 3 B. 4 C. 6 D. 9
4. Balancing Chemical Equations
Chapter 5
Section Review
5. Which coefficients correctly balance the formula
equation
NH4NO2(s) N2(g) + H2O(l)?
A. 1, 2, 2
B. 1, 1, 2
C. 2, 1, 1
D. 2, 2, 2
4. Balancing Chemical Equations
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Chapter 5
Section Review
5. Which coefficients correctly balance the formula
equation
NH4NO2(s) N2(g) + H2O(l)?
A. 1, 2, 2
B. 1, 1, 2
C. 2, 1, 1
D. 2, 2, 2
4. Balancing Chemical Equations
Chapter 5
Section Review
6. What is the formula of the compound represented by
X in the following balanced equation?
2Ag + 2H2SO4 Ag2SO4 + SO2 + 2X
4. Balancing Chemical Equations
6. H2O
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Chapter 5
Section Review
7. How many grams of water is produced from 8 g
hydrogen and 64 g oxygen gases?
4. Balancing Chemical Equations
7. 2H2 + O2 2H2OFollowing the conservation of mass lawmreactants= mproducts
8 g + 64 = 72 g H2O will be produced
Chapter 5
• Describe the following terms
Synthesis, Analysis, Decomposition, Combination,
Oxidation, Combustion, Neutralization, Displacement
• What kind of reactions exist in human body?
Warm up
5. Types of Chemical Reactions
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Chapter 5
• Whenever two or more substances combine to form a single product, the reaction is called a synthesisreaction.
• Combination reactions can be illustrated;
A + B AB
1. Combination (Synthesis) Reactions
5. Types of Chemical Reactions
• Here are some examples;C + O2 CO2
4Fe + 3O2 2Fe2O3
CaO + H2O Ca(OH)2
N2 + 3H2 2NH3
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Chapter 5
1. Combination (Synthesis) Reactions, continued
5. Types of Chemical Reactions
Chapter 5
1. Combination (Synthesis) Reactions, continued
5. Types of Chemical Reactions
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Chapter 5
1. Combination (Synthesis) Reactions, continued
5. Types of Chemical Reactions
Chapter 5
1. Combination (Synthesis) Reactions, continued
5. Types of Chemical Reactions
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Chapter 5
1. Combination (Synthesis) Reactions, continued
5. Types of Chemical Reactions
Chapter 5
1. Combination (Synthesis) Reactions, continued
5. Types of Chemical Reactions
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Chapter 5
1. Combination (Synthesis) Reactions, continued
5. Types of Chemical Reactions
Chapter 5
• In a decomposition reaction a single compound breaks down, often with the input of energy, into two or more elements or simpler compounds.
• Decomposition reactions can be illustrated;
AB A + B
2. Decomposition (Analysis) Reactions
5. Types of Chemical Reactions
• Here are some examples;
NH4NO3 N2O + 2H2O
2H2O2 2H2O + O2
2NaCl 2Na + Cl2
PCl5 PCl3 + Cl2
Electricity
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Chapter 5
2. Decomposition (Analysis) Reactions, continued
5. Types of Chemical Reactions
Chapter 5
• In a displacement reaction a single element reacts with a compound and displaces another element from the compound.
• Displacement reactions can be illustrated;
A + BC B + AC
3. Single Displacement Reactions
5. Types of Chemical Reactions
• Single displacement reactions mostly take place due to activity differences of elements. A more active element displaces a less active one.
Zn(s) + CuSO4(aq) Cu(s) + ZnSO4(aq)
Fe(s) + NaCl(aq) No reaction
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Chapter 5
3. Single Displacement Reactions, continued
5. Types of Chemical Reactions
Chapter 5
3. Single Displacement Reactions, continued
5. Types of Chemical Reactions
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Chapter 5
3. Single Displacement Reactions, continued
5. Types of Chemical Reactions
Chapter 5
3. Single Displacement Reactions, continued
5. Types of Chemical Reactions
Activity of Some Metals
Li Rb K Ba Sr Ca Na Mg Al Mn Zn Cr Cd Fe Co Ni Sn Pb H Cu Hg Ag Pt Au
Activity Decreases
Activity of Some Nonmetals
F Cl Br I Activity Decreases
• Some examples;
NaBr(aq) + Cl2(g) 2NaCl(aq) + Br2(g)
Ca(s) + 2H2O Ca(OH)2(aq) + H2(g)
Mg(s) + 2CuCl(aq) MgCl2(aq) + 2Cu(s)
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Chapter 5
3. Single Displacement Reactions, continued
5. Types of Chemical Reactions
Chapter 5
3. Single Displacement Reactions, continued
5. Types of Chemical Reactions
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Chapter 5
3. Single Displacement Reactions, continued
5. Types of Chemical Reactions
Chapter 5
• In a double-displacement reaction two compounds in aqueous solution appear to exchange ions and form two new compounds.
• One of the products must be a solid precipitate, a gas, or a molecular compound, such as water.
• Double displacement reactions can be illustrated;
AB + CD AD + CB
4. Double Displacement (Metathesis) Reactions
5. Types of Chemical Reactions
• Some examples;
HCl(aq) + NaOH(aq) HOH(l) + NaCl(aq)
Pb(NO3)2(aq) + K2CrO4(aq) PbCrO4(ppt) + 2KNO3(aq)
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Chapter 5
4. Double Displacement (Metathesis) Reactions
5. Types of Chemical Reactions
Chapter 5 5. Types of Chemical Reactions
4. Double Displacement (Metathesis) Reactions
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Chapter 5
• A reaction which absorbs energy is endothermic reactionand which release energy is exothermic reaction.
5. Endothermic and Exothermic Reactions
5. Types of Chemical Reactions
• Some examples;
Ca(s) + 2H2O(l) Ca(OH)2(aq) + H2(g) + Energy
Exothermic Reaction
H2O(l) + Energy H2(g) + O2(g)
Endothermic Reaction
Chapter 5
5. Endothermic and Exothermic Reactions
5. Types of Chemical Reactions
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Chapter 5
5. Endothermic and Exothermic Reactions
5. Types of Chemical Reactions
Chapter 5
• A combustion reaction is a reaction of a carbon-based
compound with oxygen.
6. Combustion Reactions
5. Types of Chemical Reactions
• Some examples;
C3H8 + 5O2 3CO2 + 4H2O + heat
CH3CH2OH + 3O2 2CO2 + 3H2O + heat
C6H12O6 + 6O2 6CO2 + 6H2O + heat
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Chapter 5
6. Combustion Reactions
5. Types of Chemical Reactions
Chapter 5
6. Combustion Reactions
5. Types of Chemical Reactions
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Chapter 5
6. Combustion Reactions, continued
5. Types of Chemical Reactions
Chapter 5
6. Combustion Reactions, continued
5. Types of Chemical Reactions
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Chapter 5 5. Types of Chemical Reactions
Chapter 5
Section Review
1. In what kind of reaction do two or more substances combine to form a new compound?
A. decomposition reaction
B. double-displacement reaction
C. ionic reaction
D. synthesis reaction
5. Types of Chemical Reactions
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Chapter 5
Section Review
1. In what kind of reaction do two or more substances combine to form a new compound?
A. decomposition reaction
B. double-displacement reaction
C. ionic reaction
D. synthesis reaction
5. Types of Chemical Reactions
Chapter 5
Section Review
2. In what kind of reaction does a single compound produce two or more simpler substances?
A. decomposition reaction
B. displacement reaction
C. synthesis reaction
D. ionic reaction
5. Types of Chemical Reactions
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Chapter 5
Section Review
2. In what kind of reaction does a single compound produce two or more simpler substances?
A. decomposition reaction
B. displacement reaction
C. synthesis reaction
D. ionic reaction
5. Types of Chemical Reactions
Chapter 5
Section Review
3. The reaction 2KClO3(s) 2KCl(s) + 3O2(g) is a(n)
A. synthesis reaction.
B. combustion reaction.
C. decomposition reaction.
D. ionic reaction.
5. Types of Chemical Reactions
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Chapter 5
Section Review
3. The reaction 2KClO3(s) 2KCl(s) + 3O2(g) is a(n)
A. synthesis reaction.
B. combustion reaction.
C. decomposition reaction.
D. ionic reaction.
5. Types of Chemical Reactions
Chapter 5
Section Review
4. In what kind of reaction does one element replace a
similar element in a compound?
A. displacement reaction
B. decomposition reaction
C. combustion
D. ionic reaction
5. Types of Chemical Reactions
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Chapter 5
Section Review
4. In what kind of reaction does one element replace a
similar element in a compound?
A. displacement reaction
B. decomposition reaction
C. combustion
D. ionic reaction
5. Types of Chemical Reactions
Chapter 5
Section Review
5. The reaction Cl2(g) + 2KBr(aq) 2KCl(aq) + Br2(l)
is a(n)
A. synthesis reaction.
B. displacement reaction.
C. ionic reaction.
D. combustion reaction.
5. Types of Chemical Reactions
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Chapter 5
Section Review
5. The reaction Cl2(g) + 2KBr(aq) 2KCl(aq) + Br2(l)
is a(n)
A. synthesis reaction.
B. displacement reaction.
C. ionic reaction.
D. combustion reaction.
5. Types of Chemical Reactions
Chapter 5
Section Review
6. A precipitate forms in a double-displacement reaction
when
A. hydrogen gas reacts with a metal.
B. positive ions combine with negative ions.
C. water boils out of the solution.
D. a gas escapes.
5. Types of Chemical Reactions
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Chapter 5
Section Review
6. A precipitate forms in a double-displacement reaction
when
A. hydrogen gas reacts with a metal.
B. positive ions combine with negative ions.
C. water boils out of the solution.
D. a gas escapes.
5. Types of Chemical Reactions
Chapter 5
Section Review
7. I. K2CO3 + Cr II. ZnI2 + Br2 III. CuSO4 + Zn
Which of the above reaction(s) take place underappropriate conditions?
A. I only B. II only C. II and III D. I and llI
5. Types of Chemical Reactions
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Chapter 5
Section Review
7. I. K2CO3 + Cr II. ZnI2 + Br2 III. CuSO4 + Zn
Which of the above reaction(s) take place underappropriate conditions?
A. I only B. II only C. II and III D. I and Ill
5. Types of Chemical Reactions
Chapter 5
Section Review
8. Which of the following is a combustion reaction?
A. N2 + 3H2 2NH3
B. H2O H2 + 1/2O2
C. CaCO3 + heat CaO + CO2
D. C3H8 + 5O2 3CO2 + 4H2O
5. Types of Chemical Reactions
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Chapter 5
Section Review
8. Which of the following is a combustion reaction?
A. N2 + 3H2 2NH3
B. H2O H2 + 1/2O2
C. CaCO3 + heat CaO + CO2
D. C3H8 + 5O2 3CO2 + 4H2O
5. Types of Chemical Reactions
End of the chapter