Chemical Equations and Reactions
Name:
Date:
Period:
1. A chemical equation is balanced if there is an __________________ number of each kind of
_____________________ on both sides of the equation.
2. Determine the number of atoms of each kind in each of the following:
a. CaCO3
_____ Ca, _____ C, _____ O
b. (NH4)2SO4
_____ N, _____ H, _____ S, _____ O
c. 3 H2O
_____ H, _____ O
d. 4 Mg(OH)2
_____ Mg, _____ O, _____ H
e. 5 Ba(NO3)2
_____ Ba, _____ N, _____ O
3. Now look at the following chemical equations. Count the number of atoms of each element on the
reactant and product side. Determine if the statement is a balanced equation.
a. 2 Na + 2 H2O

2 NaOH + H2
Reactants
Products
_______
Na
_______
_______
H
_______
_______
O
_______
b. 4 NH3 + 6 NO

5 N2 + 6 H2O
Reactants
Products
_______
N
_______
_______
H
_______
_______
O
_______
c. NaCl + F2
Balanced? Yes _____ No _____

Balanced? Yes _____ No _____
NaF + Cl2
Reactants
Products
_______
Na
_______
_______
Cl
_______
_______
F
_______
Balanced? Yes _____ No _____
d. 3 NaBr + H3PO4 2 HBr + Na3PO4
_______
Na
_______
_______
Br
_______
_______
H
_______
_______
P
_______
_______
O
_______
Balanced? Yes _____ No _____
e. N2H4 + N2O4  3 N2 + 4 H2O
Balanced? Yes _____ No _____
f. 2 Bi + 3 F2  2 BiF3
Balanced? Yes _____ No _____
g. Al + Ni(NO3)2  Al(NO3)3 + Ni
Balanced? Yes _____ No _____
h. 3 NaBH4 + 4 BF3  2 B2H6 + 3 NaBF4
Balanced? Yes _____ No _____
i. 4 C3H5(NO3)3  6 N2 + O2 + 12 CO2 + 10 H2O
Balanced? Yes _____ No _____
j. Ca10F2(PO4)6 + 7 H2SO4  2 HF + 3 Ca(H2PO4)2 + 7 CaSO4
Balanced? Yes _____ No _____
Directions: Balance the following reactions. Place a “B” at the end of any that are balanced as written.
4. _____ Zn + _____O2
→
5. _____HI → _____H2
+
_____ZnO
_____I2
6. _____B + _____F2 → _____BF3
7. _____N2 + _____H2 → _____NH3
8. _____Fe + _____H2O → _____Fe3O4 + _____H2
9.
H2SO4 →
BaCl2 +
O2 →
BaSO4 +
P4O10
10.
P +
11.
KClO3 →
12.
C3H8
13.
Cu +
AgNO3 →
14.
Te +
H2O →
15.
La(NO3)3 +
16.
RhO3 →
17.
Hf +
N2 →
18.
Ga +
H2SO4 →
19.
PdCl2 +
HNO3 →
20.
RbBr +
AgCl →
21.
PaI5 →
22.
Fe2O3 →
23.
Cu +
Cl2 →
24.
Na +
O2 →
Na2O
25.
H2 +
O2 →
H2O
26.
Na2SO4 +
CaCl2 →
27.
Al2O3 →
Al +
28.
C2H6 +
O2 →
CO2 +
29.
SO3 +
H2O →
H2SO4
30.
SiCl4 →
31.
C +
KCl +
O2
O2 →
+
CO2 +
TeO +
RhO +
Ag
H2
La(OH)3 +
NaNO3
O2
Hf3N4
Pa +
Ga2(SO4)3 +
H2
Pd(NO3)2 +
AgBr +
HCl
RbCl
I2
Fe
Si +
H2O
Cu(NO3)2 +
NaOH →
H2 →
HCl
+
O2
CuCl2
CaSO4 +
O2
Cl2
CH4
H2O
NaCl
32.
Br2 +
NaI →
NaBr +
I2
33.
Zn +
HCl →
ZnCl2 +
H2
34.
H2S +
O2 →
35.
Ba(NO3)2 +
36.
C5H12 +
O2 →
CO2 +
37.
HgO →
Hg +
O2
38.
H2SO4 +
Pb +
39.
C6H12O6 +
40.
Ca +
41.
C6H12O6 →
C2H5OH +
42.
HC2H3O2 +
NaHCO3 →
H2O +
SO2
Na2SO4 →
BaSO4 +
H2O
PbO2 →
O2 →
H2 O →
NaNO3
PbSO4 +
CO2 +
H2O
H2O
Ca(OH)2 +
H2
CO2
CO2 +
NaC2H3O2 +
H2O
Challenging:
O2 →
H2 O
Na2SO4 +
43.
NaCl +
SO2 +
44.
Fe2O3 +
CO →
45.
Ca3(PO4)2 +
C +
46.
C
+
O2
47.
Mg
+
48.
CuO
+
C
→
Cu
49.
NH3
+
O2
→
NO2
50.
O3
51.
Cu
52.
C8H18
53.
Sn
CO2 +
HCl
Fe
SiO2 →
CaSiO3 +
CO +
P4
More:
→
CO
O2 → MgO
→
+
CO2
+
H2O
O2
+
+
+
→
AgNO3
O2
HF
→
Cu(NO3)2
+
Ag
CO2
+
H2O
+
H2
→
SnF2
+
HCl
54.
Al(OH)3
55.
Ca3(PO4)2
56.
Fe
57.
NH4NO3
→
58.
C
Al2O3
59.
N2
60.
BaCl2
61.
C6H12O6
62.
Al
63.
CO2
64.
NO
65.
Al
+
66.
HgO
→
67.
KClO3
68.
CaBr2
69.
H2O
+
+
+
Li3PO4
73.
Ca(OH)2
74.
Al2(SO4)3
O2
+
+
H2O
Fe2O3
+
→
CO2
+
P
→
HNO3
Ca(OH)2
→
H2O
+
Ca3P2
C
Li
+
Al2O3
Li2CO3
→
→
+
H2O
H2
O2
→
O2
NaCl
O2
+
Fe
→
+
+
Al2(SO4)3
+
Na3P
+
+
Fe
→
+
CO2
NH3
KCl
+
CaSO4
CO2
BaSO4
→
→
Hg
72.
+
→
H2SO4
C2H6
Al
→
LiOH
H2
71.
H2O
→
O2
+
+
NH3
Fe2O3
C6H12O6
P
→
→
→
H2O
H3PO4
+
Na2SO4
+
+
Fe3O4
+
+
→
N2O
+
70.
75.
→
H2
+
AlCl3
H2SO4
O2
+
→
P2O5
+
+
NaBr
H2
H2 O
+
+
H2O
O2
Ca(NO3)2
→
Al(OH)3
+
H2O
+
CaSO4
76.
N2
+
77.
CH4
+
78.
Fe2O3
+
79.
AsCl3
80.
C3H8
81.
K2S
82.
Al
83.
H2S
84.
Fe
85.
Ca(NO3)2
→
H2
→
O2
+
→
+
KOH
S8
+
H2O
+
H2O
As2S3
+
CO2
→
CuBr2
O2
+
→
→
O2
+
Fe
H2S
+
CO2
→
H2
+
+
NH3
+
CuS
HCl
H 2O
+
KBr
Al2O3
→
→
Na3PO4 →
H2 O
+
K2S
Ca3(PO4)2
+
NaNO3
FeS
DIRECTIONS: Refer to the unbalanced chemical equation below to answer the following questions.
Write your answers in the space provided.
Al(NO3)3 + FeCl2
→ Fe(NO3)2 + AlCl3
86. Write the names of the reactants in this equation:
_______________________________________
_____________________________________
87. Write the names of the products in this equation:
_______________________________________
_____________________________________
88. Balance the equation above. What is the coefficient for Al(NO3)3? ___________
What is the coefficient for FeCl2?
___________
What is the coefficient for Fe(NO3)2? ___________
What is the coefficient for AlCl3?
___________
89. How many oxygen atoms are there on each side of the balanced equation? __________
90. What should you do if an equation you have written cannot be balanced? ________________________
__________________________________________________________________________________
91. How is balancing an equation related to the Law of Conservation of Matter? _____________________
___________________________________________________________________________________
92. Describe the correct way to balance an equation: ___________________________________________
___________________________________________________________________________________
93. How are the physical states of the reactants and products indicated in a chemical equation? __________
___________________________________________________________________________________
Write complete equations for the following using the state symbols!
Remember the seven diatomic elements !!!
93a.Two molecules of solid sodium chloride decompose when exposed to an electric current into two atoms
of sodium metal and 1 molecule of chlorine gas.
93b.One molecule in a barium chloride solution reacts with one molecule in a sodium sulfate solution to
produce 1 molecule of solid barium sulfate and 2 molecules of sodium chloride in solution.
93c.Two molecule of solid potassium chlorate, when heated, decompose into two molecules of solid
potassium chloride and 3 molecules of oxygen gas.
93d. One molecule of solid calcium carbonate decomposes when heated into one molecule of solid calcium
oxide and 1 molecule of carbon dioxide gas.
93e. Two molecules of solid aluminum hydroxide decomposes when heated into one molecule of solid
aluminum oxide and three molecules of water vapor .
93f. One atom of zinc metal when mixed with two molecules of a hydrochloric acid solution react and
produce one molecule of zinc chloride in solution and one molecule of hydrogen gas.
DIRECTIONS: Write balanced chemical equations for each of the following reactions. Indicate the
physical state of the reactants and products (ex – s,g,l,aq).
94. Hydrogen gas reacts with nitrogen gas to produce ammonia gas (NH3).
95. Hydrogen bromide gas reacts with oxygen gas to produce liquid water and bromine gas.
96. When a solid piece of magnesium is placed in hydrochloric acid, hydrogen gas bubbles off and
magnesium chloride is left in solution.
97. Hydrochloric acid can be added to calcium carbonate to produce calcium chloride in solution, carbon
dioxide gas and water.
98. Solid carbon disulfide can be used to form carbon dioxide gas and sulfur dioxide gas when it reacts
with oxygen gas.
99. Solid manganese dioxide reacts with hydrochloric acid to produce manganese (II) chloride, liquid
water and chlorine gas.
100. Write the equation for the following reaction: ammonia, NH3, reacts with hydrochloric acid to form
ammonium chloride.
101. When heated, calcium carbonate decomposes to form calcium oxide and carbon dioxide. Write the
equation for this reaction:
102. Write the equation for the following reaction: barium oxide reacts with water to form barium
hydroxide.
103. Acetaldehyde, CH3CHO, decomposes to form methane, CH4, and carbon monoxide. Write the
equation for this reaction.
104. Write the equation for the following reaction: zinc reacts with copper (II) nitrate to form zinc nitrate
and copper.
105. When heated, calcium sulfite decomposes to form calcium oxide and sulfur dioxide. Write an equation
for this reaction.
106. Write the equation for the following reaction: iron metal reacts with sulfuric acid to form iron (II)
sulfate and hydrogen gas.
107. Azomethane, C2H6N2, decomposes to form ethane, C2H6, and nitrogen gas at 297 °C. Write an
equation for this reaction.
108. Write out the equation for the following reaction: carbon monoxide reacts with chlorine gas to form
phosgene, COCl2.
109. Manganese (II) iodide decomposes when exposed to light to form manganese and iodine. Write an
equation for this reaction.
110. Write a balanced chemical equation for the reaction in which dinitrogen pentoxide reacts with water to
form nitric acid.
111. Magnesium reacts with titanium (IV) chloride to produce magnesium chloride and titanium. Write the
balanced equation for this reaction.
112. Write a balanced chemical equation for the reaction in which carbon reacts with zinc oxide to produce
zinc and carbon dioxide.
113. Bromine reacts with sodium iodide to form sodium bromide and iodine. Write the balanced equation
for this reaction.
114. Write a balanced chemical equation for the reaction in which phosphorus trichloride reacts with
chlorine gas to produce phosphorus pentachloride.
115. Phosphorus reacts with bromine to produce phosphorus tribromide. Write the balanced equation for
this reaction.
116. Calcium hydride reacts with water to produce calcium hydroxide and hydrogen gas. Write the
balanced equation for this reaction.
117. Write the balanced chemical equation for the reaction in which sulfuric acid reacts with potassium
hydroxide to produce potassium sulfate and water.
118. Write a balanced chemical equation for the reaction in which propane, C3H8, reacts with oxygen gas
to produce carbon dioxide and water.
119. Benzene, C6H6, reacts with oxygen gas to produce carbon dioxide and water. Write the balanced
equation for this reaction.
Synthesis Reactions
Equations
Chemical reactions are happening around you all the time. A match burns. A car rusts. Food spoils.
Leaves decay. These are just a few chemical reactions.
Probably the most important chemical reactions take place in your body. They are happening this very
moment. Digestion is a chemical process. So is respiration. In every one of your trillions of cells, chemical
reactions are taking place all the time. Life depends upon chemical reactions.
There are several kinds of chemical reactions. One kind is a synthesis reaction. “Synthesis” means putting
together. A synthesis reaction combines substances, usually elements (but sometimes smaller compounds), to
form a new, larger compound. When the compound forms, we say it has been synthesized. Below is a “model”
of a synthesis reaction.
A
+
B
→
AB
Element + Element → Compound
1. RUSTING When iron rusts, it combines with oxygen.
→
4Fe + 3O2
iron
+ oxygen →
2Fe2O3
iron oxide (rust)
link up

to form  Compound
Element + Element
2. THE BURNING OF CARBON Charcoal is made of the element carbon, C. When carbon burns, it
combines with oxygen. This produces the gas carbon dioxide, CO2.
C
+ O2
carbon
→
+ oxygen
Element + Element
CO2
→
carbon dioxide
link up

to form  Compound
A synthesis reaction is like any other kind of chemical reaction. No matter is created or destroyed. The atoms
just change their arrangement.
Equation I:
CO2 + C → 2CO2
Equation II:
CO2 + H2O → H2CO3
120. How is Equation I different from the other synthesis equations seen in this packet? ________________
___________________________________________________________________________________
121. 1. How is Equation II different from the other synthesis equations seen in this packet? _____________
___________________________________________________________________________________
122. Look at the equations below. Identify the synthesis reactions by placing a check (√) next to it.
Equation
a.
2K + Br2 → 2KBr
b.
2H2O → 2H2 + O2
c.
NaCl → Na + Cl
d.
4Au + 3O2 → 2Au2O3
e.
2Na + 2HCl → 2NaCl + H2
f.
Cu + Br2 → CuBr2
g.
ZnSO4 + FeCl2 → ZnCl2 + FeSO4
h.
2Na + Br2 → 2NaBr
i.
2HgO → 2Hg + O2
j.
CH4 + 2O2 → CO2 + 2H2O
A Synthesis
Reaction
Not a Synthesis
Reaction
Decomposition Reaction
Synthesis reactions build compounds. Anything that can be built can also ne taken apart. The breakdown of a
compound into simpler substances is called decomposition. Decomposition is a chemical process.
Let’s look at two examples:
1. Common table salt (sodium chloride) is a compound composed of the elements sodium and chlorine. It
can be melted, and if electricity is passed through melted sodium chloride, it decomposes. It changes
back into atoms of sodium and chlorine. Here is the reaction:
electricity

 2Na
breaks it into
2NaCl
sodium chloride
(compound)
sodium
(element)
+ Cl
chlorine
(element)
The decomposition of a compound by means of electricity is called electrolysis. Only certain
compounds can be decomposed by electrolysis. Usually these compounds are liquids.
2. Potassium chlorate (KClO3) is a compound composed of potassium, chlorine and oxygen. Heat
decomposes potassium chlorate into oxygen and potassium chloride (a simpler compound.) Here is the
reaction:
2KClO3
potassium chlorate
(compound)
heat

breaks down into 
2KCl
+
potassium chloride
(a simpler compound)
3O2
oxygen
(element)
Notice that the decomposition is not complete, the oxygen has been separated, but the potassium and
chlorine are still joined in the compound, potassium chloride. Another kind of decomposition reaction
can separate potassium chloride into its elements. Only certain compounds can be decomposed with
heat
Look at the diagram above and previous page. Electrolysis decomposes water. This is the equation for the
reaction:
2H2O → 2H2
+ O2
water → hydrogen + oxygen
Equation
a.
CuCl2 → Cu + Cl2
b.
3Hf + 2N2 → Hf3N4
c.
Zn + 2HCl → ZnCl2 + H2
d.
C3H8 + 5O2 → 4H2O + 3CO2
e.
2NaOH → 2Na + O2 + H2
f.
Fe + S → FeS
g.
CaCl2 + FeSO4 → Ca SO4 + FeCl2
h.
4P + 5O2 → 2P2O5
i.
3CuCl2 + 2Al → 2AlCl3 + 3Cu
A Synthesis
Reaction
A Decomposition
Reaction
Neither
Ca(OH)2 → CaO + H2O
j.
170. Identifying Synthesis and Decomposition Reactions:
Matching:
______ 123. synthesis reaction
A) breaks down compounds
______ 124. decomposition reaction
B) uses electricity
______ 125. electrolysis and heat
C) methods of decomposition
______ 126. electrolysis
D) simpler than a compound
______ 127. an element
E) builds compounds
Short Answer:
128. Does boiling decompose water? ________________
129. What does boiling do to water? _________________________________________________________
___________________________________________________________________________________
Series of Metals
Element
Lithium
Potassium
Barium
Calcium
Sodium
Magnesium
Aluminum
Manganese
Zinc
Chromium
Iron
Cobalt
Nickel
Tin
Lead
Hydrogen*
Copper
Mercury
Silver
Platinum
Gold
Ease of oxidation increases
Activity
* Hydrogen is included in the activity series of metals because it has a positive oxidation number.
Single & Double Replacement & Combustion Packet
In a Single Replacement Reaction a free element takes the place of or replaces another element that is part of a
compound. The element that was replaced is now “free.”
A
+
free element
BC
→
compound
AC
new compound
+
B
new free element
Let’s study an actual replacement reaction – one between zinc (Zn) and hydrochloric acid (HCl). The zinc is
the “free” element and the hydrochloric acid is the compound.
Zn
+
HCl
→
ZnCl2
The zinc replaces the hydrogen.
+
H2
The hydrogen gas is set free.
The reaction produces a new compound, zinc chloride (ZnCl2), and free hydrogen (H2). Notice that the
elements we started with are the elements we ended with, they are just arranged in a different way. This kind of
reaction is called a single replacement reaction where a free element replaces an element that is part of a
compound.
For example, if you do a simple experiment of placing an iron nail (Fe) in a solution of copper (II) sulfate
(CuSO4), you will see that after a few minutes the nail is coated with copper metal. Here is the equation for the
reaction:
Fe
+ CuSO4
→
FeSO4
+ Cu
Single Replacement Reactions
Decide whether each reaction is possible. Place a check next to the reactions that are possible.
130. _____
Zn + CuSO4  ZnSO4 + Cu
131. _____ Pb + Mg(NO3)2  Pb(NO3)2 + Mg
132. _____ AgCl2 + Zn  ZnCl2 + Ag
133. _____ 2HCl + Ca  CaCl2 + H2
134. _____ Pt + 2HCl  PtCl2 + H2
Write balanced equations for the following single replacement reactions. Make sure to check that each
reaction is possible on your Activity Series List.
135)
Magnesium metal reacts with hydrochloric acid to produce magnesium chloride and hydrogen gas.
136)
Sodium Chloride reacts with potassium to produce potassium chloride and sodium.
137)
Zinc Sulfate reacts with copper to produce zinc metal and copper (II) sulfate.
138)
Cobalt (II) oxide reacts with aluminum to produce aluminum oxide and cobalt.
139) Nickel (III) sulfate reacts with zinc to produce zinc sulfate and nickel
140. Identify (√) the following reactions as Synthesis (Syn), Decomposition (Decomp),Single Replacement
(SR) or None of These
Equation
a.
C + 2S → CS2
b.
2H2O2 → 2H2 + O2
c.
2Al + 6HCl → 2AlCl3 + 3H2
d.
Li3PO4 + 3NaF → 3LiF + Na3PO4
e.
Zn + PbO → ZnO + Pb
f.
CuCl2 + 2KBr → CuBr2 + 2KCl
g.
CuSO4 + Fe → Cu + FeSO4
h.
2Na + Br2 → 2NaBr
i.
2HgO → 2Hg + O2
j.
C3H8 + 5O2 → 3CO2 + 4H2O
Synthesis
Reaction
Decomposition
Reaction
Single
Replacement
Reaction
None of
These
Double Replacement Reactions:
A double replacement reaction takes place between two compounds. A part of one compound changes
place with a part of the other compound. This produces two new compounds.
AB
+
compound
→
CD
AD
compound
+
new compound
CB
new compound
The positive ion of one compound switches place with the positive part of the other compound. Let’s look at an
example of a double replacement reaction between sodium hydroxide and hydrochloric acid:
NaOH
+
HCl
→
NaCl
+
HOH
The sodium and hydrogen change places and two new compounds form, NaCl and HOH (water).
Example #1) BaCl2
barium
chloride
+
Na2SO4
→
sodium
sulfate
BaSO4 +
barium
sulfate
2NaCl
sodium
chloride
141. Identifying Double Replacement Reactions:
Equation
a.
Mg(OH)2 + 2HCl → MgCl2 + 2H2O
b.
C6H10O5 +H2O → C6H12O6
c.
Na2SO4 + BaCl2 → 2NaCl + BaSO4
d.
3Mg + N2 → Mg3N2
e.
H2SO4 + BaCl2 → 2HCl + BaSO4
f.
CH4 + 2O2 → CO2 + 2H2O
g.
ZnCO3 → ZnO + CO2
h.
CuSO4 + H2S → H2SO4 + CuS
i.
NH4NO3 → 2H2O + N2O
j.
C6H12 + 9O2 → 6CO2 + 6H2O
A Double
Replacement
Reaction
Not a Double
Replacement
Reaction
142. Identify (√) the following reactions as Synthesis (Syn), Decomposition (Decomp), Single Replacement
(SR) , Double Replacement (DR) , Other
Equation
Reaction Type
Syn.
a.
N2 + 3H2 → 2NH3
b.
2Br2 + 2H2O → 4HBr + O2
c.
Mg + 2HCl → MgCl2 + H2
d.
2KBr + H2SO4 → K2SO4 + 2HBr
e.
H2SO3 → H2O + SO2
f.
C6H12O6 + 6O2 → 6CO2 + 6H2O
g.
NaCl + AgNO3 → NaNO3 + AgCl
h.
H2 + Cl2 → 2HCl
i.
H2CO3 → H2O + CO2
j.
C3H8 + 5O2 → 3CO2 + 4H2O
Decomp.
S.R.
D.R.
Other
Combustion Reactions:
A combustion reaction takes place between a hydrocarbon (a compound made of hydrogen and carbon) and
the element oxygen. Oxygen is a diatomic element which means it is so reactive it will bond with itself.
Therefore the oxygen in the air required for combustion is O2. Carbon dioxide and water are always the
products for these types of reactions.
CH
→
+ O2
CO2
hydrocarbon oxygen
+ H2 O
carbon dioxide
water
For example, when natural gas (methane, CH4) is burned with oxygen (O2) carbon dioxide (CO2) and water
(H2O) are produced.
CH4
+ 2O2
methane
→
oxygen
CO2
+ 2H2O
carbon dioxide
water
In another example, cellular respiration, our body metabolizes glucose (C6H12O6) with oxygen (O2) and we
produce carbon dioxide (CO2) and water (H2O). In this case the “hydrocarbon” also contains oxygen.
C6H12O6 + 6O2
glucose
oxygen
→
6CO2
carbon dioxide
+ 6H2O
water
143.
A Combustion
Reaction
Equation
a.
Mg(OH)2 + 2HCl → MgCl2 + 2H2O
b.
2Br2 + 2H2O → 4HBr + O2
c.
C3H8 + 5O2 → 3CO2 + 4H2O
d.
3Mg + N2 → Mg3N2
e.
H2SO4 + BaCl2 → 2HCl + BaSO4
f.
CH4 + 2O2 → CO2 + 2H2O
g.
ZnCO3 → ZnO + CO2
h.
C6H10O5 +H2O → C6H12O6
i.
NH4NO3 → 2H2O + N2O
j.
C6H12 + 9O2 → 6CO2 + 6H2O
Not a
Combustion
Reaction
144. Identify (√) the following reactions as Synthesis (Syn), Decomposition (Decomp), Single Replacement
(SR) , Double Replacement (DR) , Combustion (C)
Reaction Type
Equation
Syn.
a.
CO2 → C + O2
b.
NaCl + AgNO3 → NaNO3 + AgCl
c.
S + Cl2 → SCl2
d.
BaCl2 + 2NaOH → 2NaCl + Ba(OH)2
e.
C3H8 + 5O2 → 3CO2 + 4H2O
f.
CH4 → C + 2H2
g.
Pb(NO3)2 + Mg → Pb + Mg(NO3)2
h.
Mg + 2HCl → MgCl2 + H2
i.
H2SO4 → H2 + S + 2O2
j.
2O2 + N2 → N2O4
k.
3CaBr2 + 2Na3P → Ca3P2 + 6NaBr
l.
2KI + Br2 → 2KBr + I2
m.
C6H12O6 → 6C + 6H2O
Decomp.
S.R.
D.R.
C
n.
C6H12 + 9O2 → 6CO2 + 6H2O
o.
Si + O2 → SiO2
p.
2NaI + Pb(NO3)2 → 2NaNO3 + PbI2
q.
2C8H18 + 25O2 → 16CO2 + 18H2O
r.
H2 + CO + O2 → H2CO3
s.
C6H12O6 + 6O2 → 6CO2 + 6H2O
t.
CS2 + 2F2 → CF4 + 2S
Types of Chemical Reactions
Directions: Label the following reactions as synthesis (S), decomposition (D),
single replacement (SR), double replacement (DR) and combustion (C).
145.
NaCl → Na + Cl2
___________
146.
Na + Cl2 → NaCl
___________
147.
C2H4 + O2 → CO2 + H2O
___________
148.
H2O → H2 + O2
___________
149.
H2 + O2 → H2O
___________
150.
C8H18 + O2 → CO2 + H2O
___________
151.
NaOH + HCl → HOH + NaCl
___________
152.
Na + HCl → H2 + NaCl
___________
153.
K + Cl2 → KCl
___________
154.
K + AgCl → Ag + KCl
___________
155.
C6H12 + O2 → CO2 + H2O
___________
156.
Ca + S → CaS
___________
157.
KOH + HNO3 → HOH + KNO3
___________
158.
Al + O2 → Al2O3
___________
159.
HgO → Hg + O2
___________
160.
161.
NaOH + H2SO4 → Na2SO4 + H2O
Fe + O2 → Fe2O3
___________
___________
162.
C6H8 + O2 → CO2 + H2O
163.
Pb(NO3)2 + K2CrO4 →PbCrO4 + KNO3
164.
H2 + N2 → NH3
165.
C3H5(NO3)3 → CO2 + N2 + H2O + O2
166.
Fe + CuCl2 → FeCl2 + Cu
___________
167.
KClO3 → KCl + O2
___________
168.
Mg + HCl → H2 + MgCl2
___________
169.
C5H10 + O2 → CO2 + H2O
___________
170.
CO2 → C + O2
___________
171.
NaCl + AgNO3 → NaNO3 + AgCl
172.
S + Cl2 → SCl2
173.
BaCl2 + NaOH → NaCl + Ba(OH)2
174.
Zn + CuSO4 → ZnSO4 + Cu
___________
175.
CH4 → C + H2
___________
176.
Pb(NO3)2 + Mg → Pb + Mg(NO3)2
___________
177.
H2SO4 → H2 + S + O2
___________
178.
C3H8 + O2 → CO2 + H2O
___________
179.
O2 + N2 → N2O4
___________
180.
CaBr2 +
181.
2KI + Br2 → 2KBr + I2
___________
182.
C6H12O6 → C + H2O
___________
183.
NaF → Na + F2
___________
184.
Si + O2 → SiO2
___________
185.
H2 + CO + O2 → H2CO3
___________
186.
C7H14 + O2 → CO2 + H2O
___________
187.
Li3PO4 → Li + P + O2
___________
Na3P → Ca3P2 + NaBr
___________
___________
___________
___________
___________
___________
___________
___________
Classifying Chemical Reactions
Part I: Matching
_______ 188. A + B → AB
A. combustion reaction
_______ 189. A + BX → AX + B
B. decomposition (analysis) reaction
_______ 190. AX + BY → AY + BX
C. double replacement reaction
_______ 191 AB → A + B
D. single replacement reaction
_______ 192. hydrocarbon + O2 → CO2 + H2O
E. synthesis (direct combination) reaction
Part II: Classifying Classify the following reactions as synthesis (S), decomposition (D),
single replacement (SR), double replacement (DR) or combustion (C).
_______ 193.
_______ 194.
_______ 195.
_______ 196.
_______ 197.
_______ 198.
_______ 199.
_______ 200.
_______ 201.
CO2 → C + O2
NaCl
+ AgNO3 → NaNO3 + AgCl
S + Cl2 → SCl2
BaCl2 + NaOH → NaCl + Ba(OH)2
C5H10 + O2 →
CO2 + H2O
Zn + CuSO4 →
ZnSO4 + Cu
CH4 →
C + H2
C3H8 + O2 →
CO2 + H2O
Pb(NO3)2 + Mg →
Pb + Mg(NO3)2
Part III: Short Answer
202. Explain why hydrogen is listed in the Activity Series even though hydrogen is not a metal.
__________________________________________________________________________________
__________________________________________________________________________________
Part IV: Write the complete (with state symbols) balanced equation for the following reactions and then
identify the type of reaction (S, D, SR, DR, C.)
203. Magnesium metal replaces mercury in a solution of mercury (II) nitrate.
204. Bromine gas combines with gaseous nitrogen to produce gaseous nitrogen tribromide.
205. A solution of potassium sulfate reacts with a solution of lead (II) nitrate.
206. Solid potassium chlorate is heated and decomposes into oxygen gas and solid potassium chloride.
207. The gas in our gas jets is methane, CH4. Write the reaction for the combustion of methane.
Equations
Directions:
Write, balance and identify the type for each of the following reactions.
______
208. silver nitrate + potassium sulfate → silver sulfate + potassium nitrate
______
209. silver cyanide + potassium → potassium cyanide + silver
______
210. nitrogen + hydrogen → ammonia
______
211. zinc carbonate → zinc oxide + carbon dioxide
Directions: Write, balance and predict the products for each of the following reactions.
212. The double replacement rxn between sodium hydroxide and calcium nitrate:
213. The double replacement rxn between hydrogen sulfide and cadmium nitrate:
214. The decomposition of aluminum chloride:
215. The decomposition of sodium chloride:
216. The single replacement rxn between aluminum and lead (II) oxide:
217. The double replacement rxn between silver acetate and potassium chromate
218. The decomposition of water to produce gaseous products:
219. The direct combination (synthesis) of iron (III) oxide from a metal and a gas:
Directions: Write, balance, identify the type, and predict the products for each of the following reactions.
220. magnesium + zinc nitrate →
221. aluminum + phosphoric acid →
222. potassium + chlorine gas →
223. chromium (III) chloride + sulfuric acid →
Predicting Products
Directions: Predict the product and balance each of these reactions. List the reaction type
abbreviation to the left of each reaction.
________ 224.
CuCl2 
________ 225.
N2
+
H2 
________ 226.
Ca
+
AlCl3
________ 227.
Al(NO3)3
________ 228.
C3H6
FeCl2 
+
+

O2 
229. Aluminum sulfate reacts with barium chloride
230. Zinc reacts with copper (I) sulfate
231. Sodium chloride decomposes.
232. Calcium metal reacts with oxygen
233. Butane, C4H10, burns in air
Balancing Practice Quiz
Identify the type, predict the products if it occurs, and balance the following reactions:
234. _____
Ba
+ O2→
235. _____
Zn
+ CuSO4
→
236. _____
Ag
+ FeSO4
→
237. _____
BaCl2 + Na3PO4 →
238. _____
C6H12O6 + O2→
239. _____
Zn
240. _____
Cu + MgSO4 →
241. _____
KClO3 →
242. _____
C4H8
+ Pb(NO3)2 →
+ O2→