Name ___________
WPHS Chemistry
Unit 4
Chemical Reactions
Bergmann-Sams
-1-
Name ___________
Chemistry: Unit 4 Outline: Chemical Reactions
Assignment
WB Page Number
Podcast 4.1 (CB 1-3)
Online
Worksheet A
pg 7-9
Podcast 4.2 (CB 5-9)
Online
Demo: Types of Reactions
In Class
Pg 10-12
Score
Out of





Worksheet B
Lab: Small Scale Single Replacement
Podcast 4.3 (CB 11-13)
Worksheet C
Lab: Small Scale Double
Pg 4
Online
Pg 13-15
Pg 5-6
100


100
Online
Pg 16
Teacher Handout
Pg 17-20
In Class


100

100
Replacement
Podcast 4.4 (CB 15-17)
Worksheet D
Technology Lab
Worksheet E (Review)
Unit 4 Exam
(You must score 85/100 on all assignments with a number to move to the next
unit. For those assignments with a check, you need to do it to the satisfaction of
your teacher)
-2-
Name ___________
Unit 4 Chemical Reactions: Composition Book Outline
8-1: Describing Chemical Change
1 Converting Word Equations into Formulaic Equations (pg 203-206)
Question: Answer the following question
 What is the difference between a word equation and a chemical equation
Define
 Catalyst
Copy: Table 8.1 on page 206
3 Balancing Chemical Equations (pg 207-211)
Read the section and: “Balancing Chemical Equations” and come up with an analogy
like the bicycle and write the balanced chemical equation.
Leave the rest of the page blank
8-2: Types of Chemical Equations
5
Reaction Types (pgs 212-216)
Define: Combination Reactions, Decomposition Reaction, Single Replacement
Reaction, Double Replacement Reaction, Combustion Reaction Do one at a time with
the examples underneath each
List: Two examples of each type (written with formulas—not words)
7
Predicting Single Replacement Reactions
Copy: Table 8.2 on page 217
9
11
13
Predicting Single Replacement Reactions
Leave blank for teacher notes
Predicting and Writing Double Replacement Reactions
Leave blank for teacher notes
Predicting and Writing Double Replacement Reactions
Leave blank for teacher notes
8-3: Reactions in Aqueous Solutions
15
17
Ionic and Net Ionic Equations (pg 225-228)
Leave blank for teacher notes
Ionic and Net Ionic Equations (pg 225-228)
Leave blank for teacher notes
-3-
Name ___________
Activity Series of Metals Lab
Purpose: To observe an activity series of different metals.
Procedure:
1. Using the well plates, select a row of wells for each solution listed in the data
table. Make sure that you write down which letter and number your wells are for
each solution. There should be three wells for each solution (one of the three for
each of the metals).
2. Put five drops of each solution in the wells chosen for that solution.
3. Put one piece of magnesium in one of the wells for each solution. For example,
you should have a well of copper sulfate with magnesium in it, a well of
magnesium sulfate with magnesium in it, and a well of sodium chloride with
magnesium in it, a well of zinc sulfate with magnesium in it and a well of silver
nitrate with magnesium in it.
4. Repeat step 3 with copper instead of magnesium.
5. Repeat step 3 with zinc instead of magnesium.
6. After l minute has passed, make observations of both the metal strips and the
solutions. Put these observations in a data table in your comp book that looks like
the one below. Label this data table as 1 minute.
7. After 5 total minutes have passed, take another set of observations. Make another
data table like the one below and label it 5 minutes.
8. After 15 total minutes have passed, take another set of observations. Again, make
another data table and label it 15 minutes.
Data Table:
CuSO4
MgSO4
NaCl
ZnCl2
AgNO3
Cu metal
Mg metal
Zn metal
Analysis Questions: (as always with labs, these questions should be written in complete
sentences)
1. Why doesn’t the metal react with the same metal solution?
2. In which wells did the appearance of the metal change? Be sure to tell your
teacher what both of the reactants of the well were.
3. Write a balanced equation for each visible reaction between a metal and it’s
solution. Be sure to identify what types of reactions these are.
4. Based on the results of your experiment construct your own activity series for the
five metals. Put the most active metal first and the least active metal last. Be sure
to include your reasoning for your rankings.
5. In a short summary paragraph, describe and explain the patterns that you see in
your reaction table.
-4-
Name ___________
Double Replacement Lab
Use Beral Pipets to add each solution on the grid. For those that have a reaction occur,
describe the reaction. For those that do not, record NVR (No visible reaction) When
done you need to:
1. Write out each complete reaction that occurs (you must balance it)
2. Write out the ionic equation for each reaction that occurs.
3. Write out the net-ionic equation for each reaction that occurs.
Put “flimsy” over the top of this page and mix all of the chemicals. Do not mix the same
chemical with the same.
Chemical NaCl
AgNO3
Pb(NO3)2 Na2SO4
BaCl2
NaOH
Na3PO4
NaCl
AgNO3
Pb(NO3)2
Na2SO4
BaCl2
NaOH
Na3PO4
X
X
X
X
X
X
XX
X
X
X X
X X
X X
X X
X X X X
X X X X
X X X X
X X
X
X X
X X
X
X X X
-5-
Name ___________
Data Table: Write in your observations here.
Chemical NaCl
AgNO3
Pb(NO3)2 Na2SO4
NaCl
AgNO3
Pb(NO3)2
Na2SO4
BaCl2
NaOH
Na3PO4
-6-
BaCl2
NaOH
Na3PO4
Name ___________
Equation Worksheet A:
Balancing Chemical Equations
Balance the following equations and identify the type of reaction: (Double Replacement,
Single Replacement, Combination, Decomposition, or Combustion)
1) __HgO

2) __HCl +
__Mg 
__H2 +
MgCl2
3) __CH4 +
__O2 
__CO2 +
__H2O Type: ________________
4) __C6H12O6
+ __O2 
__CO2 + __H2O
Type: ________________
5) __H2 +
__O2 
__H2O
Type: ________________
6) __H2 +
__N2 
__NH3
Type: ________________
7) __NO +
__O2 
__NO2
Type: ________________
8) __Al2O3

9) __CaO +
__H2O 
__Hg +
__Al
__O2
+
Type: ________________
Type: ________________
__O2 Type: ________________
__Ca(OH)2
Type: ________________
10) Hydrogen gas reacts with iodine to produce hydroiodic acid.
Type: ________________
11) Sulfur reacts with oxygen to produce sulfur dioxide.
Type: ________________
-7-
Name ___________
12) Calcium acetate reacts with sodium carbonate to produce calcium carbonate and
sodium acetate.
Type: ________________
13) Write the chemical reaction that shows how rust forms: (Iron III oxide)
Type: ________________
14) Iron combines with oxygen and water to form iron (III) hydroxide
Type: ________________
15) Sulfur trioxide is bubbled through water to produce sulfuric acid
Type: ________________
-8-
Name ___________
16) Copper metal is made by treating copper ore the following way: Copper (II)
sulfide is heated with carbon and oxygen to produce copper and sulfur dioxide
and carbon dioxide.
Type: ________________
17) Copper-bottomed cooking pans turn black because copper combines with oxygen
to form copper (II) oxide.
Type: ________________
18) Magnesium hydroxide neutralizes stomach acid, HCl, to produce magnesium
chloride and water.
Type: ________________
-9-
Name ___________
Equation Worksheet B: Single Replacement Reactions
A. Predict the products and balance the following single replacement reactions.
If no reaction occurs write N.R. For transition metals use the following charges:
Iron: Fe3+
Lead: Pb4+
Mercury: Hg2+
Copper: Cu1+
1. Fe
+
CuCl2 
2. Hg
+
Sn(SO4)2 
3. Ba
+
Ni3(PO4)2 
4. Pb
+
Au(NO3)3 
5. Li
+
HOH 
6. K
+
AgCl
7. Ca
+
NaOH 
8. Cu
+
Fe(OH)3 
9. Fe
+
Cu(OH)2 

- 10 -
Name ___________
10. Lead II Chloride + Magnesium
11. Barium Nitrate + Zinc
12. Potassium + Tin IV Nitrate
13. Copper + Silver Nitrate
14. Sodium Phosphate + Potassium
15. Gold + Hydrochloric acid
16. Magnesium + Aluminum Hydroxide
17. Iron + Copper II Sulfate
- 11 -
Name ___________
18. Iron + Nickel II Iodide
19. Sodium Permanganate + Calcium
20. hydrochloric acid + Zinc
21. Aluminum + Iron II dichromate
- 12 -
Name ___________
Equation Worksheet C: Double Replacement Reactions
Complete and Balance the following reactions. If no reaction occurs then write N.R.
1) Na2SO4 (aq) + Ba(NO3)2(aq) ---->
2) NaNO3(aq) +
NH4Cl(aq) ----->
3) Pb(NO3)2 (aq) +
Na2CrO4(aq)
4) ZnCl2(aq) + K2CO3(aq) ---->
5) Ammonium Chloride + Silver Nitrate ------>
6) Barium Acetate +
Copper II Chromate
- 13 -
Name ___________
7) Solutions of Silver Nitrate and ammonium chloride are mixed
8) Solutions of Lead II nitrate and Sodium Chloride are mixed
9) Solutions of zinc sulfate and magnesium chloride are mixed
10) Solutions of Ammonium phosphate and Zinc Chlorate are mixed
11) Solutions of Aluminum bromide and Iron II Iodide are mixed
- 14 -
Name ___________
12) Solutions of sodium sulfide and Iron II Chlorate are mixed
13) Solutions of copper II bromide and potassium phosphate are mixed
14) Solutions of barium acetate and zinc sulfate are mixed
- 15 -
Name ___________
Equation Worksheet D: Net Ionic Equation Worksheet
For the following reactions write the:
a. Complete Equation (Indicate states): Balance
b. Ionic Equation
c. Net Ionic Equation
1. ZnCl2 (aq) + Na2S (aq)  ZnS(s) + NaCl(aq)
2. (NH4)3PO4 + AgNO3 
3. Magnesium Nitrate + Potassium phosphate  Magnesium Phosphate (s) +
Potassium Nitrate.
4. Lead II Acetate + Potassium Iodide
- 16 -
Name ___________
Equations Worksheet E: Mixed Types of Reactions
Directions: For each of the following reactions:
1) Complete the reaction (Put NR if no reaction takes place)
2) Balance it
3) Identify the type of reaction (Single Replacement, combination, double replacement,
decomposition, or combustion)
4) Indicate states of matter for each reaction
1) NaCl + AgNO3 
2) Fe + CuSO4

3) C4H10 + O2 
4) Ba(NO3)2 + Na2SO4 
5) AgNO3 + Li

6) LiBr + Cu 
7) MgS + NaOH 
- 17 -
Name ___________
8) Hg + LiCl

9) Li + HgCl2

10) C3H8

+ O2
11) Ammonium Nitrate is added to sodium chloride
12) Lithium Chloride is added to Zinc Phosphate
13) Zinc is added to lithium chloride
14) Iron is added to a solution of silver nitrate
- 18 -
Name ___________
15) A solution of copper II sulfate is added to an iron nail
16) Octane (C8H18) is burned in air
17) A solution of Tin IV sulfate is added to a solution of ammonium hydroxide
18) Sodium hydroxide is added to hydrochloric acid
19) Calcium hydroxide is added to sulfuric acid
20) Nickel is added to hydrochloric acid
21) Strontium is added to water
22) Hydrochloric acid is added to copper metal
- 19 -
Name ___________
23) Solid bismuth is added to a solution of barium hydroxide.
24) Methanol (CH3OH) is burned in air
25) Solid gold is added to hydrochloric acid
- 20 -
Name ___________
Name: ______________
Period: ______________
Balancing Reactions Worksheet
Synthesis and Decomposition
Part A (Review): Balance the following reactions and indicate whether they are synthesis
or decomposition reactions.
1.
2.
3.
4.
5.
SO3 +
H2O
HgO
Al2O3(s)
P
+
H2O
--->
--->
--->
O2
--->
H2
Hg
Al(s)
--->
H2SO4
+
O2
+
O2
+
O2(g)
P2O5
Type:_____________
Type:_____________
Type:_____________
Type:_____________
Type:_____________
Part B: Predict the products and indicate type (include states):
1. KBr --->
Type:
2. Li + Cl2 --->
Type:
3. Rb2CO3 --->
Type:
4. NiO --->
Type:
5. CO2 + H2O--->
Type:
_________
_________
_________
_________
_________
Part C: Predict the products, balance, include states, and indicate type.
1. Potassium Chlorate is heated vigorously
Type: _________
2. Molten sodium is reacted with chlorine gas
Type: _________
3. Calcium is added to water
Type: _________
4. Zinc carbonate is heate
Type: _________
5. Aluminum chloride decomposes into it's elements
Type: _________
6. Cesium hydroxide is heated
Type: _________
7. Sulfurous Acid is heated
Type: _________
8. Potassium and Bromine are reacted
Type: _________
9. Potassium Oxide and Carbon dioxide react
Type: _________
10. Calcium chlorate is heated
Type: _________
11. Sodium hydroxide is heated
Type: _________
- 21 -
Name ___________
12. Iodine reacts with hydrogen
Type: _________
- 22 -
Name ___________
Balancing Chemical Equations Worksheet 1
Name
Period
Balance the following equations:
1. 2HgO 
2Hg +
O2
2. HCl +
Mg

H2
+
MgCl2
3. CH4 +
2O2 
CO2 +
2H2O
4. C6H12O6
+
6O2 
6CO2 +
6H2O
5. 2H2 +
O2

2H2O
6. 2H2 +
Cl2

2HCl
7. 3H2 +
N2

2NH3
8.
2 NO +
O2

2NO2
9. 3Al2O3

4Al
+2O2
10. CaO +
H2O 
Ca(OH)2 already balanced
11. Hydrogen gas reacts with iodine to produce hydrogen iodide.
H2+ I2 2HI
12. Sulfur reacts with oxygen to produce sulfur dioxide.
S + O2  SO2
13. Calcium acetate reacts with sodium carbonate to produce calcium carbonate and
sodium acetate.
Ca(C2H3O2)2 + Na2CO3 2NaC2H3O2 +CaCO3
14. Write the chemical reaction that shows how rust forms:
4Fe + 3O2  2Fe2O3
15. Iron combines with oxygen and water to form iron (III) hydroxide
Fe + O2 + 6H2O  4Fe(OH)3
16. Sulfur trioxide is bubbled through water to produce hydrogen sulfate
SO3+ H2O  H2SO4 already balanced
17. Copper metal is made by treating copper ore the following way:
 Copper (II) sulfide is heated with carbon and oxygen to produce copper and sulfur
dioxide and carbon dioxide.
CuS +C + 4O2  SO2 + CO2 + Cu
Copper-bottomed cooking pans turn black because copper combines with oxygen to form
copper (II) oxide.
2Cu + O2 2CuO
18. Any Group I metal reacts with water to produce hydrogen gas and the metal
hydroxide. Write the reaction that occurs when rubidium is dropped in water.
2Rb + 2HOH  2RbOH + H2
- 23 -
Name ___________
19. Magnesium hydroxide neutralizes stomach acid, HCl, to produce magnesium
chloride and water.
Mg(OH)2 + 2HCl  MgCl2 + 2H2O
20. Limestone is dissolved by acid (Remember our carbonate lab in September?). This
is why statues are dissolved by acid rain. First, the acid is formed in the
atmosphere. Second, it falls on the statue and dissolves it. Write two reactions that
show how this
happens. First, nitrogen dioxide reacts with water to form hydrogen nitrate.
Second, hydrogen nitrate combines with calcium carbonate to form carbon dioxide
and water and calcium nitrate.
4NO2+ 2H2O  4HNO3 balancing is difficult extra credit if you can
2HNO3 + CaCO3  Ca(NO3)2+ H2O+ CO2
Balancing Reactions Worksheet
Synthesis and Decomposition
Part A (Review): Balance the following reactions and indicate whether they are synthesis
or decomposition reactions.
1.
SO3
2.
+
H2O
--->
H2SO4
2H2O
--->
2H2
+
3.
4.
2HgO
2Al2O3(s)
--->
--->
2Hg +
4Al(s) +
5.
4P
5O2
--->
+
balanced
Type: synthesis
O2
Type: decomposition
O2
3O2(g)
Type: decomposition
Type: Decomposition
2P2O5
Type: Synthesis
Part B: Predict the products and indicate type (include states):
1. 2KBr --->
2K + Br2
Type: decomp
2. 2Li + Cl2 ---> 2LiCl
Type: synth
3. Rb2CO3 --->
Rb2O + CO2
Type: decomp
4. 2NiO --->
2Ni + O2
Type: decomp
5. CO2 + H2O---> H2CO3
Type: synth
Part C: Predict the products, balance, include states, and indicate type.
1) Potassium Chlorate is heated vigorously
2KClO3  2KCl + 3O2
2)
decomposition
Molten sodium is reacted with chlorine gas
- 24 -
Name ___________
2Na + Cl2  2NaCl
3) Calcium is added to water
Ca + 2HOH  Ca(OH)2
synthesis
synthesis
4) Zinc carbonate is heate
ZnCO3 ZnO + CO2
decomposition
5) Aluminum chloride decomposes into it's elements
2AlCl3 2Al + 3Cl2
decomposition
6) Cesium hydroxide is heated
4CsOH  2Cs2O + 2H2
decomposition
7) Sulfurous Acid is heated
H2SO3 H2O + SO2
decomposition
8) Potassium and Bromine are reacted
2K+ Br2  2KBr
decomposition
9. Potassium Oxide and Carbon dioxide react
K2O + CO2  K2CO3
decomposition
10. Calcium chlorate is heated
Ca(ClO3)2  CaCl2 + 3O2 decomposition
1) Sodium hydroxide is heated
4NaOH  2Na2O + 2H2 decomposition
12. Iodine reacts with hydrogen
I2 + H2  2HI
synthesis
- 25 -
Name ___________
Single Replacement Reactions Worksheet
Do work on a separate sheet of paper
Name:
A. Predict the products and balance the following single replacement reactions. If
no reaction occurs write N.R.
1) Fe
2) Hg
3) Ba
4) F2
5) Cl2
6) Pb
7) Li
8) K
9) Ca
10) Cu
11) Fe
12) Br2
+
+
+
+
+
+
+
+
+
+
+
+
CuCl2
Sn(SO4)2
Ni3(PO4)2
NaCl
NH4Br
Au(NO3)3
HOH
AgCl
NaOH
Fe(OH)3
Cu(OH)2
KI












B. Write the reactions and predict the products of each of the following single
replacement reactions. Balance all reactions. If no reaction occurs write N.R.
13) Lead II Chloride + Magnesium
14) Barium Nitrate + Zinc
15) Potassium + Tin IV Nitrate
16) Copper + Silver Nitrate
17) Sodium Phosphate + Potassium
18) Gold + Hydrogen chloride
19) Magnesium + Aluminum Hydroxide
20) Iron + Copper II Sulfate
21) Iron + Nickel II Iodide
22) Sodium Permanganate + Calcium
23) Hydrogen Chloride + Zinc
24) Aluminum + Iron II dichromate
- 26 -
Name ___________
Name:____________
Period:____________
Mixed Types of Reactions
Directions: For each of the following reactions:
5) Complete the reaction (Put NR if no reaction takes place)
6) Balance it
7) Identify the type of reaction
8) (Single Replacement, combination, double replacement, decomposition, or
combustion)
9) Indicate states of matter for each reaction
26) NaCl + AgNO3

27) Fe + CuSO4

28) C4H10 + O2

29) Ba(NO3)2 + Na2SO4

30) AgNO3 + Li

31) LiBr + Cu

32) MgS + NaOH

33) HG + LiCl

34) Li + HgCl2

35) C3H8
+ O2

36) Ammonium Nitrate is added to sodium chloride
37) Lithium Chloride is added to Zinc Phosphate
38) Zinc is added to lithium chloride
39) Iron is added to a solution of silver nitrate
40) A solution of copper II sulfate is added to an iron nail
41) Octane (C8H18) is burned in air
42) A solution of Tin IV sulfate is added to a solution of ammonium hydroxide
43) Sodium hydroxide is added to hydrochloric acid
44) Calcium hydroxide is added to sulfuric acid
45) Nickel is added to hydrochloric acid
46) Strontium is added to water
47) Hydrochloric acid is added to copper metal
48) Solid bismuth is added to a solution of barium hydroxide.
49) A solution of potassium iodide is added to liquid bromine.
50) Methanol (CH3OH) is burned in air
51) Solid gold is added to hydrochloric acid
- 27 -
Name ___________
Ws E KEY
Types of Reactions Work Sheet
Directions: For each of the following reactions:
 Complete the reaction (Put NR if no reaction takes place)
 Balance it
 Identify the type of reaction
 (Single Replacement, combination, double replacement, decomposition, or
combustion)
 Indicate states of matter for each reaction
1) Sodium chloride plus silver nitrate
NaCl(aq)+AgNO3(aq) AgCl(s) + NaNO3(aq)
Double Replacement
2) Iron plus copper II sulfate
2Fe(s) + 3CuSO4(aq)  3Cu(s) + Fe2(SO4)3(aq)
Fe(s) + CuSO4(aq)  Cu(s) + FeSO4(aq)
Single Replacement
3) Butane (C4H10) burns completely in the presence of oxygen
C4H10 (g) + 13/2O2 (g)  4CO2 (g) + 5H2O (g)
2C4H10 (g) + 13O2 (g)  8CO2 (g) + 10H2O (g)
Combustion
4) Barium Nitrate + sodium sulfate
Ba(NO3)2 (aq) + Na2SO4 (aq)  BaSO4
Double Replacement
5) Silver nitrate Plus Lithium
AgNO3(aq) + Li (s) - LiNO3
Single Replacement
(aq)
(s)
+ 2NaNO3 (aq)
+ Ag
6) Lithium bromide plus copper
LiBr (aq) + Cu  No reaction
7) Magnesium sulfide plus sodium hydroxide.
MgS (s) + NaOH (aq)  No reaction
8) Liquid mercury reacts with aqueous lithium chloride
Hg (l) + LiCl (aq)  No Reaction
9) Solid Lithium is dropped into a solution of Mercury II chloride
2Li (s) + HgCl2 (aq)  2LiCl (aq) + Hg (l)
- 28 -
Name ___________
Single Replacement
10) Propane (C3H8) is burned in the presence of air
C3H8 (g) + 5O2 (g)  3CO2 (g) + 4H2O (g)
Combustion
11) Ammonium Nitrate is added to sodium chloride
NH4NO3 (aq) + NaCl (aq)  No reaction
12) Lithium Chloride is added to Zinc Phosphate
LiCl (aq) + Zn3(PO4)2(s)  No reaction
13) Zinc is added to lithium chloride
Zn (s) + LiCl(aq)  No reaction
14) Iron is added to a solution of silver nitrate
Fe (s) + 3AgNO3(aq)  3Ag(s) + Fe(NO3)3
Fe (s) + 2AgNO3(aq)  2Ag(s) + Fe(NO3)2
Single Replacement
15) A solution of copper II sulfate is added to an iron nail
3CuSO4 (aq) + 2Fe (s)  Fe2(SO4)3 (aq) + 3Cu(s)
CuSO4 (aq) + Fe (s)  FeSO4 (aq) + Cu
Single Replacement
16) Octane (C8H18) is burned in air
C8H18(g) + 12.5O2(g)  8CO2(g) + 9H2O(g)
2C8H18(g) + 25O2(g) 
16CO2(g) + 18H2O(g)
combustion
17) A solution of Tin IV sulfate is added to a solution of ammonium hydroxide
Sn(SO4)2(aq) + 4NH4OH(aq)
Sn(OH)4(s) + 2(NH4)2SO4(aq)
double replacement
Or: No Reaction: Really a reaction will occur
18) Sodium hydroxide is added to hydrochloric acid
NaOH(aq) + HCl(aq)  H2O(l) + NaCl(aq)
double replacement
- 29 -
Name ___________
19) Calcium hydroxide is added to sulfuric acid
Ca(OH)2 (s) + H2SO4 (aq) 
CaSO4 (s) + 2H2O(l)
double replacement
20) Nickel is added to hydrochloric acid
Ni(s) + 2HCl(aq)  NiCl2(aq) + H2 (g)
2Ni(s) + 6HCl(aq)  2NiCl3(aq) + 3H2 (g)
Single Replacement
21) Strontium is added to water
Sr(s) + 2HOH(l)  Sr(OH)2(s) + H2(g)
Single replacement
22) Hydrochloric acid is added to copper metal
HCl(aq) + Cu  No reaction
23) Solid bismuth is added to a solution of barium hydroxide.
Bi(s) + Ba(OH)2(s)  No reaction
24) A solution of potassium iodide is added to liquid bromine.
2KI(aq) + Br2(l)  2KBr(aq) + I2 (s)
single replacement
25) Methanol (CH3OH) is burned in air
2CH3OH(g) + 3O2(g) 
2CO2(g) + 4H2O(g)
combustion
26) Solid gold is added to hydrochloric acid
Au(s) + HCl(aq)  no reaction
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Name ___________
Reaction Type Worksheet
Balance and then identify each of the following reactions as: combustion, synthesis,
decomposition, Single Displacement, Double Displacement.
1. Na +
Cl2  NaCl
2. AgNO3
+ NaCl  AgCl + NaNO3 Type: ______________
3. NH4CO3  (NH4)2O
3. CuSO4
5. Na3PO4 +
6. AgNO3 +
+ CO2
 Li2SO4
+ Li
4. C2H6 + O2
Type: ______________

CO2
Type: ______________
+ Cu
Type: ______________
+ H2O
Type: ______________
CuCl2  Cu3(PO4)2 + NaCl Type: ______________
Zn  Zn(NO3)2 + Ag
7. CH3OH + O2  CO2
Type: ______________
+ H2O
Type: ______________
8. CaO + CO2  CaCO3
Type: ______________
9. Pb(NO3)2 + Na2CrO4  NaNO3 + PbCrO4 Type: ______________
10. KClO3  KCl
+ O2
Type: ______________
11. Magnesium + Iron III Chloride  Magnesium Chloride + Iron
12. Nickel II Iodide + Silver I Nitrate  Silver I Iodide + Nickel II Nitrate
13. Sodium carbonate decomposes into sodium oxide and carbon dioxide
14. Butane (C4H10) reacts with oxygen to form carbon dioxide and water
15. Magnesium oxide reacts with carbon dioxide to make magnesium carbonate
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Name ___________
16. Potassium Phosphate + Chromium III Chloride
Potassium Chloride + Chromium III Phosphate
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