CP Chemistry
Mrs. Klingaman
Chapter 8:
Chemical Reactions
Name: _____________________________________
Mods: ___________________
Chapter 8: Chemical Equations and Reactions
Reading Guide
8.1 – Describing Chemical Reactions (pgs. 247-261)
1. Define chemical reaction –
2. In any chemical reaction, the original substances are known as the _____________________ and
the resulting substances are known as _______________________
3. According to the law of conservation of mass, the total mass of reactants must ______________
the total mass of products for any given chemical reaction.
4. What are chemical equations?
5. In the chemical equation below, identify the reactant(s) and the product(s):
(NH4)2Cr2O4 (s)  N2 (g) + Cr2O3 (s) + 4 H2O (g)
6. Chemical reactions have physical indicators. These indicators serve as evidence that a chemical
reaction has taken place. List the 4 indicators below (italicized words only):
(1) _______________________________________________________________________
(2) _______________________________________________________________________
(3) _______________________________________________________________________
(4) _______________________________________________________________________
7. Define precipitate –
8. Chemical equations must satisfy the law of conservation of mass. List 3 requirements for a good
chemical equation (italicized words only):
(1) _______________________________________________________________________
(2) _______________________________________________________________________
(3) _______________________________________________________________________
9. In addition to the 7 elements which occur naturally as diatomic molecules (Br2I2N2Cl2H2O2F2), what
are 2 other exceptions where an element is represented by more than just its atomic symbol?
Using Figure 1.3 (pg. 249) fill in the following table for elements that exist as diatomic molecules:
Element
Symbol
Molecular
Formula
Physical State at
Room Temperature
10. Define coefficient -
Identify the coefficient(s) in the chemical equation below:
2 Ag2O (s)  4 Ag (s) + O2 (g)
11. Define word equation -
_______, _______, _______
Using the reaction of methane with oxygen, write the word equation that describes the reaction
and then write a sentence the states how the word equation is read.
Word Equation:
Sentence the word equation would be read aloud:
12. Define formula equation -
Using the reaction for methane and oxygen, write the formula equation (not balanced):
13. Word equations and formula equations are __________________________ statements. They do
not give information about the amounts of reactants or products.
14. Writing Balanced Equations:
In order to satisfy the law of conservation of mass, there must be equal numbers and types of
atom on both sides of the chemical equation.
Below, rewrite the formula equation for reaction between methane and oxygen (see #12 above).
Next, add coefficients to some of the formulas so that there are an equal number of atoms on both
sides of the equation (this represents a balanced chemical equation). When finished, check your
answer using page 251.
# of atoms on REACTANT Side : # of atoms on PRODUCT Side
_____: Carbon : _____
_____: Hydrogen : _____
_____: Oxygen : _____
A useful tool for learning to balance chemical equations is to use a ratio-type-setup to compare the
numbers atoms on each side of the equation. (Note: the number of atoms in each chemical
formula is equal to the coefficient out front of the formula multiplied by the subscript on the atom)
15. Symbols Used in Chemical Equations:
Reactants and Products
Symbol
Meaning
(s)
solid or crystal
Reaction Conditions
Symbol
“produces” or “yields”, indicates the
result of a reaction
reaction in which products can reform
into reactants; the final result is a
mixture of products and reactants
liquid
(l)
(g)
(aq)
Meaning
gas
Δ
aqueous solution
(dissolved in
water)
solid precipitate
product forms
(very rarely used)
gaseous product
forms
(very rarely used)
or
heat
2 atm
0°C
MnO2
reactants are heated
signifies the pressure at which the
reaction is carried out (if different than
normal atmospheric pressure)
signifies the temperature at
which the reaction is carried out
(in this example, 0°C)
formula of the catalyst added to speed
up the rate of the reaction
(in this example, MnO2)
16. Write the following chemical equation as a descriptive sentence (how you would read this aloud).
Include all the information available in the equation including the states of matter.
2 HgO (s)
Δ
2 Hg (l) + O2 (g)
17. Chemical Equations show relative amounts, masses, and progression of chemical reactions.
When a chemical equation is balanced, it gives you a lot of information about the chemical
reaction. List 3 quantitative pieces of information revealed by a chemical equation:
(1) _______________________________________________________________________
(2) _______________________________________________________________________
(3) _______________________________________________________________________
18. Review Figure 1.6 on page 255 and complete the table below for the number of molecules,
moles, and mass (in grams) of the reactants and products in the following balanced equation:
H2
Cl2
HCl
Molecule(s)
Mole(s)
Gram(s)
19. List 2 pieces of information that a chemical equation does not provide:
(1) ___________________________________________________________________
(2) ___________________________________________________________________
Balancing Equations: Chemical equations can be balanced with a step-by-step inspection.
20. Using the example on page 258 (sample problem c), List the 4 steps in balancing chemical
equations as well as the word, formula, and balanced equation part that is given for each step.
(1) _______________________________________________________________________
(2) _______________________________________________________________________
(3) _______________________________________________________________________
(4) _______________________________________________________________________
8.2 – Types of Chemical Reactions (pgs. 262-270)
21. What are the 5 basic types of reactions?
22. Define Synthesis Reaction -
23. A synthesis reaction, also called a composition (or combination) reaction, is represented by the
following general equation: A + X ⟶ AX
Define the variables:
A = __________________________________
X= ___________________________________
AX = _________________________________
24. Define Decomposition Reaction -
25. A decomposition reaction is represented by the following general equation: AX ⟶ A + X
Define the variables:
AX = _________________________________
A= ___________________________________
X = __________________________________
26. Define Single Displacement Reaction (aka: single replacement reaction) -
27. A single displacement reaction is represented by the following general equation:
28. Define Double Displacement Reaction (aka: Double Replacement Reaction) -
29. A double displacement reaction is represented by the following general equation:
Define the variables:
A, X, B, and Y: __________________________________
AX = __________________________________________
BY= ___________________________________________
30. Define Combustion Reaction -
31. One way to recognize reaction types is by the products formed. Aside from the combustion of
hydrogen, what are the two products formed for combustion reactions?
8.3 – Activity Series of the Elements (pgs. 271-273)
The ability of an element to react is known as the element’s activity. NOT all reactions can occur as
they are written due to a lack of reactivity.
32. Define activity series -
33. What is the purpose of an activity series?
Rules for Balancing Chemical Equations:
1) Determine the correct chemical formulas for all the reactants and products in the reaction
(abbreviated rxn), using what you know about the elements and ionic compounds. Indicate the
state of matter in which the reactants and products exist in parentheses next to the formula.
2) Write the formulas for the reactants on the left and the formulas for the products on the right with a
yield sign () in between. If two or more reactants or products are involved, separate their
formulas with plus signs. When finished, you will have a skeleton formula equation.
3) Count the number of atoms of each element in the reactants and products. For simplicity, a
polyatomic ion appearing unchanged on both sides of the equation can be counted as a single
unit.
4) Balance each of the elements, one at a time, by using coefficients out in front of the
element/compound. When no coefficient is written, it is assumed to be 1. It is best to begin
balancing an equation with elements that appear only once on each side of the equation. You
must NEVER attempt to balance an equation by changing subscripts in the chemical formula
of a substance.
5) Check each atom or polyatomic ion to be sure that the equation is balanced.
6) Finally, make sure all the coefficients are in the lowest possible ratio that balances.
In-Class Practice
Balance the following equations using the rules above:
1) ______ KI (aq) + ______ Cl2 (g)  ______ KCl (aq) + ______ I2 (g)
2) ______ Al (s) + ______ HCl (aq)  ______ AlCl3 (aq) + ______H2 (g)
3) ______ Mg(NO3)2 (aq) + ______ K3PO4 (aq)  ______ Mg3(PO4)2 (s) + ______ KNO3 (aq)
4) ______MnO2 (s) + ______HCl (aq)  ______MnCl2 (aq) + ______H2O (l) + ______Cl2 (g)
5) ______ Zn(OH)2 (s) + ______ H3PO4 (aq)  ______ Zn3(PO4)2 (s) + ______ H2O (l)
6) ______ C3H8 (l) + ______ O2 (g)  ______ CO2 (g) + ______ H2O (g)
7) ______ C2H6 (l) + ______ O2 (g)  ______ CO2 (g) + ______ H2O (g)
8) ______ C6H12O6 (s) + ______ O2 (g)  ______ CO2 (g) + ______ H2O (g)
Balancing Equations: WS #1
1)
____ Na3PO4 (aq) + ____ KOH (aq)  ____ NaOH (aq) + ____ K3PO4 (aq)
2)
____ MgF2 (aq)+ ____ Li2CO3 (aq) ____ MgCO3 (s) + ____ LiF (aq)
3)
____ P4 (s) + ____ O2 (g)  ____ P2O3 (s)
4)
____ RbNO3 (aq) + ____ BeF2 (aq)  ____ Be(NO3)2 (aq) + ____ RbF (aq)
5)
____ AgNO3 (aq) + ____ Cu (s)  ____ Cu(NO3)2 (aq) + ____ Ag (s)
6)
____ CF4 (s)+ ____ Br2 (g) ____ CBr4 (s) + ____ F2 (g)
7)
____ HCN (aq) + ____ CuSO4 (aq)  ____ H2SO4 (aq) + ____ Cu(CN)2 (aq)
8)
____ GaF3 (aq) + ____ Cs (s) ____ CsF (aq) + ____ Ga (s)
9)
____ BaS (aq) + ____ PtF2 (aq)  ____ BaF2 (aq) + ____ PtS (s)
10)
____ N2 (g) + ____ H2 (g)  ____ NH3 (g)
11)
____ NaF (aq) + ____ Br2 (g)  ____ NaBr (aq) + ____ F2 (g)
12)
____ Pb(OH)2 (aq) + ____ HCl (aq)  ____ H2O (l) + ____ PbCl2 (s)
13)
____ AlBr3 (aq) + ____ K2SO4 (aq)  ____ KBr (aq) + ____ Al2(SO4)3 (aq)
14)
____ CH4 (g) + ____ O2 (g)  ____ CO2 (g) + ____ H2O (g)
15)
____ Na3PO4 (aq) + ____ CaCl2 (aq)  ____ NaCl (aq) + ____ Ca3(PO4)2 (aq)
16)
____ K (s) + ____ Cl2 (g)  ____ KCl (aq)
17)
____ Al (s) + ____ HCl (aq)  ____ H2 (g) + ____ AlCl3 (aq)
18)
____ N2 (g) + ____ F2 (g)  ____ NF3 (g)
19)
____ SO2 (g) + ____ Li2Se (s)  ____ SSe2 (g) + ____ Li2O (s)
20)
____ NH3 (g) + ____ H2SO4 (aq)  ____ (NH4)2SO4 (aq)
Balancing Equations: WS #2 (OPTIONAL extra practice)
1)
____ KClO3 (aq)  ____ KCl (aq) + ____ O2 (g)
2)
____ NaCl (aq) + ____ F2 (g)  ____ NaF (aq) + ____ Cl2 (g)
3)
____ H2 (g) + ____ O2 (g)  ____ H2O (g)
4)
____ C3H8 (s) + ____ O2 (g)  ____ CO2 (g) + ____ H2O (g)
5)
____ C8H18 (l) + ____ O2 (g)  ____ CO2 (g) + ____ H2O (g)
6)
____ FeCl3 (aq) + ____ NaOH (aq)  ____ Fe(OH)3 (s) + ____ NaCl (aq)
7)
____ P4 (s)+ ____O2  ____ P2O5
8)
____ Na (s) + ____ H2O (l)  ____ NaOH (aq) + ____ H2 (g)
9)
____ Ag2O (s)  ____ Ag (s) + ____ O2 (g)
10)
____ S8 (s) + ____O2 (g)  ____ SO3 (g)
11)
____ C6H12O6 (s) + ____O2 (g)  ____ CO2 (g) + ____ H2O (g)
12)
____ K (s) + ____ MgBr2 (aq)  ____ KBr (aq) + ____ Mg (s)
13)
____ HCl (aq) + ____ CaCO3 (s)  ____ CaCl2 (aq) + ____H2O (g) + ____ CO2 (g)
14)
____HNO3 (aq) + ____NaHCO3 (s)  ____NaNO3 (aq) + ____H2O (g) + ____CO2 (g)
15)
____ H2O (l) + ____ O2 (g)  ____ H2O2 (l)
16)
____ NaBr (aq) + ____ CaF2 (aq)  ____ NaF (aq) + ____ CaBr2 (aq)
17)
____ H2SO4 (aq) + ____ NaNO2 (aq)  ____ HNO2 (aq) + ____ Na2SO4 (aq)
18)
____ Al (s) + ____ Fe3N2 (aq)  ____ AlN (aq) + ____ Fe (s)
19)
____ C7H8 (s) + ____ O2 (g)  ____ CO2 (g) + ____ H2O (g)
20)
____ NaClO3 (aq)  ____ NaCl (aq) + ____ O2 (g)
Writing and Balancing Word Equations – In Class Examples
Seven Diatomic Molecules (these MUST be memorized!):
Directions: Write the following word equations as formula equations and then balance them:
1)
Hydrogen gas and oxygen gas combine to produce liquid water. (remember diatomics!)
2)
Sodium metal reacts with an aqueous solution of magnesium chloride yielding aqueous
sodium chloride and magnesium metal.
3)
A solution of aluminum bromide plus chlorine gas produces aqueous aluminum chloride and
bromine liquid.
4)
Aqueous solutions of aluminum nitrate and sodium sulfide react to form solid aluminum
sulfide and aqueous sodium nitrate.
5)
Solutions of aluminum sulfate and calcium hydroxide combine to form solid aluminum
hydroxide and aqueous calcium sulfate.
6)
Gaseous dicarbon dihydride reacts with oxygen gas to produce carbon dioxide gas and
water vapor.
7)
Aluminum metal heated in the presence of oxygen gas will form solid aluminum oxide.
8)
Iron will react with water to yield solid iron (III) oxide and hydrogen gas.
Writing and Balancing Word Equations – Homework
Directions: Write the following word equations as formula equations and then balance them:
1)
Hydrogen gas and nitrogen gas react to form gaseous nitrogen trihydride (aka: ammonia)
2)
Aqueous solutions of hydrochloric acid and sodium hydroxide yield aqueous sodium
chloride and water.
3)
A solution of lead (II) sulfate reacts with iron metal to produce lead and aqueous iron (II)
sulfate.
4)
When solid potassium chlorate is heated it will form solid potassium chloride and oxygen
gas.
5)
When heated, sulfuric acid (H2SO4) will decompose into gaseous sulfur trioxide and water
vapor.
6)
Aqueous potassium iodide reacts with bromine liquid to yield aqueous potassium bromide
and iodine solid.
7)
Solutions of sodium phosphate and calcium nitrate react to produce aqueous sodium nitrate
and solid calcium phosphate.
8)
Aqueous solutions of ammonium carbonate and zinc sulfate combine to yield solid zinc
carbonate and a solution of ammonium sulfate.
9)
Aqueous solutions of phosphoric acid and strontium hydroxide react to form solid strontium
phosphate and water.
Classification of Chemical Reactions (In-Class)
Directions: Classify the reactions below as synthesis, decomposition, hydrocarbon
combustion, single replacement, or double replacement.
1. 2H2 (g) + O2 (g)  2H2O (l)
_______________________________
2. 2H2O (l) 2H2 (g) + O2 (g)
_______________________________
3. Zn (s) + H2SO4 (aq)  ZnSO4 (aq) + H2 (l)
_______________________________
4. 2CO (g) + O2 (g)  2CO2 (g)
_______________________________
5. C3H8 (l) + 5O2 (g)  3CO2 (g) + 4H2O (g)
_______________________________
6. 2HgO (s)  2Hg (s) + O2 (g)
_______________________________
7. 2KBr (aq) + Cl2 (g)  2KCl (aq) + Br2 (g)
_______________________________
8. CaO (s) + H2O (l)  Ca(OH)2 (aq)
_______________________________
9. AgNO3 (aq) + NaCl (aq)  AgCl (s) + NaNO3 (aq) _______________________________
10. C6H12O6 (s) + 6O2 (g)  6H2O (l) + 6CO2 (g)
______________________________
11. 2H2O2 (l)  2H2O (g) + O2 (g)
______________________________
12. 2KOH (aq) + H2SO4 (aq)  K2SO4 (aq) + 2H2O (l) ______________________________
Balancing & Classifying Chemical Reactions
Directions:
First, balance each of the chemical equations below. Then, classify each reaction as synthesis,
decomposition, combustion, single-replacement, or double-replacement
1)
____ NaBr (aq) + ____ Ca(OH)2 (aq)  ___ CaBr2 (aq) + ____ NaOH (aq)
Type of reaction: _____________________________
2)
____ NH3 (g)+ ____ H2SO4 (aq)  ____ (NH4)2SO4 (aq)
Type of reaction: _____________________________
3)
____ C5H10O (l) + ____ O2 (g)  ____ CO2 (g) + ____ H2O (g)
Type of reaction: _____________________________
4)
____ Pb (s) + ____ H3PO4 (aq)  ____ H2 (g) + ____ Pb3(PO4)2 (s)
Type of reaction: _____________________________
5)
____ Li3N (aq) + ____ NH4NO3 (aq) ____ LiNO3 (aq) + ____ (NH4)3N (aq)
Type of reaction: _____________________________
6)
____ HBr (aq) + ____ Al(OH)3 (aq)  ____ H2O (g) + ____ AlBr3 (aq)
Type of reaction: _____________________________
7)
____ Sb (s) + ____ Cl2 (g)  ____ SbCl3 (s)
Type of reaction: _____________________________
8)
____NaCO3 (s)  ____Na(s) + ____CO2 (g) + ____O2 (g)
Type of reaction: _____________________________
9)
____Si (s) + ____Br2 (g)  ____SiBr4 (s)
Type of reaction: _____________________________
10)
____(NH4)2CO3 (aq) + ____Al(NO3)3 (aq)  ____NH4NO3 (aq) + ____Al2(CO3)3 (aq)
Type of reaction: _____________________________
11)
____Mg (s) + ____O2 (g)  ____MgO (s)
Type of reaction: _____________________________
12)
____C2H2 (s) + ____O2 (g)  ____CO2 (g) + ____H2O (g)
Type of reaction: _____________________________
13)
____CuCl2 (aq) + ____AgNO3 (aq)  ____Cu(NO3)2 (aq) + ____AgCl (s)
Type of reaction: _____________________________
14)
____Rb (s) + ____Cl2 (g)  ____RbCl (s)
Type of reaction: _____________________________
15)
____Ca(OH)2 (aq)  ____CaO (s) + ____H2O (l)
Type of reaction: _____________________________
16)
____ Pb(NO3)2 (aq) + ____ H2S (g)  ____ PbS (s) + ____ HNO3 (aq)
Type of reaction: _____________________________
17)
____ Fe (s) + ____ HCl (aq)  ____ FeCl2 (aq) ) + ____ H2 (g)
Type of reaction: _____________________________
Predicting the Products of Chemical Reactions (In-Class)
Directions: Predict the products for each type of reaction given below and balance the equation:
Synthesis (aka: Combination) Reactions:
Two reactants come together to form one product (typically a solid compound).
1) ______ Mg (s) + ______ N2 (g) 
2) ______ Li (s) + ______ O2 (g) 
3) ______ S8 (s) + ______ Al (s) 
Decomposition Reactions:
One reactant breaks down into two products (most simply, the reactant breaks into its elements)
4) ______ Fe2O3 (s) 
5) ______ RbCl (s) 
6) ______ H2O (s) 
Hydrocarbon Combustion Reactions:
When a hydrocarbon combusts in the presence of oxygen gas the same two products always form.
7) ______ CH4 (g) + ______ O2 (g) 
8) ______ C2H6 (g) + ______ O2 (g) 
9) ______ C4H10O (g) + ______ O2 (g) 
Predicting Products – Mixed Review
Directions:
Use the given reactants to decide which type of chemical reaction is occurring (synthesis,
decomposition, or hydrocarbon combustion). Then, predict the products of the reaction and balance
the resulting equation.
1) ______ K (s) + ______ Cl2 (g) 
2) ______ C5H12 (g) + ______ O2 (g) 
3) ______ MnS2 (s) 
4) ______ FeCl3 (s) 
5) ______ Ca (s) + ______ N2 (g) 
6) ______ C2H6 (g) + ______ O2 (g) 
7) ______ Ba (s) + ______ O2 (g) 
8) ______ V2O5 (s) 
9) ______ Sr (s) + ______ P4 (s) 
10) ______ C3H8O2 (g) + ______ O2 (g) 
Double Replacement Reactions & Solubility Table (In-Class)
1) Using solubility table, predict whether each of the following compounds is soluble (aq) or
insoluble (s) in water:
a.
NiBr2 –
f.
Co(C2H3O2)2 –
b.
Li2S –
g.
PbCl2 –
c.
Zn3(PO4)2 –
h.
Cu(OH)2 –
d.
(NH4) 2SO4 –
i.
K2CO3 –
e.
CaCO3 –
j.
AgNO3 –
2) Write a balanced chemical equation for each double replacement reaction below. If no precipitate
forms, write NR (no reaction) after the balanced equation.
a. Aqueous solutions of sodium carbonate and silver nitrate are mixed.
b. Aqueous solution of sodium hydroxide and potassium sulfate are mixed.
c. Aqueous solutions of potassium phosphate and copper (II) acetate are mixed.
d. Aqueous solutions of potassium sulfide and zinc chloride are mixed.
Double Replacement Reactions: Predicting a Precipitate
Directions:
Predict the products formed by the combination of the following aqueous solutions (including the
states of matter) and balance the resulting chemical equation. If a precipitate forms, put a box around
its chemical formula . If no precipitate forms, write NR (no reaction) after the balanced equation.
1.
____Li2CO3 (aq) + ____AgNO3 (aq) 
2.
____NaOH (aq) + ____H2SO4 (aq) 
3.
____BaCl2 (aq) + ____H3PO4 (aq) 
4.
____FeSO4 (aq) + ____Pb(NO3)2 (aq) 
5.
____Ni(C2H3O2)2 (aq) + ____(NH4)2S (aq) 
6.
____CaCl2 (aq) + ____HNO3 (aq) 
7.
____AgNO3 (aq) + ____KCl (aq) 
8.
____Al2(SO4)3 (aq) + ____(NH4)3PO4 (aq) 
9.
____CuS (aq) + ____LiBr (aq) 
10. ____Na2S + ____Pb(NO3)2 (aq) 
11. ____Al(OH)3 (s) + ____HC2H3O2 (aq) 
12. ____K2CO3 (aq) + ____BaI2 (aq) 
Single Replacement Reactions - Metals
A solid metal (or hydrogen gas) can only replace another metal which is lower than itself on the
activity series list. If the metal by itself is more reactive than the metal cation in the reactant
compound, then a reaction can occur.
Ex) Zn(s) + CuCl2(aq)  ZnCl2(aq) + Cu(s) …because Zn is above Cu, this rxn occurs
Ag(s) + CuCl2 (aq)  No Reaction (NR) … because Ag is below Cu, no rxn occurs
Directions:
Using the activity series of metals, determine if the following reactions will occur. If yes, write the
balanced molecular equation. If no reaction occurs, write NR.
1. ____ Al (s) + ____ NiCl2 (aq) 
2. ____ Pb(NO3) 2 (aq) + ____ Ag (s) 
3. ____ Cr (s) + ____ NiSO4 (aq) 
4. ____ HBr (aq) + ____ Mn (s) 
5. ____ Hg (l) + ____ Zn(NO3)2 
6. ____ H2 (g) + ____ CuCl2 (aq) 
7. ____ Li (s) + ____ H2O (l)
8. ____ HCl (aq) + ____ Pt (s) 
9. ____ Pb (s) + ____ CuSO4 (aq) 
10. ____ Ca (s) + ____ Au(NO3)3 (aq) 
11. ____ Zn (s) + ____ Mg(NO3)2 (aq) 
Single Replacement Reactions - Halogens
A halogen gas can only replace another halogen which is lower than itself on the activity series list. If
the halogen by itself is more reactive than the halogen anion in the reactant compound, then a
reaction can occur.
Ex) F2(g) + SrI2(aq)  SrF2(aq) + I2(g) …because F is above I, this rxn occurs
Br2(g) + NaCl (aq)  No Reaction (NR) … because Br is below Cl, no rxn occurs
Directions:
Using the activity series of the halogens, determine if the following reactions will occur. If yes, write
the balanced molecular equation. If no reaction occurs, write NR.
1. ____ Cl2 (g) + ____ KI (aq) 
2. ____ KF (aq) + ____ Br2 (l) 
3. ____ Cl2 (g) + ____ NaI (aq) 
4. ____ CaI2 (aq) + ____ Br2 (l) 
5. ____ Br2 (l) + ____ NaCl (aq)
6. ____ CaBr2 (aq) + ____ I2 (s) 
7. ____ F2 (g) + ____ AlCl3 (aq)
8. ____ MgI2 (aq) + ____ Cl2 (g) 
9. ____ Cl2 (g) + ____ LiF (aq)
10. ____ BaI2 (aq) + ____ F2 (g) 
Predicting Products of Reactions – Mixed Review
Directions: Using the given reactants, determine the reaction type, predict the products and balance.
1.
____ C10H16 (s) + ____ O2 (g) 
Type of Reaction: ___________________________________
2.
____ MgO (s) 
Type of Reaction: ___________________________________
3.
____ Cu (s) + ____ CaCl2 (aq) 
Type of Reaction: ___________________________________
4.
____ Al(OH)3 (s) + ____ H2SO4 (aq) 
Type of Reaction: ___________________________________
5.
____ K (s) + ____ Br2 (l) 
Type of Reaction: ___________________________________
6.
____ Na (s) + ____ H2O (l) 
Type of Reaction: ___________________________________
7.
____ Ca (s) + ____ O2 (g) 
Type of Reaction: ___________________________________
8.
____ Cl2 (g) + ____ NaI (aq) 
Type of Reaction: ___________________________________
9.
____ Hg(OH)2 (s) + ____ H3PO4 (aq) 
Type of Reaction: ___________________________________
10. ____ C3H6 (g) + ____ O2 (aq) 
Type of Reaction: ___________________________________
11. ____ K2CO3 (aq) + ____ BaCl2 (aq) 
Type of Reaction: ___________________________________
12. ____ FeCl3 (aq) 
Type of Reaction: ___________________________________