South Pasadena • Chemistry
Name
Period
Date
5 · Chemical Reactions
STATION 1
• CLASSIFYING & BALANCING
For each of the following equations, classify the reaction, then balance the equation.
C—combustion DR—double replacement
SR—single replacement
S—synthesis
DR
ZnS (aq) + 2 HCl (aq)  ZnCl2 (aq) + H2S (g)
SR
2 HCl (aq) + Zn (s)  ZnCl2 (aq) + H2 (g)
S
2 H2 (g) + O2 (g)  2 H2O (ℓ)
DR
3 Ca(OH)2 (aq) + 2 H3PO4 (aq)  Ca3(PO4)2 (s) + 6 H2O (ℓ)
D—decomposition
5 · Chemical Reactions
STATION 2
• CLASSIFYING & BALANCING
For each of the following equations, classify the reaction, then balance the equation.
C—combustion DR—double replacement
SR—single replacement
S—synthesis
SR
8 Al (s) + 3 Fe3O4 (s)  4 Al2O3 (s) + 9 Fe (s)
C
C5H12 (ℓ) + 8 O2 (g)  5 CO2 (g) + 6 H2O (ℓ)
D
2 H2O2 (aq)  2 H2O (ℓ) + … O2 (g)
S
CaO (s) + CO2 (g)  CaCO3 (s)
D—decomposition
5 · Chemical Reactions
STATION 3
Consider the following balanced equation:
Molar Masses:
• STOICHIOMETRY
C3H8(g) + 5 O2(g)  3 CO2(g) + 4 H2O(g)
44.09
32.00
44.01
18.02 g/mol
1. What mass of CO2 is formed when 100. grams of C3H8 react?
1 mol C3H8   3 mol CO2  44.01 g CO2
100. g C3H8 
= 299 g CO2
44.09
g C3H8 1 mol C3H8  1 mol CO2 

2. What volume (at STP) of O2(g) is needed to completely react with 7.55 grams of C3H8?
1 mol C3H8   5 mol O2  22.4 L O2
7.55 g C3H8 
44.09 g C3H8 1 mol C3H8  1 mol O2  = 19.2 L O2
5 · Chemical Reactions
STATION 4
Consider the following balanced equation:
Molar Masses:
• STOICHIOMETRY
3 Mg (s) + Al2(SO4)3 (aq)  2 Al (s) + 3 MgSO4 (aq)
24.30
342.1
26.98
120.4 g/mol
1. What mass of MgSO4 is formed when 80.0 grams of Mg are consumed?
1 mol Mg  3 mol MgSO4 120.4 g MgSO4
80.0 g Mg 
24.3 g Mg  3 mol Mg   1 mol MgSO4  = 396 g MgSO4
2. How many atoms of Al are formed when 19.0 g Mg are used?
1 mol Mg   2 mol Al  6.022 × 1023 atoms Al
23
19.0 g Mg 
1 mol Al
24.3 g Mg 3 mol Mg 
 = 3.14 × 10 atoms Al
5 · Chemical Reactions
STATION 5
• DOUBLE REPLACEMENT
Write the balanced equation given the following reactants. Indicate the state of each substance. Circle any
precipitates that form.
1.
Solutions of aluminum nitrate and lithium oxide are combined.
Al3+
NO3−
2 Al(NO3)3 (aq)+
2.
Li+ O2−
Al3+ O2−
3 Li2O (aq)  Al2O3 (s)
Li+ NO3−
+
6 LiNO3 (aq)
Solutions of calcium hydroxide and sulfuric acid are mixed.
Ca2+
OH−
Ca(OH)2 (aq) +
H+ SO42−
Ca2+ SO42−
H2SO4 (aq)  CaSO4 (s) +
H+ OH−
2 H2O (ℓ)
5 · Chemical Reactions
STATION 6
• DOUBLE REPLACEMENT
Write the balanced equation given the following reactants. Indicate the state of each substance. Circle any
precipitates that form.
1. Solutions of lead nitrate and hydrochloric acid are combined.
Pb2+
NO3−
Pb(NO3)2 (aq) +
H+ Cl−
Pb2+ Cl−
2 HCl (aq)  PbCl2 (s)
H+ NO3−
+
2 HNO3 (aq)
2. Solutions of magnesium acetate and water are combined.
Mg2+
C2H3O2−
Mg(C2H3O2)2 (aq)
H+ OH−
+
Mg2+
OH−
2 H2O (ℓ)  Mg(OH)2 (s)
H+ C2H3O2−
+
2 HC2H3O2 (aq)
5 · Chemical Reactions
STATION 7
1. Consider the following reaction:
Mg + Zn2+  Zn + Mg2+
Mg  Mg2+ + 2 e−
Zn2+ + 2 e−  Zn
[ positive | negative ]
[ positive | negative ]
[ gaining | losing ] electrons
[ gaining | losing ] electrons
[ oxidized | reduced ]
[ oxidized | reduced ]
Write the half reactions:
The charge is becoming more:
The element is:
So this element is being:
2. Consider the following reaction:
2 Mg + O2  2 MgO
Mg  Mg2+ + 2 e−
O2 + 4 e−  2 O2−
[ positive | negative ]
[ positive | negative ]
[ gaining | losing ] electrons
[ gaining | losing ] electrons
[ oxidized | reduced ]
[ oxidized | reduced ]
Write the half reactions:
The charge is becoming more:
The element is:
• REDOX
So this element is being:
5 · Chemical Reactions
STATION
8
•
SINGLE REPLACEMENT
1. Zinc metal is placed in a solution of hydrochloric acid.
 Write the balanced equation for the reaction.
Zn (s) + 2 HCl (aq)  H2 (g) + ZnCl2 (aq)

H is [ oxidized | reduced ] from H+ to H0.
Zn is [oxidized | reduced ] from Zn0 to Zn2+.
2. Aluminum metal is placed in a solution of ferric nitrate.
 Write the balanced equation for the reaction.
Al (s) + Fe(NO3)3 (aq)  Fe (s) + Al(NO3)3 (aq)

Al is [ oxidized | reduced ] from Al0 to Al3+.
Fe is [oxidized | reduced ] from Fe3+ to Fe0.
5 · Chemical Reactions
STATION
9
•
SINGLE REPLACEMENT
1. Nickel metal is placed in a solution of cupric chloride.
a. Write the balanced equation for the reaction.
Ni (s) + CuCl2 (aq)  Cu (s) + NiCl2 (aq)
b. Cu is [oxidized | reduced ] from Cu2+ to Cu0.
Ni is [oxidized | reduced ] from Ni0 to Ni2+.
2. Calcium metal is placed in a solution of hydrochloric acid.
a. Write the balanced equation for the reaction.
Ca (s) + 2 HCl (aq)  H2 (g) + CaCl2 (aq)
b. Ca is [ oxidized | reduced ] from Ca0 to Ca2+.
H is [oxidized | reduced ] from H+ to H0.