Practice Problems: Types of Reactions
CHEM 1A
Identify the type(s) of reaction in the following equations.
1. 2 SO2 + O2  2 SO3

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
2. 4 Al + 3 MnO2  3 Mn + 2 Al2O3
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3. Bi2S3 + 6 HCl  2 BiCl3 + 3 H2S
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

4. 2 PbO2  2 PbO + O2
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5. 3 H2SO4 + 2 Al(OH)3  6 H2O + Al2(SO4)3
6. C3H8 + 5 O2  3 CO2 + 4 H2O
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Predict the products for the following combination reactions and balance them (show your check).
The product of each reaction is a charge neutral ionic compound.
7. ___ Mg(s) + ___ O2(g) 
8. ___ Al(s) + ___ Br2(l) 
Activity Series:
9. ___ Cu(s) + ___ FeCl3(aq) 
10. ___ Al(s) + ___ HBr(aq) 
11. ___ H2(g) + ___ Al2O3(aq) 
12. ___ Cl2(g) + ___ HBr(aq) 
13. ___ I2(s) + ___ HCl(aq) 
Metals
(and Hydrogen)
form cations
K
Ca
Na
Mg
Al
Zn
Fe
Ni
Sn
Pb
H
Cu
Ag
Hg
Au
Non-Metals
(Halogens)
form anions
F2
Cl2
Br2
I2
increasing
activity
Predict the products for the following single replacement reactions
and balance them (show your check). If no reaction occurs, write
“no reaction” on the product side of the arrow.
Predict the products for the following double replacement reactions and balance them (show your
check). Use the solubility rules to determine if a precipitate (solid) will form. Label the phase of
insoluble products as solid and soluble products as aqueous.
14. ___ Cu(NO3)2(aq) + ___ FeCl3(aq) 
15. ___ Ba(C2H3O2)2(aq) + ___ (NH4)2SO4(aq) 
16. ___ KCl(aq) + ___ Pb(NO3)2(aq) 
17. ___ Na2CO3(aq) + ___ CaBr2(aq) 
18. ___ CaCl2(aq) + ___ AgNO3(aq) 
Complete the following combustion reactions (in air) and balance them (show your check).
19. ___ C2H2(g) + ___ ______(g) 
20. ___ C3H8(g) + ___ ______(g) 
21. ___ C2H5OH(l) + ___ ______(g) 
Predict the products for the following acid-base neutralization reactions and balance them (show
your check).
22. ___ HBr(aq) + ___ Al(OH)3(s) 
23. ___ HCl(aq) + ___ CaCO3(s) 
24. ___ H2SO4(aq) + ___ KOH(aq) 
25. ___ H3PO4(aq) + ___ Ba(OH)2(aq) 
Balance the following redox reactions using the ½ reaction method.
26. CH3OH(aq) + Cr2O72-(aq)  CH2O(aq) + Cr3+(aq)
Oxidation ½ Reaction:
Reduction ½ Reaction:
Balanced Redox Equation:
27. Zn(s) + HCl(aq)  Zn2+(aq) + H2(g) + Cl–(aq)
Oxidation ½ Reaction:
Balanced Redox Equation:
Reduction ½ Reaction:
28. Cl2(g)  ClO-(aq) + Cl-(aq)
(Occurring in a basic solution)
Oxidation ½ Reaction:
Note: This is a disproportionation reaction
(the same element is being reduced and oxidized)
Reduction ½ Reaction:
Balanced Redox Equation:
Write and balance the formula equation, the complete ionic equation, and the net ionic equation
for the following reaction. Include the phases in the formula equation, and circle the spectator
ions in the complete ionic equation.
29. The acid-base neutralization reaction between aqueous phosphoric acid and aqueous sodium
hydroxide