Juan R. Liwag Memorial High School
Bayanihan, Gapan City
SY: 2012-2013
FORMAL REPORT
Activity #3: Types of Reactions: Redox and Non-Redox
Group 5
I.
Objectives
II.
Science Concepts
III.
Schematic Procedure
IV.
Results and Discussions
V.
Conclusion
VI.
References
I.Objectives
 To learn to identify redox reactions.
 To study practical applications of redox reactions.
 To learn to identify substances oxidized and substances reduced, as well as oxidizing
agents and reducing agents in redox reactions.
II. Science Concepts
Types of Redox Reactions
 Combination reactions
A combination reaction is the simplest redox reactions and as the name suggests involves
the "combining" of elements to form a chemical compound. It denoted in the manner:
A+B→C
 Decomposition reactions
Decomposition reactions are the opposite of combination reactions. A decomposition
reaction leads to the breakdown of a compound into two or more components at least one of
which must be in the elemental state.
AB → A + B
 Displacement reactions
In displacement reaction, an ion in a compound is replaced by an ion of another element.
It may be noted as:
X + YZ → X Z + Y
Displacement reactions fit into two categories; metal displacement and non-metal displacement.
(a) Metal displacement
A metal in a compound can be displaced by another metal in the uncombined state. Metal
displacement reactions find many applications in metallurgical processes in which pure metals
are obtained from their compounds in ores.
(b) Non-metal displacement
The non-metal displacement redox reactions include hydrogen displacement and a rarely
occurring reaction involving oxygen displacement.
 Disproportionation reactions
Disproportionation reactions are a special type of redox reactions. The element in one
oxidation state is simultaneously oxidized and reduced. One of the reacting substances in a
disproportionation reaction always contains an element that can exist in at least three oxidation
states. The element in the form of reacting substance is in the intermediate oxidation state; and
both higher and lower oxidation states of that element are formed in the reaction.
2A → A' + A"
III. Schematic Diagram
Part A. Demonstration Videos
Watch the video clips of some experiments about redox reactions:
 Burning of natural gas, CH4, in the presence of oxygen
 Reaction of nitric acid and copper
 Metal activity series: aluminum and silver- removal of tarnish
 Reactions of Copper sulfate solutions with household chemicals
PART B. ACTUAL EXPERIMENT
1. Reaction of hydrochloric acid and zinc.
Pour 3 mL of a 6.0 mol/L HCl
solution in a beaker.
Place a piece of zinc metal in
the Erlenmeyer flask.
Cover the mouth of Erlenmeyer
flask with balloon to collect the
produced gas.
2. Reaction of Mg and Hydrochloric acid.
Pour 3 mL of a 6.0 mol/L HCl
solution in a beaker.
Place a piece of Mg metal in the
Erlenmeyer flask.
Observe what happens. Do not
smell the fume.
3. Metal activity series: zinc and copper.
Prepared 3 mL of a 0.1 mol/L
copper(II)sulfate solution.
Put a piece of zinc metal in the
beaker.
Observe the changes.
4. Metal activity series: copper and silver.
Prepared 3 mL of a 0.1 mol/L
silver nitrate solution.
Put a piece of metallic copper in
the beaker.
Observe the changes.
5. Metal activity series: Iron and copper.
Prepared 3 mL of a 0.1 mol/L
silver nitrate solution.
Put a piece of iron nail in the
beaker.
Observe the changes.
IV. RESULTS AND DISCUSSION
PART A QUESTIONS:
1. Write balanced equations for the combustion of propane, C3H8, and of gasoline, C8H18.
2 C8H18 + 25 O2  16 CO2+ 18 H2O
2. Write balanced equation for this reaction and do the redox analysis.
3Cu+ 8HNO3  3 Cu(NO3)2 + 2NO +4H2O
Oxidation, Lost 2e-, Reducing Agent: Copper
Reduction, Gained 3e-, Oxidizing Agent: Nitrogen
3. Write a balanced equation and do the redox analysis.
3 Ag2S + 2 Al  6 Ag+Al2S3
Oxidation, Lost 3e-, Reducing Agent: Aluminum
Reduction, Gained 1e-, Oxidizing Agent: Silver
PART B QUESTIONS:
Observation:
1. Reaction of Hydrochloric Acid and Zinc.
It produced gas fumes.
2. Reaction of Magnesium and Hydrochloric Acid.
It produced bubbles and the Magnesium metal disappeared.
3. Metal activity series: Zinc and Copper.
Zinc metal turned black.
4. Metal activity series: Copper and Lead
The Copper wire tarnished.
5. Metal activity series: Iron and copper.
The Iron nail formed rust.
1. Write the balanced equations and do the redox analysis for the reaction of zinc with acid.
Zn + HCl  ZnCl2 + H2
Oxidation, Lost 4e-, Reducing Agent: Zinc
Reduction, Gained 1e-, Oxidizing Agent: Hydrogen
2. Write the balanced equations and do the redox analysis for the reaction of Mg with HCl.
Mg + 2HCl  MgCl2+ H2
Oxidation, Lost 2e-, Reducing Agent: Magnesium
Reduction, Gained 1e-, Oxidizing Agent: Hydrogen
3. Write a balanced equation for this reaction and do the redox analysis. Which metal is more
active: zinc or copper?
Zn + CuSO4  ZnSO4 + Cu
Oxidation, Lost 2e-, Reducing Agent: Zinc
Reduction, Gained 2e-, Oxidizing Agent: Copper
Zinc is more active than Copper.
4. Write balanced equation for this reaction and do the redox analysis. Which metal is more
active: copper or lead?
Cu + Pb (NO3)2  no reaction
Lead is more active than Copper.
5. Write balanced equation for this reaction and do the redox analysis. Which metal is more
active: copper or silver? Which metal is more active: aluminum or silver?
Ag + CuSO4  no reaction
Copper is more active than Silver.
Aluminum is more active than Silver.
PART C. PRACTICE EXCERCISES
A. Predict the products of the following chemical reactions and then balance the reactions using
oxidation number method. Determine which of the reactions are redox and which are non-redox
by assigning oxidation numbers to each atom. Indicate the type of reaction.
1. Ag + S  Ag2S
Oxidation, Reducing Agent, Lost 1e- : Silver
Reduction, Oxidizing Agent, Gained 2e- : Sulfur
Balanced Equation: 2Ag + S  Ag2S
(Synthesis)
1x2=2
2x1=2
2. Fe2O3  Fe + O2
Oxidation, Reducing Agent, Lost 2e- : Oxygen
Reduction, Oxidizing Agent, Gained 3e- : Iron
Balanced Equation: 2Fe2O3  4Fe + 3O2
(Decomposition)
2x3=6
3x2=6
3.
Ca + O2  CaO
Oxidation, Reducing Agent, Lost 2e- : Calcium
Reduction, Oxidizing Agent, Gained 2e- : Oxygen
Balanced Equation: 2Ca + O2  2CaO
(Synthesis)
2x1=2
2x1=2
4. Al + Fe2O3  Al2O3 + Fe
Oxidation, Reducing Agent, Lost 3e- : Aluminum
Reduction, Oxidizing Agent, Gained 3e- : Iron
Balanced Equation: 2Al + Fe2O3  Al2O3 + 2 Fe
(Single Replacement)
3x1=3
3x1=3
5. CuF2 + H2SO4  CuSO4+ HF
Oxidation, Reducing Agent: None
Reduction, Oxidizing Agent, Gained 1e- : Copper
Balanced Equation: CuF2 + H2SO4 CuSO4 + 2 HF
NON-REDOX Reaction
(Double Replacement)
6. Mg + HCl  MgCl2 + H2
Oxidation, Reducing Agent, Lost 2e- : Magnesium
(Single Replacement)
2x1=2
Reduction, Oxidizing Agent, Gained 1e- : Hydrogen
Balanced Equation: Mg + 2HCl  MgCl2 + H2
1x2=2
7. C4H10 + O2  CO2 + H2O
Oxidation, Reducing Agent
Reduction, Oxidizing Agent
Balanced Equation:
NON-REDOX Reaction
(Combustion)
8. LiOH + HCl  LiCl + H2O
Oxidation, Reducing Agent: None
Reduction, Oxidizing Agent: None
Balanced Equation: LiOH + HCl  LiCl + H2O
NON-REDOX Reaction
(Neutralization)
9. Pb(OH)4 + KI  PbI4 + KOH
Oxidation, Reducing Agent: None
Reduction, Oxidizing Agent : None
Balanced Equation: Pb(OH)4 + 4KI  PbI4 +4KOH
NON-REDOX Reaction
10. C6H6 + O2 H2O + CO2
Oxidation, Reducing Agent
Reduction, Oxidizing Agent
Balanced Equation:
NON-REDOX Reaction
(Double Replacement)
(Combustion)
B. Give at least five(5) practical uses of redox reaction in our daily lives. Write the balanced
chemical reactions of each examples.
 Cellular Respiration
C6H12O6 + 6 O2  6 CO2 + 6 H2O

Steel Making
Fe2O3 + 3C  2Fe + 3CO

Rusting of Iron
4 Fe + 3 O2  2 Fe2O3

Heating Houses
CH4 + 2O2  CO2 + 2H2O

Combustion
2 C 8 H 18 + 25 O 2 → 16 CO 2 + 18 H 2 O
V. Conclusion
We can therefore conclude that redox reactions are among the most common and most
important chemical reactions in everyday life. Photosynthesis and the reverse reaction of cellular
respiration are considered one of the redox reactions. The combustion of wood in a fire is
another. These processes are essential in every aspect of human life. For this reason it is
necessary to understand what is taking place when these reactions happen.
Redox reactions, or oxidation-reduction reactions, observe the transfer of electrons between
reactants and/or products. Redox reactions are matched set -- you don't have a redox reaction
without oxidation reaction or a reduction reaction happening at the same time. If a species in a
reaction is oxidized, then something else must be reduced.
VI. References
Result of the activity
http://chemmaster.co.in
GROUP V
IV-Zara
Leader:
Leomar T. Santiago
___________________
Members:
Crissa Chirene P. Bug-os
___________________
Donna Clarisse L. Calma
___________________
Matthew Reinier W. Garcia
___________________
Christine Joy G. Jimenez
___________________
Lori Anne M. Pestaño
___________________
John Bennedick B. Quijano
___________________
Jean Ellice P. Roy
___________________
Camille R. Villania
___________________
Submitted to:
Mr. Jeffrey M.Sta Ines
Advanced Chemistry Teacher