Leader :BeejayC.Oanes
Members :
Carl Jensen delos Santos
BermhelOrgante
Robert Jeremiah Reyes
Ivan Roberto
Yanni Young
Hershey Genovania
Emma Pauline Perdiguerra
Chrisette Perez
Hannah Joy Serrano
Activity 3
Types of reaction:
redox and non-redox
I.objective: - To learn to identify redox reaction.
- To study practical application of redox reactions.
- To learn to identify substances reduced, as well as oxidizing agents and
reducing agent s in redox reaction.
Ii. theoretical background:
Redox reaction – there is a change in oxidation number in the reaction.
Non Redox – there is no change in oxidation number
Types of Redox Reaction: Synthesis, decomposition, single replacement, double replacement,
combustion and acid-base.
Iii. Schematic procedures:
Part A:DEMONSTRATION VIDEO
Watch video from youtube some
chemical reaction and write the
correct balance chemical equation
and its redox analysis.
Part B:ACTUAL EXPERIMENT
1.Reaction of hydrochloric acid and zinc.
H + Release from the reaction so the H+
occupied the unblown ballon.
3.Metal activity series: Zn & Cu
2.REACTION OF MG AND
HYDROCHLORIC ACID.
Like in zinc the H+ occupied the
unblown balloon.
4.Metal activity series: Cu & Pb(NO3)2
5.Metal activity series: Fe and CuSO4
PART C.PRACTICE EXERCISE:
Make some exercise about redox and non
redox
Ex: Ag + S
Ag2S
IV.RESULTS AND DISCUSSION:
PART A: demonstration video
1. Burning of natural gas, CH4 in the presence of oxygen.
CH4
+ 2O2
CO2 + 2H2O (hydrocarbon combustion)
2. Reaction of nitric acid and copper.
2 HNO3 + 2Cu
2CuNO3 + H2 (single replacement)
3.Metal activity series:aluminum and silver – removal of tarnish.
3Ag2S
+ 2Al
6Ag + Al2S3 (single replacement)
4. Reaction of copper sulfate solutions with household chemicals.
CuCO3 + 2NaHSO4
CuSO4 + Na2CO3+ SO2+ O2
PART b: actual experiment
1.Reaction of HCl(aq) and Zn (single replacement .Zn is more active than Cl so it replace Cl)
Zn
+ 2HCl(aq)
ZnCl2
+ H2
2. Reaction of HCl(aq) and Mg
Mg + 2HCl
MgCl2 + H2
(o)
(+2)(-1)
(+1)(-1)
(0)
gain e- = 1 e-
lose = 2e-
3. Metal activity series: Zn & Cu
Zn + CuSO4
(o) (+2) (+6) (-1)
ZnSO4 + Cu
gain=2e-
(+2)(+6)(-2) (0)
lose=2e-
4. Metal activity series: Cu & Pb(NO3)2
Cu + Pb(NO3)2
No reaction happen because Pb is more active than Cu
5. Metal activity series: Fe and CuSO4
Fe + CuSO4
(0)
gain=2e-
FeSO4 + Cu
(+2)(+6)(-2)
(+2)(+6)(-2)
lose=2e-
(0)
Part c: practice exercise
A.Detemine w/c of the reaction are redox and non redox and the type of reaction.
1. 2Ag + S
(0)
(0)
2. 2Ca + O2
(0)
(0)
Ag2S REDOX
(Synthesis)
(+1)(-2)
2CaO
REDOX (Synthesis)
(+2)(-2)
3.Mg + 2 HCl
MgCl2
+ H2
(+2)(-1)
(0)
(0)
(+1)(-1)
4. CuF2 + H2SO4
(+2)(-1)
REDOX (single replacement)
CuSO4 + HF REDOX (double replacement)
(+1)(+6)(-2)
(+2)(+6)(-2) (+1)(-1)
5.LiOH + HCl
LiCl
(+1)(-2)(+1) (+1)(-1)
+ H2O NOT REDOX (double replacement)
(+1)(-1)
(+1)(-2)
B. 2 Example of redox reaction in our daily lives.
1 INSIDE THE FUEL TANK:
2H2O2
H20
+ ENERGY
2.RUSTING OF IRON
Fe + O2
Fe2O3
V.CONCLUSION
We determine whether the reaction ia a redox or not redox and we determine which element is
more active to replace another element in a reaction.