Taewoong Moon
Oxidation- Reduction Reactions- Design Lab
Experiment Question: In oxidation-reduction reactions, or redox reactions, are strengths of reducing and oxidizing agents different from each reaction?
Theory of an experiment:
1. Determine the relative strengths of oxidizing agents and reducing agents.
2. Study some simple oxidation-reduction reactions
Hypothesis: Relative strengths of reducing and oxidizing agents differ from each reaction.
Background Information:
Whenever electrons are lost by one substance, they must be gained by another. Reactions involving the exchange or transfer of electrons from atoms or ions of one substance to those of another substance are called oxidation-reduction reaction. The substance that is oxidized is called the reducing agent. The substance that is reduced (gaining electrons) is called oxidizing agent.
Because they are made up of two distinct processes redox reactions can be represented by two half reactions.
Independent Variable
Dependent Variable
Controlled Variable
Structure of test tube
Volume of test tube
Temperature
Pressure
Materials:
1. Test tube, 18*100mm
2. Test tube holder
3. Graduated cylinder-10ml
4. Dropper pipet.
5. Bunsen burner
6. Safety goggles
7. Lab coat
8. 0.1 M AgNO3
9.
Safety:
Handle the hydrochloric acid with extreme care. Avoid spills on your skin or clothing.
Always wear safety goggles and a lab coat or apron when working in the lab.
Procedures
Relative activity of some metals.
1. Add 5ml of 0,1 M AgNO3, to a clean, dry tube. Add a piece of copper metal into this solution. Add 5ml of 0.1 M solution. Record your observations
2. Add 5ml of 0.1 M Cu(No3)2 to each tube. Place of strip of Zn and Pb in each tube. Record your observations
3. Repeat step 2 using 0.1 M Pb(NO3)2 and strips of Cu and Zn. Record your observations
4. Repeat the step again using 0.1 M Zn(NO3)2 and strips of Cu and Pb.
Reaction of iron metals and ions
1. Place 5ml of 0.1M FeCl3 in a clean dry test tube. Drop SnCl2. Record your observations
Data and Observations 1. Cu+AgNo3 Ag + Cu(No3)2 2. Zn + Cu(No3)2
Pb+ Cu(No3)2
3. Cu+ Pb(No3)2 Zn+ Pb(No3)2
4. Cu+ Zn(No3)2 Pb+ Zn (No3)2
5. Fe3+ + Sn2+
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