Redox Reaction Lab
Purpose – to observe and study a spontaneous reduction oxidation reaction
Introduction – A chemical reaction can often be recognized by the rearrangement of electrons in the valence shell of the reactants. Often, these rearrangements involve the loss or gain of electrons, giving us what we call a redox, or reduction-oxidation reaction. The elements which gain electrons are reduced, and those that lose electrons are oxidized. This occurs because some elements are able to gain electrons easier than others. For metals, we say that the more active a metal, the easier it is for it to give up electrons. Thus, the most active metals are those which give up their electrons the easiest.
Materials
Beakers Aluminum Foil CuCl2(aq)
Water Stirring Rod Filter set-up
Procedure
1. Pour approximately 50mL of copper (II) chloride solution into the small beaker.
2. Tear the aluminum into tiny bits.
3. Observe both of the reactants.
4. Collect the bits of aluminum and place them all in the beaker with the solution.
5. Stir the mixture until the reaction is complete.
6. Set-up a filter apparatus and filter the mixture.
7. Collect the filtrate in the larger beaker.
8. Observe both products (filtrate and residue).
Observations
Both reactants before reaction
Both products after reaction and filtering
Calculations
o Write out a balanced reaction equation for the reaction between aluminum and copper (II) chloride.
o Write out a balanced net ionic equation for this redox reaction.
o Write out balanced half reactions for this redox reaction.
Conclusion
In paragraph form, answer the following questions:
o Write a conclusion statement mentioning the purpose.
o As the reaction proceeds, you see less and less aluminum foil, what is happening to the aluminum? (Where is it going?)
o What is the orange-brown solid and where did it come from?
o Identify which elements are gaining electrons and which are losing electrons.
o Identify which elements are being reduced and which are being oxidized.