Reaction of Copper (II) Chloride Dihydrate and Aluminum
Procedure: Write and balance a chemical equation for the reaction. Calculate the amount of
copper (II) chloride dehydrate needed to completely react with the aluminum sample given.
Crumple the aluminum foil to separate any coating on the aluminum; tear into small pieces. Place
the predetermined quantity of copper (II) chloride dihydrate into a 250 mL beaker. Add
approximately 150 mL of water to the solid and stir to dissolve. Add the torn pieces of
aluminum to the solution and continue to stir until the reaction is complete. Filter the solution
through a pre-weighed piece of filter paper. Discard the filtrate, and dry the residue in the
drying oven before recording the final mass. (Note: a few drops of concentrated hydrochloric
acid might be needed to facilitate the reaction process.)
Calculations and Questions:
1. Provide tables for both qualitative and quantitative data.
2. Write and balance a chemical equation for the reaction between copper (II)
chloride and aluminum. Include states of matter.
3. Calculate the amount of copper (II) chloride dihydrate needed to completely react all
of the aluminum. Determine the Molarity of the solution.
4. Write the complete ionic and net ionic equations; identify the driving force and
spectator ions.
5. Write the chemical formula for copper (II) chloride. Identify the cation and
anion.
6. When the copper (II) chloride is dissolved in water, is the substance present
as an ionic compound or as ions in solution? Explain. Is
7. Identify the type(s) of reaction (considering the types of reactions studied in
class). If it is a redox reaction, identify what is oxidized and what is reduced.
8. Is the reaction endothermic or exothermic? How do you know?
9. What evidence allows you to determine that a chemical change has occurred?
10. What substance is present in the filtrate at the end of the reaction? How do you
know?
11. What is the mass of the residue formed?
12. Calculate the theoretical yield, % yield and % error.
13.Is there a limiting reagent and an excess reagent present? If so, what are they?
14.What are the possible sources of error in this experiment?