Aluminum Reaction with Copper (II) Chloride LAB
Background Information
In this experiment, you will take a piece of aluminum foil
and place it into a solution of copper (II) chloride. You will
observe its behavior by measuring the temperature at the
beginning and end of the experiment. You will be able to
qualitatively investigate any changes that occur.
Copper (II) chloride is an ionic compound which is bluegreen in its hydrated form, CuCl2. 2 H2O, and is brown in its
anhydrous form, CuCl2. This compound melts at 498oC but does
not have a measurable boiling point because the liquid
decomposes before the temperature gets high enough for it to
boil. Aluminum metal will react with the CuCl2 in a single replacement reaction to form copper
metal and aluminum chloride.
A single replacement reaction is a type of reaction where the more reactive metal
replaces the less reactive metal dissolved in the solution.
Hypothesis
Materials
Safety goggles
Lab apron
CuCl2 crystals
Beaker, 100 ml
Funnel
Erlenmeyer flask
distilled water bottle
folded filter paper with staples
stirring rod
Aluminum foil square
Procedure:
1. Wear safety goggles and apron at all times
2. Measure 25 mL of distilled water in the graduated cylinder.
3. Get a pre-measured portion of CuCl2. (about 2.0 g)
Aluminum Reaction with Copper (II) Chloride LAB
4. Place the folded filter paper with staples in the Erlenmeyer flask. Add the 2.0 g of CuCl 2 into
the filter paper. Pour the 25 mL of distilled water over the CuCl2, being careful not to overfill the
funnel all at once. After all the CuCl2 has been dissolved by the distilled water, describe as
completely as you can anything that happens. Include the staples and what happened to them
in your observations.
Observations:
5. Pour the solution from the Erlenmeyer flask into the 50 mL beaker. Place the thermometer
in the beaker and record the temperature of the solution.
Temperature
6. Obtain a small piece of aluminum foil and, using the stirring rod, hold it under the liquid in
the beaker. You may need to add small pieces of aluminum foil to complete the reaction.
Record the temperature of the solution during the reaction. Describe what happens thoroughly.
Temperature
Observations:
7. Repeat until the aluminum fails to react.
8. Clean up all equipment used and leave lab tables the way you found them. Place the copper
solution in a collecting beaker designated by your teacher. Complete your lab questions and
place in your lab books for grading.
Aluminum Reaction with Copper (II) Chloride LAB
Post Lab Questions
1. Write a paragraph on your observations in this lab. Try to organize all observations into
physical or chemical properties.
2. What eventually happens when you put the aluminum in the copper (II) chloride?
3. Is the reaction exothermic or endothermic?
4. Aluminum reacts with copper (II) chloride, CuCl2, to form copper metal and aluminum
chloride, AlCl3. Identify the reactants and the products for the experiment.
Reactants:
Products:
5. Write a word equation for the reaction based in the above statement.
6. Write the equation using formulas for the reactants and products.
7. What type of reaction is taking place (single replacement, double replacement, synthesis,
combustion, decomposition)?