Lab: Production and Isolation of Copper
A Reaction between Copper II Chloride and Aluminum
Purpose:
 Observe and describe the reaction between Copper II chloride and Aluminum
 Use experimental data to practice mole/mole, mole/mass and mass/mass calculations
Discussion:
The basic idea behind balancing equations is to show that matter is not created or destroyed in
chemical reactions. Balanced equations and the mole concept allow for exact calculation of amounts
of reactants and amounts of products. Aluminum is more reactive than copper so in this reaction, it
will replace the copper in the Copper II Chloride, producing Copper and Aluminum Chloride.
Student Task (Pre-Lab Questions):
1. What are some signs that a chemical reaction has occurred?
2. The expected reaction is:
CuCl2 (aq)+ Al (s)  AlCl3 (aq) + Cu (s)
Balance this chemical equation.
3. Use the balanced equation to set up a table of conversion factors.
REACTANTS
PRODUCTS
Balanced Equation
Mols
Molar Mass (MM) (g/mol)
Mass Conserved (MC) (g)
(Mols X MM = MC)
EXPERIMENTAL DESIGN
Safety:
I will adhere to all safety precautions including wearing safety goggles and not fooling around. ________(initials)
(Treat all school property including lab supplies and equipment with respect. If you break or damage anything, you will be
charged.)
Materials:
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Apparatus (Equipment)
Digital Balance
250 mL Beaker
50 mL measuring cylinder
Thermometer
Funnel
Empty water bottle
Filter Paper
250 ml Erlenmeyer Flask
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Reagents
Copper II Chloride (CuCl2)
Alumininum (Al)
Water
Procedure: Write down each step as you do them in your notebook and check off that you have
completed that step!
Day 1
1. Pour 25 ml of water into a graduated cylinder. Record the temperature of the water.
2. Tare a weigh boat. Place approximately 1.5 gram of copper chloride crystals into the weigh boat.
Accurately record the mass of the copper II chloride. Add the copper II chloride to a 250 ml beaker
3. Add the 25mL of water to the flask. Swirl gently till all crystals are dissolved. Record observations
and take another temperature reading. Leave the thermometer in the flask.
4. Record the mass of your aluminum wire. Record the mass of your dry filter paper.
5. Bend the wire into a loop and place it into the copper chloride solution. Wait about 10-15 minutes
making observations during this time. Record all evidence of a chemical reaction.
6. Continue to watch the thermometer and once it stops changing record a final temperature reading.
7. After the reaction has stopped, carefully separate the newly formed copper from the aluminum and
isolate it from the remaining solution using the funnel, filter paper and water bottle. Rinse the copper
carefully with water, and filter again.
8. Place the newly formed copper and filter paper on the class tray, and allow to dry overnight.
9. Clean up your lab area and return all materials.
Day 2
Determine the mass of the new copper you have made. (Don’t forget to subtract the mass of dry filter
paper).
STUDENT TASK: OBSERVATIONS AND DATA: (Include all units) Be sure this data table and data
are written in your notebook!
Mass of Copper II Chloride (CuCl2) used
Mass of Aluminum (Al) used
Mass of Copper (Cu) produced
Mass of dry Filter Paper
Temperature of Water Only
Temperature of Aqueous Copper II Chloride {CuCl2 (aq)}
Final Temperature of Reaction Vessel
STUDENT TASK: ANALYSIS: Copy and answer these questions in your notebook.
Day 1
1. What are three observations you made that indicated a chemical reaction occurred?
2. a) Given your measured mass of Aluminum, what mass of Copper II Chloride (CuCl2)
would you need to completely use it up? b) Did you have enough Al?
3. Given your measured mass of Aluminum, what mass of copper do you expect to produce?
(This value is the theoretical yield of copper produced in grams.)
4. Convert your measured mass of Aluminum to moles. Given your moles of Aluminum,
how many moles of Aluminum Chloride (AlCl3) do you expect to produce?
Day 2
5. Obtain the mass of copper produced. This is your actual yield. Compare it to your theoretical
yield. {Percent Yield = (Actual yield/Theoretical yield) X 100} %.
6. Error Analysis: What unavoidable experimental errors might be factors in a percent yield that
is less than or greater than 100%.
STUDENT TASK: CONCLUSION, REFLECTION AND ACTIVE PARTICIPATION:
Summarize what you did and learned. How has this experiment helped you in your understanding of
mass/mole calculations? What was your job? Rate your behavior on a scale of 1-10. Include any
recommendations for improving this experiment.