My PBL Project
Al displaces Cu
Introduction
In the project I am going to see how Al (aluminum) displace Cu(copper) by displacement.
Materials
Beakers, Pyrex®, 600-mL, 3
Graduated cylinder, 250-mL
Spatula
Stirring rod
Thermometer (or Temp Probe)
Wood splint and matches
Aluminum foil, 6" x 12", 2 pieces
Copper(II) chloride solution, CuCl2, 1.0 M, 140 mL
Copper(II) sulfate solution, CuSO4, 1.0 M, 140 mL
Sodium chloride solution, NaCl, 1.0 M, 140 mL*
Water, distilled, 420 mL
Procedures
Section 1: Aluminum and Copper(II) chloride
1. Place a 600-mL Pyrex® beaker on the work table.
2. Use a graduated cylinder to measure 140 mL of 1.0 M CuCl2 solution. Pour this
solution into the beaker.
3. Measure and add 140 mL of distilled water to the beaker. The solution is now 0.5 M
CuCl2 solution.
4. Cut a piece of aluminum foil approximately 6" x 12". Loosely crumple the foil enough
to fit into the beaker but do not crush the foil tightly into a ball as this will slow the
reaction and much of the aluminum will remain unreacted.
5. Measure the temperature of the CuCl2 solution before adding the foil.
6. Place the piece of crumpled foil into the beaker. Using a stirring rod, push it down
completely into the solution. Measure the temperature of the reaction mixture again.
7. Observe all changes that occur including a change in temperature. Record your
observations/data in detail.
8. Discuss if a reaction occurred and what are the reactants and products based on
your observations. Also discuss if the reaction is exothermic or endothermic. Test
your hypothesis about the identity of the products and reactants in this reaction by
conducting Section 2.
Section 2: Aluminum and Copper(II) sulfate
9. Repeat the procedure (steps 1-8) from Section 1 in a different 600-mL beaker,
except this time using 70 mL of 1.0 M CuSO4 solution and 70 mL of distilled water.
The solution is now 0.5 M CuSO4.
10. Discuss if a reaction occurred and what are the reactants and products based on
your observations. Also discuss if the reaction is exothermic or endothermic. Test
your hypothesis about the identity of the products and reactants in this reaction by
conducting Section 3. : Set the beaker from Section 2 aside for use in Section 4.
Section 3: Aluminum and Sodium chloride
11. Repeat the procedure (steps 1-8) from Section 1 in a different 600-mL beaker,
except this time using 70 mL of 1.0 M NaCl solution and 70 mL of distilled water.
The solution is now 0.5 M NaCl
12. Discuss if a reaction occurred and what are the reactants and products based on
your observations. Also discuss if the reaction is exothermic or endothermic. Test
your hypothesis about the identity of the products and reactants in this reaction by
conducting Section 4. Set the beaker from Section 3 aside for use in Section 4.
Section 4: Aluminum and Copper(II) Sulfate and Sodium Chloride
13. Place the beaker from Section 2 on the work table.
14. Add 70 mL of 1.0 M NaCI solution and 70 mL of distilled water to the beaker.
15. Discuss the role of various chemicals in the reaction and if the hypotheses put forth
in previous sections was validated or disproved based on observations and data.
16. Write the chemical equation for the reaction. If chloride ions are not in the equation,
what is the purpose of the chloride ions? Discuss the role of a catalyst in a reaction.
Predict what would happen if CuSO4 were added to the beaker from Section 3.
17. Then, try it out. Place the beaker from Section 3 on the work table. This beaker
contains the unreacted aluminum foil in the 0.5 M NaCI solution.
18. Add 70 mL of 1.0 M CuSO4 solution and 70 mL of distilled water to the beaker.
19. Discuss observations and hypotheses about the identity of the products and
reactants in this reaction. Write chemical equations and your explanations for the
reactions.
Scientific Principle
Chemical reactions (single displacement) causing change and forming a new compound; changing temperature, color, and odor.
The reaction of certain elements with each other causes them to go through a chemical reaction known as displacement.
e.g.
Any metal that is higher in the "electromotive series" will displace copper sulphate. Aluminum, is an example of that.
*electromotive series: any element who has a tendency to give up electrons.
CuSO4(aq) + Al(s) ----> Al2SO4(aq) + Cu(s)
Safety Precautions
Copper( II) chloride solution and copper( II) sulfate solution are toxic by ingestion. Small
quantities of hydrogen gas are produced from the reaction. Hydrogen is a highly flammable
gas; keep flammable materials away from the reaction mixture. Wear chemical splash
goggles, chemical-resistant gloves, and a chemical-resistant apron. This activity requires
the use of hazardous chemicals and/or has the potential for hazardous reactions. Please
review the Safety Precautions section and relevant Material Safety Data Sheets before
beginning this activity.