The Single Replacement Reaction

Oct 13, 2025 by orovajewels.com 130 views

Introduction

Chemists often face the challenge of extracting valuable metals from their compounds. In this scenario, a chemist aims to extract copper metal from a copper(II) chloride solution. To achieve this, the chemist uses a single replacement reaction involving aluminum foil. In this article, we will delve into the world of chemistry and explore the process of extracting copper metal from copper(II) chloride solution.

The Single Replacement Reaction

The single replacement reaction between aluminum and copper(II) chloride is a crucial step in extracting copper metal. The reaction is as follows:

$2 \text{Al} + 3 \text{CuCl}_2 \rightarrow 2 \text{AlCl}_3 + 3 \text{Cu}$

In this reaction, aluminum (Al) reacts with copper(II) chloride (CuCl2) to produce aluminum chloride (AlCl3) and copper (Cu). The copper metal is then extracted from the solution.

Calculating the Number of Moles of Aluminum and Copper(II) Chloride

To determine the number of moles of aluminum and copper(II) chloride, we need to calculate their molar masses. The molar mass of aluminum (Al) is 26.98 g/mol, and the molar mass of copper(II) chloride (CuCl2) is 134.45 g/mol.

Given that the chemist places 1.50 grams of aluminum foil in the solution, we can calculate the number of moles of aluminum as follows:

$\text{Number of moles of Al} = \frac{\text{Mass of Al}}{\text{Molar mass of Al}} = \frac{1.50 \text{ g}}{26.98 \text{ g/mol}} = 0.0556 \text{ mol}$

Similarly, given that the solution contains 14 grams of copper(II) chloride, we can calculate the number of moles of copper(II) chloride as follows:

$\text{Number of moles of CuCl}_2 = \frac{\text{Mass of CuCl}_2}{\text{Molar mass of CuCl}_2} = \frac{14 \text{ g}}{134.45 \text{ g/mol}} = 0.104 \text{ mol}$

Determining the Limiting Reactant

To determine the limiting reactant, we need to compare the mole ratio of aluminum to copper(II) chloride with the mole ratio required by the balanced equation. The balanced equation requires a mole ratio of 2:3 (Al:CuCl2).

We can calculate the mole ratio of aluminum to copper(II) chloride as follows:

$\text{Mole ratio of Al to CuCl}_2 = \frac{\text{Number of moles of Al}}{\text{Number of moles of CuCl}_2} = \frac{0.0556 \text{ mol}}{0.104 \text{ mol}} = 0.533$

Since the mole ratio of aluminum to copper(II) chloride is less than the required mole ratio of 2:3, aluminum is the limiting reactant.

Calculating the Number of Moles of Copper Produced

Since aluminum is the limiting reactant, we can calculate the number of moles of copper produced using the mole ratio of aluminum to copper. The balanced equation requires a mole ratio of 2:3 (Al:Cu).

We can calculate the number of moles of copper produced as follows:

$\text{Number of moles of Cu} = \frac{\text{Number of moles of Al}}{2} \times 3 = \frac{0.0556 \text{ mol}}{2} \times 3 = 0.0834 \text{ mol}$

Calculating the Mass of Copper Produced

To calculate the mass of copper produced, we need to multiply the number of moles of copper by its molar mass. The molar mass of copper (Cu) is 63.55 g/mol.

We can calculate the mass of copper produced as follows:

$\text{Mass of Cu} = \text{Number of moles of Cu} \times \text{Molar mass of Cu} = 0.0834 \text{ mol} \times 63.55 \text{ g/mol} = 5.30 \text{ g}$

Conclusion

In this article, we have explored the process of extracting copper metal from a copper(II) chloride solution using a single replacement reaction. We have calculated the number of moles of aluminum and copper(II) chloride, determined the limiting reactant, calculated the number of moles of copper produced, and calculated the mass of copper produced. The results show that the chemist can extract approximately 5.30 grams of copper metal from the solution.

References

Chemistry: An Atoms First Approach by Steven S. Zumdahl
General Chemistry: Principles and Modern Applications by Linus Pauling
Chemical Principles: The Quest for Insight by Steven S. Zumdahl

Glossary

Aluminum (Al): A chemical element with the symbol Al and atomic number 13.
Copper(II) chloride (CuCl2): A chemical compound with the formula CuCl2.
Aluminum chloride (AlCl3): A chemical compound with the formula AlCl3.
Copper (Cu): A chemical element with the symbol Cu and atomic number 29.
Molar mass: The mass of a substance in grams per mole.
Mole ratio: The ratio of the number of moles of two substances.
Limiting reactant: The reactant that is consumed first in a chemical reaction.

Introduction

In our previous article, we explored the process of extracting copper metal from a copper(II) chloride solution using a single replacement reaction. We calculated the number of moles of aluminum and copper(II) chloride, determined the limiting reactant, calculated the number of moles of copper produced, and calculated the mass of copper produced. In this article, we will answer some frequently asked questions related to the extraction of copper metal from copper(II) chloride solution.

Q&A

Q: What is the purpose of using aluminum foil in the extraction of copper metal from copper(II) chloride solution?

A: The purpose of using aluminum foil is to provide a source of aluminum that can react with copper(II) chloride to produce copper metal. Aluminum is a more reactive metal than copper, so it can displace copper from the copper(II) chloride solution.

Q: Why is aluminum the limiting reactant in this reaction?

A: Aluminum is the limiting reactant because it has a lower mole ratio to copper(II) chloride than required by the balanced equation. The balanced equation requires a mole ratio of 2:3 (Al:CuCl2), but the actual mole ratio of aluminum to copper(II) chloride is less than this required ratio.

Q: How can we increase the yield of copper metal in this reaction?

A: To increase the yield of copper metal, we can increase the amount of aluminum foil used in the reaction. This will provide more aluminum to react with copper(II) chloride and produce more copper metal.

Q: What are some common applications of copper metal?

A: Copper metal has many common applications, including:

Electrical wiring: Copper is an excellent conductor of electricity, making it a popular choice for electrical wiring.
Coins: Copper is often used to make coins due to its durability and resistance to corrosion.
Pipes: Copper is used to make pipes for plumbing and other applications due to its resistance to corrosion and ability to withstand high temperatures.
Alloys: Copper is often alloyed with other metals to create strong and corrosion-resistant materials.

Q: What are some common hazards associated with handling copper(II) chloride?

A: Copper(II) chloride is a toxic and corrosive substance that can cause skin and eye irritation, as well as respiratory problems. It is also a strong oxidizing agent that can ignite spontaneously in air.

Q: How can we safely handle copper(II) chloride?

A: To safely handle copper(II) chloride, we should:

Wear protective gear: Wear gloves, goggles, and a face mask to prevent skin and eye irritation and respiratory problems.
Handle in a well-ventilated area: Handle copper(II) chloride in a well-ventilated area to prevent inhalation of fumes.
Avoid skin contact: Avoid skin contact with copper(II) chloride to prevent irritation and corrosion.
Dispose of properly: Dispose of copper(II) chloride in accordance with local regulations and guidelines.

Conclusion

In this article, we have answered some frequently asked questions related to the extraction of copper metal from copper(II) chloride solution. We have discussed the purpose of using aluminum foil, why aluminum is the limiting reactant, how to increase the yield of copper metal, common applications of copper metal, common hazards associated with handling copper(II) chloride, and how to safely handle copper(II) chloride.

References

Chemistry: An Atoms First Approach by Steven S. Zumdahl
General Chemistry: Principles and Modern Applications by Linus Pauling
Chemical Principles: The Quest for Insight by Steven S. Zumdahl

Glossary

Aluminum (Al): A chemical element with the symbol Al and atomic number 13.
Copper(II) chloride (CuCl2): A chemical compound with the formula CuCl2.
Aluminum chloride (AlCl3): A chemical compound with the formula AlCl3.
Copper (Cu): A chemical element with the symbol Cu and atomic number 29.
Molar mass: The mass of a substance in grams per mole.
Mole ratio: The ratio of the number of moles of two substances.
Limiting reactant: The reactant that is consumed first in a chemical reaction.