A Chemist Wants To Extract Copper Metal From A Copper Chloride Solution. The Chemist Places 1.50 Grams Of Aluminum Foil In A Solution Of 14 Grams Of Copper (II) Chloride. A Single Replacement Reaction Takes Place:$[ 2 \text{Al} + 3 \text{CuCl}_2

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 chloride solution. To achieve this, the chemist employs a single replacement reaction, which involves the reaction of aluminum foil with copper (II) chloride. In this article, we will delve into the details of this reaction, exploring the chemical principles behind it and the calculations involved.

The Single Replacement Reaction

The single replacement reaction between aluminum foil and copper (II) chloride can be represented by the following equation:

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

In this reaction, aluminum (Al) displaces copper (Cu) from the copper (II) chloride solution, resulting in the formation of aluminum chloride (AlCl3) and copper metal (Cu). This reaction is a classic example of a single replacement reaction, where one element displaces another element from a compound.

Calculating the Number of Moles of Aluminum

To calculate the number of moles of aluminum, we need to know the molar mass of aluminum. The molar mass of aluminum is 26.98 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:

${ \text{Number of moles of Al} = \frac{\text{Mass of Al}}{\text{Molar mass of Al}} }$

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

${ \text{Number of moles of Al} = 0.0556 \text{ mol} }$

Calculating the Number of Moles of Copper (II) Chloride

To calculate the number of moles of copper (II) chloride, we need to know the molar mass of copper (II) chloride. The molar mass of copper (II) chloride is 170.48 g/mol. Given that the solution contains 14 grams of copper (II) chloride, we can calculate the number of moles of copper (II) chloride as follows:

${ \text{Number of moles of CuCl}_2 = \frac{\text{Mass of CuCl}_2}{\text{Molar mass of CuCl}_2} }$

${ \text{Number of moles of CuCl}_2 = \frac{14 \text{ g}}{170.48 \text{ g/mol}} }$

${ \text{Number of moles of CuCl}_2 = 0.0821 \text{ mol} }$

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:

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

${ \text{Mole ratio of Al to CuCl}_2 = \frac{0.0556 \text{ mol}}{0.0821 \text{ mol}} }$

${ \text{Mole ratio of Al to CuCl}_2 = 0.678 }$

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

Calculating the Mass of Copper Metal Produced

To calculate the mass of copper metal produced, we need to know the molar mass of copper. The molar mass of copper is 63.55 g/mol. Since aluminum is the limiting reactant, we can calculate the number of moles of copper metal produced as follows:

${ \text{Number of moles of Cu} = \frac{\text{Number of moles of Al}}{2} }$

${ \text{Number of moles of Cu} = \frac{0.0556 \text{ mol}}{2} }$

${ \text{Number of moles of Cu} = 0.0278 \text{ mol} }$

We can then calculate the mass of copper metal produced as follows:

${ \text{Mass of Cu} = \text{Number of moles of Cu} \times \text{Molar mass of Cu} }$

${ \text{Mass of Cu} = 0.0278 \text{ mol} \times 63.55 \text{ g/mol} }$

${ \text{Mass of Cu} = 1.77 \text{ g} }$

Conclusion

In this article, we have explored the single replacement reaction between aluminum foil and copper (II) chloride. We have calculated the number of moles of aluminum and copper (II) chloride, determined the limiting reactant, and calculated the mass of copper metal produced. This reaction is a classic example of a single replacement reaction, where one element displaces another element from a compound. The chemist's quest to extract copper metal from copper chloride solution has been successfully achieved.

References

• Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2006). General Chemistry: Principles and Modern Applications. Pearson Prentice Hall.
• Atkins, P. W., & De Paula, J. (2006). Physical Chemistry. Oxford University Press.

Further Reading

• Single replacement reactions: A comprehensive review of single replacement reactions, including examples and applications.
• Copper (II) chloride: A detailed discussion of the properties and reactions of copper (II) chloride.
• Aluminum: A comprehensive review of the properties and reactions of aluminum.
  A Chemist's Quest: Extracting Copper Metal from Copper Chloride Solution - Q&A ====================================================================

Introduction

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

Q: What is the purpose of using aluminum foil in this reaction?

A: The purpose of using aluminum foil in this reaction is to displace copper from the copper (II) chloride solution. Aluminum is a more reactive metal than copper, and it can displace copper from its compounds.

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

A: Aluminum is the limiting reactant in this reaction 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 is 0.678:1 (Al:CuCl2). This means that there is not enough aluminum to react with all of the copper (II) chloride, making aluminum the limiting reactant.

Q: What is the significance of the mole ratio in this reaction?

A: The mole ratio is significant in this reaction because it determines the amount of product that will be formed. In this case, the mole ratio of aluminum to copper (II) chloride determines the amount of copper metal that will be produced.

Q: Can this reaction be used to extract copper metal from other copper compounds?

A: Yes, this reaction can be used to extract copper metal from other copper compounds. However, the reaction conditions and the amount of reactants required may vary depending on the specific compound being used.

Q: What are some potential applications of this reaction?

A: Some potential applications of this reaction include:

• Extracting copper metal from copper-rich ores
• Producing copper metal for use in electronics and other industries
• Developing new methods for extracting copper metal from copper compounds

Q: What are some potential hazards associated with this reaction?

A: Some potential hazards associated with this reaction include:

• The release of toxic gases, such as hydrogen chloride, during the reaction
• The formation of highly reactive compounds, such as aluminum chloride
• The potential for fires or explosions if the reaction is not properly controlled

Q: How can this reaction be scaled up for industrial use?

A: This reaction can be scaled up for industrial use by increasing the amount of reactants and using larger reaction vessels. However, it is also important to consider the potential hazards associated with the reaction and to take steps to mitigate them.

Conclusion

In this article, we have answered some frequently asked questions related to the single replacement reaction between aluminum foil and copper (II) chloride. We have discussed the purpose of using aluminum foil in this reaction, why aluminum is the limiting reactant, the significance of the mole ratio, and some potential applications and hazards associated with this reaction. We hope that this article has provided a useful overview of this reaction and its potential uses.

References

• Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2006). General Chemistry: Principles and Modern Applications. Pearson Prentice Hall.
• Atkins, P. W., & De Paula, J. (2006). Physical Chemistry. Oxford University Press.

Further Reading

• Single replacement reactions: A comprehensive review of single replacement reactions, including examples and applications.
• Copper (II) chloride: A detailed discussion of the properties and reactions of copper (II) chloride.
• Aluminum: A comprehensive review of the properties and reactions of aluminum.