Calculating the Number of Moles of Copper Produced

Oct 13, 2025 by thesweetdesigns.com 48 views

Introduction

Hydrogen gas is a highly reactive substance that can react with various metal oxides to form metals and water vapor. One such reaction involves hydrogen gas reacting with copper(II) oxide to form copper metal and water vapor. This reaction is a classic example of a redox reaction, where hydrogen gas acts as a reducing agent and copper(II) oxide acts as an oxidizing agent. In this article, we will delve into the details of this reaction and explore how to calculate the number of moles of copper produced when 255 L of hydrogen gas reacts with copper(II) oxide.

The Reaction

The reaction between hydrogen gas and copper(II) oxide is as follows:

{ \text{CuO} + \text{H}_2 \rightarrow \text{Cu} + \text{H}_2\text{O} \}

In this reaction, one mole of copper(II) oxide reacts with one mole of hydrogen gas to produce one mole of copper metal and one mole of water vapor. This reaction is a simple example of a redox reaction, where the oxidation state of copper changes from +2 to 0.

Calculating the Number of Moles of Copper Produced

To calculate the number of moles of copper produced, we need to know the volume of hydrogen gas used in the reaction. The given volume of hydrogen gas is 255 L. We also need to know the molar volume of hydrogen gas at standard temperature and pressure (STP), which is 22.4 L/mol.

Step 1: Convert the Volume of Hydrogen Gas to Moles

To convert the volume of hydrogen gas to moles, we can use the following formula:

{ \text{moles} = \frac{\text{volume (L)}}{\text{molar volume (L/mol)}} \}

Substituting the given values, we get:

{ \text{moles} = \frac{255 \text{ L}}{22.4 \text{ L/mol}} = 11.4 \text{ mol} \}

Step 2: Calculate the Number of Moles of Copper Produced

Since one mole of hydrogen gas reacts with one mole of copper(II) oxide to produce one mole of copper metal, the number of moles of copper produced is equal to the number of moles of hydrogen gas used in the reaction. Therefore, the number of moles of copper produced is also 11.4 mol.

Conclusion

In conclusion, when 255 L of hydrogen gas reacts with copper(II) oxide, 11.4 mol of copper metal is produced. This calculation demonstrates the importance of understanding the stoichiometry of chemical reactions and how to apply it to real-world problems.

Understanding the Stoichiometry of Chemical Reactions

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. It is a crucial concept in chemistry that helps us understand the amounts of substances involved in a reaction. In this article, we have seen how to calculate the number of moles of copper produced when hydrogen gas reacts with copper(II) oxide. This calculation demonstrates the importance of understanding the stoichiometry of chemical reactions and how to apply it to real-world problems.

Applications of Hydrogen Gas in Industry

Hydrogen gas has numerous applications in industry, including the production of chemicals, fuels, and energy. Some of the major applications of hydrogen gas include:

Production of chemicals: Hydrogen gas is used as a reducing agent in the production of chemicals such as ammonia, methanol, and hydrogen peroxide.
Production of fuels: Hydrogen gas is used as a fuel in the production of hydrogen fuel cells, which are used to power vehicles and other devices.
Production of energy: Hydrogen gas is used as a source of energy in the production of electricity, particularly in the form of hydrogen fuel cells.

Conclusion

In conclusion, hydrogen gas is a highly reactive substance that can react with various metal oxides to form metals and water vapor. The reaction between hydrogen gas and copper(II) oxide is a classic example of a redox reaction, where hydrogen gas acts as a reducing agent and copper(II) oxide acts as an oxidizing agent. By understanding the stoichiometry of chemical reactions, we can calculate the number of moles of copper produced when hydrogen gas reacts with copper(II) oxide. This calculation demonstrates the importance of understanding the stoichiometry of chemical reactions and how to apply it to real-world problems.

References

CRC Handbook of Chemistry and Physics: This reference book provides a comprehensive collection of physical and chemical data, including the molar volume of hydrogen gas at STP.
Chemical Reactions and Stoichiometry: This textbook provides a detailed explanation of the stoichiometry of chemical reactions and how to apply it to real-world problems.

Glossary

Molar volume: The volume of one mole of a substance at standard temperature and pressure (STP).
Redox reaction: A chemical reaction in which one substance is reduced (gains electrons) and another substance is oxidized (loses electrons).
Stoichiometry: The branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions.
Hydrogen Gas Reacts with Copper(II) Oxide: A Comprehensive Q&A ====================================================================

Introduction

In our previous article, we explored the reaction between hydrogen gas and copper(II) oxide, and calculated the number of moles of copper produced when 255 L of hydrogen gas reacts with copper(II) oxide. In this article, we will answer some frequently asked questions related to this reaction.

Q: What is the reaction between hydrogen gas and copper(II) oxide?

A: The reaction between hydrogen gas and copper(II) oxide is as follows:

{ \text{CuO} + \text{H}_2 \rightarrow \text{Cu} + \text{H}_2\text{O} \}

In this reaction, one mole of copper(II) oxide reacts with one mole of hydrogen gas to produce one mole of copper metal and one mole of water vapor.

Q: What is the molar volume of hydrogen gas at standard temperature and pressure (STP)?

A: The molar volume of hydrogen gas at STP is 22.4 L/mol.

Q: How many moles of copper are produced when 255 L of hydrogen gas reacts with copper(II) oxide?

A: To calculate the number of moles of copper produced, we need to know the volume of hydrogen gas used in the reaction. We can use the following formula:

{ \text{moles} = \frac{\text{volume (L)}}{\text{molar volume (L/mol)}} \}

Substituting the given values, we get:

{ \text{moles} = \frac{255 \text{ L}}{22.4 \text{ L/mol}} = 11.4 \text{ mol} \}

Therefore, 11.4 mol of copper metal is produced when 255 L of hydrogen gas reacts with copper(II) oxide.

Q: What is the significance of understanding the stoichiometry of chemical reactions?

A: Understanding the stoichiometry of chemical reactions is crucial in chemistry as it helps us understand the quantitative relationships between reactants and products in chemical reactions. It is essential in calculating the amounts of substances involved in a reaction, which is critical in various industrial and scientific applications.

Q: What are some of the major applications of hydrogen gas in industry?

A: Hydrogen gas has numerous applications in industry, including:

Production of chemicals: Hydrogen gas is used as a reducing agent in the production of chemicals such as ammonia, methanol, and hydrogen peroxide.
Production of fuels: Hydrogen gas is used as a fuel in the production of hydrogen fuel cells, which are used to power vehicles and other devices.
Production of energy: Hydrogen gas is used as a source of energy in the production of electricity, particularly in the form of hydrogen fuel cells.

Q: What is the difference between a redox reaction and a non-redox reaction?

A: A redox reaction is a chemical reaction in which one substance is reduced (gains electrons) and another substance is oxidized (loses electrons). A non-redox reaction, on the other hand, is a chemical reaction in which no electrons are transferred between substances.

Q: What is the importance of understanding the concept of molar volume?

A: Understanding the concept of molar volume is crucial in chemistry as it helps us calculate the number of moles of a substance present in a given volume. It is essential in various industrial and scientific applications, including the production of chemicals, fuels, and energy.

Conclusion

In conclusion, the reaction between hydrogen gas and copper(II) oxide is a classic example of a redox reaction, where hydrogen gas acts as a reducing agent and copper(II) oxide acts as an oxidizing agent. By understanding the stoichiometry of chemical reactions, we can calculate the number of moles of copper produced when hydrogen gas reacts with copper(II) oxide. This calculation demonstrates the importance of understanding the stoichiometry of chemical reactions and how to apply it to real-world problems.

References

CRC Handbook of Chemistry and Physics: This reference book provides a comprehensive collection of physical and chemical data, including the molar volume of hydrogen gas at STP.
Chemical Reactions and Stoichiometry: This textbook provides a detailed explanation of the stoichiometry of chemical reactions and how to apply it to real-world problems.

Glossary

Molar volume: The volume of one mole of a substance at standard temperature and pressure (STP).
Redox reaction: A chemical reaction in which one substance is reduced (gains electrons) and another substance is oxidized (loses electrons).
Stoichiometry: The branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions.