Calculating the Molar Mass of Copper Carbonate

Oct 13, 2025 by pynkocean.com 144 views

Introduction

Copper carbonate is a chemical compound that decomposes into copper oxide and carbon dioxide through a thermal decomposition reaction. The reaction is as follows:

${ CuCO_3 \rightarrow CuO + CO_2 }$

In this reaction, copper carbonate (CuCO3) decomposes into copper oxide (CuO) and carbon dioxide (CO2). The relative formula masses of the compounds involved in this reaction are essential in determining the amount of copper oxide produced when a given mass of copper carbonate decomposes.

Calculating the Molar Mass of Copper Carbonate

To calculate the amount of copper oxide produced, we first need to determine the molar mass of copper carbonate (CuCO3). The relative formula masses of the elements involved in copper carbonate are:

Copper (Cu): 63.5 g/mol
Carbon (C): 12.0 g/mol
Oxygen (O): 16.0 g/mol

The molar mass of copper carbonate (CuCO3) is calculated as follows:

Molar mass of CuCO3 = (1 x 63.5) + (1 x 12.0) + (3 x 16.0) Molar mass of CuCO3 = 63.5 + 12.0 + 48.0 Molar mass of CuCO3 = 123.5 g/mol

Calculating the Molar Mass of Copper Oxide

Next, we need to determine the molar mass of copper oxide (CuO). The relative formula masses of the elements involved in copper oxide are:

Copper (Cu): 63.5 g/mol
Oxygen (O): 16.0 g/mol

The molar mass of copper oxide (CuO) is calculated as follows:

Molar mass of CuO = (1 x 63.5) + (1 x 16.0) Molar mass of CuO = 63.5 + 16.0 Molar mass of CuO = 79.5 g/mol

Calculating the Amount of Copper Oxide Produced

Given that 247 g of copper carbonate fully decomposes, we can calculate the amount of copper oxide produced using the following steps:

Calculate the number of moles of copper carbonate: Number of moles of CuCO3 = mass of CuCO3 / molar mass of CuCO3 Number of moles of CuCO3 = 247 g / 123.5 g/mol Number of moles of CuCO3 = 2.00 mol
Since the reaction is a 1:1 decomposition, the number of moles of copper oxide produced is equal to the number of moles of copper carbonate: Number of moles of CuO = number of moles of CuCO3 Number of moles of CuO = 2.00 mol
Calculate the mass of copper oxide produced: Mass of CuO = number of moles of CuO x molar mass of CuO Mass of CuO = 2.00 mol x 79.5 g/mol Mass of CuO = 159 g

Conclusion

In conclusion, when 247 g of copper carbonate fully decomposes, 159 g of copper oxide is produced. This calculation is based on the relative formula masses of the compounds involved in the decomposition reaction and the stoichiometry of the reaction.

Limitations and Future Work

This calculation assumes that the copper carbonate is pure and that the decomposition reaction is 100% efficient. In reality, the purity of the copper carbonate and the efficiency of the decomposition reaction may affect the actual amount of copper oxide produced. Future work could involve investigating the effects of impurities and reaction efficiency on the amount of copper oxide produced.

Applications of Copper Oxide

Copper oxide has several applications, including:

Catalysts: Copper oxide is used as a catalyst in various chemical reactions, including the production of nitric acid and the oxidation of ammonia.
Electrodes: Copper oxide is used as an electrode material in batteries and fuel cells.
Pigments: Copper oxide is used as a pigment in paints and coatings.
Antimicrobial agents: Copper oxide has antimicrobial properties and is used in medical applications, such as wound dressings and implantable devices.

Conclusion

In conclusion, the calculation of the amount of copper oxide produced when 247 g of copper carbonate fully decomposes is a straightforward application of the principles of stoichiometry and the relative formula masses of the compounds involved. The result of this calculation has implications for the production and application of copper oxide in various fields.

Introduction

In our previous article, we discussed the decomposition reaction of copper carbonate (CuCO3) into copper oxide (CuO) and carbon dioxide (CO2). We also calculated the amount of copper oxide produced when 247 g of copper carbonate fully decomposes. In this article, we will address some frequently asked questions related to this topic.

Q: What is the purpose of calculating the molar mass of copper carbonate?

A: The molar mass of copper carbonate is calculated to determine the number of moles of copper carbonate present in a given mass. This is essential in calculating the amount of copper oxide produced in the decomposition reaction.

Q: Why is the molar mass of copper oxide important?

A: The molar mass of copper oxide is important because it is used to calculate the mass of copper oxide produced in the decomposition reaction. This is essential in determining the amount of copper oxide produced.

Q: What is the significance of the 1:1 decomposition ratio in the reaction?

A: The 1:1 decomposition ratio in the reaction means that for every mole of copper carbonate that decomposes, one mole of copper oxide is produced. This is essential in calculating the amount of copper oxide produced.

Q: Can the decomposition reaction of copper carbonate be affected by external factors?

A: Yes, the decomposition reaction of copper carbonate can be affected by external factors such as temperature, pressure, and the presence of impurities. These factors can affect the rate and efficiency of the reaction.

Q: What are some common applications of copper oxide?

A: Copper oxide has several applications, including:

Catalysts: Copper oxide is used as a catalyst in various chemical reactions, including the production of nitric acid and the oxidation of ammonia.
Electrodes: Copper oxide is used as an electrode material in batteries and fuel cells.
Pigments: Copper oxide is used as a pigment in paints and coatings.
Antimicrobial agents: Copper oxide has antimicrobial properties and is used in medical applications, such as wound dressings and implantable devices.

Q: Can copper oxide be produced through other methods?

A: Yes, copper oxide can be produced through other methods, including:

Reduction of copper(II) sulfate: Copper oxide can be produced by reducing copper(II) sulfate with a reducing agent such as hydrogen gas.
Thermal decomposition of copper(II) nitrate: Copper oxide can be produced by thermally decomposing copper(II) nitrate.

Q: What are some common sources of copper carbonate?

A: Copper carbonate can be found in nature in the form of minerals such as azurite and malachite. It can also be synthesized in the laboratory through the reaction of copper(II) oxide with carbon dioxide.

Q: Can copper carbonate be used as a source of copper?

A: Yes, copper carbonate can be used as a source of copper. It can be decomposed to produce copper oxide, which can then be reduced to produce copper metal.

Conclusion

In conclusion, the decomposition reaction of copper carbonate into copper oxide and carbon dioxide is an important chemical reaction with several applications. The calculation of the amount of copper oxide produced when 247 g of copper carbonate fully decomposes is a straightforward application of the principles of stoichiometry and the relative formula masses of the compounds involved. We hope that this Q&A article has provided a better understanding of this topic and its significance in chemistry.