Calculating the Number of Moles of CH4

Oct 13, 2025 by orovajewels.com 107 views

Introduction

The combustion of methane (CH4) is a fundamental chemical reaction that produces carbon dioxide (CO2) and water (H2O) as byproducts. Understanding the stoichiometry of this reaction is crucial in various fields, including chemistry, environmental science, and engineering. In this article, we will explore the production of carbon dioxide from the combustion of 110 g of CH4.

The Combustion Reaction

The combustion reaction of CH4 is represented by the following equation:

${CH_4 + 2 O_2 \rightarrow CO_2 + 2 H_2O}$

This equation indicates that one mole of CH4 reacts with two moles of O2 to produce one mole of CO2 and two moles of H2O.

Molar Mass of CH4

To determine the number of moles of CH4, we need to calculate its molar mass. The atomic masses of C and H are 12.01 g/mol and 1.008 g/mol, respectively. Therefore, the molar mass of CH4 is:

${M_{CH_4} = 12.01 + 4(1.008) = 16.042 \text{ g/mol}}$

Calculating the Number of Moles of CH4

Given that we have 110 g of CH4, we can calculate the number of moles using the following formula:

${n_{CH_4} = \frac{m_{CH_4}}{M_{CH_4}}}$

where ${n_{CH_4}}$ is the number of moles of CH4, ${m_{CH_4}}$ is the mass of CH4, and ${M_{CH_4}}$ is the molar mass of CH4.

Plugging in the values, we get:

${n_{CH_4} = \frac{110 \text{ g}}{16.042 \text{ g/mol}} = 6.87 \text{ mol}}$

Stoichiometry of the Reaction

According to the combustion reaction equation, one mole of CH4 produces one mole of CO2. Therefore, the number of moles of CO2 produced is equal to the number of moles of CH4.

Calculating the Number of Moles of CO2

Using the number of moles of CH4 calculated earlier, we can determine the number of moles of CO2 produced:

${n_{CO_2} = n_{CH_4} = 6.87 \text{ mol}}$

Conclusion

In conclusion, the combustion of 110 g of CH4 produces 6.87 moles of CO2. This calculation is based on the stoichiometry of the combustion reaction and the molar mass of CH4.

Limitations and Future Directions

While this calculation provides a quantitative understanding of the production of CO2 from the combustion of CH4, there are several limitations and future directions to consider. For example, the calculation assumes that the reaction occurs under ideal conditions, which may not be the case in real-world scenarios. Additionally, the calculation does not take into account the presence of other reactants or products that may affect the stoichiometry of the reaction.

References

[1] Lide, D. R. (2004). CRC Handbook of Chemistry and Physics. CRC Press.
[2] Atkins, P. W., & de Paula, J. (2010). Physical Chemistry. Oxford University Press.

Additional Resources

[1] National Institute of Standards and Technology (NIST). (n.d.). Molar Mass of CH4.
[2] Chemistry LibreTexts. (n.d.). Combustion Reaction of Methane.

Keywords

CH4
CO2
Combustion reaction
Stoichiometry
Molar mass
Chemical reaction
Environmental science
Engineering

Introduction

In our previous article, we explored the production of carbon dioxide (CO2) from the combustion of 110 g of methane (CH4). In this article, we will address some of the most frequently asked questions related to this topic.

Q1: What is the combustion reaction of CH4?

A1: The combustion reaction of CH4 is represented by the following equation:

${CH_4 + 2 O_2 \rightarrow CO_2 + 2 H_2O}$

This equation indicates that one mole of CH4 reacts with two moles of O2 to produce one mole of CO2 and two moles of H2O.

Q2: What is the molar mass of CH4?

A2: The molar mass of CH4 is 16.042 g/mol, which is calculated by adding the atomic masses of C and H:

${M_{CH_4} = 12.01 + 4(1.008) = 16.042 \text{ g/mol}}$

Q3: How many moles of CH4 are produced from 110 g of CH4?

A3: To calculate the number of moles of CH4, we use the following formula:

${n_{CH_4} = \frac{m_{CH_4}}{M_{CH_4}}}$

where ${n_{CH_4}}$ is the number of moles of CH4, ${m_{CH_4}}$ is the mass of CH4, and ${M_{CH_4}}$ is the molar mass of CH4.

Plugging in the values, we get:

${n_{CH_4} = \frac{110 \text{ g}}{16.042 \text{ g/mol}} = 6.87 \text{ mol}}$

Q4: How many moles of CO2 are produced from the combustion of 110 g of CH4?

A4: According to the combustion reaction equation, one mole of CH4 produces one mole of CO2. Therefore, the number of moles of CO2 produced is equal to the number of moles of CH4:

${n_{CO_2} = n_{CH_4} = 6.87 \text{ mol}}$

Q5: What are some of the limitations of this calculation?

A5: While this calculation provides a quantitative understanding of the production of CO2 from the combustion of CH4, there are several limitations to consider. For example, the calculation assumes that the reaction occurs under ideal conditions, which may not be the case in real-world scenarios. Additionally, the calculation does not take into account the presence of other reactants or products that may affect the stoichiometry of the reaction.

Q6: What are some of the applications of this calculation?

A6: This calculation has several applications in various fields, including:

Environmental science: Understanding the production of CO2 from the combustion of CH4 is crucial in assessing the impact of human activities on the environment.
Engineering: This calculation is used in the design of combustion systems, such as engines and furnaces.
Chemistry: This calculation is used in the study of chemical reactions and the development of new fuels.

Q7: How can I calculate the mass of CO2 produced from the combustion of CH4?

A7: To calculate the mass of CO2 produced, we need to multiply the number of moles of CO2 by its molar mass. The molar mass of CO2 is 44.01 g/mol. Therefore, the mass of CO2 produced is:

${m_{CO_2} = n_{CO_2} \times M_{CO_2} = 6.87 \text{ mol} \times 44.01 \text{ g/mol} = 301.5 \text{ g}}$

Q8: What are some of the safety considerations when working with CH4 and CO2?

A8: When working with CH4 and CO2, it is essential to follow proper safety protocols to avoid accidents and injuries. Some of the safety considerations include:

Handling CH4 and CO2 in well-ventilated areas to prevent the buildup of flammable gases.
Using proper equipment and protective gear when handling CH4 and CO2.
Following proper procedures for storing and disposing of CH4 and CO2.

Conclusion

In conclusion, the combustion of CH4 produces CO2 as a byproduct. Understanding the stoichiometry of this reaction is crucial in various fields, including environmental science, engineering, and chemistry. This Q&A article provides a comprehensive overview of the combustion reaction of CH4 and the production of CO2.

References

[1] Lide, D. R. (2004). CRC Handbook of Chemistry and Physics. CRC Press.
[2] Atkins, P. W., & de Paula, J. (2010). Physical Chemistry. Oxford University Press.

Additional Resources

[1] National Institute of Standards and Technology (NIST). (n.d.). Molar Mass of CH4.
[2] Chemistry LibreTexts. (n.d.). Combustion Reaction of Methane.

Keywords

CH4
CO2
Combustion reaction
Stoichiometry
Molar mass
Chemical reaction
Environmental science
Engineering