Methane Combusts, Releasing 890.1 KJ Of Energy. How Much Methane In Liters Would Be Needed To Generate 2950 KJ Of Energy?a. Is This Reaction Exothermic Or Endothermic?b. Write The $\Delta H$ With The Correct Sign.c. Write The Full, Balanced

Introduction

Methane (CH4) is a potent greenhouse gas that plays a crucial role in various industrial processes, including energy production. When methane combusts, it releases a significant amount of energy, which can be harnessed to generate power. In this article, we will explore the energy released during methane combustion and calculate the amount of methane required to generate a specific amount of energy. We will also analyze the thermodynamic properties of the reaction and determine whether it is exothermic or endothermic.

Methane Combustion Reaction

The combustion reaction of methane is as follows:

CH4 + 2O2 → CO2 + 2H2O

This reaction releases a significant amount of energy, which can be calculated using the enthalpy change (ΔH) of the reaction. The enthalpy change is a measure of the energy released or absorbed during a chemical reaction.

Energy Released During Methane Combustion

The energy released during methane combustion is given as 890.1 kJ per mole of methane. This value represents the enthalpy change (ΔH) of the reaction.

Calculating the Amount of Methane Required

To calculate the amount of methane required to generate 2950 kJ of energy, we can use the following equation:

Amount of methane (in moles) = Energy required (in kJ) / Energy released per mole (in kJ)

Substituting the values, we get:

Amount of methane (in moles) = 2950 kJ / 890.1 kJ/mol = 3.31 mol

Converting Moles to Liters

To convert the amount of methane from moles to liters, we need to know the molar volume of methane at standard temperature and pressure (STP). The molar volume of methane at STP is 22.4 liters per mole.

Therefore, the amount of methane required to generate 2950 kJ of energy is:

Amount of methane (in liters) = 3.31 mol x 22.4 L/mol = 74.1 L

Is the Reaction Exothermic or Endothermic?

An exothermic reaction is one that releases energy, while an endothermic reaction is one that absorbs energy. Since the combustion reaction of methane releases energy, it is an exothermic reaction.

Writing the ΔH with the Correct Sign

The enthalpy change (ΔH) of an exothermic reaction is negative, indicating that energy is released during the reaction. Therefore, the ΔH of the methane combustion reaction is:

ΔH = -890.1 kJ/mol

Full, Balanced Equation

The full, balanced equation for the methane combustion reaction is:

CH4 + 2O2 → CO2 + 2H2O

Conclusion

In this article, we calculated the amount of methane required to generate 2950 kJ of energy and analyzed the thermodynamic properties of the reaction. We determined that the reaction is exothermic and wrote the ΔH with the correct sign. The full, balanced equation for the methane combustion reaction is also provided.

References

• [1] CRC Handbook of Chemistry and Physics, 97th Edition.
• [2] Atkins, P. W., & de Paula, J. (2010). Physical Chemistry. Oxford University Press.

Additional Information

• The energy released during methane combustion is a significant contributor to the greenhouse effect.
• Methane combustion is a major source of energy production, particularly in the form of natural gas.
• The thermodynamic properties of the methane combustion reaction are critical in understanding the energy released during the reaction.
  Methane Combustion: Q&A =========================

Q: What is the primary source of energy released during methane combustion?

A: The primary source of energy released during methane combustion is the breaking of chemical bonds between the carbon and hydrogen atoms in the methane molecule.

Q: How does the energy released during methane combustion compare to other energy sources?

A: The energy released during methane combustion is comparable to other fossil fuels, such as coal and oil. However, methane has a higher energy density than these fuels, making it a more efficient energy source.

Q: What are the environmental implications of methane combustion?

A: Methane combustion releases carbon dioxide, a greenhouse gas, into the atmosphere, contributing to climate change. Additionally, the combustion process can release other pollutants, such as nitrogen oxides and particulate matter, which can have negative impacts on air quality and human health.

Q: Can methane combustion be used to generate electricity?

A: Yes, methane combustion can be used to generate electricity through the use of gas turbines or internal combustion engines. The energy released during combustion is converted into mechanical energy, which is then used to drive a generator and produce electricity.

Q: What are the advantages of using methane combustion for energy production?

A: The advantages of using methane combustion for energy production include:

• High energy density: Methane has a high energy density, making it a efficient energy source.
• Wide availability: Methane is widely available, particularly in the form of natural gas.
• Low emissions: Compared to other fossil fuels, methane combustion has relatively low emissions of pollutants and greenhouse gases.

Q: What are the disadvantages of using methane combustion for energy production?

A: The disadvantages of using methane combustion for energy production include:

• Greenhouse gas emissions: Methane combustion releases carbon dioxide, a greenhouse gas, into the atmosphere.
• Air pollution: The combustion process can release other pollutants, such as nitrogen oxides and particulate matter, which can have negative impacts on air quality and human health.
• Energy efficiency: The energy efficiency of methane combustion can be lower than other energy sources, such as solar or wind power.

Q: Can methane combustion be used in combination with other energy sources?

A: Yes, methane combustion can be used in combination with other energy sources, such as solar or wind power, to create a hybrid energy system. This can help to reduce greenhouse gas emissions and improve energy efficiency.

Q: What are the future prospects for methane combustion as an energy source?

A: The future prospects for methane combustion as an energy source are uncertain. While methane has a high energy density and is widely available, the environmental implications of its combustion are a major concern. As the world transitions to cleaner energy sources, such as solar and wind power, the role of methane combustion in energy production may decline.

Q: Can methane combustion be used in transportation?

A: Yes, methane combustion can be used in transportation, particularly in the form of compressed natural gas (CNG) or liquefied natural gas (LNG). CNG and LNG are used as fuels for vehicles, such as buses and trucks, and can offer a cleaner alternative to traditional fossil fuels.

Q: What are the safety considerations for methane combustion?

A: The safety considerations for methane combustion include:

• Explosion risk: Methane is a highly flammable gas, and its combustion can be explosive if not handled properly.
• Fire risk: Methane combustion can also be a fire hazard if not properly contained.
• Ventilation: Proper ventilation is essential to prevent the accumulation of methane and other gases in enclosed spaces.

Q: Can methane combustion be used in industrial processes?

A: Yes, methane combustion can be used in industrial processes, such as in the production of chemicals and fuels. The high energy density of methane makes it an attractive fuel for industrial applications.

Q: What are the economic implications of methane combustion?

A: The economic implications of methane combustion include:

• Cost: The cost of methane combustion can be lower than other energy sources, particularly in the form of natural gas.
• Energy efficiency: The energy efficiency of methane combustion can be lower than other energy sources, which can impact its overall cost-effectiveness.
• Environmental regulations: The environmental implications of methane combustion are subject to regulations, which can impact its cost and feasibility.