Determining the Amount of Energy Released

Oct 13, 2025 by recoveryshake.com 120 views

Understanding the Combustion Reaction

The combustion of ethene, C2H4, is a chemical reaction that involves the reaction of ethene with oxygen to produce carbon dioxide and water. This reaction is exothermic, meaning that it releases energy in the form of heat. The balanced chemical equation for the combustion of ethene is:

C2H4 + 3O2 → 2CO2 + H2O

ΔH = -1390 kJ

Determining the Amount of Energy Released

To determine the amount of energy released when 2.3 moles of ethene is combusted, we need to use the given balanced chemical equation and the value of ΔH. The equation shows that 1 mole of ethene releases 1390 kJ of energy when it is combusted. To find the amount of energy released when 2.3 moles of ethene is combusted, we can multiply the value of ΔH by the number of moles of ethene.

Calculating the Energy Released

To calculate the energy released, we can use the following formula:

Energy Released = ΔH x Number of Moles

Plugging in the values, we get:

Energy Released = -1390 kJ x 2.3 moles

Energy Released = -3193 kJ

Interpreting the Results

The negative sign in the result indicates that the reaction is exothermic, meaning that it releases energy. The magnitude of the result, 3193 kJ, indicates the amount of energy released when 2.3 moles of ethene is combusted.

Significance of the Results

The combustion of ethene is an important reaction in various industrial processes, such as the production of plastics and other organic compounds. The energy released during this reaction can be harnessed and used to power machinery or generate electricity.

Conclusion

In conclusion, the combustion of ethene is an exothermic reaction that releases a significant amount of energy. By using the balanced chemical equation and the value of ΔH, we can determine the amount of energy released when a given number of moles of ethene is combusted. This information can be useful in various industrial and scientific applications.

Limitations of the Study

One limitation of this study is that it assumes that the reaction is carried out under ideal conditions, with no losses due to heat transfer or other factors. In reality, the reaction may not be as efficient, and the actual energy released may be different from the calculated value.

Future Directions

Future studies could investigate the effects of different conditions, such as temperature and pressure, on the energy released during the combustion of ethene. Additionally, researchers could explore the use of ethene as a fuel source in various applications, such as power generation or transportation.

References

[1] ChemGuide. (n.d.). Combustion of ethene. Retrieved from https://www.chemguide.co.uk/inorganic/analysis/combustion/ethene.html
[2] Wikipedia. (n.d.). Ethene. Retrieved from https://en.wikipedia.org/wiki/Ethene

Glossary

Exothermic reaction: A chemical reaction that releases energy in the form of heat.
ΔH: The change in enthalpy, which is a measure of the energy released or absorbed during a reaction.
Mole: A unit of measurement that represents 6.022 x 10^23 particles (such as atoms or molecules).
Combustion: A chemical reaction that involves the reaction of a fuel with oxygen to produce heat and light.

Understanding the Combustion Reaction

C2H4 + 3O2 → 2CO2 + H2O

ΔH = -1390 kJ

Q&A: The Combustion of Ethene

Q: What is the combustion of ethene?

A: The combustion of ethene is a chemical reaction that involves the reaction of ethene with oxygen to produce carbon dioxide and water.

Q: Is the combustion of ethene an exothermic reaction?

A: Yes, the combustion of ethene is an exothermic reaction, meaning that it releases energy in the form of heat.

Q: What is the balanced chemical equation for the combustion of ethene?

A: The balanced chemical equation for the combustion of ethene is:

C2H4 + 3O2 → 2CO2 + H2O

Q: What is the value of ΔH for the combustion of ethene?

A: The value of ΔH for the combustion of ethene is -1390 kJ.

Q: How can we determine the amount of energy released when 2.3 moles of ethene is combusted?

A: We can determine the amount of energy released by multiplying the value of ΔH by the number of moles of ethene.

Q: What is the significance of the combustion of ethene?

A: The combustion of ethene is an important reaction in various industrial processes, such as the production of plastics and other organic compounds. The energy released during this reaction can be harnessed and used to power machinery or generate electricity.

Q: What are some limitations of this study?

A: One limitation of this study is that it assumes that the reaction is carried out under ideal conditions, with no losses due to heat transfer or other factors. In reality, the reaction may not be as efficient, and the actual energy released may be different from the calculated value.

Q: What are some future directions for this study?

A: Future studies could investigate the effects of different conditions, such as temperature and pressure, on the energy released during the combustion of ethene. Additionally, researchers could explore the use of ethene as a fuel source in various applications, such as power generation or transportation.

Glossary

Exothermic reaction: A chemical reaction that releases energy in the form of heat.
ΔH: The change in enthalpy, which is a measure of the energy released or absorbed during a reaction.
Mole: A unit of measurement that represents 6.022 x 10^23 particles (such as atoms or molecules).
Combustion: A chemical reaction that involves the reaction of a fuel with oxygen to produce heat and light.

References

[1] ChemGuide. (n.d.). Combustion of ethene. Retrieved from https://www.chemguide.co.uk/inorganic/analysis/combustion/ethene.html
[2] Wikipedia. (n.d.). Ethene. Retrieved from https://en.wikipedia.org/wiki/Ethene

Additional Resources

National Institute of Standards and Technology. (n.d.). Enthalpy of combustion of ethene. Retrieved from https://webbook.nist.gov/cgi/cbook.cgi?ID=C74-85-1&Units=SI&Mask=0#Thermo
Chemical Abstracts Service. (n.d.). Ethene. Retrieved from https://pubchem.ncbi.nlm.nih.gov/compound/Ethene