Which Of The Following Statements About The Combustion Of Glucose With Oxygen To Form Water And Carbon Dioxide ($C_6H_{12}O_6 + 6O_2 \rightarrow 6CO_2 + 6H_2O$) Is Correct?A. The Entropy Of The Universe Decreases As The Result Of This

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Introduction

The combustion of glucose with oxygen is a fundamental chemical reaction that has been extensively studied in the field of chemistry. This reaction is a classic example of a redox reaction, where glucose (C6H12O6) reacts with oxygen (O2) to form carbon dioxide (CO2) and water (H2O). In this article, we will examine the statements about this reaction and determine which one is correct.

The Balanced Chemical Equation

The balanced chemical equation for the combustion of glucose with oxygen is:

C6H12O6 + 6O2 → 6CO2 + 6H2O

This equation indicates that one molecule of glucose reacts with six molecules of oxygen to produce six molecules of carbon dioxide and six molecules of water.

Entropy and the Second Law of Thermodynamics

Entropy is a measure of the disorder or randomness of a system. The second law of thermodynamics states that the total entropy of an isolated system will always increase over time. However, in the case of the combustion of glucose with oxygen, the entropy of the universe does not decrease.

Statement A: The Entropy of the Universe Decreases

The entropy of the universe is a measure of the total disorder or randomness of the universe. In the case of the combustion of glucose with oxygen, the entropy of the universe does not decrease. Instead, the entropy of the system (the glucose and oxygen molecules) increases as the reaction proceeds.

Explanation

When glucose and oxygen react, the bonds between the atoms are broken and new bonds are formed. This process increases the disorder or randomness of the system, resulting in an increase in entropy. The entropy of the universe, on the other hand, is determined by the total disorder or randomness of the universe, including the system and its surroundings.

The Surroundings

The surroundings of the system include the environment in which the reaction takes place. In the case of the combustion of glucose with oxygen, the surroundings include the air, the container, and any other objects that may be present. The entropy of the surroundings also increases as the reaction proceeds, as the heat and light released by the reaction increase the disorder or randomness of the surroundings.

Conclusion

In conclusion, the entropy of the universe does not decrease as a result of the combustion of glucose with oxygen. Instead, the entropy of the system and its surroundings increases as the reaction proceeds. This is in accordance with the second law of thermodynamics, which states that the total entropy of an isolated system will always increase over time.

Additional Considerations

There are several additional considerations that are relevant to the combustion of glucose with oxygen. These include:

  • Energy Release: The combustion of glucose with oxygen releases a significant amount of energy in the form of heat and light. This energy is released as the bonds between the atoms are broken and new bonds are formed.
  • Carbon Dioxide Emissions: The combustion of glucose with oxygen produces carbon dioxide as a byproduct. This is a greenhouse gas that contributes to climate change.
  • Water Production: The combustion of glucose with oxygen produces water as a byproduct. This is a valuable resource that is essential for life.

Conclusion

In conclusion, the combustion of glucose with oxygen is a complex process that involves the breaking and forming of bonds between atoms. The entropy of the universe does not decrease as a result of this reaction, but instead increases as the system and its surroundings become more disordered or random. This is in accordance with the second law of thermodynamics, which states that the total entropy of an isolated system will always increase over time.

References

  • Levine, I. N. (2008). Physical Chemistry. 6th ed. New York: McGraw-Hill.
  • Atkins, P. W. (2007). Physical Chemistry. 9th ed. New York: Oxford University Press.
  • Kotz, J. C. (2008). Chemistry and Chemical Reactivity. 8th ed. New York: Thomson Brooks/Cole.

Glossary

  • Entropy: A measure of the disorder or randomness of a system.
  • Second Law of Thermodynamics: A law that states that the total entropy of an isolated system will always increase over time.
  • Redox Reaction: A chemical reaction in which one substance is oxidized and another substance is reduced.
  • Carbon Dioxide: A greenhouse gas that contributes to climate change.
  • Water: A valuable resource that is essential for life.
    Q&A: The Combustion of Glucose with Oxygen =============================================

Introduction

In our previous article, we discussed the combustion of glucose with oxygen and the concept of entropy. In this article, we will answer some frequently asked questions about this topic.

Q: What is the purpose of the combustion of glucose with oxygen?

A: The combustion of glucose with oxygen is a fundamental chemical reaction that releases energy in the form of heat and light. This energy is essential for many biological processes, including the production of ATP (adenosine triphosphate), which is the energy currency of the cell.

Q: What is the role of oxygen in the combustion of glucose?

A: Oxygen plays a crucial role in the combustion of glucose. It is the reactant that allows the glucose molecule to break down and release energy. Without oxygen, the glucose molecule would not be able to undergo combustion and release energy.

Q: What is the byproduct of the combustion of glucose with oxygen?

A: The byproducts of the combustion of glucose with oxygen are carbon dioxide and water. Carbon dioxide is a greenhouse gas that contributes to climate change, while water is a valuable resource that is essential for life.

Q: Is the combustion of glucose with oxygen an exothermic reaction?

A: Yes, the combustion of glucose with oxygen is an exothermic reaction. This means that it releases energy in the form of heat and light. The energy released during this reaction is what makes it possible for many biological processes to occur.

Q: What is the significance of the second law of thermodynamics in the combustion of glucose with oxygen?

A: The second law of thermodynamics states that the total entropy of an isolated system will always increase over time. In the case of the combustion of glucose with oxygen, the entropy of the system and its surroundings increases as the reaction proceeds. This is in accordance with the second law of thermodynamics.

Q: Can the combustion of glucose with oxygen be used to produce energy?

A: Yes, the combustion of glucose with oxygen can be used to produce energy. This is because the reaction releases energy in the form of heat and light. However, it is not a very efficient way to produce energy, as most of the energy released is lost as heat.

Q: What are some of the limitations of the combustion of glucose with oxygen?

A: Some of the limitations of the combustion of glucose with oxygen include:

  • Low energy yield: The combustion of glucose with oxygen releases a relatively small amount of energy compared to other energy-producing reactions.
  • Carbon dioxide emissions: The combustion of glucose with oxygen produces carbon dioxide as a byproduct, which contributes to climate change.
  • Water production: The combustion of glucose with oxygen produces water as a byproduct, which can be a problem in certain environments.

Q: Can the combustion of glucose with oxygen be used to produce biofuels?

A: Yes, the combustion of glucose with oxygen can be used to produce biofuels. Biofuels are fuels that are produced from organic matter, such as plants and microorganisms. The combustion of glucose with oxygen can be used to produce biofuels, such as ethanol and butanol.

Conclusion

In conclusion, the combustion of glucose with oxygen is a complex process that involves the breaking and forming of bonds between atoms. The entropy of the universe does not decrease as a result of this reaction, but instead increases as the system and its surroundings become more disordered or random. This is in accordance with the second law of thermodynamics. The combustion of glucose with oxygen can be used to produce energy, but it is not a very efficient way to do so. Additionally, it has several limitations, including low energy yield, carbon dioxide emissions, and water production.

References

  • Levine, I. N. (2008). Physical Chemistry. 6th ed. New York: McGraw-Hill.
  • Atkins, P. W. (2007). Physical Chemistry. 9th ed. New York: Oxford University Press.
  • Kotz, J. C. (2008). Chemistry and Chemical Reactivity. 8th ed. New York: Thomson Brooks/Cole.

Glossary

  • Entropy: A measure of the disorder or randomness of a system.
  • Second Law of Thermodynamics: A law that states that the total entropy of an isolated system will always increase over time.
  • Redox Reaction: A chemical reaction in which one substance is oxidized and another substance is reduced.
  • Carbon Dioxide: A greenhouse gas that contributes to climate change.
  • Water: A valuable resource that is essential for life.
  • Biofuels: Fuels that are produced from organic matter, such as plants and microorganisms.