A Major Component Of Gasoline Is Octane \left( C_8H_{18} \right ]. When Liquid Octane Is Burned In Air, It Reacts With Oxygen \left( O_2 \right ] Gas To Produce Carbon Dioxide Gas And Water.Determine The Moles Of Octane Needed To
Introduction
Gasoline is a complex mixture of hydrocarbons, and octane is one of the major components. It is a highly volatile liquid with the chemical formula C8H18. When liquid octane is burned in air, it reacts with oxygen gas to produce carbon dioxide gas and water. This chemical reaction is a crucial aspect of combustion, and understanding the stoichiometry of this reaction is essential in various fields, including chemistry, engineering, and environmental science.
The Chemical Reaction of Octane
The chemical reaction of octane can be represented by the following equation:
C8H18 + 12.5O2 → 8CO2 + 9H2O
In this equation, one mole of octane reacts with 12.5 moles of oxygen gas to produce 8 moles of carbon dioxide gas and 9 moles of water.
Determining the Moles of Octane Needed
To determine the moles of octane needed to produce a certain amount of carbon dioxide, we can use the stoichiometry of the reaction. Let's assume we want to produce 8 moles of carbon dioxide. According to the balanced equation, 1 mole of octane produces 8 moles of carbon dioxide. Therefore, to produce 8 moles of carbon dioxide, we need 1 mole of octane.
Calculating the Moles of Octane Needed
To calculate the moles of octane needed, we can use the following formula:
moles of octane = moles of carbon dioxide / 8
Let's assume we want to produce 100 moles of carbon dioxide. Using the formula above, we get:
moles of octane = 100 moles / 8 = 12.5 moles
Therefore, to produce 100 moles of carbon dioxide, we need 12.5 moles of octane.
The Role of Oxygen in the Reaction
Oxygen plays a crucial role in the combustion reaction of octane. According to the balanced equation, 12.5 moles of oxygen gas are needed to produce 8 moles of carbon dioxide. This means that oxygen is the limiting reactant in this reaction, and it determines the amount of octane that can be burned.
The Importance of Stoichiometry in Chemistry
Stoichiometry is a fundamental concept in chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. Understanding stoichiometry is essential in various fields, including chemistry, engineering, and environmental science. In this article, we have seen how stoichiometry can be used to determine the moles of octane needed to produce a certain amount of carbon dioxide.
Conclusion
In conclusion, the chemical reaction of octane is a complex process that involves the combustion of liquid octane in air to produce carbon dioxide gas and water. Understanding the stoichiometry of this reaction is essential in various fields, including chemistry, engineering, and environmental science. By using the balanced equation and the formula for calculating the moles of octane needed, we can determine the amount of octane required to produce a certain amount of carbon dioxide.
Frequently Asked Questions
- What is the chemical formula of octane?
- C8H18
- What is the balanced equation for the combustion reaction of octane?
- C8H18 + 12.5O2 → 8CO2 + 9H2O
- What is the role of oxygen in the combustion reaction of octane?
- Oxygen is the limiting reactant in this reaction, and it determines the amount of octane that can be burned.
- How can we determine the moles of octane needed to produce a certain amount of carbon dioxide?
- We can use the balanced equation and the formula for calculating the moles of octane needed.
References
- Chemistry: An Atoms First Approach, by Steven S. Zumdahl
- General Chemistry: Principles and Modern Applications, by Linus Pauling
- Chemistry: The Central Science, by Theodore L. Brown
Further Reading
- The combustion reaction of octane is a complex process that involves the combustion of liquid octane in air to produce carbon dioxide gas and water.
- Understanding the stoichiometry of this reaction is essential in various fields, including chemistry, engineering, and environmental science.
- By using the balanced equation and the formula for calculating the moles of octane needed, we can determine the amount of octane required to produce a certain amount of carbon dioxide.
Glossary
- Octane: A highly volatile liquid with the chemical formula C8H18.
- Combustion reaction: A chemical reaction that involves the burning of a substance in air to produce carbon dioxide gas and water.
- Stoichiometry: A fundamental concept in chemistry that deals with the quantitative relationships between reactants and products in chemical reactions.
- Limiting reactant: The reactant that determines the amount of product that can be formed in a chemical reaction.
Introduction
In our previous article, we discussed the chemical reaction of octane, a major component of gasoline. We explored the balanced equation, the role of oxygen in the reaction, and how to determine the moles of octane needed to produce a certain amount of carbon dioxide. In this article, we will answer some frequently asked questions related to the chemical reaction of octane.
Q&A
Q: What is the chemical formula of octane?
A: The chemical formula of octane is C8H18.
Q: What is the balanced equation for the combustion reaction of octane?
A: The balanced equation for the combustion reaction of octane is:
C8H18 + 12.5O2 → 8CO2 + 9H2O
Q: What is the role of oxygen in the combustion reaction of octane?
A: Oxygen is the limiting reactant in this reaction, and it determines the amount of octane that can be burned.
Q: How can we determine the moles of octane needed to produce a certain amount of carbon dioxide?
A: We can use the balanced equation and the formula for calculating the moles of octane needed.
Q: What is the significance of the balanced equation in the combustion reaction of octane?
A: The balanced equation is essential in understanding the stoichiometry of the reaction, which is crucial in determining the amount of octane needed to produce a certain amount of carbon dioxide.
Q: Can we use the balanced equation to determine the amount of water produced in the combustion reaction of octane?
A: Yes, we can use the balanced equation to determine the amount of water produced in the combustion reaction of octane. According to the balanced equation, 9 moles of water are produced for every 8 moles of carbon dioxide.
Q: What is the relationship between the amount of octane and the amount of carbon dioxide produced in the combustion reaction?
A: According to the balanced equation, 1 mole of octane produces 8 moles of carbon dioxide.
Q: Can we use the balanced equation to determine the amount of oxygen needed to produce a certain amount of carbon dioxide?
A: Yes, we can use the balanced equation to determine the amount of oxygen needed to produce a certain amount of carbon dioxide. According to the balanced equation, 12.5 moles of oxygen are needed to produce 8 moles of carbon dioxide.
Q: What is the significance of the limiting reactant in the combustion reaction of octane?
A: The limiting reactant determines the amount of product that can be formed in the reaction. In this case, oxygen is the limiting reactant, and it determines the amount of octane that can be burned.
Q: Can we use the balanced equation to determine the amount of heat released in the combustion reaction of octane?
A: Yes, we can use the balanced equation to determine the amount of heat released in the combustion reaction of octane. However, this requires additional information about the enthalpy of formation of the reactants and products.
Conclusion
In conclusion, the chemical reaction of octane is a complex process that involves the combustion of liquid octane in air to produce carbon dioxide gas and water. Understanding the stoichiometry of this reaction is essential in various fields, including chemistry, engineering, and environmental science. By using the balanced equation and the formula for calculating the moles of octane needed, we can determine the amount of octane required to produce a certain amount of carbon dioxide.
Frequently Asked Questions
- What is the chemical formula of octane?
- C8H18
- What is the balanced equation for the combustion reaction of octane?
- C8H18 + 12.5O2 → 8CO2 + 9H2O
- What is the role of oxygen in the combustion reaction of octane?
- Oxygen is the limiting reactant in this reaction, and it determines the amount of octane that can be burned.
- How can we determine the moles of octane needed to produce a certain amount of carbon dioxide?
- We can use the balanced equation and the formula for calculating the moles of octane needed.
References
- Chemistry: An Atoms First Approach, by Steven S. Zumdahl
- General Chemistry: Principles and Modern Applications, by Linus Pauling
- Chemistry: The Central Science, by Theodore L. Brown
Further Reading
- The combustion reaction of octane is a complex process that involves the combustion of liquid octane in air to produce carbon dioxide gas and water.
- Understanding the stoichiometry of this reaction is essential in various fields, including chemistry, engineering, and environmental science.
- By using the balanced equation and the formula for calculating the moles of octane needed, we can determine the amount of octane required to produce a certain amount of carbon dioxide.
Glossary
- Octane: A highly volatile liquid with the chemical formula C8H18.
- Combustion reaction: A chemical reaction that involves the burning of a substance in air to produce carbon dioxide gas and water.
- Stoichiometry: A fundamental concept in chemistry that deals with the quantitative relationships between reactants and products in chemical reactions.
- Limiting reactant: The reactant that determines the amount of product that can be formed in a chemical reaction.