Calculate the number of moles of C9H20

Oct 13, 2025 by ludoplayers7.com 48 views

Determine the Mass in Grams of CO2 Produced by the Complete Reaction of C9H20

Understanding the Combustion Reaction

The combustion reaction of nonane (C9H20) is a complex process that involves the reaction of the hydrocarbon with oxygen to produce carbon dioxide and water. The balanced chemical equation for this reaction is:

C9H20(l) + 14O2(g) → 9CO2(g) + 10H2O(l)

In this reaction, 1 mole of nonane reacts with 14 moles of oxygen to produce 9 moles of carbon dioxide and 10 moles of water.

Calculating the Mass of CO2 Produced

To determine the mass of CO2 produced by the complete reaction of 11.65 grams of C9H20, we need to follow these steps:

Calculate the number of moles of C9H20: The molar mass of C9H20 is 128.23 g/mol. We can calculate the number of moles of C9H20 using the formula:

moles = mass / molar mass

moles = 11.65 g / 128.23 g/mol = 0.0908 mol

Calculate the number of moles of CO2 produced: According to the balanced chemical equation, 1 mole of C9H20 produces 9 moles of CO2. Therefore, the number of moles of CO2 produced is:

moles CO2 = 9 × moles C9H20 moles CO2 = 9 × 0.0908 mol = 0.8172 mol

Calculate the mass of CO2 produced: The molar mass of CO2 is 44.01 g/mol. We can calculate the mass of CO2 produced using the formula:

mass CO2 = moles CO2 × molar mass mass CO2 = 0.8172 mol × 44.01 g/mol = 36.01 g

Therefore, the mass of CO2 produced by the complete reaction of 11.65 grams of C9H20 is 36.01 grams.

Understanding the Limiting Reactant

In a combustion reaction, the limiting reactant is the reactant that is consumed first and determines the amount of product formed. In this case, the limiting reactant is C9H20. The amount of C9H20 consumed is equal to the amount of CO2 produced.

Calculating the Percentage Yield of CO2

The percentage yield of CO2 is the ratio of the actual mass of CO2 produced to the theoretical mass of CO2 produced. The theoretical mass of CO2 produced is the mass of CO2 that would be produced if all the C9H20 were converted to CO2.

Theoretical mass CO2 = moles CO2 × molar mass Theoretical mass CO2 = 0.8172 mol × 44.01 g/mol = 36.01 g

The percentage yield of CO2 is:

Percentage yield = (actual mass CO2 / theoretical mass CO2) × 100% Percentage yield = (36.01 g / 36.01 g) × 100% = 100%

Therefore, the percentage yield of CO2 is 100%, indicating that all the C9H20 was converted to CO2.

Conclusion

In conclusion, the mass of CO2 produced by the complete reaction of 11.65 grams of C9H20 is 36.01 grams. The limiting reactant is C9H20, and the percentage yield of CO2 is 100%. This calculation demonstrates the importance of understanding the balanced chemical equation and the limiting reactant in a combustion reaction.

References

Chemistry: An Atoms First Approach, Steven S. Zumdahl, 2014
General Chemistry: Principles and Modern Applications, John W. Hill, 2010

Additional Resources

Online calculators for calculating the mass of CO2 produced
Online resources for understanding combustion reactions and limiting reactants

Frequently Asked Questions

Q: What is the molar mass of C9H20? A: The molar mass of C9H20 is 128.23 g/mol.
Q: What is the molar mass of CO2? A: The molar mass of CO2 is 44.01 g/mol.
Q: What is the percentage yield of CO2? A: The percentage yield of CO2 is 100%.
Frequently Asked Questions: Combustion Reactions and Limiting Reactants

Q: What is a combustion reaction?

A: A combustion reaction is a chemical reaction in which a substance reacts with oxygen to produce heat and light. Combustion reactions typically involve the reaction of a hydrocarbon with oxygen to produce carbon dioxide and water.

Q: What is the balanced chemical equation for the combustion reaction of C9H20?

A: The balanced chemical equation for the combustion reaction of C9H20 is:

C9H20(l) + 14O2(g) → 9CO2(g) + 10H2O(l)

Q: What is the limiting reactant in a combustion reaction?

A: The limiting reactant in a combustion reaction is the reactant that is consumed first and determines the amount of product formed. In the case of the combustion reaction of C9H20, the limiting reactant is C9H20.

Q: How do I calculate the mass of CO2 produced in a combustion reaction?

A: To calculate the mass of CO2 produced in a combustion reaction, you need to follow these steps:

Calculate the number of moles of the hydrocarbon (C9H20) using the formula: moles = mass / molar mass
Calculate the number of moles of CO2 produced using the balanced chemical equation
Calculate the mass of CO2 produced using the formula: mass CO2 = moles CO2 × molar mass

Q: What is the molar mass of C9H20?

A: The molar mass of C9H20 is 128.23 g/mol.

Q: What is the molar mass of CO2?

A: The molar mass of CO2 is 44.01 g/mol.

Q: What is the percentage yield of CO2 in a combustion reaction?

A: The percentage yield of CO2 in a combustion reaction is the ratio of the actual mass of CO2 produced to the theoretical mass of CO2 produced. If all the hydrocarbon is converted to CO2, the percentage yield is 100%.

Q: How do I determine the limiting reactant in a combustion reaction?

A: To determine the limiting reactant in a combustion reaction, you need to compare the mole ratio of the reactants to the mole ratio of the products. The reactant that is consumed first is the limiting reactant.

Q: What are some common mistakes to avoid when calculating the mass of CO2 produced in a combustion reaction?

A: Some common mistakes to avoid when calculating the mass of CO2 produced in a combustion reaction include:

Not balancing the chemical equation
Not calculating the number of moles of the hydrocarbon correctly
Not using the correct molar masses of the reactants and products
Not calculating the mass of CO2 produced correctly

Q: How can I improve my understanding of combustion reactions and limiting reactants?

A: To improve your understanding of combustion reactions and limiting reactants, you can:

Practice calculating the mass of CO2 produced in different combustion reactions
Study the balanced chemical equations for different combustion reactions
Learn about the different types of combustion reactions and their applications
Practice determining the limiting reactant in different combustion reactions

Q: What are some real-world applications of combustion reactions and limiting reactants?

A: Some real-world applications of combustion reactions and limiting reactants include:

Power generation: Combustion reactions are used to generate electricity in power plants.
Transportation: Combustion reactions are used to power vehicles.
Industrial processes: Combustion reactions are used in various industrial processes, such as the production of chemicals and fuels.

Q: How can I use combustion reactions and limiting reactants in my everyday life?

A: You can use combustion reactions and limiting reactants in your everyday life by:

Understanding the combustion reaction that occurs in your car engine
Understanding the combustion reaction that occurs in your home furnace
Understanding the combustion reaction that occurs in your kitchen stove
Using the concept of limiting reactants to optimize your cooking and baking recipes.

Conclusion

In conclusion, combustion reactions and limiting reactants are important concepts in chemistry that have many real-world applications. By understanding these concepts, you can improve your understanding of chemical reactions and their applications in everyday life.