If 8.73 Mol Of $C_5H_{12}$ Reacts With Excess $O_2$, How Many Moles Of \$CO_2$[/tex\] Will Be Produced By The Following Combustion Reaction?$\[C_5H_{12} + 8O_2 \longrightarrow 6H_2O + 5CO_2\\]Moles Of

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In this article, we will delve into the world of chemical reactions and explore the combustion of C5H12 with excess O2. We will examine the given reaction equation, identify the limiting reactant, and calculate the number of moles of CO2 produced.

The Combustion Reaction Equation

The given reaction equation is:

C5H12+8O2⟶6H2O+5CO2{C_5H_{12} + 8O_2 \longrightarrow 6H_2O + 5CO_2}

This equation represents the combustion of C5H12 with excess O2, resulting in the production of 6 moles of H2O and 5 moles of CO2.

Identifying the Limiting Reactant

To determine the limiting reactant, we need to identify the reactant that will be completely consumed first. In this case, we have excess O2, which means that C5H12 is the limiting reactant.

Calculating the Number of Moles of CO2 Produced

To calculate the number of moles of CO2 produced, we need to use the mole ratio of C5H12 to CO2 from the balanced equation. The balanced equation shows that 1 mole of C5H12 produces 5 moles of CO2.

Given that we have 8.73 mol of C5H12, we can calculate the number of moles of CO2 produced as follows:

Moles of CO2=Moles of C5H12×51{ \text{Moles of CO2} = \text{Moles of C5H12} \times \frac{5}{1} }

Moles of CO2=8.73 mol×51{ \text{Moles of CO2} = 8.73 \, \text{mol} \times \frac{5}{1} }

Moles of CO2=43.65 mol{ \text{Moles of CO2} = 43.65 \, \text{mol} }

Therefore, the number of moles of CO2 produced is 43.65 mol.

Conclusion

In conclusion, when 8.73 mol of C5H12 reacts with excess O2, the number of moles of CO2 produced is 43.65 mol. This calculation is based on the balanced equation and the mole ratio of C5H12 to CO2.

Understanding the Importance of Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. In this article, we have applied stoichiometric principles to calculate the number of moles of CO2 produced.

Key Takeaways

  • The combustion reaction of C5H12 with excess O2 produces 6 moles of H2O and 5 moles of CO2.
  • C5H12 is the limiting reactant in this reaction.
  • The number of moles of CO2 produced can be calculated using the mole ratio of C5H12 to CO2 from the balanced equation.
  • Stoichiometry is essential in calculating the number of moles of products produced in a chemical reaction.

Real-World Applications

The combustion reaction of C5H12 with excess O2 has several real-world applications, including:

  • Internal Combustion Engines: The combustion of C5H12 (gasoline) with O2 is the primary mechanism of energy production in internal combustion engines.
  • Fuel Cells: Fuel cells use the combustion reaction of C5H12 with O2 to produce electricity.
  • Industrial Processes: The combustion reaction of C5H12 with O2 is used in various industrial processes, such as the production of chemicals and plastics.

Conclusion

In this article, we will address some of the most frequently asked questions about the combustion reaction of C5H12 with excess O2.

Q: What is the balanced equation for the combustion reaction of C5H12 with excess O2?

A: The balanced equation for the combustion reaction of C5H12 with excess O2 is:

C5H12+8O2⟶6H2O+5CO2{C_5H_{12} + 8O_2 \longrightarrow 6H_2O + 5CO_2}

Q: What is the limiting reactant in the combustion reaction of C5H12 with excess O2?

A: In the combustion reaction of C5H12 with excess O2, C5H12 is the limiting reactant.

Q: How many moles of CO2 are produced when 8.73 mol of C5H12 reacts with excess O2?

A: According to the balanced equation, 1 mole of C5H12 produces 5 moles of CO2. Therefore, when 8.73 mol of C5H12 reacts with excess O2, the number of moles of CO2 produced is:

Moles of CO2=Moles of C5H12×51{ \text{Moles of CO2} = \text{Moles of C5H12} \times \frac{5}{1} }

Moles of CO2=8.73 mol×51{ \text{Moles of CO2} = 8.73 \, \text{mol} \times \frac{5}{1} }

Moles of CO2=43.65 mol{ \text{Moles of CO2} = 43.65 \, \text{mol} }

Q: What is the role of O2 in the combustion reaction of C5H12?

A: O2 is the oxidizing agent in the combustion reaction of C5H12. It reacts with C5H12 to produce CO2 and H2O.

Q: What are the products of the combustion reaction of C5H12 with excess O2?

A: The products of the combustion reaction of C5H12 with excess O2 are 6 moles of H2O and 5 moles of CO2.

Q: What is the significance of the combustion reaction of C5H12 with excess O2?

A: The combustion reaction of C5H12 with excess O2 is a complex process that has several real-world applications, including internal combustion engines, fuel cells, and industrial processes.

Q: How can the combustion reaction of C5H12 with excess O2 be used in real-world applications?

A: The combustion reaction of C5H12 with excess O2 can be used in various real-world applications, including:

  • Internal Combustion Engines: The combustion of C5H12 (gasoline) with O2 is the primary mechanism of energy production in internal combustion engines.
  • Fuel Cells: Fuel cells use the combustion reaction of C5H12 with O2 to produce electricity.
  • Industrial Processes: The combustion reaction of C5H12 with O2 is used in various industrial processes, such as the production of chemicals and plastics.

Q: What are some of the limitations of the combustion reaction of C5H12 with excess O2?

A: Some of the limitations of the combustion reaction of C5H12 with excess O2 include:

  • Energy Efficiency: The combustion reaction of C5H12 with excess O2 is not very energy efficient, as a significant amount of energy is lost as heat.
  • Environmental Impact: The combustion reaction of C5H12 with excess O2 produces greenhouse gases, such as CO2, which contribute to climate change.
  • Safety Concerns: The combustion reaction of C5H12 with excess O2 can be hazardous, as it can produce flammable gases and heat.

Conclusion

In conclusion, the combustion reaction of C5H12 with excess O2 is a complex process that has several real-world applications. However, it also has some limitations, including energy efficiency, environmental impact, and safety concerns. By understanding the combustion reaction of C5H12 with excess O2, we can develop more efficient and sustainable energy production methods.