The Combustion Reaction of Acetylene

Oct 13, 2025 by magicalceylontours.com 3 views

Introduction

Acetylene, a highly flammable gas, is widely used in various industrial applications, including welding and cutting metals. The combustion reaction of acetylene is a crucial process that involves the reaction of acetylene with oxygen to produce carbon dioxide and water vapor. In this article, we will discuss the combustion reaction of acetylene and calculate the limiting reactant when 37.0 mol of acetylene and 81.0 mol of oxygen are available.

The Combustion Reaction of Acetylene

The combustion reaction of acetylene is represented by the following equation:

${2 C_2H_2(l) + 5 O_2(g) \rightarrow 4 CO_2(g) + 2 H_2O(g)}$

In this reaction, 2 moles of acetylene react with 5 moles of oxygen to produce 4 moles of carbon dioxide and 2 moles of water vapor.

Calculating the Limiting Reactant

To determine the limiting reactant, we need to calculate the number of moles of acetylene and oxygen required to react completely. We can do this by dividing the number of moles of each reactant by the coefficient in the balanced equation.

For acetylene:

${ \text{Moles of acetylene required} = \frac{5 \text{ mol of oxygen}}{2 \text{ mol of acetylene}} \times \text{Moles of acetylene available} }$

${ \text{Moles of acetylene required} = \frac{5}{2} \times 37.0 \text{ mol} }$

${ \text{Moles of acetylene required} = 92.5 \text{ mol} }$

Since we have 37.0 mol of acetylene available, which is less than the required amount, acetylene is the limiting reactant.

Calculating the Amount of Product Formed

Now that we have determined the limiting reactant, we can calculate the amount of product formed. Since acetylene is the limiting reactant, we will use the number of moles of acetylene available to calculate the amount of product formed.

For carbon dioxide:

${ \text{Moles of carbon dioxide formed} = \frac{4 \text{ mol of carbon dioxide}}{2 \text{ mol of acetylene}} \times \text{Moles of acetylene available} }$

${ \text{Moles of carbon dioxide formed} = \frac{4}{2} \times 37.0 \text{ mol} }$

${ \text{Moles of carbon dioxide formed} = 74.0 \text{ mol} }$

For water vapor:

${ \text{Moles of water vapor formed} = \frac{2 \text{ mol of water vapor}}{2 \text{ mol of acetylene}} \times \text{Moles of acetylene available} }$

${ \text{Moles of water vapor formed} = \frac{2}{2} \times 37.0 \text{ mol} }$

${ \text{Moles of water vapor formed} = 37.0 \text{ mol} }$

Conclusion

In conclusion, the combustion reaction of acetylene is a complex process that involves the reaction of acetylene with oxygen to produce carbon dioxide and water vapor. By calculating the limiting reactant and the amount of product formed, we can determine the amount of product that will be formed when 37.0 mol of acetylene and 81.0 mol of oxygen are available. This calculation is essential in understanding the combustion reaction of acetylene and its applications in various industrial processes.

References

Chemical Equations and Reactions by OpenStax
General Chemistry by Linus Pauling

Additional Resources

Combustion Reaction of Acetylene by Chemistry LibreTexts
Acetylene by Wikipedia
Frequently Asked Questions (FAQs) about the Combustion Reaction of Acetylene ====================================================================================

Q: What is the combustion reaction of acetylene?

A: The combustion reaction of acetylene is a chemical reaction that involves the reaction of acetylene with oxygen to produce carbon dioxide and water vapor. The balanced equation for this reaction is:

${2 C_2H_2(l) + 5 O_2(g) \rightarrow 4 CO_2(g) + 2 H_2O(g)}$

Q: What is the role of oxygen in the combustion reaction of acetylene?

A: Oxygen plays a crucial role in the combustion reaction of acetylene. It reacts with acetylene to produce carbon dioxide and water vapor. The amount of oxygen required for the reaction is 5 moles for every 2 moles of acetylene.

Q: What is the limiting reactant in the combustion reaction of acetylene?

A: The limiting reactant in the combustion reaction of acetylene is the reactant that is present in the smallest amount. In the case of 37.0 mol of acetylene and 81.0 mol of oxygen, acetylene is the limiting reactant.

Q: How do you calculate the amount of product formed in the combustion reaction of acetylene?

A: To calculate the amount of product formed, you need to divide the number of moles of the product by the coefficient in the balanced equation. For example, to calculate the amount of carbon dioxide formed, you would divide the number of moles of carbon dioxide by 4 (the coefficient in the balanced equation).

Q: What are the products of the combustion reaction of acetylene?

A: The products of the combustion reaction of acetylene are carbon dioxide and water vapor.

Q: What are the applications of the combustion reaction of acetylene?

A: The combustion reaction of acetylene has various applications in industrial processes, including welding and cutting metals.

Q: Is the combustion reaction of acetylene exothermic or endothermic?

A: The combustion reaction of acetylene is exothermic, meaning that it releases heat energy.

Q: What are the safety precautions to be taken while handling acetylene?

A: When handling acetylene, it is essential to take safety precautions, such as wearing protective gear, ensuring proper ventilation, and following the manufacturer's instructions.

Q: Can the combustion reaction of acetylene be used to produce electricity?

A: Yes, the combustion reaction of acetylene can be used to produce electricity through a process called fuel cell technology.

Q: What are the environmental implications of the combustion reaction of acetylene?

A: The combustion reaction of acetylene produces carbon dioxide and water vapor as products, which can contribute to greenhouse gas emissions and climate change.

Q: Can the combustion reaction of acetylene be used to produce hydrogen?

A: Yes, the combustion reaction of acetylene can be used to produce hydrogen through a process called steam methane reforming.

Conclusion

In conclusion, the combustion reaction of acetylene is a complex process that involves the reaction of acetylene with oxygen to produce carbon dioxide and water vapor. By understanding the reaction, its products, and its applications, we can appreciate the importance of this process in various industrial and environmental contexts.