Read The Given Chemical Reaction:${ 2 C_2 H_6 + 7 O_2 \rightarrow 4 CO_2 + 6 H_2 O }$How Many Moles Of { H_2 O $}$ Are Produced During The Complete Combustion Of 1.4 Moles Of { C_2 H_6 $}$?A. 4.2 Moles B. 5.6 Moles C.
Introduction
Chemical reactions are the foundation of chemistry, and understanding the stoichiometry of these reactions is crucial in various fields, including chemistry, physics, and engineering. In this article, we will delve into the complete combustion of ethane (C2H6) and analyze the production of water (H2O) during this process.
The Chemical Reaction
The given chemical reaction is:
This reaction represents the complete combustion of ethane, where two moles of ethane react with seven moles of oxygen to produce four moles of carbon dioxide and six moles of water.
Understanding the Reaction
To understand the reaction, let's break it down into its constituent parts. The reactants are ethane (C2H6) and oxygen (O2), while the products are carbon dioxide (CO2) and water (H2O). The reaction is a combustion reaction, where the ethane molecule reacts with oxygen to produce carbon dioxide and water.
Stoichiometry of the Reaction
Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. In this reaction, the stoichiometric coefficients of the reactants and products are:
- 2 moles of C2H6
- 7 moles of O2
- 4 moles of CO2
- 6 moles of H2O
Calculating the Moles of H2O Produced
Now, let's calculate the moles of H2O produced during the complete combustion of 1.4 moles of C2H6. To do this, we need to use the stoichiometric coefficients of the reaction.
From the reaction equation, we can see that 2 moles of C2H6 produce 6 moles of H2O. Therefore, the mole ratio of C2H6 to H2O is:
To calculate the moles of H2O produced, we can multiply the mole ratio by the number of moles of C2H6:
Therefore, the complete combustion of 1.4 moles of C2H6 produces 4.2 moles of H2O.
Conclusion
In conclusion, the complete combustion of ethane (C2H6) produces water (H2O) as a byproduct. By analyzing the stoichiometry of the reaction, we can calculate the moles of H2O produced during the combustion of a given amount of C2H6. In this article, we calculated the moles of H2O produced during the complete combustion of 1.4 moles of C2H6 and found that it produces 4.2 moles of H2O.
References
- Chemistry: An Atoms First Approach, by Steven S. Zumdahl
- General Chemistry: Principles and Modern Applications, by Linus Pauling
Discussion
What do you think about the complete combustion of ethane? Have you ever worked with ethane or any other hydrocarbons? Share your thoughts and experiences in the comments below!
Related Articles
- Complete Combustion of Methane: A Stoichiometric Analysis
- Stoichiometry of Chemical Reactions: A Guide
- Chemical Reactions: A Comprehensive Guide
Q&A: Complete Combustion of Ethane =====================================
Introduction
In our previous article, we discussed the complete combustion of ethane (C2H6) and analyzed the production of water (H2O) during this process. In this article, we will answer some frequently asked questions related to the complete combustion of ethane.
Q: What is the complete combustion of ethane?
A: The complete combustion of ethane is a chemical reaction where ethane reacts with oxygen to produce carbon dioxide and water. The reaction is represented by the equation:
Q: What are the products of the complete combustion of ethane?
A: The products of the complete combustion of ethane are carbon dioxide (CO2) and water (H2O). The reaction produces 4 moles of CO2 and 6 moles of H2O for every 2 moles of C2H6 that react.
Q: How many moles of H2O are produced during the complete combustion of 1.4 moles of C2H6?
A: To calculate the moles of H2O produced, we can use the mole ratio of C2H6 to H2O, which is:
Multiplying this ratio by the number of moles of C2H6 (1.4 moles) gives us:
Q: What is the role of oxygen in the complete combustion of ethane?
A: Oxygen plays a crucial role in the complete combustion of ethane. It reacts with ethane to produce carbon dioxide and water. The reaction requires a sufficient amount of oxygen to proceed, and the amount of oxygen required is proportional to the amount of ethane that reacts.
Q: Can the complete combustion of ethane be used to produce energy?
A: Yes, the complete combustion of ethane can be used to produce energy. The reaction releases a significant amount of energy, which can be harnessed to produce electricity or heat. However, the combustion of ethane also produces greenhouse gases, such as carbon dioxide, which contribute to climate change.
Q: What are the safety precautions when handling ethane?
A: When handling ethane, it is essential to take safety precautions to prevent accidents and exposure to the gas. Some of the safety precautions include:
- Handling ethane in a well-ventilated area
- Wearing protective clothing and gloves
- Avoiding exposure to the gas
- Following proper storage and handling procedures
Conclusion
In conclusion, the complete combustion of ethane is a complex process that involves the reaction of ethane with oxygen to produce carbon dioxide and water. By understanding the stoichiometry of the reaction and the role of oxygen, we can calculate the moles of H2O produced during the combustion of a given amount of C2H6. We hope that this Q&A article has provided you with a better understanding of the complete combustion of ethane.
References
- Chemistry: An Atoms First Approach, by Steven S. Zumdahl
- General Chemistry: Principles and Modern Applications, by Linus Pauling
Discussion
Do you have any questions about the complete combustion of ethane? Share your thoughts and experiences in the comments below!
Related Articles
- Complete Combustion of Methane: A Stoichiometric Analysis
- Stoichiometry of Chemical Reactions: A Guide
- Chemical Reactions: A Comprehensive Guide