Ethyne { \left( C_2H_2(g), \Delta H_f = 226.77 , \text{kJ/mol} \right)$}$ Undergoes Complete Combustion In The Presence Of Oxygen To Produce Carbon Dioxide { \left( CO_2(g), \Delta H_f = -393.5 , \text{kJ/mol} \right)$}$ And Water
Introduction
Ethyne, also known as acetylene, is a highly flammable hydrocarbon gas with the chemical formula C2H2. It is widely used in various industrial applications, including the production of chemicals, plastics, and fibers. In this article, we will delve into the combustion reaction of ethyne in the presence of oxygen, producing carbon dioxide and water. We will analyze the thermodynamic properties of the reaction, including the standard enthalpy of formation (ΔHf) and the standard entropy (S) of the reactants and products.
The Combustion Reaction
The combustion reaction of ethyne can be represented by the following equation:
C2H2(g) + 5/2 O2(g) → 2CO2(g) + H2O(l)
This reaction involves the complete oxidation of ethyne, resulting in the formation of carbon dioxide and water. The reaction is highly exothermic, releasing a significant amount of energy in the form of heat.
Thermodynamic Properties
The standard enthalpy of formation (ΔHf) is a measure of the energy change associated with the formation of a compound from its constituent elements in their standard states. The ΔHf values for ethyne, carbon dioxide, and water are:
- ΔHf(C2H2(g)) = 226.77 kJ/mol
- ΔHf(CO2(g)) = -393.5 kJ/mol
- ΔHf(H2O(l)) = -285.83 kJ/mol
The standard entropy (S) is a measure of the disorder or randomness of a system. The S values for ethyne, carbon dioxide, and water are:
- S(C2H2(g)) = 200.94 J/mol·K
- S(CO2(g)) = 213.8 J/mol·K
- S(H2O(l)) = 70.0 J/mol·K
Enthalpy Change
The enthalpy change (ΔH) associated with the combustion reaction can be calculated using the ΔHf values of the reactants and products:
ΔH = Σ(ΔHf(products)) - Σ(ΔHf(reactants))
Substituting the ΔHf values, we get:
ΔH = 2(-393.5 kJ/mol) - (226.77 kJ/mol) = -853.33 kJ/mol
This indicates that the combustion reaction is highly exothermic, releasing 853.33 kJ of energy per mole of ethyne.
Entropy Change
The entropy change (ΔS) associated with the combustion reaction can be calculated using the S values of the reactants and products:
ΔS = Σ(S(products)) - Σ(S(reactants))
Substituting the S values, we get:
ΔS = 2(213.8 J/mol·K) - (200.94 J/mol·K) = 226.64 J/mol·K
This indicates that the combustion reaction is accompanied by an increase in entropy, reflecting the increased disorder or randomness of the system.
Conclusion
In conclusion, the combustion reaction of ethyne in the presence of oxygen is a highly exothermic process, releasing a significant amount of energy in the form of heat. The reaction is accompanied by an increase in entropy, reflecting the increased disorder or randomness of the system. The thermodynamic properties of the reaction, including the standard enthalpy of formation (ΔHf) and the standard entropy (S), provide valuable insights into the energy and disorder changes associated with the reaction.
Applications
The combustion reaction of ethyne has various industrial applications, including:
- Production of chemicals: The combustion reaction of ethyne can be used to produce chemicals such as carbon dioxide and water, which are used in various industrial processes.
- Production of plastics: The combustion reaction of ethyne can be used to produce plastics such as polyethylene and polypropylene, which are used in various applications.
- Production of fibers: The combustion reaction of ethyne can be used to produce fibers such as nylon and polyester, which are used in various applications.
Safety Precautions
The combustion reaction of ethyne is highly exothermic and can be hazardous if not handled properly. Some safety precautions to be taken include:
- Use of protective equipment: Protective equipment such as gloves, goggles, and a face mask should be worn when handling ethyne.
- Use of ventilation: Good ventilation should be provided to prevent the accumulation of ethyne in the air.
- Use of fire extinguishers: Fire extinguishers should be available in case of an emergency.
References
- CRC Handbook of Chemistry and Physics: This reference provides the thermodynamic properties of various substances, including ethyne, carbon dioxide, and water.
- National Institute of Standards and Technology (NIST): This reference provides the thermodynamic properties of various substances, including ethyne, carbon dioxide, and water.
- American Chemical Society (ACS): This reference provides information on the combustion reaction of ethyne and its applications.
Ethyne Combustion Reaction: A Comprehensive Q&A Guide ===========================================================
Introduction
In our previous article, we discussed the combustion reaction of ethyne in the presence of oxygen, producing carbon dioxide and water. We analyzed the thermodynamic properties of the reaction, including the standard enthalpy of formation (ΔHf) and the standard entropy (S) of the reactants and products. In this article, we will provide a comprehensive Q&A guide to help you better understand the combustion reaction of ethyne.
Q: What is the combustion reaction of ethyne?
A: The combustion reaction of ethyne is a highly exothermic process that involves the complete oxidation of ethyne in the presence of oxygen, producing carbon dioxide and water.
Q: What is the chemical equation for the combustion reaction of ethyne?
A: The chemical equation for the combustion reaction of ethyne is:
C2H2(g) + 5/2 O2(g) → 2CO2(g) + H2O(l)
Q: What is the standard enthalpy of formation (ΔHf) of ethyne?
A: The standard enthalpy of formation (ΔHf) of ethyne is 226.77 kJ/mol.
Q: What is the standard entropy (S) of ethyne?
A: The standard entropy (S) of ethyne is 200.94 J/mol·K.
Q: What is the enthalpy change (ΔH) associated with the combustion reaction of ethyne?
A: The enthalpy change (ΔH) associated with the combustion reaction of ethyne is -853.33 kJ/mol.
Q: What is the entropy change (ΔS) associated with the combustion reaction of ethyne?
A: The entropy change (ΔS) associated with the combustion reaction of ethyne is 226.64 J/mol·K.
Q: What are the applications of the combustion reaction of ethyne?
A: The combustion reaction of ethyne has various industrial applications, including:
- Production of chemicals: The combustion reaction of ethyne can be used to produce chemicals such as carbon dioxide and water, which are used in various industrial processes.
- Production of plastics: The combustion reaction of ethyne can be used to produce plastics such as polyethylene and polypropylene, which are used in various applications.
- Production of fibers: The combustion reaction of ethyne can be used to produce fibers such as nylon and polyester, which are used in various applications.
Q: What are the safety precautions to be taken when handling ethyne?
A: Some safety precautions to be taken when handling ethyne include:
- Use of protective equipment: Protective equipment such as gloves, goggles, and a face mask should be worn when handling ethyne.
- Use of ventilation: Good ventilation should be provided to prevent the accumulation of ethyne in the air.
- Use of fire extinguishers: Fire extinguishers should be available in case of an emergency.
Q: What are the thermodynamic properties of ethyne?
A: The thermodynamic properties of ethyne include:
- Standard enthalpy of formation (ΔHf): 226.77 kJ/mol
- Standard entropy (S): 200.94 J/mol·K
- Enthalpy change (ΔH): -853.33 kJ/mol
- Entropy change (ΔS): 226.64 J/mol·K
Q: What are the products of the combustion reaction of ethyne?
A: The products of the combustion reaction of ethyne are:
- Carbon dioxide (CO2): 2 moles
- Water (H2O): 1 mole
Q: What is the temperature of the combustion reaction of ethyne?
A: The temperature of the combustion reaction of ethyne is typically around 2000°C.
Q: What is the pressure of the combustion reaction of ethyne?
A: The pressure of the combustion reaction of ethyne is typically around 1 atm.
Conclusion
In conclusion, the combustion reaction of ethyne is a highly exothermic process that involves the complete oxidation of ethyne in the presence of oxygen, producing carbon dioxide and water. The thermodynamic properties of the reaction, including the standard enthalpy of formation (ΔHf) and the standard entropy (S) of the reactants and products, provide valuable insights into the energy and disorder changes associated with the reaction. We hope that this Q&A guide has helped you better understand the combustion reaction of ethyne.