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In the complete combustion of butanol (C4H9OH(l))
- a)ΔH < ΔE
- b)ΔH = ΔE
- c)ΔH > ΔE
- d)ΔH and ΔE relation cannot be predicated
Correct answer is option 'C'. Can you explain this answer?
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In the complete combustion of butanol (C4H9OH(l))a)ΔH < &Delt...
H=E+nRT
H>E
bcz of additional value of no. of moles of gases present in producrt
H>E
bcz of additional value of no. of moles of gases present in producrt
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In the complete combustion of butanol (C4H9OH(l))a)ΔH < &Delt...
Understanding Combustion and Energy Changes
In the complete combustion of butanol (C4H9OH), the reaction involves the burning of butanol with oxygen to produce carbon dioxide and water.
Key Concepts of Energy Changes
- Enthalpy Change (ΔH): This represents the heat absorbed or released during a chemical reaction at constant pressure.
- Internal Energy Change (ΔE): This refers to the total energy change of the system, including both heat and work done.
Relationship Between ΔH and ΔE
- For reactions involving gases, the difference between ΔH and ΔE can be significant due to the work done against atmospheric pressure when gases are formed.
- In the case of combustion, the formation of gaseous products (CO2 and H2O) from a liquid reactant (butanol) implies that ΔH will generally be greater than ΔE because additional energy is required to account for the work done by the expanding gases.
Why Option C is Correct
- The complete combustion of butanol produces gaseous products, leading to a situation where:
ΔH (heat of combustion) > ΔE (internal energy change)
- This is a common characteristic of combustion reactions involving liquid reactants and gaseous products.
Conclusion
In summary, the correct answer is option 'C' because the combustion of butanol results in gaseous products, which means the heat change (ΔH) is greater than the internal energy change (ΔE) due to additional work done during the reaction. This relationship is fundamental in thermodynamics, especially in combustion chemistry.
In the complete combustion of butanol (C4H9OH), the reaction involves the burning of butanol with oxygen to produce carbon dioxide and water.
Key Concepts of Energy Changes
- Enthalpy Change (ΔH): This represents the heat absorbed or released during a chemical reaction at constant pressure.
- Internal Energy Change (ΔE): This refers to the total energy change of the system, including both heat and work done.
Relationship Between ΔH and ΔE
- For reactions involving gases, the difference between ΔH and ΔE can be significant due to the work done against atmospheric pressure when gases are formed.
- In the case of combustion, the formation of gaseous products (CO2 and H2O) from a liquid reactant (butanol) implies that ΔH will generally be greater than ΔE because additional energy is required to account for the work done by the expanding gases.
Why Option C is Correct
- The complete combustion of butanol produces gaseous products, leading to a situation where:
ΔH (heat of combustion) > ΔE (internal energy change)
- This is a common characteristic of combustion reactions involving liquid reactants and gaseous products.
Conclusion
In summary, the correct answer is option 'C' because the combustion of butanol results in gaseous products, which means the heat change (ΔH) is greater than the internal energy change (ΔE) due to additional work done during the reaction. This relationship is fundamental in thermodynamics, especially in combustion chemistry.
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In the complete combustion of butanol (C4H9OH(l))a)ΔH < ΔEb)ΔH = ΔEc)ΔH > ΔEd)ΔH and ΔE relation cannot be predicatedCorrect answer is option 'C'. Can you explain this answer?
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