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At 298 K and 1 atm, the molar enthalpies of combustion of Cyclopropane and propene are – 2091 kJ mol–1 and –2058 kJ mol–1, respectively. The enthalpy change (in kJ mol–1) for the conversion of one mole of propene to one mole of Cyclopropane is _________.
Correct answer is '33'. Can you explain this answer?
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At 298 K and 1 atm, the molar enthalpies of combustion of Cyclopropane...
=Molar Enthalpy of combustion of Propene - Molar Enthalpy of combustion of Cylcopropane
=-2058-(-2091)
=33
=-2058-(-2091)
=33
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At 298 K and 1 atm, the molar enthalpies of combustion of Cyclopropane...
**Given information:**
- Molar enthalpy of combustion of Cyclopropane (C3H6) = 2091 kJ/mol
- Molar enthalpy of combustion of Propene (C3H6) = 2058 kJ/mol
**Enthalpy change for the conversion of propene to cyclopropane:**
To find the enthalpy change for the conversion of one mole of propene to one mole of cyclopropane, we need to calculate the difference between their molar enthalpies of combustion.
Enthalpy change = Molar enthalpy of combustion of cyclopropane - Molar enthalpy of combustion of propene
Enthalpy change = 2091 kJ/mol - 2058 kJ/mol
Enthalpy change = 33 kJ/mol
Therefore, the enthalpy change for the conversion of one mole of propene to one mole of cyclopropane is 33 kJ/mol.
This positive enthalpy change indicates that the conversion of propene to cyclopropane is an endothermic process. It requires the input of energy to break the bonds in propene and form the new bonds in cyclopropane.
**Explanation:**
Cyclopropane and propene are both hydrocarbons with different molecular structures. The conversion of propene to cyclopropane involves breaking and forming chemical bonds, which leads to a change in the enthalpy of the system.
In the process of combustion, hydrocarbons react with oxygen to produce carbon dioxide and water. The enthalpy of combustion is the energy released when one mole of a substance is completely burned in excess oxygen.
The molar enthalpy of combustion of cyclopropane (2091 kJ/mol) and propene (2058 kJ/mol) represents the energy released when one mole of each compound is combusted.
To find the enthalpy change for the conversion of propene to cyclopropane, we subtract the molar enthalpy of combustion of propene from the molar enthalpy of combustion of cyclopropane. The positive value of 33 kJ/mol indicates that the conversion process requires the input of 33 kJ/mol of energy.
This energy is needed to break the carbon-carbon double bond in propene and form the carbon-carbon single bonds in cyclopropane. The conversion process is endothermic because it requires energy to proceed.
In summary, the enthalpy change for the conversion of one mole of propene to one mole of cyclopropane is 33 kJ/mol, indicating an endothermic process.
- Molar enthalpy of combustion of Cyclopropane (C3H6) = 2091 kJ/mol
- Molar enthalpy of combustion of Propene (C3H6) = 2058 kJ/mol
**Enthalpy change for the conversion of propene to cyclopropane:**
To find the enthalpy change for the conversion of one mole of propene to one mole of cyclopropane, we need to calculate the difference between their molar enthalpies of combustion.
Enthalpy change = Molar enthalpy of combustion of cyclopropane - Molar enthalpy of combustion of propene
Enthalpy change = 2091 kJ/mol - 2058 kJ/mol
Enthalpy change = 33 kJ/mol
Therefore, the enthalpy change for the conversion of one mole of propene to one mole of cyclopropane is 33 kJ/mol.
This positive enthalpy change indicates that the conversion of propene to cyclopropane is an endothermic process. It requires the input of energy to break the bonds in propene and form the new bonds in cyclopropane.
**Explanation:**
Cyclopropane and propene are both hydrocarbons with different molecular structures. The conversion of propene to cyclopropane involves breaking and forming chemical bonds, which leads to a change in the enthalpy of the system.
In the process of combustion, hydrocarbons react with oxygen to produce carbon dioxide and water. The enthalpy of combustion is the energy released when one mole of a substance is completely burned in excess oxygen.
The molar enthalpy of combustion of cyclopropane (2091 kJ/mol) and propene (2058 kJ/mol) represents the energy released when one mole of each compound is combusted.
To find the enthalpy change for the conversion of propene to cyclopropane, we subtract the molar enthalpy of combustion of propene from the molar enthalpy of combustion of cyclopropane. The positive value of 33 kJ/mol indicates that the conversion process requires the input of 33 kJ/mol of energy.
This energy is needed to break the carbon-carbon double bond in propene and form the carbon-carbon single bonds in cyclopropane. The conversion process is endothermic because it requires energy to proceed.
In summary, the enthalpy change for the conversion of one mole of propene to one mole of cyclopropane is 33 kJ/mol, indicating an endothermic process.
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At 298 K and 1 atm, the molar enthalpies of combustion of Cyclopropane and propene are 2091 kJ mol1 and 2058 kJ mol1, respectively. The enthalpy change (in kJ mol1) for the conversion of one mole of propene to one mole of Cyclopropane is _________.Correct answer is '33'. Can you explain this answer?
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At 298 K and 1 atm, the molar enthalpies of combustion of Cyclopropane and propene are 2091 kJ mol1 and 2058 kJ mol1, respectively. The enthalpy change (in kJ mol1) for the conversion of one mole of propene to one mole of Cyclopropane is _________.Correct answer is '33'. Can you explain this answer? for IIT JAM 2024 is part of IIT JAM preparation. The Question and answers have been prepared according to the IIT JAM exam syllabus. Information about At 298 K and 1 atm, the molar enthalpies of combustion of Cyclopropane and propene are 2091 kJ mol1 and 2058 kJ mol1, respectively. The enthalpy change (in kJ mol1) for the conversion of one mole of propene to one mole of Cyclopropane is _________.Correct answer is '33'. Can you explain this answer? covers all topics & solutions for IIT JAM 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for At 298 K and 1 atm, the molar enthalpies of combustion of Cyclopropane and propene are 2091 kJ mol1 and 2058 kJ mol1, respectively. The enthalpy change (in kJ mol1) for the conversion of one mole of propene to one mole of Cyclopropane is _________.Correct answer is '33'. Can you explain this answer?.
At 298 K and 1 atm, the molar enthalpies of combustion of Cyclopropane and propene are 2091 kJ mol1 and 2058 kJ mol1, respectively. The enthalpy change (in kJ mol1) for the conversion of one mole of propene to one mole of Cyclopropane is _________.Correct answer is '33'. Can you explain this answer? for IIT JAM 2024 is part of IIT JAM preparation. The Question and answers have been prepared according to the IIT JAM exam syllabus. Information about At 298 K and 1 atm, the molar enthalpies of combustion of Cyclopropane and propene are 2091 kJ mol1 and 2058 kJ mol1, respectively. The enthalpy change (in kJ mol1) for the conversion of one mole of propene to one mole of Cyclopropane is _________.Correct answer is '33'. Can you explain this answer? covers all topics & solutions for IIT JAM 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for At 298 K and 1 atm, the molar enthalpies of combustion of Cyclopropane and propene are 2091 kJ mol1 and 2058 kJ mol1, respectively. The enthalpy change (in kJ mol1) for the conversion of one mole of propene to one mole of Cyclopropane is _________.Correct answer is '33'. Can you explain this answer?.
Solutions for At 298 K and 1 atm, the molar enthalpies of combustion of Cyclopropane and propene are 2091 kJ mol1 and 2058 kJ mol1, respectively. The enthalpy change (in kJ mol1) for the conversion of one mole of propene to one mole of Cyclopropane is _________.Correct answer is '33'. Can you explain this answer? in English & in Hindi are available as part of our courses for IIT JAM.
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