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Two moles of an ideal gas is expanded isothermally and reversibly at 300 K from 1L to 10 L. The enthalpy change in kJ is
- a)11.4 kJ
- b)4.8 kJ
- c)-11.4 kJ
- d)zero kJ
Correct answer is option 'D'. Can you explain this answer?
Most Upvoted Answer
Two moles of an ideal gas is expanded isothermally and reversibly at ...
The enthalpy change at constant pressure is given as
ΔH = CpΔT
For isothermal expansion
ΔT = 0
∴ ΔH = 0
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Two moles of an ideal gas is expanded isothermally and reversibly at ...
Solution:
Isothermal expansion of ideal gas is a reversible process.
The enthalpy change for an ideal gas during an isothermal process is zero.
Enthalpy is defined as H = U + PV, where U is the internal energy of the gas, P is the pressure, and V is the volume.
For an ideal gas, internal energy is a function of temperature only, and it does not depend on volume or pressure.
During an isothermal process, the temperature remains constant, and hence, internal energy remains constant.
Since internal energy remains constant, enthalpy change during an isothermal process is zero.
Therefore, the enthalpy change for the given process is zero.
Hence, the correct option is D.
Isothermal expansion of ideal gas is a reversible process.
The enthalpy change for an ideal gas during an isothermal process is zero.
Enthalpy is defined as H = U + PV, where U is the internal energy of the gas, P is the pressure, and V is the volume.
For an ideal gas, internal energy is a function of temperature only, and it does not depend on volume or pressure.
During an isothermal process, the temperature remains constant, and hence, internal energy remains constant.
Since internal energy remains constant, enthalpy change during an isothermal process is zero.
Therefore, the enthalpy change for the given process is zero.
Hence, the correct option is D.
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Two moles of an ideal gas is expanded isothermally and reversibly at 300 K from 1L to 10 L. The enthalpy change in kJ isa)11.4 kJb)4.8 kJc)-11.4 kJd)zero kJCorrect answer is option 'D'. Can you explain this answer?
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Two moles of an ideal gas is expanded isothermally and reversibly at 300 K from 1L to 10 L. The enthalpy change in kJ isa)11.4 kJb)4.8 kJc)-11.4 kJd)zero kJCorrect answer is option 'D'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about Two moles of an ideal gas is expanded isothermally and reversibly at 300 K from 1L to 10 L. The enthalpy change in kJ isa)11.4 kJb)4.8 kJc)-11.4 kJd)zero kJCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Two moles of an ideal gas is expanded isothermally and reversibly at 300 K from 1L to 10 L. The enthalpy change in kJ isa)11.4 kJb)4.8 kJc)-11.4 kJd)zero kJCorrect answer is option 'D'. Can you explain this answer?.
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