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For an ideal gas, the relation between the enthalpy change and internal energy change at constant temperature is given by
- a)H = E + PV
- b)Δ H = Δ E + Δ n R T
- c)Δ H = Δ E + P Δ V
- d)Δ H = Δ G + T Δ S
Correct answer is option 'B'. Can you explain this answer?
Most Upvoted Answer
For an ideal gas, the relation between the enthalpy change and interna...
Explanation:
Enthalpy and Internal Energy Change for an Ideal Gas:
- For an ideal gas, the relation between enthalpy change (ΔH) and internal energy change (ΔE) at constant temperature is given by the equation: ΔH = ΔE + ΔnRT.
- Here, Δn represents the change in moles of gas, R is the gas constant, and T is the temperature in Kelvin.
- This equation is derived from the first law of thermodynamics, which states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system.
Significance of the Equation:
- The equation ΔH = ΔE + ΔnRT is important in understanding the relationship between enthalpy and internal energy changes for an ideal gas.
- It helps in determining how the enthalpy of a system changes with respect to the internal energy and the number of moles of gas present.
- This equation is particularly useful in the study of thermodynamics and in calculating the heat transfer and work done in various chemical reactions involving ideal gases.
Conclusion:
- The equation ΔH = ΔE + ΔnRT is a fundamental relationship for an ideal gas that connects the enthalpy change with the internal energy change at constant temperature.
- Understanding this equation is essential for analyzing and predicting the behavior of ideal gases in different thermodynamic processes.
Enthalpy and Internal Energy Change for an Ideal Gas:
- For an ideal gas, the relation between enthalpy change (ΔH) and internal energy change (ΔE) at constant temperature is given by the equation: ΔH = ΔE + ΔnRT.
- Here, Δn represents the change in moles of gas, R is the gas constant, and T is the temperature in Kelvin.
- This equation is derived from the first law of thermodynamics, which states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system.
Significance of the Equation:
- The equation ΔH = ΔE + ΔnRT is important in understanding the relationship between enthalpy and internal energy changes for an ideal gas.
- It helps in determining how the enthalpy of a system changes with respect to the internal energy and the number of moles of gas present.
- This equation is particularly useful in the study of thermodynamics and in calculating the heat transfer and work done in various chemical reactions involving ideal gases.
Conclusion:
- The equation ΔH = ΔE + ΔnRT is a fundamental relationship for an ideal gas that connects the enthalpy change with the internal energy change at constant temperature.
- Understanding this equation is essential for analyzing and predicting the behavior of ideal gases in different thermodynamic processes.
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For an ideal gas, the relation between the enthalpy change and internal energy change at constant temperature is given bya)H = E + PVb)Δ H = Δ E + Δ n R Tc)Δ H = Δ E + P Δ Vd)Δ H = Δ G + T Δ SCorrect answer is option 'B'. 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 For an ideal gas, the relation between the enthalpy change and internal energy change at constant temperature is given bya)H = E + PVb)Δ H = Δ E + Δ n R Tc)Δ H = Δ E + P Δ Vd)Δ H = Δ G + T Δ SCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for For an ideal gas, the relation between the enthalpy change and internal energy change at constant temperature is given bya)H = E + PVb)Δ H = Δ E + Δ n R Tc)Δ H = Δ E + P Δ Vd)Δ H = Δ G + T Δ SCorrect answer is option 'B'. Can you explain this answer?.
For an ideal gas, the relation between the enthalpy change and internal energy change at constant temperature is given bya)H = E + PVb)Δ H = Δ E + Δ n R Tc)Δ H = Δ E + P Δ Vd)Δ H = Δ G + T Δ SCorrect answer is option 'B'. 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 For an ideal gas, the relation between the enthalpy change and internal energy change at constant temperature is given bya)H = E + PVb)Δ H = Δ E + Δ n R Tc)Δ H = Δ E + P Δ Vd)Δ H = Δ G + T Δ SCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for For an ideal gas, the relation between the enthalpy change and internal energy change at constant temperature is given bya)H = E + PVb)Δ H = Δ E + Δ n R Tc)Δ H = Δ E + P Δ Vd)Δ H = Δ G + T Δ SCorrect answer is option 'B'. Can you explain this answer?.
Solutions for For an ideal gas, the relation between the enthalpy change and internal energy change at constant temperature is given bya)H = E + PVb)Δ H = Δ E + Δ n R Tc)Δ H = Δ E + P Δ Vd)Δ H = Δ G + T Δ SCorrect answer is option 'B'. Can you explain this answer? in English & in Hindi are available as part of our courses for JEE.
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