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The reversible expansion of an ideal gas under adiabatic and isothermal conditions is shown in the figure. Which of the following statement(s) is (are) correct ?
 
  • a)
    T1 = T2 (2012 - II)
  • b)
    T3 > T1
  • c)
    wisothermal > wadiabatic
  • d)
    ΔUisothermal > ΔUadiabatic
Correct answer is option 'A,C,D'. Can you explain this answer?
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Verified Answer
The reversible expansion of an ideal gas under adiabatic and isotherma...
T1 = T2 because process is isothermal.
Work done in adiabatic process is less than in isothermal process because area covered by isothermal curve is more than the area covered by the adiabatic curve.
In adiabatic process expansion occurs by using internal energy, hence, it decreases while in isothermal process temperature remains constant that's why no change in internal energy.
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Most Upvoted Answer
The reversible expansion of an ideal gas under adiabatic and isotherma...
T1 = T2 because process is isothermal.
Work done in adiabatic process is less than in isothermal process because area covered by isothermal curve is more than the area covered by the adiabatic curve.
In adiabatic process expansion occurs by using internal energy, hence, it decreases while in isothermal process temperature remains constant that's why no change in internal energy.
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Community Answer
The reversible expansion of an ideal gas under adiabatic and isotherma...
A is correct because the temperature is constant in the isothermal process
C is correct because area under the curve is greater for isothermal process.. which represents the work done
D is correct because for isothermal delta U is zero and this case for adiabatic process it is negative..
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A gaseous sample is generally allowed to do only expansion/compression type of work against its surroundings. The work done in case of an irreversible expansion (in the intermediate stages, of expansion/compression the states of gases are not define d). The work done can be calculated usingdW = NextdVwhile in case of reversible process the work done can be calculated using dw = PdV where P is pressure of gas at some intermediate stages. Like for an isothermal reversible process.Since d w = P d V so magnitude of worked one can also be calculated by, calculating the area under the PV curve of the reversible process in PV diagram.Q.If four identical samples of an ideal gas initially at similar state (P0, Vo, T0) are allowed to expand to double their volumes by four different processes..I : by isothermal irreversible process II : by reversible process having equation P2V = constant III : by reversible adiabatic process IV: by irreversible adiabatic expansion against constant external pressure.Then in the graph shown the final state is represented by four different points then, the correct match can be

A gaseous sample is generally allowed to do only expansion/compression type of work against its surroundings. The work done in case of an irreversible expansion (in the intermediate stages, of expansion/compression the states of gases are not define d). The work done can be calculated usingdW = NextdVwhile in case of reversible process the work done can be calculated using dw = PdV where P is pressure of gas at some intermediate stages. Like for an isothermal reversible process.Since d w = P d V so magnitude of worked one can also be calculated by, calculating the area under the PV curve of the reversible process in PV diagram.Q.Two samples (initially under same states) of an ideal gas are first allowed to expand to double their volume using irreversible isothermal expansion against constant external pressure, then samples are returned back to their original volume first by reversible adiabatic process and second by reversible process having equation PV2 = constant then

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The reversible expansion of an ideal gas under adiabatic and isothermal conditions is shown in the figure. Which of the following statement(s) is (are) correct ?a)T1 = T2 (2012 - II)b)T3 > T1c)wisothermal > wadiabaticd)ΔUisothermal > ΔUadiabaticCorrect answer is option 'A,C,D'. Can you explain this answer?
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The reversible expansion of an ideal gas under adiabatic and isothermal conditions is shown in the figure. Which of the following statement(s) is (are) correct ?a)T1 = T2 (2012 - II)b)T3 > T1c)wisothermal > wadiabaticd)ΔUisothermal > ΔUadiabaticCorrect answer is option 'A,C,D'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about The reversible expansion of an ideal gas under adiabatic and isothermal conditions is shown in the figure. Which of the following statement(s) is (are) correct ?a)T1 = T2 (2012 - II)b)T3 > T1c)wisothermal > wadiabaticd)ΔUisothermal > ΔUadiabaticCorrect answer is option 'A,C,D'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The reversible expansion of an ideal gas under adiabatic and isothermal conditions is shown in the figure. Which of the following statement(s) is (are) correct ?a)T1 = T2 (2012 - II)b)T3 > T1c)wisothermal > wadiabaticd)ΔUisothermal > ΔUadiabaticCorrect answer is option 'A,C,D'. Can you explain this answer?.
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