Four samples of ideal gas containing same moles and initially at same temperature and pressure are subjected to four different processes.
(A) Isothermal reversible expansion
(B) Isothermal irreversible expansion against final pressure
(C) Adiabatic reversible expansion
(D) Adiabatic irreversible expansion against final pressure.
If in all the cases, final pressure is same then what will be the order of final temperature in the above cases.

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$T_{a} = T_{b} > T_{c} = T_{d}$

$T_{a} > T_{b} > T_{c} > T_{d}$

$T_{a} = T_{b} < T_{c} < T_{d}$

$T_{a} = T_{b} > T_{d} > T_{c}$

answer is D.

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Detailed Solution

In isothermal process, temperature remains constant, while, in adiabatic expansion, temperature $↓$ , as work is done at the cost of internal energy. T Bnal of rev. adiabatic expansion is least because more work is done in reversible than irreversible adiabatic expansion.

$\Rightarrow T_{a} = T_{b} > T_{d} > T_{c}$