List - I List - II (P) Isothermal reversible expansion of an ideal gas (1) Δ S system 0 (Q) Isothermal free expansion of an ideal gas (2) Δ S system

Question

List - I List - II (P) Isothermal reversible expansion of an ideal gas (1) Δ S system ​ > 0 (Q) Isothermal free expansion of an ideal gas (2) Δ S system ​ < 0 (R) Adiabatic reversible expansion of an ideal gas (3) Δ S surrounding ​ = 0 (S) Adiabatic irreversible compression of an ideal gas (4) Δ S universe ​ > 0 (5) Δ S universe ​ = 0

TestHub · Accepted Answer

For isothermal reversible expansion, entropy of the system increases, and the process is reversible, so $Δ S_{t o t a l} = 0$ . Hence, P → 1, 5.

In free expansion, gas expands spontaneously, so $Δ S_{t o t a l} > 0$ . The surroundings are unchanged, and $Δ S_{s u rr} = 0$ . Thus, Q → 1, 3, 4.

Adiabatic reversible expansion has no heat exchange and is reversible; therefore, $Δ S_{s u rr} = 0$ and $Δ S_{t o t a l} = 0$ . Hence, R → 3, 5.

In adiabatic irreversible compression, entropy generation occurs, so $Δ S_{t o t a l} > 0$ . System entropy also increases due to irreversibility. Thus, S → 1, 3, 4.

Therefore, Option (A) is correct.

List - I	List - II
(P) Isothermal reversible expansion of an ideal gas	(1) $Δ S_{system} > 0$
(Q) Isothermal free expansion of an ideal gas	(2) $Δ S_{system} < 0$
(R) Adiabatic reversible expansion of an ideal gas	(3) $Δ S_{surrounding} = 0$
(S) Adiabatic irreversible compression of an ideal gas	(4) $Δ S_{universe} > 0$
	(5) $Δ S_{universe} = 0$

Chemistry - Thermodynamics - II Question with Solution | TestHub

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