For an irreversible isothermal expansion of an ideal gas:

Δ S_{s y s} = Δ S_{s u r r}

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Δ S_{s y s} = - Δ S_{s u r r}

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| Δ S_{s y s} | = | Δ S_{s u r r} |

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None of these

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Solution

The correct option is D None of these
Solution:- (D) None of these
For an irreversible process,
${Δ S}_{Total} = {Δ S}_{Sys.} + {Δ S}_{Surr.} = + v e$
$∴ ∣ ∣ {Δ S}_{Sys.} ∣ ∣ > | {Δ S}_{Surr.} |$

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Similar questions

Δ S_{s y s} + Δ S_{s u r r}

List - I (Process)	List - II
(I) Reversible isothermal expansion of an ideal gas.	(P) $Δ S_{s y s} = 0$
(II) Reversible adiabatic compression of a real gas.	(Q) $Δ H = Δ U = Δ S_{total} = 0$
(III) Adiabatic free expansion.	(R) $Δ S_{total} > 0$
(IV) Isothermal free expansion	(S) $q = 0$
	(T) $Δ S_{surr.} = 0$
	(U) $Δ S_{s y s} > 0$

List - I (Process)	List - II
(I) Reversible isothermal expansion of an ideal gas.	(P) $Δ S_{s y s} = 0$
(II) Reversible adiabatic compression of a real gas.	(Q) $Δ H = Δ U = Δ S_{total} = 0$
(III) Adiabatic free expansion	(R) $Δ S_{total} > 0$
(IV) Isothermal free expansion	(S) $q = 0$
	(T) $Δ S_{surr} = 0$
	(U) $Δ S_{s y s} > 0$