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Enthalpy

Which of the ...

Question

Which of the following is always true for an isothermal expansion of an ideal gas?

△ S = 0

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△ U = 0

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q = 0

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w = 0

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Solution

The correct option is B $△ U = 0$
Solution:- (B) $Δ U = 0$
In an isothermal process, the temperature remains constant.
Therefore,
$Δ U = Δ H = 0$

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q, w, Δ U

1.0 b a r

0.1 b a r

273 K

q

w

△ U

27^{o} C

10 d m^{3}

20 d m^{3}

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) $Δ S_{s y s} > 0$

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