For a spontaneous process, which of the following is true?

Δ S_{s y s}

is positive

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Δ S_{s u r r}

is positive

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Δ S_{t o t a l}

is positive

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Δ S_{t o t a l}

is negative

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Solution

The correct option is C $Δ S_{t o t a l}$ is positive
$Δ G = Δ H - T Δ S$

$Δ G < 0$ for spontaneous reaction, i.e., $Δ H < T Δ S$ .

Hence, $Δ S_{t o t a l}$ is positive for spontaneous reaction.

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Similar questions

The value of ∆S for spontaneous process is

Q. The total entropy change

(△ S_{t o t a l})

for the system and the surrounding of a spontaneous process is given by:

Q. The total entropy change (

Δ S_{t o t a l}

) for the system and surroundings of a spontaneous process is given by :

Which of the following is not correct?
(a) $Δ$ G is zero for a reversible reaction.
(b) $Δ$ G is positive for a spontaneous reaction.
(c) $Δ$ G is negative for a spontaneous reaction.
(d) $Δ$ G is positive for a non-spontaneous reaction.

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) $Δ S_{s y s} > 0$

Which of the following options has the incorrect combination considering List - I and List - II.

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For a spontaneous process, which of the following is true?

The correct option is C ΔStotal is positiveΔG=ΔH−TΔSΔG<0 for spontaneous reaction, i.e., ΔH<TΔS.Hence, ΔStotal is positive for spontaneous reaction.

The correct option is C $Δ S_{t o t a l}$ is positive
$Δ G = Δ H - T Δ S$

$Δ G < 0$ for spontaneous reaction, i.e., $Δ H < T Δ S$ .

Hence, $Δ S_{t o t a l}$ is positive for spontaneous reaction.