The total entropy change ( $Δ S_{t o t a l}$ ) for the system and surroundings of a spontaneous process is given by :

Δ S_{t o t a l} = Δ S_{s y s t e m} + Δ S_{s u r r} > 0

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Δ S_{t o t a l} = Δ S_{s y s t e m} + Δ S_{s u r r} < 0

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Δ S_{s y s t e m} = Δ S_{t o t a l} + Δ S_{s u r r} > 0

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Δ S_{s u r r} = Δ S_{t o t a l} + Δ S_{s y s t e m} < 0

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Solution

The correct option is A $Δ S_{t o t a l} = Δ S_{s y s t e m} + Δ S_{s u r r} > 0$
According to Second Law Of Thermodynamics, for a spontaneous process, total change in entropy (system + surrounding) should be positive.

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(△ S_{t o t a l})

The value of ∆S for spontaneous process is

Δ S_{s y s t e m}, Δ S_{s u r r}

Δ S_{t o t a l}

Δ S_{T o t a l} = - 40 k J / m o l \times K

Δ H_{s y s} = 2000 k J / m o l

T = 400 K

Δ S_{s y s t e m}

{Δ S}_{s y s t e m} + {Δ S}_{s u r r .}

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