The transformation H2Ol,−10∘C⟶H2Os,−10∘C at 1atm pressure is accompanied with Δsys S∘=−20.5 J K−1.• Which of the following facts will hold good for the change in entropy of surrounding ΔsurS∘?

Since the transformation H2O1,−10∘C⟶H2Os,−10∘C is irreversible or spontaneous, Δtotal S∘=Δsys S∘+Δsurr S∘>0.From this, it follows that Δsum S∘>Δsys S∘

The transformation H2Ol,−10∘C⟶H2Os,−10∘C at 1atm pressure is accompanied with Δsys S∘=−20.5 J K−1.• Which of the following facts will hold good for the change in entropy of surrounding ΔsurS∘?

Since the transformation H2O1,−10∘C⟶H2Os,−10∘C is irreversible or spontaneous, Δtotal S∘=Δsys S∘+Δsurr S∘>0.From this, it follows that Δsum S∘>Δsys S∘

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The transformation $H_{2} O (l, - 10^{\circ} C) ⟶ H_{2} O (s, - 10^{\circ} C)$ at $1 atm$ pressure is accompanied with $Δ_{sys} S^{\circ} = - 20.5$ $J K^{- 1}$ .• Which of the following facts will hold good for the change in entropy of surrounding $(Δ_{sur} S^{\circ}) ?$

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$Δ_{surr} S^{\circ} < |Δ_{sys} S^{\circ}|$

$Δ_{surr} S^{\circ} = 0$

$Δ_{sur} S^{\circ} = |Δ_{s y s} S^{\circ}|$

$Δ_{surr} S^{\circ} > |Δ_{sys} S^{\circ}|$

answer is B.

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Detailed Solution

Since the transformation $H_{2} O (1, - 10^{\circ} C) ⟶ H_{2} O (s, - 10^{\circ} C)$ is irreversible or spontaneous, $Δ_{total} S^{\circ} = Δ_{sys} S^{\circ} +$ $Δ_{surr} S^{\circ} > 0$ .From this, it follows that $Δ_{sum} S^{\circ} > |Δ_{sys} S^{\circ}|$