The latent heat of fusion of ice is 5-99 KJ-mol at its melting point- The values of - S for fusion of 900 gm ice and - S for freezing of liquid water are respectively-

The correct option is C 1097 JK^ 1 ; 21.9 J mol^ 1K^ 1 Δ H_Fusion=TΔ S_Fusion = nbsp;5.99 nbsp;KJ/mol nbsp; ∴Δ S_Fusion=Δ H_FusionT ...

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Standard VII

Physics

Effects of Heat

The latent he...

Question

The latent heat of fusion of ice is $5.99 K J / m o l$ at its melting point. The values of $Δ S$ for fusion of $900 g m$ ice and $Δ S$ for freezing of liquid water are respectively:

8698

J K^{- 1}

; 16.8 J

m o l^{- 1} K^{- 1}

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9269

J K^{- 1}

; 12.6 J

m o l^{- 1} K^{- 1}

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1097

J K^{- 1}

; 21.9 J

m o l^{- 1} K^{- 1}

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1236

J K^{- 1}

; 28.6 J

m o l^{- 1} K^{- 1}

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Solution

The correct option is C 1097 $J K^{- 1}$ ; 21.9 J $m o l^{- 1} K^{- 1}$
$Δ H_{F u s i o n} = T Δ S_{F u s i o n} = 5.99 K J / m o l$
$∴ Δ S_{F u s i o n} = \frac{Δ H_{F u s i o n}}{T}$
$= \frac{5.99 \times 10^{3}}{273}$ J/K
$= 21.9 J / K m o l^{- 1}$
For $900 g m$ ice i.e., $\frac{900}{18} = 50$ moles,
$Δ S = 50 \times 21.9$
$=> 1097 J K^{- 1}$

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The latent heat of fusion of ice is 5.99KJ/mol at its melting point. The values of ΔS for fusion of 900 gm ice and ΔS for freezing of liquid water are respectively:

The correct option is C 1097 JK−1; 21.9 J mol−1K−1ΔHFusion=TΔSFusion=5.99KJ/mol ∴ΔSFusion=ΔHFusionT=5.99×103273 J/K=21.9J/Kmol−1For 900 gm ice i.e., 90018=50 moles, ΔS=50×21.9=>1097JK−1

The latent heat of fusion of ice is $5.99 K J / m o l$ at its melting point. The values of $Δ S$ for fusion of $900 g m$ ice and $Δ S$ for freezing of liquid water are respectively: