Calculate the entropy change when 1 mol of ice 0- C is converted into water at 0- C- The change in heat is 1436 cal per mol-None of these-

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Entropy of Phase Change

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Calculate the entropy change when 1 mol of ice $0^{\circ} C$ is converted into water at $0^{\circ} C$ . The change in heat is 1436 cal per mol.

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None of these

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0^{\circ} C

0^{\circ} C

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

0^{o} C

Calculate the entropy change accompanying the following change of state.

$H_{2} O (s, - 10^{\circ} C, 1 a t m) \to H_{2} O (l, 10^{\circ} C, 1 a t m)$
$C_{P}$ for ice = $9 c a l d e g^{- 1} m o l^{- 1}$

$C_{P}$ for $H_{2} O$ = $18 c a l d e g^{- 1} m o l^{- 1}$

Latent heat of fusion of ice = $1440 c a l m o l^{- 1}$ at $0^{\circ} C$

0^{o} C

H_{2} O (s) ⟶ H_{2} O (l)

6 k J {m o l}^{- 1}

1 k g

0^{o} C

0^{o} C

80 c a l / C^{o}

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