Calculate the entropy change `(DeltaS)` when `1 mol` of ice at `0^(@)C` is converted into water at `0^(@)C`. Heat of fusion of ice at `0^(@)C` is `1436 cal` per mol.

Calculate the entropy change `(DeltaS)` when `1 mol` of ice at `0^(@)C

1.	Calculate the entropy change `(DeltaS)` when `1 mol` of ice at `0^(@)C` is converted into water at `0^(@)C`. Heat of fusion of ice at `0^(@)C` is `1436 cal` per mol.
Answer» Entropy change `(DeltaS)` for the change of state of a substance is given by dividing the heat change by the absolute temperature at which the change takes place reversibly, i.e., at the melting point in this case. Hence, `DeltaS = (q_(rev))/(T) = (1436)/(237) = 5.26 cal deg^(-1) mol^(-1)`

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Calculate the entropy change `(DeltaS)` when `1 mol` of ice at `0^(@)C` is converted into water at `0^(@)C`. Heat of fusion of ice at `0^(@)C` is `1436 cal` per mol.

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