One mole of ice is converted into water at `273K`. The entropies of `H_2O(s)` and `H_2O(l)` are `38.20` and `60.01Jmol^(-1)K^(-1)` respectively. The enthalpy change for the conversion is:A. `59.54 J mol^(-1)`B. `5954 J mol^(-1)`C. `595.4 J mol^(-1)`D. `320.6 J mol^(-1)`

One mole of ice is converted into water at `273K`. The entropies of `H

1.	One mole of ice is converted into water at `273K`. The entropies of `H_2O(s)` and `H_2O(l)` are `38.20` and `60.01Jmol^(-1)K^(-1)` respectively. The enthalpy change for the conversion is:A. `59.54 J mol^(-1)`B. `5954 J mol^(-1)`C. `595.4 J mol^(-1)`D. `320.6 J mol^(-1)`
Answer» Correct Answer - B `DeltaG=DeltaH-TDeltaS`, at equilibrium `DeltaG=0 :. DeltaH=TDeltaS` Or `DeltaH=273xx(60.01-38.20)` `=5954.13 J mol^(-1)`

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One mole of ice is converted into water at `273K`. The entropies of `H_2O(s)` and `H_2O(l)` are `38.20` and `60.01Jmol^(-1)K^(-1)` respectively. The enthalpy change for the conversion is:A. `59.54 J mol^(-1)`B. `5954 J mol^(-1)`C. `595.4 J mol^(-1)`D. `320.6 J mol^(-1)`

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