One mole of ice is converted into water at 273 K. The entropies of `H_(2)O(s)` and `H_(2)O(l)` are 38.20 and 60.01 J `mol^(-1)K^(-1)` respectively. Calculate the enthalpy change for this conversion a ?

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

1.	One mole of ice is converted into water at 273 K. The entropies of `H_(2)O(s)` and `H_(2)O(l)` are 38.20 and 60.01 J `mol^(-1)K^(-1)` respectively. Calculate the enthalpy change for this conversion a ?
Answer» At 273 K ice and water are in equilibrium with each other and at equilibrium `Delta G = 0` `because Delta G = Delta H-T Delta S " " Delta H=T Delta S =273xx(60.01-38.20)=5954.13 J mol^(-1)`

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One mole of ice is converted into water at 273 K. The entropies of `H_(2)O(s)` and `H_(2)O(l)` are 38.20 and 60.01 J `mol^(-1)K^(-1)` respectively. Calculate the enthalpy change for this conversion a ?

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