Enthalpy change for the process,
`H_(2)O"(ice")hArr H_(2)O"(water)"`
is `"6.01 kJ mol"^(-1)`. The entropy change of 1 mole of ice at its melting point will be

Enthalpy of fusion of water is 6.01 kJ mol^(-1) . The entropy change of 1 mole of ice at its melting point will be:

The molar enthlpy of fusion of water is 6.01KJ mol^(-1) . The entropy change of 1 mol of water at its melting point will be

The enthalpy change for the reaction, H_2 O_((s))to H_2 O_((l)),Delta H=+6.01 kJ mol^(-1) at 0^@C is called enthalpy of _______ .

The enthalpy of fusion of water is 1.435 kcal/mol. The molar entropy change for the melting of ice at 0°C is ?

One mole of ice is coverted 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. The enthaply change for the conversion is

Latent heat of fusion of ice is 6 kJ mol^(-1) . Calculate the entropy change in the fusion of ice.