What is entropy change for the conversion of one gram of ice to water at 273 K and one atmospheric pressure?
`(DeltaH_("fusion")=6.025kJ" "mol^(-1))`

What is the entropy change for the conversion of one gram of ice to water at 167 K and one atmospheric pressure ? [Delta H_("fussion") = 6.025 kJ mol^(-1)]

Calculate the entropy change during the melting of one mole of ice into water at 0^@C and 1 atm pressure. Enthalpy of fusion of ice is 6008 J "Mole"^(-1)

Calculate the entropy change during the melting of one mole of ice into water at 0^@C and 1 atm pressure. Enthalpy of fusion of ice is 6008 "J mol"^(-1) .

Calculate the entropy change for the conservation of following: (a) 1g ice to water at 273K , DeltaH_f for ice=6.025kJmol^(-1) . (b) 36g water to vapour at 373K, DeltaH_v for H_2O=40.63kJmol(-1)

Entropy change involved in the conversion of 1 mole of liquid water at 373 K to vapour at the same temperature will be ____ ( DeltaH_"vap"=2.257 kJ g^(-1) )