Entropy change involved in the conversion of1 mole of liquid water at 373 K to vapour at the same temperature will be ____ (DeltaH_"vap"=2.257 kJ g^(-1))

Entropy change involved in the conversion of1 mole of liquid water at

1.	Entropy change involved in the conversion of1 mole of liquid water at 373 K to vapour at the same temperature will be ____ (DeltaH_"vap"=2.257 kJ g^(-1))
Answer» Solution :`DeltaH_"vap"=2.257 K J G^(-1)` 1 mole of `H_2O`=18 g `therefore DeltaH_"vap"` for a1 mole = `2.257xx18=40.626 k J g^(-1)` . `T_b` =373 K `DeltaS_"vap"=40.626/373=0.1089 "KJ mol"^(-1)` `=0.109 "kJ mol"^(-1)`