Calculate the entropy change involved in the converion of one mole of liquid water at 373 K to vapour at the same temperature ( latenet heat of vaporization of water Delta_(vap) H = 2.257 kJ //g)

Calculate the entropy change involved in the converion of one mole of

1.	Calculate the entropy change involved in the converion of one mole of liquid water at 373 K to vapour at the same temperature ( latenet heat of vaporization of water Delta_(vap) H = 2.257 kJ //g)
Answer» Solution : For the conversion of water `rarr` vapour , the entropy change is given by `Delta_(vap) S = (Delta_(vap) H)/( T_(b))` Here, `Delta_(vap) H=2.257 kJ //g = 2.257 xx18 kJ //mol =40.626 kJ //mol, T_(b) = 373 K` `:. Delta _(vap ) S = (40.626k J mol^(-1))/( 373K) = 0.1089K J K^(-1) mol^(-1) = 108.9 J K^(-1) mol^(-1)`