Entropy change involve in conversion of `1` mole of liquid water at `373K` to vapour at the same temperature (latent heat of vaporisation of water=`2.257kJg^(-1))`

Options

A. `30.7JK^(-1)mol^(-1)`
B. `60.3JK^(-1)mol^(-1)`
C. `90.8JK^(-1)mol^(-1)`
D. `108.9JK^(-1)mol^(-1)`

Answer

C

Explanation

`DeltaH_(vap)=2.257KJ//g=(2.257xx18)Kjmol^(-1)=40.626KJmol^(-1)`
`DeltaS_(vap)=(40.626)/(373)=0.1089KJK^(-1)mol^(-1)`