Correct Answer - 3
`DeltaW_(vap)=40850J mol^(-1),T_(b)=373K`
`DeltaS_(vap)=(DeltaH_(vap))/(T_(b))=(40850J mol^(-1))/(373K)=109.5K^(-1)mol^(-1)`
`DeltaS_(vap)` per gram`=(505.5JK^(-1)mol^(-1))/(18gmol^(-1))=6.083JK^(-1)g^(-1)`
Entropy change for `3.6g` water `=6.083JK^(-1)g^(-1)xx3.5g=21.69JK^(-1)`