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)`

Explanation

`DeltaS_("fusion")=(DeltaH_(f))/T=(6.025xx10^(3))/273`
`=22.1 JK^(-1) mol^(-1)`
Now,
`18 g` ice melts showing a change in entropy =`22.1`
`:. 1 g` ice melts showing a change in entropy
`22.1/18xx1=1.227 JK^(-1)`
(b) `DeltaS_(V)=(DeltaH_(V))/T=(40.63xx10^(3))/373`
`=108.9 KJ^(-1)mol^(-1)`
`18 g H_(2)O` vaporises to show a change in entropy `=108.9`
`:. 36 g H_(2)O` vaporises to show a change in entropy `=(108.9xx36)/18=217.85 JK^(-1)`