Heat of neutralisation of strong acid and strong base under `1 atm` and `25^@C` is `-13.7 kcal`. If standard Gibbs energy change for dissociation of water to `H^+` and `OH^-` is `-19.14 kcal`, the change in standard entropy for dissociation of water is:

Options

A. `18.25 calK^(-1) mol^(-1)`
B. `110.2 calK^(-1) mol^(-1)`
C. `-18.25 calK^(-1) mol^(-1)`
D. `-110.2 calK^(-1) mol^(-1)`

Answer

B

Explanation

`:' DeltaG^(@)=DeltaH^(@)-TDeltaS^(@)`
`:. DeltaH^(@)` for `H_(2)OhArrH^(+)+OH^(-)` is`+13.7 kcal`
`:. DeltaS^(@)=(DeltaH^(@)-DeltaG^(@))/T`
`=(+13.7+19.14)/298=110.2 calK^(-1) mol^(-1)`