What is the entropy change (in `JK^(-1)mol^(-1)`) when one mole of ice is converted into water at `0^(@)C`?
(The enthalpy change for the conversion of ice to liquid water is `6.0KJmol^(-1)` at `0^(@)C`)

Options

A. `2.198 JK^(-1) "mol"^(-1)`
B. `21.98 JK^(-1) "mol"^(-1)`
C. `20.13 JK^(-1) "mol"^(-1)`
D. `2.013 JK^(-1) "mol"^(-1)`

Answer

B

Explanation

Given , `DeltaH_(f)=6.0 KJ "mol"^(-1)`
`T=0+273=273 K`
`DeltaH_(f)=(6.0)/(273) = 0.02198 JK^(-1) "mol"^(-1)`
`(T=0^(@) C + 273 K =273 K )`
`=0.02198 xx 1000 JK^(-1) "mol"^(-1)`
`=21.98 JK^(-1) "mol"^(-1)`