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. `21.98`
B. `20.13`
C. `2.013`
D. `2.198`

Answer

A

Explanation

`DeltaH=6.0 kJ mol^(-1)=6xx10^(3)J mol^(-1)`
`T=0^(@)C=273 K`
`DeltaS=(DeltaH)/(T)` (For a reversible process)
`DeltaS=(6xx10^(3)J mol^(-1))/(273 K)=21.98 JK^(-1)mol^(-1)`.