The change of entropy $(dS)$ is defined as

$3$ moles of water is boiled at $373 \ K$ and is changed to vapour state having the same temperature. What will be the change in entropy of the system (in $kJ/K$)? [ The molar heat of vaporization of water is $40.668 \ kJ/mol$ ]

For which one of the following reactions, the entropy change is positive?

Find the change in entropy for the fusion of $1 \, mol$ of ice in $J \, K^{-1} \, mol^{-1}$. The melting point of water is $273 \, K$ and the molar enthalpy of fusion for water is $6.0 \, kJ \, mol^{-1}$.

For which one of the following reactions is the entropy change positive?

The enthalpy of fusion of water is $1.435 \ kcal/mol$. The molar entropy change for the melting of ice at $0 \ ^\circ C$ is