In a spontaneous process,the entropy of the system and its surroundings

The enthalpy change for the transition of liquid water to steam is $37.3 \ kJ \ mol^{-1}$ at $373 \ K$. Find $\Delta S$ in $J \ mol^{-1} \ K^{-1}$.

For a process to occur spontaneously,

One mole of ice is converted into water at $273 \, K$. The entropy of $H_2O_{(s)}$ and $H_2O_{(l)}$ are $38.20 \, J \, mol^{-1} \, K^{-1}$ and $60.01 \, J \, mol^{-1} \, K^{-1}$ respectively. The enthalpy change for the conversion is $....... \, J \, mol^{-1}$.

The standard entropies of $CO_{2(g)}$,$C_{(s)}$,and $O_{2(g)}$ are $213.5$,$5.740$,and $205 \ J \ K^{-1} \ mol^{-1}$ respectively. The standard entropy of formation of $CO_{2(g)}$ is $...... \ J \ K^{-1} \ mol^{-1}$.

What happens to the entropy of water when it freezes to form an ice cube?