Calculate the entropy change for the melting of $1 \, kg$ of ice at $0 \, ^\circ C$ in $SI$ units. (Latent heat of fusion of ice = $80 \, cal \, g^{-1}$) (in $.67$)

In which of the following reactions,standard reaction entropy change $(\Delta S^o)$ is positive and standard Gibb's energy change $(\Delta G^o)$ decreases sharply with increasing temperature?

Which of the following substances has the highest entropy?

Which of the following processes is non-spontaneous?

One mole of an ideal gas expands adiabatically and reversibly from its initial pressure to half of its initial pressure. What will be the value of $\Delta S$ in $J \ K^{-1} \ mol^{-1}$? $[ln 2 = 0.693$ and $R = 8.314 \ J \ mol^{-1} \ K^{-1}]$

One mole of ice is converted into water at $1 \ atm$ and $273 \ K$. The entropies of $H_2O_{(s)}$ and $H_2O_{(\ell)}$ are $38.2$ and $60.01 \ J \ mol^{-1} \ K^{-1}$ respectively. The enthalpy change for the conversion is ...... $J \ mol^{-1}$.