The latent heat of melting of ice at $0^{\circ} C$ is $6 \, kJ \, mol^{-1}$. The entropy change during the melting in $J \, K^{-1} \, mol^{-1}$ is closest to

If the enthalpy change for the following reaction at $300 \ K$ is $+7 \ kJ \ mol^{-1}$,find the entropy change of the surrounding (in $J \ K^{-1}$)?
$H_2O_{(s)} \longrightarrow H_2O_{(l)}$

The $\Delta S$ for the vaporisation of $1 \ mol$ of water is $88.3 \ J/mol \ K$. The value of $\Delta S$ for the condensation of $1 \ mol$ of vapour will be.......$ J/mol \ K$

Given $\Delta _rS^o = -266 \ J \ K^{-1}$ and the listed $S_m^o$ values,calculate $S^o$ for $Fe_3O_{4(s)}$ for the reaction: $4 Fe_3O_{4(s)} + O_{2(g)} \to 6 Fe_2O_{3(s)}$. Given $S_m^o(Fe_2O_3) = 87 \ J \ K^{-1} \ mol^{-1}$ and $S_m^o(O_2) = 205 \ J \ K^{-1} \ mol^{-1}$.

At the boiling point of water,$900 \ J/g$ of heat is exchanged. What is the increase in entropy in $J \ K^{-1} \ mol^{-1}$?

Calculate the entropy change for melting $1 \ g$ of ice at $0^{\circ} C$ in $J \ g^{-1} K^{-1}$,if the heat of fusion of ice at $0^{\circ} C$ is $80 \ J \ g^{-1}$.