For a reversible spontaneous change,$\Delta S$ is:

What is the entropy change (in $J\, K^{-1}\, mol^{-1}$) when one mole of ice is converted into water at $0^{\circ}C$? (The enthalpy change for the conversion of ice to liquid water is $6.0\, kJ\, mol^{-1}$ at $0^{\circ}C$)

Calculate the entropy change in $JK^{-1}$ for the reversible expansion of $5 \ mol$ of an ideal gas at $27 \ ^oC$ from $8 \ dm^3$ to $80 \ dm^3$.

Calculate the entropy change in $J \, mol^{-1} K^{-1}$ for the isothermal reversible expansion of $2 \, mol$ of an ideal gas from a volume of $10 \, dm^3$ to $100 \, dm^3$ at $27 \, ^oC$.

Calculate $\Delta S_{total}$ for a certain reaction at $298 \ K$ if $\Delta H^{\circ} = -208.6 \ kJ$ and $\Delta S^{\circ} = -36 \ J \ K^{-1}$. (in $J \ K^{-1}$)

Which of the following statements is correct?