The enthalpy change for the transition of liquid water to steam at $100\,^oC$ is $40.8\, kJ\, mol^{-1}$. The entropy change for this process is .... $J\, K^{-1}\, mol^{-1}$.

When the same quantity of heat is absorbed by a system at two different temperatures $T_{1}$ and $T_{2}$,such that $T_{1} > T_{2}$,the changes in entropy are $\Delta S_{1}$ and $\Delta S_{2}$ respectively. Then:

What happens to the entropy during the melting of ice to water?

Fill in the blanks:
$(i)$ The entropy of one mole of a substance at a fixed temperature and standard state is called ........ .
$(ii)$ The unit of molar entropy is .......... .
$(iii)$ The process of conversion of graphite into diamond is of ........ type.

Enthalpy of vaporization of benzene is $+35.3 \ kJ \ mol^{-1}$ at its boiling point,$80^{\circ} C$. The entropy change in the transition of the vapour to liquid at its boiling point in $[J \ K^{-1} \ mol^{-1}]$ is

Considering entropy $(S)$ as a thermodynamic parameter,what are the necessary conditions for a process to be spontaneous?