If the enthalpy change for the transition of liquid water to steam is $30 \ kJ \ mol^{-1}$ at $27 \ ^oC,$ the entropy change for the process would be ............. $J \ mol^{-1} \ K^{-1}$

For which one of the following reactions, the entropy change is positive?

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 ...... $J \ mol^{-1}$.

The entropy change in the isothermal reversible expansion of $2$ moles of an ideal gas from $10 \ L$ to $100 \ L$ at $300 \ K$ is: (in $JK^{-1}$)

The enthalpy of vapourization of a liquid is $30 \ kJ \ mol^{-1}$ and entropy of vapourization is $75 \ J \ mol^{-1} \ K^{-1}$. The boiling point of the liquid at $1 \ atm$ is.......$K$

In which of the following processes is $\Delta S$ negative?