The enthalpy of vaporization of water is $186.5 \, kJ \, mol^{-1}$. What is the entropy of vaporization in $kJ \, K^{-1} \, mol^{-1}$?

Which state functions are required to understand the second law of thermodynamics?

The enthalpy of vaporisation of a certain liquid at its boiling point of $35^{\circ} C$ is $24.64 \ kJ \ mol^{-1}$. The value of change in entropy for the process is

When a liquid boils,there is

In which of the following processes does entropy increase?

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