One mole of an ideal gas is expanded isothermally and reversibly to half of its initial pressure. $\Delta S$ for the process in $J \ K^{-1} \ mol^{-1}$ is $[ln \ 2 = 0.693$ and $R = 8.314 \ J \ mol^{-1} \ K^{-1}]$

The standard molar entropy of $H_{2}O_{(l)}$ is $70 \ J \ K^{-1} \ mol^{-1}$. Will the standard molar entropy of $H_{2}O_{(s)}$ be more or less than $70 \ J \ K^{-1} \ mol^{-1}$?

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

For the conversion $C$ (graphite) $\to C$ (diamond),the $\Delta S$ is:

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

Calculate the entropy change of the surrounding if $2 \ moles$ of $H_2$ and $1 \ mole$ of $O_2$ gas combine to form $2 \ moles$ of liquid water by releasing $525 \ kJ$ of heat to the surrounding at constant pressure and at $300 \ K$. (in $J \ K^{-1}$)