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 $JK^{-1}$)

Identify the reaction/process in which the entropy increases.

What is the melting point of benzene if $\Delta H_{fusion} = 9.95 \ kJ/mol$ and $\Delta S_{fusion} = 35.7 \ J/K \cdot mol$?

$A$ container is divided into two compartments by a removable partition as shown below:
In the first compartment,$n_{1}$ moles of ideal gas $He$ is present in a volume $V_{1}$. In the second compartment,$n_{2}$ moles of ideal gas $Ne$ is present in a volume $V_{2}$. The temperature and pressure in both the compartments are $T$ and $p$,respectively. Assuming $R$ is the gas constant,the total change in entropy upon removing the partition when the gases mix irreversibly is:

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:

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