The enthalpy change for the conversion of water into vapor at $27^\circ C$ is $30 \ kJ/mol$. The entropy change for this process in $J/mol \ K$ is:

At $10\, ^oC$,$1\, mol$ of an ideal gas is allowed to expand reversibly and adiabatically from $10\, L$ to $200\, L$. Calculate the change in entropy in $cal/K$.

For the reaction $MgCO_3(s) \rightarrow MgO(s) + CO_2(g)$,the value of $\Delta S$ is:

Entropy of the universe is

For the vaporization of water at $1 \, \text{atm}$ pressure,the liquid water and water vapor are in equilibrium. What is the temperature in $K$?
$H_2O_{(l)} \rightleftharpoons H_2O_{(g)}$ [at $1 \, \text{atm}$ pressure] [$\Delta S = 120 \, J K^{-1}$ and $\Delta H = +45.0 \, kJ$]

Two moles of an ideal gas undergo free expansion from $10 \ L$ to $100 \ L$ at $300 \ K$. The values of $\Delta S_{system}$ and $\Delta S_{surroundings}$ are ($R$ is universal gas constant)