The total entropy change for a system and its surroundings increases,if the process 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 $\Delta H = +45.0 \, kJ$]

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

Of the following,the largest value of entropy at $25^{\circ} C$ and $1 \ atm$ is that of

One mole of an ideal diatomic gas $(C_V = 5 \ cal)$ was transformed from initial $25 \ ^{\circ}C$ and $1 \ L$ to the state when temperature is $100 \ ^{\circ}C$ and volume $10 \ L$. The entropy change of the process can be expressed as $(R = 2 \ cal / mol \cdot K)$ :-

Which of the following is correct regarding entropy?