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

What is the change in entropy when an ideal gas expands into a vacuum?

$3$ moles of water is boiled at $373 \ K$ and is changed to vapour state having the same temperature. What will be the change in entropy of the system (in $kJ/K$)? [ The molar heat of vaporization of water is $40.668 \ kJ/mol$ ]

$A$ reversible adiabatic process is one in which:

The entropy change involved in the conversion of $1 \, \text{mole}$ of liquid water at $373 \, K$ to vapour at the same temperature will be $[\Delta H_{vap} = 2.257 \, kJ/g]$. (in $, kJ/K$)

Identify the correct statement regarding a spontaneous process: