For a spontaneous process,the correct statement is

$3$ 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 $40.668 \ kJ/mol$ ]

Which of the following reactions exhibits a decrease in entropy?

Give the mathematical equation for entropy change.

What is the entropy change (in $J\, K^{-1}\, mol^{-1}$) when one mole of ice is converted into water at $0^{\circ}C$? (The enthalpy change for the conversion of ice to liquid water is $6.0\, kJ\, mol^{-1}$ at $0^{\circ}C$)

The molar heat of vaporisation of a liquid is $6 \ kJ \ mol^{-1}$. If the entropy change is $16 \ J \ mol^{-1} \ K^{-1}$,the boiling point of the liquid is: