What happens to the total entropy of the system and surroundings during a spontaneous irreversible process?

$STATEMENT-1:$ There is a natural asymmetry between converting work to heat and converting heat to work.
$STATEMENT-2:$ No process is possible in which the sole result is the absorption of heat from a reservoir and its complete conversion into work.

For which of the following processes,$\Delta S$ is negative?

Calculate the entropy change of the surrounding if $2 \ moles$ of $H_2$ and $1 \ mole$ of $O_2$ gas combine to form $2 \ moles$ of liquid water by releasing $525 \ kJ$ of heat to the surrounding at constant pressure and at $300 \ K$. (in $J \ K^{-1}$)

What is the entropy of vaporisation of water at $100\,^{\circ}C$,if the molar heat of vaporisation is $9710\,cal/mol$?

What is entropy? Explain its role in spontaneity.