For the reaction H 2 O ( l ) ⟶ H 2 O ( g ) at T = 100 ° C and P = 1   atm , choose the…

The given reaction is:

${\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{l}\right)} \to {\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{g}\right)}$

It is the equilibrium reaction

We know that at equilibrium position

$∆{\mathrm{S}}_{\mathrm{universe}} = 0$         $\left(\mathrm{i}\right)$

Also, the relation between entropies of system and surrounding is

$$\begin{gathered} ∆{\mathrm{S}}_{\mathrm{universe}} =∆{\mathrm{S}}_{\mathrm{system}}+∆{\mathrm{S}}_{\mathrm{surrounding}} \\ 0 =∆{\mathrm{S}}_{\mathrm{system}}+∆{\mathrm{S}}_{\mathrm{surrounding}} \\ ∆{\mathrm{S}}_{\mathrm{system}}=-∆{\mathrm{S}}_{\mathrm{surrounding}} \end{gathered}$$

So, from the given option

${\mathrm{\Delta S}}_{\mathrm{system} }>0 \& {\mathrm{\Delta S}}_{\mathrm{surroundings} }<0$