The increase in entropy in $J K^{-1}$ of a substance when it absorbs $1 \ kJ$ of heat energy at $3 \ K$ is

At $25\,^oC$ and $1\,atm$ pressure,mercury reacts with chlorine to form mercurous chloride: $2Hg + Cl_2 \to Hg_2Cl_2; \Delta H = -31.3\,kcal$. What is the entropy change of the reaction at $25\,^oC$?

$9.0 \, g$ of $H_2O$ is vaporized at $100 \, ^\circ C$ and $1 \, atm$ pressure. If the latent heat of vaporization of water is $x \, J / g$,then $\Delta S$ is given by :-

Which of the following processes is associated with a decrease in entropy?

For an isolated system,$\Delta U = 0,$ what will be $\Delta S?$

$STATEMENT-1:$ 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.