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 $25\,^oC$?

Give the mathematical equation for entropy change.

An irreversible process occurring isothermally in an isolated system leads to

Of the following,the largest value of entropy at $25^{\circ} C$ and $1 \ atm$ is that of

Identify the incorrect statements from the following:
$I. \quad \Delta S_{\text{system}} = (\Delta S_{\text{total}} + \Delta S_{\text{surr.}})$
$II. A_{(l)} \rightarrow A_{(s)}$: for this process entropy change decreases
$III.$ Entropy units are $J K^{-1} mol^{-1}$

Statement-$1$: For a process at equilibrium,the total entropy is maximum and the change in total entropy is zero.
Statement-$2$: For a reversible process,if the same amount of heat is supplied to a system at two different temperatures,then the entropy change is less at a lower temperature.