The entropy values (in $J K^{-1} mol^{-1}$) of $H_{2(g)} = 130.6$,$Cl_{2(g)} = 223.0$ and $HCl_{(g)} = 186.7$ at $298 \ K$ and $1 \ atm$ pressure. Then entropy change for the reaction $H_{2(g)} + Cl_{2(g)} \to 2HCl_{(g)}$ is :-

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 $J K^{-1} mol^{-1}$

If the standard molar entropies $(S^o)$ for $H_2$,$Cl_2$,and $HCl$ are $0.13$,$0.22$,and $0.19 \, kJ \, K^{-1} \, mol^{-1}$ respectively,what is the total change in standard entropy $(\Delta S^o)$ for the reaction $H_2 + Cl_2 \rightarrow 2HCl$ in $J \, K^{-1} \, mol^{-1}$?

The enthalpy change for the transition of liquid water to steam,$\Delta H_{vap} = 37.3 \ kJ \ mol^{-1}$ at $373 \ K$. The entropy change for the process is......$J \ mol^{-1} K^{-1}$.

When two gases are mixed,the entropy $......$

Which of the following is the least $random$ state of water?