The entropy change in the isothermal reversible expansion of $2$ moles of an ideal gas from $10 \ L$ to $100 \ L$ at $300 \ K$ is: (in $JK^{-1}$)

Identify from the following physical transformations that exhibits a decrease in entropy.

Standard entropy of $X_2, Y_2$ and $XY_3$ are $60, 40$ and $50 \ J \ K^{-1} \ mol^{-1},$ respectively. For the reaction,$\frac{1}{2}X_2 + \frac{3}{2}Y_2 \to XY_3, \ \Delta H = -30 \ kJ,$ to be at equilibrium,the temperature will be ............... $K$.

The $S^o$ of the following substances are:
$CH_{4(g)} : 186.2 \ J \ K^{-1} \ mol^{-1}$
$O_{2(g)} : 205.2 \ J \ K^{-1} \ mol^{-1}$
$CO_{2(g)} : 213.6 \ J \ K^{-1} \ mol^{-1}$
$H_2O_{(l)} : 69.9 \ J \ K^{-1} \ mol^{-1}$
The entropy change $\Delta S^o$ . . . . . . $J \ K^{-1} \ mol^{-1}$ for the reaction
$CH_{4(g)} + 2O_{2(g)} \to CO_{2(g)} + 2H_2O_{(l)}$ is

For the reaction $2 H_{2(g)} + O_{2(g)} \longrightarrow 2 H_2O_{(g)}$,at $300 \ K$,$\Delta G$ and $\Delta H$ of water are $-228.4 \ kJ \ mol^{-1}$ and $-241.60 \ kJ \ mol^{-1}$,respectively. Calculate the value of change in entropy for the given reaction.

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