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 $JK^{-1}$)

$A$ reversible adiabatic process is one in which:

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

In a reversible adiabatic process $\Delta S$ is :-

When the value of entropy is greater,then the ability of work

Which of the following processes is associated with an increase in entropy?
$(I)$ Melting of a solid
$(II)$ Mixing of gases
$(III)$ Compression of a gas
$(IV)$ Expansion of a gas