Calculate the maximum work done in expanding $16 \ g$ of oxygen $(O_2)$ at $300 \ K$ and occupying a volume of $5 \ dm^3$ isothermally until the volume becomes $25 \ dm^3$. (in $J$)

For the reaction $Ag_2O_{(s)} \rightarrow 2Ag_{(s)} + 1/2 O_{2_{(g)}}$,the value of $\Delta H = 30.56 \, kJ \, mol^{-1}$ and $\Delta S = 66 \, J \, K^{-1} \, mol^{-1}$. At what temperature $(K)$ will the change in free energy for the reaction be zero?

For the reaction $x + y \rightarrow z$,the process is spontaneous at room temperature,and the reverse reaction is spontaneous at high temperature. Which of the following is true?

The condition of spontaneity of a process is

Identify the correct statement for the change in Gibbs energy $(\Delta G_{\text{system}})$ for a system at constant temperature and pressure.

Values of $\Delta H$ and $\Delta S$ for five different reactions are given below. On the basis of these values,predict which one of these will be spontaneous at all temperatures.

Reaction	$\Delta H \ (kJ \ mol^{-1}) / \Delta S \ (J \ K^{-1} \ mol^{-1})$
$I$	$+98.0, +14.8$
$II$	$-55.5, -84.6$
$III$	$+28.3, -17.0$
$IV$	$-40.5, +24.6$
$V$	$+34.7, 0.0$