$A$ process is taking place at constant temperature and pressure. Then

Gibbs free energy $G$,enthalpy $H$ and entropy $S$ are interrelated as in

Based on the provided table, which of the following options correctly identifies the spontaneous reactions?

	$\Delta_r H^{\circ}$	$\Delta_r S^{\circ}$	$\Delta_r G^{\circ}$	Spontaneity of the reaction
$A$	$+$	$+$	$+$	Spontaneous at low $T$
$B$	$+$	$+$	$-$	Spontaneous at high $T$
$C$	$-$	$-$	$-$	Spontaneous at low $T$
$D$	$+$	$-$	$+$	Spontaneous at high $T$

The occurrence of a reaction is impossible if

When $\Delta H_{vap} = 30 \ kJ \ mol^{-1}$ and $\Delta S_{vap} = 75 \ J \ mol^{-1} \ K^{-1}$,then the temperature of vapour,at one atmosphere is . . . . $K$.

The free energy for a reaction having $\Delta H = 31400 \, cal$ and $\Delta S = 32 \, cal \, K^{-1} \, mol^{-1}$ at $1000 \, ^oC$ is ....... $cal$.