Gibbs free energy $(G)$ is defined as

For the reaction $H_{2(g)} + \frac{1}{2}O_{2(g)} \to H_2O_{(l)}$,$\Delta H = -285.8 \ kJ \ mol^{-1}$,$\Delta S = -0.163 \ kJ \ mol^{-1} K^{-1}$. What is the value of free energy change at $27 \ ^\circ C$ for the reaction in $kJ \ mol^{-1}$?

Which of the following conditions regarding a chemical process ensures its spontaneity at all temperatures?

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 $T$

What is the relationship between Gibbs free energy change,enthalpy change,and entropy change?

If a chemical reaction is known to be non-spontaneous at $298 \ K$ but spontaneous at $350 \ K$,then which among the following conditions is true for the reaction?