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

For a reaction at $25 \, ^oC$,the enthalpy change and entropy change are $-11.7 \times 10^3 \, J \, mol^{-1}$ and $-105 \, J \, mol^{-1} \, K^{-1}$ respectively. What is the Gibbs free energy in $kJ$?

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 $J$)

Describe Gibbs energy and spontaneity.

At $273 \ K$ the maximum work done when pressure on $10 \ g$ of hydrogen is reduced from $10 \ atm$ to $1 \ atm$ under isothermal,reversible conditions is (Assume the gas behaves ideally) $(R=8.3 \ J \ K^{-1} \ mol^{-1})$

Compare the following criteria for spontaneity of a reaction based on the values of $\Delta_{\text{r}}H^0$,$\Delta_{\text{r}}S^0$,and $\Delta_{\text{r}}G^0$:

$\Delta_{\text{r}}H^0$	$\Delta_{\text{r}}S^0$	$\Delta_{\text{r}}G^0$	Description
$(a) (+)$	$(-)$	$(+)$	$(i) \text{ Non-spontaneous at all temperatures}$
$(b) (-)$	$(-)$	$(-)$	$(ii) \text{ Spontaneous at low temperatures}$
$(c) (-)$	$(+)$	$(-)$	$(iii) \text{ Spontaneous at all temperatures}$