Spontaneity of a chemical reaction is decided by the negative change in

For a reaction to be spontaneous at any temperature,which of the following is true?

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
$(a) (+)$	$(-)$	$(+)$	$(i) \text{ Non-spontaneous at all temperatures}$
$(b) (-)$	$(-)$	$(-)$	$(ii) \text{ Spontaneous at low temperatures}$
$(c) (-)$	$(+)$	$(-)$	$(iii) \text{ Spontaneous at all temperatures}$

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

What is the free energy change $\Delta G$ when $1.0 \ mole$ of water at $100 \ ^oC$ and $1 \ atm$ pressure is converted into steam at $100 \ ^oC$ and $1 \ atm$ pressure?

For a certain reaction,the enthalpy change and entropy change are $40.63 \ kJ \ mol^{-1}$ and $100 \ J \ K^{-1} \ mol^{-1}$ respectively. What will be the value of $\Delta G$ at $27 \ ^oC$?