In which of the following conditions will a reaction always be spontaneous at all temperatures?

The essential condition for the feasibility of a reaction is that

For a certain reaction,$\Delta H = -210 \ kJ$ and $\Delta S = -150 \ J \ K^{-1}$. Find the temperature so that $\Delta G = 0$. (in $K$)

Describe Gibbs energy and spontaneity.

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?

For a given chemical reaction $A \rightarrow B$ at $300 \ K$,the free energy change is $-49.4 \ kJ \ mol^{-1}$ and the enthalpy of reaction is $51.4 \ kJ \ mol^{-1}$. The entropy change of the reaction is $..... \ J \ K^{-1} \ mol^{-1}$.