Which of the following formulas is correct for Gibbs free energy $(G)$?

$A$ reaction has both $\Delta H$ and $\Delta S$ negative. The rate of reaction

The signs of $\Delta_r H^{\circ}$ and $\Delta_r S^{\circ}$ for a reaction to be spontaneous at all temperatures respectively are

The criterion for a spontaneous process is

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 $kJ$?

The spontaneous nature of a reaction is impossible if