Identify from the following the correct set of thermodynamic conditions for the reaction to be non-spontaneous at all temperatures.

Which of the following conditions results in a spontaneous chemical reaction?

Under what conditions will a reaction become spontaneous at all temperatures?

For the reaction $A \to B$,$\Delta H = 4 \, kcal \, mol^{-1}$ and $\Delta S = 10 \, cal \, K^{-1} \, mol^{-1}$. At what temperature $(K)$ will the reaction become spontaneous?

$\Delta H$ and $\Delta S$ for a reaction are $+30.0 \ kJ \ mol^{-1}$ and $0.06 \ kJ \ K^{-1} \ mol^{-1}$ at $1 \ atm$ pressure. The temperature at which free energy change is equal to zero and the nature of the reaction below this temperature are:

$\Delta G$ is net energy available to do useful work and is thus a measure of "free energy". Show mathematically that $\Delta G$ is a measure of free energy. Find the unit of $\Delta G$. If a reaction has positive enthalpy change and positive entropy change,under what condition will the reaction be spontaneous?