State the criteria for a spontaneous process in terms of $\Delta G$ at constant pressure and temperature.

Which of the following set of thermodynamic conditions is true for the reaction to be spontaneous at high temperature?

For vaporization of water at $1$ atmospheric pressure,the values of $\Delta H$ and $\Delta S$ are $40.63 \ kJ \ mol^{-1}$ and $108.8 \ J \ K^{-1} \ mol^{-1},$ respectively. The temperature when Gibb's energy change $(\Delta G)$ for this transformation will be zero,is ............ $K$. (in $.4$)

Which of the following conditions will always lead to a non-spontaneous change?

What is the relationship between Gibbs free energy change,enthalpy change,and entropy change?

The temperature in $K$ at which $\Delta G = 0$, for a given reaction with $\Delta H = -20.5 \ kJ \ mol^{-1}$ and $\Delta S = -50.0 \ J \ K^{-1} \ mol^{-1}$ is: