For the decomposition reaction of $N_2O_4$,$\Delta H = 58.04 \, kJ$ and $\Delta S = 176.7 \, J/K$. Calculate $\Delta G$ in $kJ$ at $T = 298 \, K$.

For a spontaneous process, the incorrect statement is

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

For a spontaneous process,which of the following conditions is most favorable?

Identify from the following the correct set of thermodynamic conditions for the reaction to be spontaneous below equilibrium temperature.

What is the nature of the reaction at $298 \ K$,if the entropy change and enthalpy change for a chemical reaction are $7.4 \ cal \ K^{-1}$ and $-2.5 \times 10^3 \ cal$,respectively?