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,which of the following conditions is most favorable?

$\Delta H$ 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:

For the reaction $A \longrightarrow B$,$\Delta H^{\circ} = 7.5 \, kJ \, mol^{-1}$ and $\Delta S^{\circ} = 25 \, J \, K^{-1} \, mol^{-1}$. The value of $\Delta G^{\circ}$ and the temperature at which the reaction reaches equilibrium are,respectively:

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

For the reaction occurring in the gaseous phase: $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,which of the following conditions is correct for the reaction to be spontaneous at high temperatures?