$A$ minus sign of the free energy change denotes that

For a reaction,$\Delta H = +3 \, kJ$ and $\Delta S = +10 \, J/K$. At what minimum temperature (in $K$) will the reaction become spontaneous?

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

For the reaction $2 \ NO_{2(g)} \rightleftharpoons N_2O_{4(g)}$,when $\Delta S = -176.0 \ J \ K^{-1} \ mol^{-1}$ and $\Delta H = -57.8 \ kJ \ mol^{-1}$,the magnitude of $\Delta G$ at $298 \ K$ for the reaction is $...... \ kJ \ mol^{-1}$. (Nearest integer)

Conversion of oxygen into ozone is non-spontaneous at

For an endothermic reaction at constant temperature $T$ and pressure $P$,if the process is spontaneous,which of the following is true?