At a temperature of $298 \ K$,if $\Delta H < T \Delta S$,what is the value of the equilibrium constant $K$?

For a given chemical reaction $A \rightarrow B$ at $300 \ K$,the free energy change is $-49.4 \ kJ \ mol^{-1}$ and the enthalpy of reaction is $51.4 \ kJ \ mol^{-1}$. The entropy change of the reaction is $..... \ J \ K^{-1} \ mol^{-1}$.

For a reaction $\Delta H = 9.08 \ kJ \ mol^{-1}$ and $\Delta S = 35.7 \ J \ K^{-1} \ mol^{-1}$. Which of the following statements is correct for the reaction?

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:

Which of the following pairs of a chemical reaction is certain to result in a spontaneous reaction?

For a process occurring at constant temperature and pressure,which of the following is true at equilibrium?