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

Which of the following reactions is expected to never be spontaneous?

Calculate the work done when $1 \text{ mole}$ of an ideal gas is expanded reversibly and isothermally from an initial pressure $P_1 = 10 \text{ bar}$ to a final pressure $P_2 = 1 \text{ bar}$ at a constant temperature $T = 300 \text{ K}$. $[R = 8.314 \text{ J K}^{-1} \text{ mol}^{-1}]$ (in $\text{ kJ}$)

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?

The maximum work done in expanding $16 \ g$ of oxygen at $300 \ K$ from an initial volume of $5 \ dm^3$ to a final volume of $25 \ dm^3$ isothermally and reversibly is $(\log_{10} 5 = 0.699)$.

For the reaction $H_2O_{(l)} \rightleftharpoons H_2O_{(g)}$ at $373 \ K$ and $1 \ atm$ pressure,which of the following is true?