The Second Law of Thermodynamics

Standard entropies of ${\mathrm{X}}_2,{\mathrm{Y}}_2$ and ${\mathrm{XY}}_3$ are $60,40$ and $50 \mathrm{J}/K/\mathrm{mol}$ respectively. At what temperature the following reaction will be at equilibrium

If a chemical reaction is known to be non-spontaneous at $298 \mathrm{K}$ but spontaneous at $350 \mathrm{K}$, then which among the following conditions is true for the reaction?

For the reaction ${\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{l}\right)}⟶{\mathrm{H}}_2{\mathrm{O}}_{\left(g\right)}$ at $T=100°\mathrm{C}$ and $\mathrm{P}=1 \mathrm{atm}$, choose the correct option:

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

At the temperature $\mathrm{T}\left(\mathrm{K}\right)$ for the reaction ${\mathrm{X}}_2{\mathrm{O}}_4 \left(\mathrm{l}\right)\to 2{\mathrm{XO}}_2 \left(\mathrm{g}\right) \mathrm{\Delta U}=\mathrm{x} \mathrm{kJ} {\mathrm{mol}}^{-1}$ $\mathrm{\Delta S}=\mathrm{y} {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}$. Gibbs energy change for the reaction is
$($Assume ${\mathrm{X}}_2{\mathrm{O}}_4, {\mathrm{XO}}_2$ are ideal gases$)$

For the reaction. $2{\mathrm{H}}_2 \left(\mathrm{g}\right)+{\mathrm{O}}_2 {\left(\mathrm{g}\right)}_{}⟶2{\mathrm{H}}_2\mathrm{O} {\left(\mathrm{g}\right)}_{}, \mathrm{at} 300 \mathrm{K}, \mathrm{\Delta G}$ and $\mathrm{\Delta H}$ of water are $-228.4 \mathrm{kJ}.{\mathrm{mol}}^{-1}$  and $-241.60 \mathrm{kJ}.{\mathrm{mol}}^{-1}$, respectively. Then calculate the value of change in entropy for the given reaction.