Which of the following set of thermodynamic conditions is true for the reaction to be spontaneous at high temperature?

For the conversion of limestone to lime,$CaCO_{3(s)} \rightarrow CaO_{(s)} + CO_{2(g)}$,the values of $\Delta H^{\circ}$ and $\Delta S^{\circ}$ at $298 \, K$ and $1 \, bar$ pressure are $+179.1 \, kJ \, mol^{-1}$ and $160.2 \, J \, K^{-1} \, mol^{-1}$ respectively. Assuming $\Delta H^{\circ}$ and $\Delta S^{\circ}$ do not change with temperature,at what temperature (in $K$) will the conversion of limestone to lime become spontaneous (in $, K$)?

For $2 \ mol$ of $He$ (ideal gas),find the work done in a process where it is heated from $200 \ K$ to $400 \ K$ such that the enthalpy of the gas varies as : $H = 10 \ V^2$ (in $R$)

What is the work done when $1 \, \text{mole}$ of a gas expands isothermally and reversibly from $25 \, \text{L}$ to $250 \, \text{L}$ at a temperature of $300 \, \text{K}$? (in $J$)

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:

For a certain reaction,the enthalpy change and entropy change are $40.63 \ kJ \ mol^{-1}$ and $100 \ J \ K^{-1} \ mol^{-1}$ respectively. What will be the value of $\Delta G$ at $27 \ ^oC$?