If a process is non-spontaneous,which of the following options is correct?

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

Consider the graph of $Gibbs$ free energy $G$ vs. Extent of reaction. The number of statement$(s)$ from the following which are true with respect to points $(a)$,$(b)$,and $(c)$ is $.................$
$A$. Reaction is spontaneous at $(a)$ and $(b)$
$B$. Reaction is at equilibrium at point $(b)$ and non-spontaneous at point $(c)$
$C$. Reaction is spontaneous at $(a)$ and non-spontaneous at $(c)$
$D$. Reaction is non-spontaneous at $(a)$ and $(b)$

For the reaction $CaCO_{3(s)} \to CaO_{(s)} + CO_{2(g)}$,given $\Delta H^o = 178.3 \, kJ$ and $\Delta S^o = 160 \, J \cdot K^{-1}$. At what temperature will the reaction become spontaneous?

For a reaction to be spontaneous,the required conditions are

For the vaporization of water at $1 \ atm$ pressure,the values of $\Delta H$ and $\Delta S$ are $40.63 \ kJ/mol$ and $108.8 \ J/K \cdot mol$ respectively. At what temperature $(K)$ will the change in Gibbs energy $(\Delta G)$ be zero (in $.4$)?