Calculate $\Delta H^{\circ}$ for a reaction at $298 \ K$ if $\Delta S^{\circ} = 120 \ J \ K^{-1}$ and $\Delta G^{\circ} = 28000 \ J$. (in $kJ$)

In which of the following conditions will a reaction always be spontaneous at all temperatures?

What is the relationship between Gibbs free energy change,enthalpy change,and entropy change?

For a spontaneous process, the incorrect statement is

$A$ spontaneous process is impossible if ........

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 $, K$)?