For a certain reaction, ΔH⁰ and ΔS⁰ respectively are 400 KJ & 200 J/mol/K. The process is non-spontaneous at

 

$$\begin{gathered} ∆{\mathrm{G}}^0=∆{\mathrm{H}}^0-\mathrm{T}∆{\mathrm{S}}^0; \\ ∆{\mathrm{G}}^0=+\mathrm{ve}-\mathrm{T}\left(+\mathrm{ve}\right); \\ ∆{\mathrm{G}}^0 \mathrm{will} \mathrm{be} \mathrm{positive} \mathrm{only} \mathrm{when} \mathrm{T}<{\mathrm{T}}_{\mathrm{eq}}; \end{gathered}$$