For a chemical reaction A + B ⇌ C + D (Δ_r H^ =80 kJ mol^-1) the entropy change Δ_r S^ depends on the temperature T (in K ) as Δ_r S^ =2 T ( J K^-1…

For a chemical reaction $\displaystyle \mathrm{A}+\mathrm{B} \rightleftharpoons \mathrm{C}+\mathrm{D}$ $\displaystyle \left(\Delta_{\mathrm{r}} \mathrm{H}^{\ominus}=80 \mathrm{~kJ} \mathrm{~mol}^{-1}\right)$ the entropy change $\displaystyle \Delta_{\mathrm{r}} \mathrm{S}^{\ominus}$ depends on the temperature T (in K ) as $\displaystyle \Delta_{\mathrm{r}} \mathrm{S}^{\ominus}=2 \mathrm{~T}\left(\mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$. Minimum temperature at which it will become spontaneous is \_\_\_\_ K. (Integer)