For the reaction CO(g)+12O2(g)→CO2(g),ΔH and ΔS are −283 kJ and −87 J K−1 mol−1 respectively. It was intended to carry out this reaction at 1000,1500,3000 and 3500 K. At which of these temperatures would this reaction be thermodynamically spontaneous?

For the reaction CO(g)+12O2(g)→CO2(g),ΔH and ΔS are −283 kJ and

1.	For the reaction CO(g)+12O2(g)→CO2(g),ΔH and ΔS are −283 kJ and −87 J K−1 mol−1 respectively. It was intended to carry out this reaction at 1000,1500,3000 and 3500 K. At which of these temperatures would this reaction be thermodynamically spontaneous?
Answer» For the reaction $C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g), Δ H$ and $Δ S$ are $- 283 kJ$ and $- 87 {J K}^{- 1} {mol}^{- 1}$ respectively. It was intended to carry out this reaction at $1000, 1500, 3000$ and $3500 K$ . At which of these temperatures would this reaction be thermodynamically spontaneous?