Assuming $\Delta$S° and $\Delta$H° do not vary with temperature, at what temperature will the reaction shown below become spontaneous? C(s)+ H₂O(g)$\rarr$H₂(g)+ CO(s)($\Delta$S° = 133.6 J/K·mol; $\Delta$H° = 131.3 kJ/mol)

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The Answer of Assuming $\Delta$S° and $\Delta$H° do not vary with temperature, at what temperature will the reaction shown below become spontaneous? C(s)+ H₂O(g)$\rarr$H₂(g)+ CO(s)($\Delta$S° = 133.6 J/K·mol; $\Delta$H° = 131.3 kJ/mol)

Assuming Δ\DeltaΔ S° And Δ\DeltaΔ H° Do Not Vary with Temperature, at What Temperature Will

Assuming $\Delta$ S° And $\Delta$ H° Do Not Vary with Temperature, at What Temperature Will