Consider the reaction 2Fe₂O₃(s)+ 3C(s)$\rightarrow$ 4Fe(s)+ 3CO₂(g), $\Delta$H^$\omicron$= 462 kJ, $\Delta$S^$\omicron$= 558 J . K ^- ¹ Calculate the equilibrium constant for this reaction at 525^$\omicron$C.

Question

Quizplus · Accepted Answer

The equilibrium constant can be calculated using the Gibbs free energy change, $\Delta G^\omicron = \Delta H^\omicron - T\Delta S^\omicron$, and the relation $\Delta G^\omicron = -RT \ln K$. At 525°C (798 K), $\Delta G^\omicron$ is calculated and then used to find $K$.

Consider the Reaction 2Fe2O3(s)+ 3C(s) →\rightarrow→ 4Fe(s)+ 3CO2(g) Δ\DeltaΔ H ο\omicronο = 462 KJ

Consider the Reaction
2Fe₂O₃(s)+ 3C(s) $\rightarrow$ 4Fe(s)+ 3CO₂(g) $\Delta$ H^$\omicron$= 462 KJ