Using Delta G_f deg at 298 K (kJ/mol): Fe2O3 -742.2; CO -137.2; CO2 -394.4, calculate Delta G deg and log_10K for Fe2O3 + 3CO -> 2Fe + 3CO2 at 298 K (R = 8.314 J K^-1 mol^-1).

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Using $Δ G_{f}^{\circ}$ at 298 K (kJ/mol): $Fe X_{2} O X_{3}$ $- 742.2$ ; $CO$ $- 137.2$ ; $CO X_{2}$ $- 394.4$ , calculate $Δ G^{\circ}$ and $lo g_{10} K$ for $Fe X_{2} O X_{3} + 3 CO 2 Fe + 3 CO X_{2}$ at 298 K ( $R = 8.314 J K^{- 1} mo l^{- 1}$ ).

Δ G^{\circ} = 3 (- 394.4) - (- 742.2) - 3 (- 137.2) = - 29.4

kJ.

lo g_{10} K = - Δ G^{\circ} / (2.303 RT) = 29400/ (2.303 \times 8.314 \times 298) = 5.15

. The reduction by CO is thermodynamically favourable even at 298 K, though slow.