For oxide formation (per mole of O2, in kJ, T in K): 2M + O2 -> 2MO, Delta G deg=-560+0.20 T; 2C + O2 -> 2CO, Delta G deg=-225-0.175 T. The Delta G deg of MO + C -> M + CO at 1200 K, per mole of MO, is

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For oxide formation (per mole of $O X_{2}$ , in $kJ$ , $T$ in K): $2 M + O X_{2} 2 MO$ , $Δ G^{\circ} = - 560 + 0.20 T$ ; $2 C + O X_{2} 2 CO$ , $Δ G^{\circ} = - 225 - 0.175 T$ . The $Δ G^{\circ}$ of $MO + C M + CO$ at 1200 K, per mole of $MO$ , is

At 1200 K,

Δ G_{CO} = - 225 - 210 = - 435

and

Δ G_{MO} = - 560 + 240 = - 320 kJ

. The coupled reaction for 2 mol

MO

- 435 - (- 320) = - 115

kJ, so per mole of

MO

it is

- 57.5 kJ

. Negative, so carbon reduces the oxide at 1200 K.