At temperatures above $1073 \ K$,coke can be used to reduce $FeO$ to $Fe$. How can you justify this reduction with an Ellingham diagram?

(N/A) In an Ellingham diagram,the line representing the oxidation of carbon to carbon monoxide $(2C + O_2 \rightarrow 2CO)$ slopes downwards,while the line for the oxidation of iron to iron$(II)$ oxide $(2Fe + O_2 \rightarrow 2FeO)$ slopes upwards.
At temperatures above $1073 \ K$,the Gibbs free energy of formation for $CO$ becomes more negative than that for $FeO$,i.e.,$\Delta_{f} G^{\ominus}_{(C, CO)} < \Delta_{f} G^{\ominus}_{(Fe, FeO)}$.
Since the reduction of $FeO$ by $C$ $(2FeO + 2C \rightarrow 2Fe + 2CO)$ is the sum of the two reactions,the overall $\Delta G^{\ominus}$ becomes negative,making the reduction thermodynamically feasible.