Given below are two statements :
Statement I : According to the Ellingham diagram, any metal oxide with higher $$\Delta G°$$ is more stable than the one with lower $$\Delta G°$$.
Statement II : The metal involved in the formation of oxide placed lower in the Ellingham diagram can reduce the oxide of a metal placed higher in the diagram.
In the light of the above statements, choose the most appropriate answer from the options given below

We need to evaluate two statements about the Ellingham diagram.

Evaluate Statement I.

Statement I: According to the Ellingham diagram, any metal oxide with higher $$\Delta G°$$ is more stable than the one with lower $$\Delta G°$$.

This is incorrect. In the Ellingham diagram, $$\Delta G°$$ values are plotted (which are negative for spontaneous oxide formation). A more negative (i.e., lower) $$\Delta G°$$ indicates a more thermodynamically stable oxide. So the oxide with lower $$\Delta G°$$ (more negative) is more stable, not the one with higher $$\Delta G°$$.

Evaluate Statement II.

Statement II: The metal involved in the formation of oxide placed lower in the Ellingham diagram can reduce the oxide of a metal placed higher in the diagram.

This is correct. In the Ellingham diagram, the oxide placed lower has a more negative $$\Delta G°$$, meaning its metal has a greater affinity for oxygen. Therefore, a metal whose oxide line lies lower in the diagram can reduce the oxide of a metal whose line lies higher (less negative $$\Delta G°$$). For example, aluminium (lower in the diagram) can reduce iron oxide (higher in the diagram) — this is the thermite reaction.

Conclusion.

Statement I is incorrect and Statement II is correct.

The correct answer is Option D: Statement I is incorrect but Statement II is correct.