TG EAMCET 3 May 2025 Shift 2 Paper

Statement I Analysis:
Ellingham diagrams plot the standard Gibbs free energy change (∆G⊖) for the formation of various metal oxides as a function of temperature. The principle driving the choice of reducing agent is based on the relative thermodynamic stability of the oxides. A metal can reduce the oxide of another metal if the ∆G⊖ for the formation of its own oxide is more negative (i.e., its line is lower on the diagram) than the ∆G⊖ for the formation of the oxide to be reduced, at a given temperature. This means that the overall reduction reaction will have a negative ∆G⊖, making it thermodynamically feasible. Therefore, Ellingham diagrams are indeed used to predict the choice of reducing agent.
Statement I is correct.
Statement II Analysis:
The thermodynamic stability of a compound is inversely related to its standard Gibbs free energy of formation ( ∆G⊖ ). A more negative (lower) value of ∆G⊖ for the formation of a compound indicates greater thermodynamic stability of that compound. Conversely, a higher (less negative or more positive) value of ∆G⊖ indicates lower stability. Therefore, a metal oxide with a higher ∆G⊖ is less stable than an oxide with a lower ∆G⊖.
Statement II is incorrect.
Based on the analysis:
Statement I is correct.
Statement II is not correct.
This corresponds to Option B.