TG EAMCET 3 May 2025 Shift 2 Paper

Statement I Analysis:Ellingham diagrams plot the standard Gibbs free energy change $(\Delta G^{\ominus})$ 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 $\Delta G^{\ominus}$ for the formation of its own oxide is more negative (i.e., its line is lower on the diagram) than the $\Delta G^{\ominus}$ for the formation of the oxide to be reduced, at a given temperature. This means that the overall reduction reaction will have a negative $\Delta G^{\ominus}$, 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 ( $\Delta G^{\ominus}$ ). A more negative (lower) value of $\Delta G^{\ominus}$ for the formation of a compound indicates greater thermodynamic stability of that compound. Conversely, a higher (less negative or more positive) value of $\Delta G^{\ominus}$ indicates lower stability. Therefore, a metal oxide with a higher $\Delta G^{\ominus}$ is less stable than an oxide with a lower $\Delta G^{\ominus}$.Statement II is incorrect.Based on the analysis:Statement I is correct.Statement II is not correct.This corresponds to Option B.