Question:
Two statements are given below.
Statement I: The reaction Cr$_2$O$_3$ + 2Al → 2Cr + Al$_2$O$_3$ (ΔG° = -421 kJ) is thermodynamically feasible.
Statement II: The above reaction occurs at room temperature.
The correct answer is
Two statements are given below.
Statement I: The reaction Cr$_2$O$_3$ + 2Al → 2Cr + Al$_2$O$_3$ (ΔG° = -421 kJ) is thermodynamically feasible.
Statement II: The above reaction occurs at room temperature.
The correct answer is
Statement I: The reaction Cr$_2$O$_3$ + 2Al → 2Cr + Al$_2$O$_3$ (ΔG° = -421 kJ) is thermodynamically feasible.
Statement II: The above reaction occurs at room temperature.
The correct answer is
Show Hint
For reactions with a negative Gibbs free energy (ΔG°), the reaction is thermodynamically feasible. However, the reaction may still require high temperatures or activation energy to occur.
Updated On: Mar 24, 2025
- Both the statements I \& II are correct.
- Both the statements I \& II are not correct.
- Statement I is correct, but statement II is not correct.
- Statement I is not correct, but statement II is correct.
Show Solution
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The Correct Option is C
Solution and Explanation
Aluminothermic Reaction Analysis
- Statement I: The reaction \( \text{Cr}_2\text{O}_3 + 2\text{Al} \rightarrow 2\text{Cr} + \text{Al}_2\text{O}_3 \) is thermodynamically feasible as the Gibbs free energy change \( (\text{G}^\circ = -421 \text{ kJ}) \) is negative, indicating that the reaction is spontaneous. Therefore, Statement I is correct.
- Statement II: The reaction does not occur at room temperature because it is an aluminothermic reaction, which requires high temperatures to overcome the activation energy barrier. Therefore, Statement II is incorrect.
Conclusion:
Hence, the correct answer is that Statement I is correct, but Statement II is not correct.
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