Given below are two statements:
Statement I: \( \text{S}_8 \) solid undergoes disproportionation reaction under alkaline conditions to form \( \text{S}^{2-} \) and \( \text{S}_2\text{O}_3^{2-} \).
Statement II: \( \text{ClO}_4^- \) can undergo disproportionation reaction under acidic condition.
In the light of the above statements, choose the most appropriate answer from the options given below:
Statement I: \( \text{S}_8 \) solid undergoes disproportionation reaction under alkaline conditions to form \( \text{S}^{2-} \) and \( \text{S}_2\text{O}_3^{2-} \).
Statement II: \( \text{ClO}_4^- \) can undergo disproportionation reaction under acidic condition.
In the light of the above statements, choose the most appropriate answer from the options given below:
- Statement I is correct but statement II is incorrect.
- Statement I is incorrect but statement II is correct
- Both statement I and statement II are incorrect
- Both statement I and statement II are correct
The Correct Option is A
Approach Solution - 1
To evaluate the given statements and determine which is correct, let's analyze each statement based on known chemical reactions and principles.
- Statement I: \(S_8\) solid undergoes disproportionation reaction under alkaline conditions to form \(S^{2-}\) and \(S_2O_3^{2-}\).
- Disproportionation is a specific type of redox (reduction-oxidation) reaction in which a single substance is simultaneously reduced and oxidized to form two different products.
- In alkaline conditions, elemental sulfur \((S_8)\) can actually disproportionate. The reaction is:
\(3S_8 + 6OH^- \rightarrow 2S_2O_3^{2-} + 4S^{2-} + 3H_2O\)
- This confirms that under alkaline conditions, sulfur can indeed form \(S^{2-}\) (sulfide) and \(S_2O_3^{2-}\) (thiosulfate).
- Statement II: \(ClO_4^-\\) can undergo disproportionation reaction under acidic conditions.
- Perchlorate ion \((ClO_4^-)\) is known for being very stable, especially under acidic conditions. It is already in its highest oxidation state, where chlorine is +7.
- Generally, in a disproportionation reaction, a substance must be capable of existing in a higher as well as a lower oxidation state. However, chlorine in \(ClO_4^-\) cannot oxidize further (higher than +7 is unfeasible under normal conditions).
- Therefore, no disproportionation reaction of \(ClO_4^-\) occurs under acidic conditions, confirming that Statement II is incorrect.
Based on the analysis above:
- Statement I is correct as sulfur in \(S_8\) can undergo disproportionation to form \(S^{2-}\) and \(S_2O_3^{2-}\) under alkaline conditions.
- Statement II is incorrect as \(ClO_4^-\\) does not undergo disproportionation under acidic conditions.
Therefore, the correct answer is: Statement I is correct but statement II is incorrect.
Approach Solution -2
To determine which of the given statements are correct, let's analyze each statement individually and understand the chemical processes involved.
Statement I: \( \text{S}_8 \) solid undergoes disproportionation reaction under alkaline conditions to form \( \text{S}^{2-} \) and \( \text{S}_2\text{O}_3^{2-} \).
Disproportionation reactions involve a substance being simultaneously oxidized and reduced. The reaction for sulfur in \( \text{S}_8 \) under alkaline conditions can be represented as follows:
\[ \text{3S}_8 + \text{12OH}^- \rightarrow \text{4S}_2\text{O}_3^{2-} + \text{2S}^{2-} + \text{6H}_2\text{O} \]
In this reaction:
- Sulfur is reduced from \( \text{S}_8 \) (0 oxidation state) to \( \text{S}^{2-} \) (-2 oxidation state).
- Sulfur is also oxidized from \( \text{S}_8 \) (0 oxidation state) to \( \text{S}_2\text{O}_3^{2-} \) (+2.5 oxidation state).
This confirms that \( \text{S}_8 \) undergoes a disproportionation reaction under alkaline conditions. Hence, Statement I is correct.
Statement II: \( \text{ClO}_4^- \) can undergo disproportionation reaction under acidic condition.
\( \text{ClO}_4^- \), or perchlorate ion, is already in its highest oxidation state (+7 for chlorine). In a disproportionation reaction, an element must be able to undergo both oxidation and reduction. Since chlorine in \( \text{ClO}_4^- \) is in its highest oxidation state, it cannot be oxidized further; hence, it cannot participate in a disproportionation reaction under normal conditions, regardless of the acidity of the medium.
Therefore, Statement II is incorrect.
Conclusion:
Based on the analysis:
- Statement I is correct because \( \text{S}_8 \) indeed undergoes disproportionation under alkaline conditions to form \( \text{S}^{2-} \) and \( \text{S}_2\text{O}_3^{2-} \).
- Statement II is incorrect as \( \text{ClO}_4^- \) cannot undergo disproportionation under any condition.
Thus, the correct answer is: Statement I is correct but statement II is incorrect.
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