Given below are two statements:

Statement I: The decomposition of hydrogen peroxide to form water and oxygen is an example of a disproportionation reaction.

Statement II: The oxygen of peroxides is in \(-1\) oxidation state and it is converted to zero oxidation state in \(O_2\) and \(-2\) oxidation state in \(H_2O\)

In the light of the above statements, choose the most appropriate answer from the options given below:

Both Statement I and Statement II are correct and Statement II is the correct explanation of Statement I.

The correct answer is option 1. Both Statement I and Statement II are correct and Statement II is the correct explanation of Statement I.

Let us analyze each statement regarding the decomposition of hydrogen peroxide:

Statement I: The decomposition of hydrogen peroxide to form water and oxygen is an example of a disproportionation reaction.

This statement is correct. A disproportionation reaction is a specific type of redox reaction in which a single substance is simultaneously oxidized and reduced, forming two different products. In the decomposition of hydrogen peroxide (\(H_2O_2\)), the reaction is as follows:

\(2H_2O_2 \rightarrow 2H_2O + O_2\)

Here, the oxygen in \(H_2O_2\) has an oxidation state of -1. During the reaction, it is both oxidized to \(O_2\) (where the oxidation state is 0) and reduced to \(H_2O\) (where the oxidation state is -2). This qualifies as a disproportionation reaction.

Statement II: The oxygen of peroxides is in -1 oxidation state and it is converted to zero oxidation state in \(O_2\) and -2 oxidation state in \(H_2O\).

This statement is correct. In hydrogen peroxide (\(H_2O_2\)), the oxidation state of oxygen is -1. When \(H_2O_2\) decomposes, the oxygen atoms are converted to two different oxidation states: 0 in \(O_2\) and -2 in \(H_2O\).

Conclusion:

Both statements are correct:

Statement I is correct because the decomposition of hydrogen peroxide is indeed a disproportionation reaction.

Statement II is correct because it accurately describes the changes in the oxidation states of oxygen during the reaction.

Furthermore, Statement II provides the specific details that explain why the reaction in Statement I is a disproportionation reaction, linking the oxidation states of oxygen in \(H_2O_2\), \(O_2\), and \(H_2O\).

Therefore, the correct answer is:

Option 1: Both Statement I and Statement II are correct and Statement II is the correct explanation of Statement I.

Statement II correctly explains the oxidation state changes that make the reaction described in Statement I a disproportionation reaction.