The oxidation state of oxygen of `H_(2)O_(2)` in the final products when it reacts with `ClO_(3)^(ɵ)` is

Options

A. 0
B. 1
C. `-1`
D. `-2`

Explanation

To determine the oxidation state of oxygen in \( H_2O_2 \) when it reacts with \( ClO_3^- \), we can follow these steps:

### Step 1: Identify the Reactants and Products
The reactants are hydrogen peroxide (\( H_2O_2 \)) and chlorate ion (\( ClO_3^- \)). The products of this reaction can vary based on the conditions (acidic, basic, etc.), but typically, \( H_2O_2 \) can be oxidized, and \( ClO_3^- \) can be reduced.

### Step 2: Determine Possible Products
In this reaction, \( H_2O_2 \) can react with \( ClO_3^- \) to produce either chlorine gas (\( Cl_2 \)) or chloride ion (\( Cl^- \)), along with oxygen gas (\( O_2 \)).

### Step 3: Analyze the Final Products
The final products include \( O_2 \). We need to find the oxidation state of oxygen in this product.

### Step 4: Determine the Oxidation State of Oxygen in \( O_2 \)
In elemental form, the oxidation state of any element is always zero. Therefore, in molecular oxygen (\( O_2 \)), the oxidation state of oxygen is 0.

### Conclusion
Thus, the oxidation state of oxygen from \( H_2O_2 \) in the final product when it reacts with \( ClO_3^- \) is **0**.

### Final Answer
The oxidation state of oxygen in the final products is **0**.

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