In the reaction
`2H_(2)O_(2) rarr 2H_(2)O+O_(2)`

Options

A. Oxygen is oxidised only
B. Oxygen is reduced only
C. Oxygen is neither oxidised nor reduced
D. Oxygen is both oxidised and reduced

Answer

To analyze the reaction \( 2H_2O_2 \rightarrow 2H_2O + O_2 \) and determine the oxidation states of the elements involved, we can follow these steps:

### Step 1: Identify the Reactants and Products
The reaction involves hydrogen peroxide (\( H_2O_2 \)), water (\( H_2O \)), and oxygen (\( O_2 \)).

### Step 2: Assign Oxidation States
- **For \( H_2O_2 \)**:
- Hydrogen (H) has an oxidation state of +1.
- Oxygen (O) in peroxides has an oxidation state of -1.
- Therefore, the oxidation state of \( H_2O_2 \) is:
\[ 2(+1) + 2(-1) = 0 \]

- **For \( H_2O \)**:
- Hydrogen (H) has an oxidation state of +1.
- Oxygen (O) has an oxidation state of -2.
- Therefore, the oxidation state of \( H_2O \) is:
\[ 2(+1) + (-2) = 0 \]

- **For \( O_2 \)**:
- Oxygen (O) in its elemental form has an oxidation state of 0.

### Step 3: Determine Changes in Oxidation States
- In the reaction, the oxidation states of oxygen change as follows:
- From \( H_2O_2 \) (O = -1) to \( H_2O \) (O = -2) — this is a reduction (gain of electrons).
- From \( H_2O_2 \) (O = -1) to \( O_2 \) (O = 0) — this is an oxidation (loss of electrons).

### Step 4: Identify the Type of Reaction
Since the same element (oxygen) is undergoing both oxidation and reduction, this reaction is classified as a **disproportionation reaction**.

### Step 5: Conclusion
Based on the analysis:
- Oxygen is both oxidized and reduced in this reaction.

Thus, the correct statement is:
**Oxygen is oxidized and reduced.**

### Final Answer
The correct option is that oxygen is oxidized and reduced.

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