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 state of oxygen, follow these steps:

### Step 1: Identify the oxidation states of oxygen in the reactants and products.
- In hydrogen peroxide (\(H_2O_2\)), the oxidation state of oxygen is \(-1\).
- In water (\(H_2O\)), the oxidation state of oxygen is \(-2\).
- In molecular oxygen (\(O_2\)), the oxidation state of oxygen is \(0\).

### Step 2: Write down the oxidation states.
- For \(H_2O_2\):
- Each oxygen: \(-1\)
- For \(H_2O\):
- Each oxygen: \(-2\)
- For \(O_2\):
- Each oxygen: \(0\)

### Step 3: Analyze the changes in oxidation states.
- In the reaction, oxygen in \(H_2O_2\) changes from \(-1\) to \(-2\) in \(H_2O\) (reduction).
- Simultaneously, oxygen changes from \(-1\) in \(H_2O_2\) to \(0\) in \(O_2\) (oxidation).

### Step 4: Determine if oxygen is oxidized or reduced.
- The oxygen that goes from \(-1\) to \(0\) is oxidized (loss of electrons).
- The oxygen that goes from \(-1\) to \(-2\) is reduced (gain of electrons).

### Conclusion:
Since oxygen is both oxidized and reduced in this reaction, the correct answer is that oxygen is both oxidized and reduced.

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