`H_(2)O_(2)rarr H_(2)O+O_(2)`
This represents

Options

A. Oxidetion of `H_(2)O_(2)`
B. Reducton of `H_(2)O_(2)`
C. Disproportionation of oxygen
D. Acidic nature of `H_(2)O_(2)`

Answer

To analyze the reaction \( H_2O_2 \rightarrow H_2O + O_2 \) and determine what it represents, we can follow these steps:

### Step 1: Identify the Reaction Type
The given reaction shows the decomposition of hydrogen peroxide (\( H_2O_2 \)) into water (\( H_2O \)) and oxygen gas (\( O_2 \)).

**Hint:** Look for the products formed from a single reactant to identify if it is a decomposition reaction.

### Step 2: Determine the Oxidation States
Next, we need to find the oxidation states of oxygen in the different species involved:
- 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.

**Hint:** Remember that oxidation states can change during a reaction, indicating oxidation or reduction.

### Step 3: Analyze the Changes in Oxidation States
From the oxidation states determined:
- The oxygen in \( H_2O_2 \) changes from -1 to -2 in \( H_2O \) (reduction).
- The oxygen in \( H_2O_2 \) changes from -1 to 0 in \( O_2 \) (oxidation).

**Hint:** A decrease in oxidation state indicates reduction, while an increase indicates oxidation.

### Step 4: Identify the Disproportionation Reaction
Since the same element (oxygen) is undergoing both oxidation and reduction (changing to two different oxidation states), this reaction is classified as a disproportionation reaction.

**Hint:** Disproportionation occurs when a single substance is both oxidized and reduced, leading to the formation of two different products.

### Step 5: Conclusion
Based on the analysis, the reaction \( H_2O_2 \rightarrow H_2O + O_2 \) represents a disproportionation reaction of hydrogen peroxide.

**Final Answer:** The reaction represents the disproportionation of oxygen.