`H_(2)O_(2) overset(R.T.) to H_(2)O+(1)/(2)O_(2)`

Options

A. For disproportionation reaction.
B. For comproportionation reaction.
C. For either intermolecular redox reaction or displacement reaction
D. For either thermal combination redox reaction or thermal decomposition redox reaction.

Answer

To determine the type of reaction represented by the equation \( H_2O_2 \overset{R.T.}{\rightarrow} H_2O + \frac{1}{2}O_2 \), we can analyze the changes in oxidation states of the elements involved. Here’s a step-by-step breakdown of the solution:

### Step 1: Identify the Reactants and Products
The reactant is hydrogen peroxide (\( H_2O_2 \)), and the products are water (\( H_2O \)) and oxygen gas (\( O_2 \)).

### Step 2: Determine Oxidation States
- In \( H_2O_2 \):
- Hydrogen (H) has an oxidation state of +1.
- Oxygen (O) has an oxidation state of -1.

- In \( H_2O \):
- Hydrogen (H) remains +1.
- Oxygen (O) has an oxidation state of -2.

- In \( O_2 \):
- Oxygen (O) has an oxidation state of 0 (as it is in its elemental form).

### Step 3: Analyze Changes in Oxidation States
- For oxygen in \( H_2O_2 \) to \( H_2O \):
- The oxidation state changes from -1 to -2 (reduction).

- For oxygen in \( H_2O_2 \) to \( O_2 \):
- The oxidation state changes from -1 to 0 (oxidation).

### Step 4: Classify the Reaction
Since one species (oxygen in \( H_2O_2 \)) is undergoing both oxidation (increase in oxidation state) and reduction (decrease in oxidation state), this reaction is classified as a **disproportionation reaction**.

### Step 5: Identify Other Characteristics
Additionally, since \( H_2O_2 \) decomposes to form two different products (\( H_2O \) and \( O_2 \)), it can also be classified as a **decomposition reaction**.

### Conclusion
Thus, the reaction \( H_2O_2 \rightarrow H_2O + \frac{1}{2}O_2 \) is both a **disproportionation reaction** and a **decomposition reaction**.

---