`I_(2)+KIrarrKI_(3)`
In the above reaction :-

Options

A. Only oxidation taken place
B. Only reduction takes place
C. Both the above
D. None of the above

Answer

To analyze the reaction \( I_2 + KI \rightarrow KI_3 \) and determine whether it involves oxidation, reduction, or both, we can follow these steps:

### Step 1: Write the Reaction
The reaction is given as:
\[ I_2 + KI \rightarrow KI_3 \]

### Step 2: Assign Oxidation States
- In \( I_2 \), the oxidation state of iodine (I) is 0 because it is in its elemental form.
- In potassium iodide (KI), potassium (K) has an oxidation state of +1 and iodine (I) has an oxidation state of -1.
- In potassium triiodide (KI_3), we need to calculate the oxidation state of iodine in this compound.

### Step 3: Calculate the Oxidation State of Iodine in KI_3
The formula for KI_3 consists of one potassium ion (K) and three iodine ions (I). The overall charge of the compound is neutral (0).

Let the oxidation state of iodine in KI_3 be \( x \):
\[ 1 \cdot (+1) + 3 \cdot x = 0 \]
This simplifies to:
\[ 1 + 3x = 0 \]
\[ 3x = -1 \quad \Rightarrow \quad x = -\frac{1}{3} \]

### Step 4: Compare Oxidation States
- The oxidation state of iodine changes from 0 in \( I_2 \) to -\(\frac{1}{3}\) in \( KI_3 \).
- The oxidation state of iodine in \( KI \) is -1.

### Step 5: Identify Oxidation and Reduction
- The change from 0 to -\(\frac{1}{3}\) indicates a reduction (gain of electrons).
- The change from -1 to -\(\frac{1}{3}\) indicates an increase in oxidation state, which is oxidation (loss of electrons).

### Conclusion
Since both oxidation and reduction processes are occurring in this reaction, we conclude that both are happening.

### Final Answer
Both oxidation and reduction are occurring in the reaction \( I_2 + KI \rightarrow KI_3 \).