The reaction, `2K_(2)MnO_(4) + Cl_(2) rarr 2KMnO_(4) + 2KCl` is an example of -

Options

A. Oxidation
B. Reduction
C. Redox
D. Chlorination

Answer

To determine the type of reaction represented by the equation `2K2MnO4 + Cl2 → 2KMnO4 + 2KCl`, we will analyze the oxidation states of the elements involved in the reaction.

### Step-by-Step Solution:

1. **Identify the Reactants and Products**:
- Reactants: `2K2MnO4` and `Cl2`
- Products: `2KMnO4` and `2KCl`

2. **Assign Oxidation States**:
- For `K2MnO4`:
- Potassium (K) has an oxidation state of +1.
- Oxygen (O) has an oxidation state of -2.
- Let the oxidation state of Manganese (Mn) be X.
- The equation for the oxidation state becomes:
\[ 2(+1) + X + 4(-2) = 0 \implies 2 + X - 8 = 0 \implies X = +6 \]
- Thus, Mn in `K2MnO4` is in the +6 oxidation state.

- For `Cl2`:
- Chlorine (Cl) in its elemental form has an oxidation state of 0.

- For `KMnO4`:
- Again, K is +1, O is -2, and let the oxidation state of Mn be Y.
- The equation becomes:
\[ +1 + Y + 4(-2) = 0 \implies 1 + Y - 8 = 0 \implies Y = +7 \]
- Thus, Mn in `KMnO4` is in the +7 oxidation state.

- For `KCl`:
- K is +1 and Cl is -1.

3. **Determine Changes in Oxidation States**:
- Manganese changes from +6 (in `K2MnO4`) to +7 (in `KMnO4`):
- This is an **oxidation** (increase in oxidation state).
- Chlorine changes from 0 (in `Cl2`) to -1 (in `KCl`):
- This is a **reduction** (decrease in oxidation state).

4. **Conclusion**:
- Since both oxidation and reduction are occurring in this reaction, it is classified as a **redox reaction**.

### Final Answer:
The reaction `2K2MnO4 + Cl2 → 2KMnO4 + 2KCl` is an example of a **redox reaction**.