`Cl_(2)+NaoH to NaCl+NaOCl`

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 \( \text{Cl}_2 + \text{NaOH} \rightarrow \text{NaCl} + \text{NaOCl} \), we will analyze the oxidation states of the elements involved in the reaction.

### Step 1: Identify the oxidation states of the reactants and products.

1. **For \( \text{Cl}_2 \)**: Chlorine in its elemental form has an oxidation state of 0.
2. **For \( \text{NaOH} \)**:
- Sodium (Na) has an oxidation state of +1.
- Oxygen (O) has an oxidation state of -2.
- Hydrogen (H) has an oxidation state of +1.
3. **For \( \text{NaCl} \)**:
- Sodium (Na) has an oxidation state of +1.
- Chlorine (Cl) has an oxidation state of -1.
4. **For \( \text{NaOCl} \)**:
- Sodium (Na) has an oxidation state of +1.
- Oxygen (O) has an oxidation state of -2.
- Let the oxidation state of chlorine (Cl) be \( x \). The compound is neutral, so:
\[ +1 + (-2) + x = 0 \implies x = +1 \]
Thus, chlorine in \( \text{NaOCl} \) has an oxidation state of +1.

### Step 2: Analyze the changes in oxidation states.

- The oxidation state of chlorine in \( \text{Cl}_2 \) changes from 0 to -1 in \( \text{NaCl} \) (reduction).
- The oxidation state of chlorine in \( \text{Cl}_2 \) changes from 0 to +1 in \( \text{NaOCl} \) (oxidation).

### Step 3: Determine the type of reaction.

Since one species (chlorine) undergoes both oxidation (to +1) and reduction (to -1), this reaction is classified as a **disproportionation reaction**. In disproportionation reactions, a single substance is simultaneously oxidized and reduced.

### Conclusion:

The type of reaction represented by \( \text{Cl}_2 + \text{NaOH} \rightarrow \text{NaCl} + \text{NaOCl} \) is a **disproportionation reaction**.

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