In the reaction of `Cl_2` with `Na_2 SO_3`, chlorine acts as

Options

A. Reductant
B. Oxidant
C. Both oxidant and reductant
D. Neither oxidant nor reductnat

Answer

To determine how chlorine acts in the reaction with sodium sulfite (Na₂SO₃), we need to analyze the chemical reaction and the changes in oxidation states. Here’s a step-by-step solution:

### Step 1: Write the Reaction
The reaction between chlorine (Cl₂) and sodium sulfite (Na₂SO₃) can be represented as follows:
\[ \text{Na}_2\text{SO}_3 + 4\text{Cl}_2 + 5\text{H}_2\text{O} \rightarrow 2\text{NaHSO}_4 + 8\text{HCl} \]

### Step 2: Identify Oxidation States
In this reaction, we need to identify the oxidation states of chlorine in its elemental form (Cl₂) and in hydrochloric acid (HCl):
- In Cl₂, the oxidation state of chlorine is 0 (elemental state).
- In HCl, the oxidation state of chlorine is -1.

### Step 3: Determine the Change in Oxidation State
The change in oxidation state for chlorine can be summarized as follows:
- Chlorine goes from an oxidation state of 0 in Cl₂ to -1 in HCl.
- This indicates a decrease in the oxidation state.

### Step 4: Define Reduction and Oxidation
According to the principles of oxidation and reduction:
- A decrease in oxidation state indicates reduction.
- The species that undergoes reduction is considered an oxidizing agent (oxidant).

### Step 5: Conclusion
Since chlorine is reduced from an oxidation state of 0 to -1, it acts as an oxidizing agent (oxidant) in this reaction. Therefore, the correct answer to the question is that chlorine acts as an oxidant.

### Final Answer
Chlorine acts as an oxidant in the reaction with sodium sulfite (Na₂SO₃).

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