Chlorine oxidises `H_2 S` to 

Options

A. `S`
B. `SO_2`
C. `H_2SO_4`
D. `H_2SO_3`

Answer

To solve the question "Chlorine oxidizes H₂S to", we will follow these steps:

### Step 1: Identify the reactants and products
Chlorine (Cl₂) is the oxidizing agent, and hydrogen sulfide (H₂S) is the reducing agent. The reaction involves the oxidation of H₂S.

### Step 2: Determine the oxidation states
In H₂S, sulfur (S) has an oxidation state of -2. When it is oxidized, its oxidation state will increase.

### Step 3: Write the balanced chemical equation
The reaction can be represented as:
\[ \text{Cl}_2 + \text{H}_2\text{S} \rightarrow \text{HCl} + \text{S} \]
In this reaction, chlorine oxidizes H₂S to produce hydrochloric acid (HCl) and elemental sulfur (S).

### Step 4: Identify the products
From the balanced equation, we see that the products of the reaction are hydrochloric acid (HCl) and sulfur (S).

### Step 5: Conclusion
Thus, when chlorine oxidizes H₂S, it produces HCl and leaves behind sulfur.

### Final Answer
Chlorine oxidizes H₂S to form HCl and sulfur.

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