(A): Conc.`H_(2)SO_(4)` reacts with KCl to give `Cl_(2)` gas
(R): HCI cannot be oxidised by conc.`H_(2)SO_(4)` 

Options

A. Both A & R are true, R is the correct explanation of A
B. Both A & R are true, R is not correct explanation of A
C. A is true, R is false
D. A is false, R is true

Answer

To solve the assertion and reason question, we will analyze both parts step by step.

### Step 1: Analyze the Assertion
The assertion states that concentrated H₂SO₄ reacts with KCl to give Cl₂ gas.

1. **Reaction of H₂SO₄ with KCl**:
- When concentrated sulfuric acid (H₂SO₄) is added to potassium chloride (KCl), the reaction can be represented as:
\[ 2 \text{KCl} + \text{H}_2\text{SO}_4 \rightarrow \text{K}_2\text{SO}_4 + 2 \text{HCl} \]
- This reaction produces potassium sulfate (K₂SO₄) and hydrochloric acid (HCl).

2. **Oxidation of HCl**:
- HCl is a mild reducing agent. In the presence of concentrated H₂SO₄, it can potentially be oxidized to chlorine gas (Cl₂):
\[ 2 \text{HCl} + \text{H}_2\text{SO}_4 \rightarrow \text{Cl}_2 + \text{H}_2\text{O} + \text{SO}_2 \]
- However, the assertion claims that Cl₂ gas is produced directly from the reaction with KCl, which is misleading because Cl₂ is not produced in the initial reaction with KCl.

### Conclusion for Assertion:
The assertion is **false** because while H₂SO₄ can react with KCl, it does not directly produce Cl₂ gas.

### Step 2: Analyze the Reason
The reason states that HCl cannot be oxidized by concentrated H₂SO₄.

1. **Understanding HCl's Reducing Properties**:
- HCl is indeed a mild reducing agent, and concentrated H₂SO₄ is a strong oxidizing agent. However, in the context of the reaction, HCl does not get oxidized to Cl₂ when it is produced from the reaction with KCl and H₂SO₄.

2. **Conclusion for Reason**:
- The reason is **true** because HCl cannot be oxidized by concentrated H₂SO₄ to produce Cl₂ gas under these conditions.

### Final Conclusion:
- The assertion (A) is **false**.
- The reason (R) is **true**.

### Answer:
A is false, R is true.

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