STATEMENT-1: when 2 faraday of charge is passed through 0.1 M `H_2SO_4` (aq) ,11.2 litre `O_2` evolved at STP.
STATEMENT-2: Molecular mass of oxygen is 32

Options

A. If both the statements are TRUE and STATEMENTS-2 is the correct explantion of STATEMENTS-1
B. If both the statements are TRUE but STATEMENTS-2 is NOT the correct explanation of STATEMENTS-2
C. If STATEMENTS-1 is TRUE and STATEMENTS-2 is FALSE
D. If STATEMENT-1 is FALSE and STATEMENT-2 is TRUE

Answer

To solve the question, we need to analyze both statements provided and verify their correctness step by step.

### Step 1: Analyze Statement 1
**Statement 1:** When 2 Faraday of charge is passed through 0.1 M H₂SO₄ (aq), 11.2 liters of O₂ is evolved at STP.

1. **Understanding Faraday's Law:** According to Faraday's first law of electrolysis, the amount of substance liberated or deposited at an electrode is directly proportional to the quantity of electricity passed through the electrolyte.

2. **Electrolysis of H₂SO₄:** In the electrolysis of dilute sulfuric acid, water is also involved. The reactions at the electrodes are:
- At the anode (oxidation): 4OH⁻ → 2H₂O + O₂ + 4e⁻
- At the cathode (reduction): 2H⁺ + 2e⁻ → H₂

3. **Moles of O₂ Produced:**
- From the reaction at the anode, 4 moles of electrons produce 1 mole of O₂.
- 2 Faraday corresponds to 2 moles of electrons (since 1 Faraday = 1 mole of electrons).
- Therefore, 2 moles of electrons will produce 0.5 moles of O₂.

4. **Volume of O₂ at STP:**
- At STP, 1 mole of any gas occupies 22.4 liters.
- Thus, 0.5 moles of O₂ will occupy:
\[ 0.5 \text{ moles} \times 22.4 \text{ L/mole} = 11.2 \text{ L} \]

5. **Conclusion for Statement 1:** The statement is correct because passing 2 Faraday of charge through 0.1 M H₂SO₄ does indeed evolve 11.2 liters of O₂ at STP.

### Step 2: Analyze Statement 2
**Statement 2:** The molecular mass of oxygen is 32.

1. **Molecular Mass Calculation:**
- The atomic mass of oxygen (O) is approximately 16 g/mol.
- Since O₂ consists of two oxygen atoms, the molecular mass of O₂ is:
\[ 2 \times 16 \text{ g/mol} = 32 \text{ g/mol} \]

2. **Conclusion for Statement 2:** This statement is also correct.

### Step 3: Determine Relationship Between Statements
- Both statements are true.
- However, Statement 2 does not explain Statement 1. Statement 1 is about the electrolysis process and the volume of gas produced, while Statement 2 merely states the molecular mass of oxygen.

### Final Conclusion
Both statements are true, but Statement 2 is not the correct explanation for Statement 1.

### Answer:
Both statements are true, but Statement 2 is not the correct explanation for Statement 1.