Statement-1: Bond energy of Hl is smaller than that of HBr.
Statement-2: HBr is stronger acid than Hl.

Options

A. Statement-1 is true, statement-2 is true, statement-2 is a correct explanation for statement-1
B. Statement-1 is true, statement-2 is true, statement-2 is not correct explanation for statement-1
C. Statement-1 is true, statement-2 is false
D. Statement-1 is false, statement-2 is true

Answer

To analyze the given statements, we need to evaluate each statement based on our understanding of bond energies and acid strengths.

### Step 1: Evaluate Statement 1
**Statement 1:** The bond energy of HI is smaller than that of HBr.

- **Explanation:**
- Bond energy is the energy required to break a bond between two atoms.
- As we move down the group in the periodic table (from Br to I), the size of the atoms increases.
- A larger atomic size leads to a longer bond length, which results in a weaker bond.
- Therefore, the bond energy of HI (which has a longer bond length due to the larger iodine atom) will indeed be smaller than that of HBr.

**Conclusion:** Statement 1 is **True**.

### Step 2: Evaluate Statement 2
**Statement 2:** HBr is a stronger acid than HI.

- **Explanation:**
- An acid is defined as a substance that can donate a proton (H⁺).
- The strength of an acid is often related to how easily it can release H⁺ ions.
- Since the bond energy of HI is lower than that of HBr, it means that HI can break apart more easily and release H⁺ ions with less energy input.
- Thus, HI is actually a stronger acid than HBr because it dissociates more readily.

**Conclusion:** Statement 2 is **False**.

### Final Conclusion
- Statement 1 is **True**: The bond energy of HI is smaller than that of HBr.
- Statement 2 is **False**: HBr is not a stronger acid than HI; HI is the stronger acid.