STATEMENT 1: Electroysis of molten `PbBr` using plantinum electrodes produces `Br_(2) at anode and
STATEMENT 2: `Br_(2)` is obtained in gaseous state at room temperature

Options

A. Statement 1 is ture , Statement 2 is true Statement 2 is correct explanation for Statement 2
B. Statement 1 is true Statement 2 is ture Statement 2 is NOT a correct explantion for Statement 2
C. Statement 1 is true statement 2 is ture
D. Statement 1 is false Statement 2 is true

Answer

To solve the question, we need to analyze both statements regarding the electrolysis of molten lead(II) bromide (PbBr2) and the state of bromine (Br2) at room temperature.

### Step-by-Step Solution:

1. **Understanding Electrolysis of PbBr2**:
- When molten PbBr2 is subjected to electrolysis, it dissociates into its ions: Pb²⁺ and Br⁻.
- The electrolysis process involves two electrodes: the anode (positive electrode) and the cathode (negative electrode).

2. **Reactions at the Electrodes**:
- **At the Cathode**: Reduction occurs. The Pb²⁺ ions gain electrons to form lead (Pb).
\[ \text{Pb}^{2+} + 2e^- \rightarrow \text{Pb (s)} \]
- **At the Anode**: Oxidation occurs. The Br⁻ ions lose electrons to form bromine (Br2).
\[ 2\text{Br}^- \rightarrow \text{Br}_2 (g) + 2e^- \]

3. **Analyzing Statement 1**:
- Statement 1 claims that electrolysis of molten PbBr2 using platinum electrodes produces Br2 at the anode.
- This statement is **true** because bromine gas (Br2) is indeed produced at the anode during the electrolysis of PbBr2.

4. **Analyzing Statement 2**:
- Statement 2 claims that Br2 is obtained in the gaseous state at room temperature.
- This statement is **false** because at room temperature, bromine exists as a liquid (Br2) and not as a gas. While Br2 can exist as a gas at higher temperatures, it is a liquid at standard room temperature (around 25°C).

5. **Conclusion**:
- Therefore, Statement 1 is true, and Statement 2 is false.

### Final Answer:
- Statement 1 is true, and Statement 2 is false.