State True or false
Molten `Na_(2)SO_(4)` is a good conductor because of mobile electrons.

Answer

To determine whether the statement "Molten Na₂SO₄ is a good conductor because of mobile electrons" is true or false, we can analyze the properties of molten sodium sulfate and the reasons behind its conductivity.

### Step-by-Step Solution:

1. **Understanding the Composition of Na₂SO₄**:
- Sodium sulfate (Na₂SO₄) is composed of sodium ions (Na⁺) and sulfate ions (SO₄²⁻).

2. **State of Na₂SO₄**:
- In its solid state, Na₂SO₄ does not conduct electricity well because the ions are fixed in place within the crystal lattice and cannot move freely.

3. **Melting of Na₂SO₄**:
- When Na₂SO₄ is heated to its melting point, it transitions into a molten state. In this state, the ionic bonds are broken, allowing the ions to move freely.

4. **Conductivity in the Molten State**:
- The mobility of these ions in the molten state allows Na₂SO₄ to conduct electricity effectively. The presence of free-moving ions is what enables the conduction of electric current, not mobile electrons.

5. **Analyzing the Statement**:
- The statement claims that molten Na₂SO₄ is a good conductor because of mobile electrons. However, in ionic compounds like Na₂SO₄, it is the movement of ions (Na⁺ and SO₄²⁻) that facilitates conduction, not electrons.

6. **Conclusion**:
- Therefore, the statement is **False**. The correct reason for the conductivity of molten Na₂SO₄ is due to the mobility of ions, not mobile electrons.

### Final Answer:
**False**