`Na_(2)S_(3)+2Ooverset(Delta)to Na_(2)SO_(4)+2S`.

Explanation

To analyze the reaction given in the question, we need to break down the process step by step.

### Step-by-Step Solution:

1. **Identify the Reactants and Products**:
The reactants in the reaction are sodium trisulfide (Na₂S₃) and oxygen (O₂). The products mentioned are sodium sulfate (Na₂SO₄) and sulfur (S).

2. **Write the Balanced Chemical Equation**:
The reaction can be represented as:
\[ \text{Na}_2\text{S}_3 + 2\text{O}_2 \rightarrow \text{Na}_2\text{SO}_4 + 2\text{S} \]

3. **Analyze the Reaction**:
- Sodium trisulfide (Na₂S₃) contains sulfur in a -2 oxidation state.
- When Na₂S₃ reacts with oxygen, sulfur is oxidized to a higher oxidation state (in Na₂SO₄, sulfur is in the +6 oxidation state).
- The reaction suggests that sulfur is being oxidized to form sodium sulfate while elemental sulfur is also produced.

4. **Check for Accuracy**:
The products listed in the question include sodium sulfate and sulfur. However, when sodium trisulfide reacts with oxygen, it typically produces sodium sulfate and sulfur dioxide (SO₂) rather than elemental sulfur.

5. **Conclusion**:
Since the products listed in the question do not accurately reflect the expected products of the reaction, we conclude that the statement is **False**.

### Final Answer:
The statement given in the question is **False**.

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