Which equation of statements is/are correct?

Options

A. `SO_(3)^(2-) + Sto S_2O_(3)^(2-)`
B. `S_(2)O_(3)^(2-)+ 2H to H_2SO_(3)+ S`
C. S has different oxidation states in `S_2O_(3)^(2-)`
D. All of the above

Answer

To determine which equations of statements are correct, we will analyze the reactions involving sulfur and its various oxidation states step by step.

### Step-by-Step Solution:

1. **Analyzing the First Reaction**:
- The first reaction involves the conversion of sulfide (S²⁻) into thiosulfate (S₂O₃²⁻) when it reacts with elemental sulfur (S).
- The balanced equation can be represented as:
\[ S^{2-} + S \rightarrow S_2O_3^{2-} \]
- In this reaction, we check the charge balance:
- Left side: Charge = 2⁻ (from sulfide) + 0 (from elemental sulfur) = 2⁻
- Right side: Charge = 2⁻ (from thiosulfate)
- The charge is balanced on both sides.
- Now, we check the oxidation states:
- Sulfide (S²⁻) has an oxidation state of -2.
- Elemental sulfur (S) has an oxidation state of 0.
- In thiosulfate (S₂O₃²⁻), one sulfur is at +4 and the other is at 0.
- Since the oxidation states are balanced and the charges are equal, this reaction is correct.

**Hint**: Check the charge balance and oxidation states to confirm the correctness of the reaction.

2. **Analyzing the Second Reaction**:
- The second reaction involves thiosulfate (S₂O₃²⁻) in an acetic medium undergoing disproportionation.
- The reaction can be represented as:
\[ S_2O_3^{2-} \rightarrow SO_3^{2-} + S \]
- In this reaction, we analyze the oxidation states of sulfur:
- In thiosulfate, the average oxidation state of sulfur is +2.
- In sulfite (SO₃²⁻), sulfur has an oxidation state of +4.
- Elemental sulfur (S) has an oxidation state of 0.
- Here, sulfur undergoes both oxidation (from +2 to +4) and reduction (from +2 to 0), which is characteristic of a disproportionation reaction.
- Therefore, this reaction is also correct.

**Hint**: Identify the changes in oxidation states to determine if a disproportionation reaction is occurring.

3. **Conclusion**:
- Both reactions have been analyzed, and we found that:
- The first reaction is correct as the charges and oxidation states are balanced.
- The second reaction is also correct as it involves the disproportionation of sulfur.
- Thus, all statements regarding these reactions are correct.

### Final Answer:
All the above statements are correct. Therefore, the answer is option **D**.