`{:("LIST - 1","LIST - 2"),("A) "H_(2)SO_(4),"1) "+4),("B) "H_(2)(S)_(n)O_(6),"2) "+3),("C) "H_(2)SO_(3),"3) "+2"," -2),("D) "H_(2)S_2O_(4),"4) "+6),(,"5) "+5","0):}`
The correct match is

Options

A. `{:(A,B,C,D),(2,5,2,4):}`
B. `{:(A,B,C,D),(3,2,1,4):}`
C. `{:(A,B,C,D),(4,5,1,2):}`
D. `{:(A,B,C,D),(2,3,1,5):}`

Answer

To solve the problem of matching the sulfur oxides from List 1 with their corresponding oxidation states from List 2, we will analyze each compound and determine the oxidation state of sulfur in each case.

### Step-by-Step Solution:

1. **Identify the Compounds and Their Structures**:
- A) \( H_2SO_4 \) (Sulfuric Acid)
- B) \( H_2(S_nO_6) \) (Thiosulfuric Acid)
- C) \( H_2SO_3 \) (Sulfurous Acid)
- D) \( H_2S_2O_4 \) (Dithionic Acid)

2. **Calculate the Oxidation State for Each Compound**:
- **For A) \( H_2SO_4 \)**:
- The structure has 4 oxygen atoms. Each oxygen has an oxidation state of -2.
- Total contribution from oxygen: \( 4 \times (-2) = -8 \).
- The two hydrogen atoms contribute \( 2 \times (+1) = +2 \).
- Let the oxidation state of sulfur be \( x \).
- The equation becomes:
\[ 2 + x - 8 = 0 \implies x = +6 \]
- Thus, the oxidation state of sulfur in \( H_2SO_4 \) is **+6**.

- **For B) \( H_2(S_nO_6) \)**:
- The structure is complex, but we can deduce that the sulfur atoms are in different oxidation states.
- The overall oxidation state can be calculated similarly, but for simplification, we find that the average oxidation state of sulfur here is **+5**.

- **For C) \( H_2SO_3 \)**:
- Again, with 3 oxygen atoms, the total contribution from oxygen is \( 3 \times (-2) = -6 \).
- The two hydrogen atoms contribute \( 2 \times (+1) = +2 \).
- Let the oxidation state of sulfur be \( x \).
- The equation becomes:
\[ 2 + x - 6 = 0 \implies x = +4 \]
- Thus, the oxidation state of sulfur in \( H_2SO_3 \) is **+4**.

- **For D) \( H_2S_2O_4 \)**:
- The structure has 4 oxygen atoms contributing \( 4 \times (-2) = -8 \).
- The two hydrogen atoms contribute \( 2 \times (+1) = +2 \).
- Let the oxidation state of sulfur be \( x \). Since there are two sulfur atoms, the equation becomes:
\[ 2 + 2x - 8 = 0 \implies 2x - 6 = 0 \implies x = +3 \]
- Thus, the oxidation state of sulfur in \( H_2S_2O_4 \) is **+3**.

3. **Match the Compounds with Their Oxidation States**:
- A) \( H_2SO_4 \) → +6 (matches with 4)
- B) \( H_2(S_nO_6) \) → +5 (matches with 5)
- C) \( H_2SO_3 \) → +4 (matches with 3)
- D) \( H_2S_2O_4 \) → +3 (matches with 2)

### Final Matching:
- A → 4
- B → 5
- C → 3
- D → 2

### Conclusion:
The correct match is:
- A) \( H_2SO_4 \) → 4
- B) \( H_2(S_nO_6) \) → 5
- C) \( H_2SO_3 \) → 3
- D) \( H_2S_2O_4 \) → 2