The oxidation numbers of the sulphur atoms in pcroxy- monosulphuric acid `(H_(2)SO_(5))` and peroxydisulphuric acid `(H_(2)S_(2)O_(8))` are respectively.

Options

A. `+8 , +7`
B. `+3 , +3`
C. `+6, +6`
D. `+4, +6`

Explanation

To find the oxidation numbers of the sulfur atoms in peroxymonosulphuric acid (H₂SO₅) and peroxydisulphuric acid (H₂S₂O₈), we will follow these steps:

### Step 1: Determine the oxidation number of sulfur in H₂SO₅

1. **Identify the formula**: H₂SO₅ consists of 2 hydrogen (H) atoms, 1 sulfur (S) atom, and 5 oxygen (O) atoms.
2. **Assign known oxidation states**:
- Hydrogen (H) has an oxidation state of +1.
- In peroxides, oxygen (O) has an oxidation state of -1. In H₂SO₅, there are 2 oxygen atoms in the peroxide form.
- The remaining 3 oxygen atoms have an oxidation state of -2 (as they are not in peroxide form).
3. **Set up the equation**: Let the oxidation number of sulfur be \( x \).
\[ 2(+1) + x + 2(-1) + 3(-2) = 0 \]
Simplifying this gives:
\[ 2 + x - 2 - 6 = 0 \implies x - 6 = 0 \implies x = +6 \]
4. **Conclusion**: The oxidation number of sulfur in H₂SO₅ is +6.

### Step 2: Determine the oxidation number of sulfur in H₂S₂O₈

1. **Identify the formula**: H₂S₂O₈ consists of 2 hydrogen (H) atoms, 2 sulfur (S) atoms, and 8 oxygen (O) atoms.
2. **Assign known oxidation states**:
- Hydrogen (H) has an oxidation state of +1.
- There are 2 oxygen atoms in the peroxide form, which have an oxidation state of -1.
- The remaining 6 oxygen atoms have an oxidation state of -2.
3. **Set up the equation**: Let the oxidation number of sulfur be \( x \).
\[ 2(+1) + 2x + 2(-1) + 6(-2) = 0 \]
Simplifying this gives:
\[ 2 + 2x - 2 - 12 = 0 \implies 2x - 12 = 0 \implies 2x = 12 \implies x = +6 \]
4. **Conclusion**: The oxidation number of sulfur in H₂S₂O₈ is also +6.

### Final Answer
The oxidation numbers of the sulfur atoms in peroxymonosulphuric acid (H₂SO₅) and peroxydisulphuric acid (H₂S₂O₈) are +6 and +6, respectively.

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