In the following reaction
`As_(2)S_(3)+NO_(3)^(ɵ)+H_(2)OtoAsO_(4)^(3-)+SO_(4)^(2-)+NO+H^(o+)` The number of electrons involved in the oxidation reaction is

Options

A. 22
B. 24
C. 26
D. 28

Explanation

To solve the problem of determining the number of electrons involved in the oxidation reaction of the given reaction:

**Given Reaction:**
\[ \text{As}_2\text{S}_3 + \text{NO}_3^- + \text{H}_2\text{O} \rightarrow \text{AsO}_4^{3-} + \text{SO}_4^{2-} + \text{NO} + \text{H}^+ \]

### Step-by-Step Solution:

1. **Identify Oxidation States:**
- For \( \text{As}_2\text{S}_3 \):
- Arsenic (As): Let the oxidation state be \( x \).
- Sulfur (S): Oxidation state is \(-2\).
- Equation: \( 2x + 3(-2) = 0 \) → \( 2x - 6 = 0 \) → \( x = +3 \).
- Therefore, As is in +3 oxidation state and S is in -2 oxidation state.

- For \( \text{NO}_3^- \):
- Nitrogen (N): Let the oxidation state be \( y \).
- Oxygen (O): Oxidation state is \(-2\).
- Equation: \( y + 3(-2) = -1 \) → \( y - 6 = -1 \) → \( y = +5 \).
- Therefore, N is in +5 oxidation state.

- For \( \text{AsO}_4^{3-} \):
- Arsenic (As): Let the oxidation state be \( z \).
- Equation: \( z + 4(-2) = -3 \) → \( z - 8 = -3 \) → \( z = +5 \).
- Therefore, As is in +5 oxidation state.

- For \( \text{SO}_4^{2-} \):
- Sulfur (S): Let the oxidation state be \( w \).
- Equation: \( w + 4(-2) = -2 \) → \( w - 8 = -2 \) → \( w = +6 \).
- Therefore, S is in +6 oxidation state.

- For \( \text{NO} \):
- Nitrogen (N): Let the oxidation state be \( v \).
- Equation: \( v + (-2) = 0 \) → \( v - 2 = 0 \) → \( v = +2 \).
- Therefore, N is in +2 oxidation state.

2. **Determine Changes in Oxidation States:**
- Arsenic (As): Changes from +3 to +5 (oxidation).
- Sulfur (S): Changes from -2 to +6 (oxidation).
- Nitrogen (N): Changes from +5 to +2 (reduction).

3. **Calculate Electrons for Oxidation:**
- For Arsenic:
- Change: \( +5 - (+3) = +2 \) (2 electrons lost per As atom).
- Since there are 2 As atoms in \( \text{As}_2\text{S}_3 \): \( 2 \times 2 = 4 \) electrons.

- For Sulfur:
- Change: \( +6 - (-2) = +8 \) (8 electrons lost per S atom).
- Since there are 3 S atoms in \( \text{As}_2\text{S}_3 \): \( 3 \times 8 = 24 \) electrons.

4. **Total Electrons in Oxidation Reaction:**
- Total electrons lost in oxidation = Electrons from Arsenic + Electrons from Sulfur = \( 4 + 24 = 28 \) electrons.

### Final Answer:
The number of electrons involved in the oxidation reaction is **28 electrons**.

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