Find the number of reducing agents from the following
`H_(2)S,SO_(3),CrO_(4)^(2-),Fe^(2+),MnO_(4)^(Θ)`

Explanation

To determine the number of reducing agents from the given species: \( H_2S, SO_3, CrO_4^{2-}, Fe^{2+}, MnO_4^{\Theta} \), we will analyze each species to see if it can act as a reducing agent.

### Step-by-Step Solution:

1. **Understanding Reducing Agents**:
- A reducing agent is a substance that donates electrons to another substance, thereby reducing it while itself being oxidized.

2. **Analyzing Each Species**:
- **\( H_2S \)**:
- Hydrogen sulfide can donate electrons and is known to act as a reducing agent.
- **Conclusion**: \( H_2S \) is a reducing agent.

- **\( SO_3 \)**:
- Sulfur trioxide typically acts as an oxidizing agent rather than a reducing agent.
- **Conclusion**: \( SO_3 \) is not a reducing agent.

- **\( CrO_4^{2-} \)**:
- Chromate ion is a strong oxidizing agent and can oxidize other substances.
- **Conclusion**: \( CrO_4^{2-} \) is not a reducing agent.

- **\( Fe^{2+} \)**:
- Ferrous ion can donate electrons and is known to act as a reducing agent.
- **Conclusion**: \( Fe^{2+} \) is a reducing agent.

- **\( MnO_4^{\Theta} \)**:
- Permanganate ion is a very strong oxidizing agent and does not act as a reducing agent.
- **Conclusion**: \( MnO_4^{\Theta} \) is not a reducing agent.

3. **Counting the Reducing Agents**:
- From the analysis, the reducing agents identified are \( H_2S \) and \( Fe^{2+} \).
- Therefore, the total number of reducing agents is **2**.

### Final Answer:
The number of reducing agents from the given species is **2**.

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