For reducing 1 mole of ferrous ions to iron the number of faradays of electricity required will be

Options

A. 1
B. 2
C. 3
D. 1.5

Explanation

To determine the number of Faradays of electricity required to reduce 1 mole of ferrous ions (Fe²⁺) to iron (Fe), we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Ferrous Ion**:
- The ferrous ion is represented as Fe²⁺.

2. **Determine the Reduction Reaction**:
- The reduction of ferrous ions to iron can be represented by the half-reaction:
\[ \text{Fe}^{2+} + 2e^- \rightarrow \text{Fe} \]
- This equation shows that 1 mole of ferrous ions requires 2 moles of electrons (2e⁻) to be reduced to 1 mole of iron.

3. **Calculate Moles of Electrons Required**:
- From the reaction, we see that to reduce 1 mole of Fe²⁺, we need 2 moles of electrons.

4. **Relate Moles of Electrons to Faradays**:
- According to Faraday's law of electrolysis, 1 mole of electrons corresponds to 1 Faraday of electricity.
- Therefore, if 2 moles of electrons are required, this translates to:
\[ 2 \text{ moles of electrons} = 2 \text{ Faradays} \]

5. **Final Answer**:
- Thus, the number of Faradays of electricity required to reduce 1 mole of ferrous ions to iron is **2 Faradays**.

### Summary:
To reduce 1 mole of ferrous ions (Fe²⁺) to iron (Fe), **2 Faradays** of electricity are required.