How much electricity in terms of Faraday is required to produce `40.0 g` of `Al` from molter `Al_(2)O_(3)`?

Explanation

To determine how much electricity in terms of Faraday is required to produce 40.0 g of aluminum from molten aluminum oxide (Al₂O₃), we can follow these steps:

### Step 1: Write the Reduction Reaction
The reduction reaction for aluminum from aluminum oxide can be represented as:
\[ \text{Al}_2\text{O}_3 + 6e^- \rightarrow 2\text{Al} + \frac{3}{2}\text{O}_2 \]
This indicates that 6 moles of electrons are required to produce 2 moles of aluminum.

### Step 2: Calculate the Molar Mass of Aluminum
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