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

Explanation

To calculate the amount of electricity in terms of Faraday required to produce 40.0 g of aluminum (Al) from molten aluminum oxide (Al₂O₃), we can follow these steps:

### Step 1: Determine the moles of aluminum produced
First, we need to calculate the number of moles of aluminum (Al) that corresponds to 40.0 g.

\[ \text{Molar mass of Al} = 27 \, \text{g/mol} \]
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