Calculate the number of coulombs required to deposit 5.4g of Al when the electrode reaction is :
`Al^(3+) +3e^(-) to Al` [Atomic weight of Al = 27 g/mol]

Explanation

To calculate the number of coulombs required to deposit 5.4 g of aluminum (Al) using the given electrode reaction, we can follow these steps:

### Step 1: Determine the moles of aluminum deposited
First, we need to calculate the number of moles of aluminum deposited using its atomic weight.

\[ \text{Moles of Al} = \frac{\text{mass of Al}}{\text{molar mass of Al}} = \frac{5.4 \, \text{g}}{27 \, \text{g/mol}} = 0.2 \, \text{mol} \]
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