What is the amount of `Al` deposited on the electrolysis of molten `Al_(2)O_(3)` when a current of `9.65 A` is passed for `10.0 s` .

Explanation

To solve the problem of determining the amount of aluminum (Al) deposited during the electrolysis of molten Al₂O₃ when a current of 9.65 A is passed for 10.0 s, we can follow these steps:

### Step 1: Understand Faraday's First Law of Electrolysis
According to Faraday's First Law, the amount of substance deposited or liberated at an electrode during electrolysis is directly proportional to the total electric charge passed through the electrolyte.

### Step 2: Calculate the Total Charge (Q)
The total charge (Q) can be calculated using the formula:
\[ Q = I \times t \]
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