A sample of `Al_(2)O_(3)` dissolved in a molten fluoride bath is electrolysed using a current of 1.20 A. What is the rate of production of Al in g/hour ? The oxygen liberated at the positive carbon electrode reacts with the carbon to form `CO_(2)`. What mass of `CO_(2)` is produced per hour ?

Explanation

To solve the problem, we will follow these steps:

### Step 1: Calculate the total charge passed during electrolysis.
The formula for charge (Q) is given by:
\[ Q = I \times t \]
where:
- \( I \) = current in amperes (A)
- \( t \) = time in seconds (s)
...