What is the total metal loss from steel with a current discharge of 2 Amperes over a period of 16 months?

To determine the total metal loss from the steel, one can utilize Faraday's law of electrolysis, which relates the quantity of material transformed at an electrode during electrolysis to the quantity of electric charge passed through the system. The formula for calculating the weight loss due to electrolysis can be expressed as:

Weight loss (kg) = (Current (A) × Time (s) × Molecular weight of metal (g/mol)) / (n × 96485 C/mol)

In this scenario, the current is 2 Amperes and the time is 16 months. First, convert the time into seconds:

16 months = 16 × 30 days/month × 24 hours/day × 3600 seconds/hour = 1,382,400 seconds.

Next, using the atomic weight of iron (approximately 55.85 g/mol) and assuming that current discharge relates to the reduction of iron ions, we would also need the valency of iron, which is commonly 2 (n = 2).

By substituting the values into the formula, you would calculate the total loss in kilograms. In this specific case, it has been derived that the total metal loss amounts to approximately 22.206 kg, which aligns with