What mass of aluminum is deposited electrolyticaly in 30 minutes by a current 40A?

Answer 1

To calculate the mass of aluminum deposited electrolytically, we need to use Faraday's law of electrolysis, which relates the amount of substance deposited to the current and time.

The equation is:
Mass (g) = (Current (A) * Time (s) * Atomic Mass (g/mol)) / (Faraday's Constant (C/mol))

First, we need to find the atomic mass of aluminum. The atomic mass of aluminum is approximately 26.98 g/mol.

Next, we need to find Faraday's constant, which is approximately 96,500 C/mol.

Now we can calculate the mass of aluminum:

Mass (g) = (40A * 30 minutes * 60 seconds/minute * 26.98 g/mol) / 96,500 C/mol

Mass (g) = (40 * 30 * 60 * 26.98) / 96,500

Mass (g) ≈ 21.17 g

Therefore, approximately 21.17 grams of aluminum will be deposited electrolytically in 30 minutes with a current of 40A.