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