what mass of Almunium is deposited electrolytically in 30minute by a current 40 A
To determine the mass of aluminum deposited electrolytically, we need to use Faraday's law of electrolysis.
The formula to calculate the mass of a substance deposited during electrolysis is:
Mass (g) = (Current (A) × Time (s) × Molar mass (g/mol)) / (1 Coulomb × Faraday's constant (C/mol))
First, convert 30 minutes to seconds:
30 minutes = 30 × 60 seconds = 1800 seconds
The molar mass of aluminum (Al) is 26.98 g/mol.
The value of Faraday's constant is 96,485 C/mol.
Now we can substitute the given values into the formula:
Mass (g) = (40 A × 1800 s × 26.98 g/mol) / (1 C × 96,485 C/mol)
Mass (g) = 215,520 g / 96,485
Mass (g) ≈ 2.236 g
Therefore, approximately 2.236 grams of aluminum will be deposited electrolytically in 30 minutes with a current of 40 A.