What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt by a current of 24 amps?

All i need is the moles of Aluminum per moles of electons. thanks

1 Al per 3 e-

To determine the moles of aluminum per mole of electrons, we need to use Faraday's law of electrolysis. Faraday's law states that the amount of substance produced or consumed in an electrolysis process is directly proportional to the amount of electricity passed through the electrolyte.

The equation relating the amount of substance produced (in moles) to the amount of electricity passed (in coulombs) is:

moles = (coulombs) / (Faraday constant)

The Faraday constant is the charge of one mole of electrons, which is equal to 96,485 coulombs/mol.

Given that we have a current of 24 amps and a time of 1 hour (3600 seconds), we can calculate the total charge passed in coulombs using the formula:

charge (in coulombs) = current (in amps) x time (in seconds)

charge = 24 A x 3600 s = 86,400 coulombs

Now we can calculate the moles of aluminum produced:

moles of aluminum = (charge) / (Faraday constant)

moles of aluminum = 86,400 C / 96,485 C/mol = 0.896 mol

Therefore, in the electrolysis of a molten aluminum salt by a current of 24 amps, approximately 0.896 moles of aluminum can be produced per hour.

To determine the mass of aluminum produced per hour in the electrolysis of a molten aluminum salt, we first need to calculate the number of moles of aluminum produced per mole of electrons.

The balanced equation for the electrolysis of molten aluminum salt (AlX) is:

2AlX(l) → 2Al(l) + X2(g)

From the equation, we can see that 2 moles of aluminum are produced per mole of the aluminum salt.

Next, we need to determine the number of moles of electrons required for the reduction of each mole of aluminum.

From the equation, we see that the reduction of each mole of aluminum requires two moles of electrons. This means that for every mole of aluminum produced, two moles of electrons are consumed.

Now, the molar mass of aluminum is approximately 26.98 g/mol.

Given a current of 24 amps, we can determine the number of moles of electrons per hour using Faraday's law:

1 Faraday = 96,485 C/mol e-
1 hour = 3,600 seconds

The charge (Q) passed in Coulombs (C) can be calculated using the formula:

Q = I × t

Where:
I = current in amperes
t = time in seconds

Q = 24 A × 3,600 s = 86,400 C

To find the number of moles of electrons, divide the total charge by the charge per mole of electrons:

Number of moles of electrons = Q / (96,485 C/mol e-) = 86,400 C / 96,485 C/mol e- = 0.896 mol e-

Now, to determine the moles of aluminum produced per hour, we simply multiply the moles of electrons by the ratio of aluminum to electrons:

Moles of aluminum = 0.896 mol e- × (2 mol Al / 2 mol e-) = 0.896 mol Al

Finally, to find the mass of aluminum produced, we calculate the mass by multiplying the moles of aluminum by the molar mass of aluminum:

Mass of aluminum = 0.896 mol Al × 26.98 g/mol = 24.15 g

Therefore, approximately 24.15 grams of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt by a current of 24 amps.