How many minutes will it take a current of 37.779 Ampères to deposit 46.053 grams of aluminum? Can ANYONE HELP

Question

How many minutes will it take a current of 37.779 Ampères to deposit 46.053 grams of aluminum (26.981538 g/mol)

CAN ANYONE HELP ME PLZ!

Answer 1

convert amps to volts....and i think volts should tell you something about how fast the reaction is happening (volts = force of electron movement)

Answer 2

The electrical current (in amperes, amps) is the rate of flow of charge.  1 amp = 1 coulomb/sec.

Another important value is the charge on a mole of electrons.  That is the Faraday, or 96,500 coulombs / mol.

The last piece of the puzzle is the number of electrons needed to deposit an atom of aluminum.  That would be three.  Also, we can say that a 3 moles of electrons will deposit 1 mole of aluminum.

A few conversion factors later and we'll have the time needed to deposit 46.053 grams

46.053 g Al x (1 mol Al / 26.9815 g Al) x (3 mole e- / mol Al) x (96,500 coulombs / mol e-) x (1 second / 37.779 coulombs) x (1 minute / 60 seconds) = 217.99 minutes