Calculate the current that must be passed into a solution of aluminum salt for 1 hour 30minutes in order to deposit 1.5kg of aluminum (Al = 27)
To calculate the current required to deposit 1.5kg of aluminum in 1 hour 30 minutes, we need to convert the time into seconds and use Faraday's law of electrolysis.
1 hour = 60 minutes = 3600 seconds
30 minutes = 30 * 60 = 1800 seconds
Total time = 3600 seconds + 1800 seconds = 5400 seconds
First, we need to calculate the number of moles of aluminum:
1.5kg = 1500g
Number of moles = mass / molar mass
Number of moles of aluminum = 1500g / 27g/mol = 55.56 moles
According to Faraday's law of electrolysis, the amount of substance (in moles) produced or consumed during electrolysis is directly proportional to the amount of charge passed through the solution. The formula used is:
Amount of substance = Charge / (Faraday's constant * Number of electrons)
The Faraday's constant is equal to 96500 C/mol.
Since aluminum has a +3 charge, it requires 3 electrons to be deposited as aluminum metal.
Let's calculate the charge required:
Charge = Amount of substance * (Faraday's constant * Number of electrons)
Charge = 55.56 moles * (96500 C/mol * 3 electrons)
Charge = 160135400 C
Now, let's calculate the current:
Current = Charge / Time
Current = 160135400 C / 5400 s
Current = 29698.04 A
Therefore, the current that must be passed into the solution of aluminum salt for 1 hour 30 minutes in order to deposit 1.5kg of aluminum is approximately 29700 A.