Calculate the current that must be passed into a solution of aluminum salt for 1hr 30 min in other to deposit 1.5g of aluminum [Al=27]

Answer 1

To calculate the current required to deposit 1.5g of aluminum, we need to use Faraday's law of electrolysis.

The equation is as follows:

mass of substance deposited = (current × time × atomic mass) / (Faraday's constant × valency)

Given:
mass of aluminum deposited (m) = 1.5g
atomic mass of aluminum (M) = 27g/mol
time (t) = 1hr 30min = 1.5 hours
Faraday's constant (F) = 96500 C/mol
valency of aluminum (z) = 3 (since aluminum has a valency of 3)

Plugging in the values into the formula:

1.5g = (current × 1.5 hours × 27g/mol) / (96500 C/mol × 3)

Rearranging the formula to solve for current (I):

I = (1.5g × 96500 C/mol × 3) / (1.5 hours × 27g/mol)

Simplifying the equation:

I = 6455.56 C/h

Therefore, the current that must be passed into the solution of aluminum salt for 1hr 30 min in order to deposit 1.5g of aluminum is approximately 6455.56 C/h.