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]
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.
To calculate the current required to deposit 1.5g of aluminum, we need to use Faraday's law of electrolysis and the molar mass of aluminum.
1. Determine the number of moles of aluminum:
Moles of aluminum (n) = mass of aluminum (m) / molar mass of aluminum (M)
Given: m = 1.5g, M = 27 g/mol
n = 1.5g / 27 g/mol
n = 0.0556 mol
2. Use Faraday's law to calculate the total charge:
Total charge (Q) = n * F
where F is Faraday's constant (96500 C/mol)
Q = 0.0556 mol * 96500 C/mol
Q ≈ 5367 C
3. Determine the time in seconds:
1 hour 30 min = (1 * 60 * 60) + (30 * 60) seconds
1 hour 30 min = 5400 seconds
4. Calculate the current:
Current (I) = Q / t
where t is the time in seconds
I = 5367 C / 5400 s
I ≈ 0.993 A
Therefore, to deposit 1.5g of aluminum in a solution of aluminum salt, a current of approximately 0.993 Amps must be passed for 1 hour 30 minutes.