Question

How many coulombs of current is required to deposit 4.5 gm of aluminium from molten alumina?

Answer 1

Answer:First we need the equation for elektrolyse of AlCl3 solution

(-) : Al3+ + 3e → Al

(+) : 2 Cl- → Cl 2

From the first equation we can derive that for 1,0 mewl Al you need 3,0 mewl e (electrons)

We don't need the second equation

1.0 mole = 6.02x10^23 particles

charge of one electron = 1.60x10^-19 coulomb

3.0 mole e has an electric charge of 3.0 x 6.02x10^23 x1.60x10^-19 = 2.89x10^5 Coulomb

That is what you need to produce 1.0 mole aluminium

Instead of using the number of particles and electron charge we could also apply the Faraday constant. This is the electric charge of 1.0 mole electrons in coulomb : F = 96,485 coulomb/mole

Explanation:please mark a s brainliest