Question

how many coulombs of electricity required to oxidise one mole of al to al3

Answer 1

1 mole of electrons carry a charge of 1.6E-19 *6.022E23 coulomb, which equals 96500 C and is called 1 Faraday. For 1 mole of Al3+, we need 3 moles of electrons and that is equal to 3 Faraday of charge i.e. 3*96500 C.

Answer 2

289500C electricity is required.

Given: Oxidation of Al to $Al^{+3}$.

To find: We have to find the electricity required

Solution:

The oxidation reaction is given as-

$Al\rightarrow Al^{+3}+3e^-$.

Thus three electrons are removed from Al to ionise it.

Thus 3F of charge is required for the oxidation of Al to $Al^{+3}$.

Now we know that one F is equal to 96500 Columb.

Thus the amount of electricity required for the oxidation is given as-

$3 \times 96500 = 289500$

289500C electricity is required.