read the following content

Practice examples

A current of 2 amperes was passed through an electrolytic cell for 20 minutes. Calculate the quantity of electric charge produced.

Working:

Quantity of electricity(in Coulombs) = Current(I) x time(t)

Substituting /converting time to second =>

2 x (20 x 60)

= 2400 C

A current of 2 amperes was passed through an electrolytic cell.96500 coulombs of charge were produced. Calculate the time taken.

Working:

Time(t) in seconds= Quantity of electricity Current(I) in amperes

Substituting = 96500

= 48250 seconds

96500 coulombs of charge were produced after 10 minutes in an electrolytic cell . Calculate the amount of current used.

Working:

Current(I) in amperes = Quantity of electricity Time(t) in seconds

Substituting/converting time to second=> 96500

10 x 60

=160.8333 Amperes

Feedback

The quantity of electricity required for one mole of electrons at the anode/cathode is called the Faraday constant(F).

It is about 96500 Coulombs.i.e

The number of Faradays used /required is equal to the number of electrons used at cathode/anode during the electrolytic process.

Cu2+ require to gain 2 moles of electrons=2 Faradays =2 x 96500 coulombs of electricity at the cathode.

Mg2+ require to gain 2 moles of electrons=2 Faradays =2 x 96500 coulombs of electricity at the cathode.

Al3+ require to gain 3 moles of electrons=3 Faradays =3 x 96500 coulombs of electricity at the cathode

Fe3+ require to gain 3 moles of electrons=3 Faradays =3 x 96500 coulombs of electricity at the cathode

Na+ require to gain 1 moles of electrons=1 Faradays =1 x 96500 coulombs of electricity at the cathode

2H+ require to gain 2 moles of electrons=2 Faradays =2 x 96500 coulombs of electricity at the cathode to form 1molecule of hydrogen gas

2Cl- require to lose/donate 2 moles of electrons=2 Faradays =2 x 96500 coulombs of electricity at the anode to form 1molecule of Chlorine Cl2 gas

2O2- require to lose/donate 4 moles of electrons=4 Faradays =4 x 96500 coulombs of electricity at the anode to form 1molecule of Oxygen O2 gas.

4OH- require to lose/donate 4 moles of electrons=4 Faradays =4 x 96500 coulombs of electricity at the anode to form 1molecule of Oxygen gas and 2 molecules of water.