Question

What volume of dry oxygen gas at STP could be generated at the anode by the electrolysis of water over a 6.0 hour period with a current of 1.5 ampere

Answer 1

ANSWER

When 30 amperes is passed for 193 minutes, the quantity of current passed =193×60×30=347400 coulombs.

=347400/96500=3.6 Faradays.

H

2

O

electrolysis

H

2

+0.5O

2

So on passing 1 Faraday of electricity, 1 mole of Hydrogen and 0.5 mole of Oxygen are produced.

On passing 3.6 Faradays of electricity 3.6 moles of Hydrogen and (3.6×0.5)=1.8 moles of Oxygen will be formed.

So the volume of Hydrogen produced at STP =3.6×22.4=80.64 liters.

Volume of oxygen produced at STP =1.8×22.4=40.32 liters.