Question

during electrolysis of a sample of water the amount of h2 produced at the cathode is 6l. amount of o2 produced at anode
CORRECT AND QUICK ANSWER WILL BE MARKED AS BRAINIEST.
PLEASE

Answer 1

H2O is the formula

3l/molecule of h

3×8=24l

Answer 2

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Answer

Step by step solution by experts to help you in doubt clearance & scoring excellent marks in exams.Explanation:

Solution

Cathode :2H⊕+2e−→H2

⇒2F≡1molofH2≡22400mL

or 1F≡0.5molofH2≡11200mL

Anode:Oc−H→O2+4e−+2H2O

⇒4F≡1molofO2≡22400mL

or 1F≡0.25molofO2≡11200mL

From two electrode reactions , it is clear that hydrogen and oxygen are evolved in the mole ration of 2:1, hence their volumes will also be in the same ratio.

⇒ Volume of H2=2/3(33.6)=22.4mL

As 2F≡22400mLH2

⇒0.002F of charge is passed through the electrolytic cell.

⇒ Amount of electricity =0.002×96500C

=193.0C

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.