Asked by A

In the process of electrolysis, electrical power is used to separate water into oxygen and hydrogen molecules via the reaction:

H2O --> H2 + ½O2

This is very much like running a hydrogen fuel cell in reverse. We assume that only the activation potential for the hydrogen reaction is non-negligible. All other potentials are negligible. Hence the relevant parameters are :

PO2 :1 atm
PH2: 1 atm
Temp: 350K
j0(H2): 0.1A/cm2
£\(H2): 0.50

1. What is the current density in A/cm2 at a voltage of 1.5 V?

2. What area of the cell, in cm2, do we need in order to get a rate of H2 production of 1 mol/sec?
Answered by kakarot
1 - 1.23v
Answered by A
how are about b,c? can you calculate it?
Answered by bujaga
for b you use Butler Volmer equation and for c you use eq: I=n*F*dH2/dt
Answered by A
yes, I know...but I don't know how to find n and eta? can you teach me how to find it?
Answered by A
Thank you. I can find it now. But can you tell me how to do 2d,e , please?
Answered by Chris
What is the answer for b and c?
Please Help.
Answered by Paul
Guys, I would be glad if you post the answer for this questions.
Thank you so much.!
Answered by Unknown
plz... post all the answers you know so that other people will be benefited.....
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