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

Question

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?

Answer 1

1 - 1.23v

Answer 2

how are about b,c? can you calculate it?

Answer 3

for b you use Butler Volmer equation and for c you use eq: I=n*F*dH2/dt

Answer 4

yes, I know...but I don't know how to find n and eta? can you teach me how to find it?

Answer 5

Thank you. I can find it now. But can you tell me how to do 2d,e , please?

Answer 6

What is the answer for b and c?
Please Help.

Answer 7

Guys, I would be glad if you post the answer for this questions.
Thank you so much.!

Answer 8

plz... post all the answers you know so that other people will be benefited.....