Chemistry Forum

Here's the issue...I'm very rusty on my highschool and college chem. I came up with a great idea, but need some things answered to make sure it would work.

So, here's the problem, question and the parts needed to be answered.

Problem: I want to use hydro electric to power a electrolysis process of sea water.

Questions:
1. How much energy is needed to electrolysis any given volume of sea water?
2. What cathode and anode would be most efficient at electrolysis of sea water?
3. How much would you get of hydrogen and oxygen at any given volume of sea water @ given energy rate?
4. How much byproduct of unwanted gas is generated?
5. How much has the anode and cathode degraded over any given volume of sea water?
6. What factors may increase rate of electrolysis of same volume of water at same given rate of energy?


Answer what you can! Anything is appreciated. Leave evidence as to how you came to your answers and thx!

If you use seawater which contains NaCl you will create Chlorine Gas.
The other things can be calculated. 1mol H₂ need two electrons.
E = U*I*t = U*Q

ChenBeier wrote: ↑Sat Nov 13, 2021 12:02 pm If you use seawater which contains NaCl you will create Chlorine Gas.
The other things can be calculated. 1mol H₂ need two electrons.
E = U*I*t = U*Q

I did assume NaCl would be a byproduct.
I am hoping to understand how much on average would be produced given a specific volume of water and a specific rate of energy.

Here would be a given example.

If I used 1 kw/h on a 100 liters of sea water, how long will it take for the 100 liters to be used and does surface area of cathode and anode end points in the water, distance between endpoints, or other factors play an efficiency role?

NaCl ist not a product its an educt. It is already present. In average the contant is 35 g/l. Its a lot.
100 l =100 kg = 5,55 kmol H₂O = 11,11 kg H₂
Faraday m= Q*c
c = 0,0376 g/Ah for H+ or 0,0188 g/Ah for H₂
Q = 11111g/0,0188 g/Ah = 590957 Ah
For 10 V it is 5909570 Wh = 5909,57 kWh
1 KWh = 0,00188 kg = 1,88 g

ChenBeier wrote: ↑Sat Nov 13, 2021 3:15 pm NaCl ist not a product its an educt. It is already present. In average the contant is 35 g/l. Its a lot.
100 l =100 kg = 5,55 kmol H₂O = 11,11 kg H₂
Faraday m= Q*c
c = 0,0376 g/Ah for H+ or 0,0188 g/Ah for H₂
Q = 11111g/0,0188 g/Ah = 590957 Ah
For 10 V it is 5909570 Wh = 5909,57 kWh
1 KWh = 0,00188 kg = 1,88 g

What is g/Ah?
What is 1KWh producing 1.88g of?

c = is the electrochemical equivalent the unit is g/Ah
https://second.wiki/wiki/elektrochemisc ... 4quivalent

1,88 g hydrogen

ChenBeier wrote: ↑Sat Nov 13, 2021 3:15 pm NaCl ist not a product its an educt. It is already present. In average the contant is 35 g/l. Its a lot.
100 l =100 kg = 5,55 kmol H₂O = 11,11 kg H₂
Faraday m= Q*c
c = 0,0376 g/Ah for H+ or 0,0188 g/Ah for H₂
Q = 11111g/0,0188 g/Ah = 590957 Ah
For 10 V it is 5909570 Wh = 5909,57 kWh
1 KWh = 0,00188 kg = 1,88 g

so the 100 L is converted into 5.55 Kmol of h20? Then turned into Kg or just h2? Something seems off with these conversions. How are you going from 5.55 kmol to 11.11 kg h2?

5,55 kmol H₂O = 5,55 kmol H₂ . The molar mass of H₂ is 2g/mol or 2kg/ kmol so it will be 11,11 kg H₂