Electrolysis of Water: Oxygen & Hydrogen Travel

In summary, when the water molecule splits, the oxygen and hydrogen would have to travel to their electrodes, so why don't you see them do this? When the water molecule splits, the oxygen and hydrogen would have to travel to their electrodes, so why don't you see them do this?According to the speaker, when the water molecule splits, the oxygen and hydrogen would have to travel to their electrodes. This is why you don't see bubbles traveling in the water to the electrodes.
  • #1
cragar
2,552
3
When you see the bubbles coming off of the 2 electrodes in the water, why don't you see bubbles traveling in the water to the electrodes? When the water molecule splits, the oxygen and hydrogen would have to travel to their electrodes, so why don't you see them do this?
And also what causes the water molecule to split. Is the E field created from the current enough to split the polarized water molecule apart?
 
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  • #2
Water molecules react directly on the electrodes, not in the bulk of the solution. Reaction requires charge transfer, they are not being "torn out" by the electric field.
 
  • #3
When you say the reaction happens at the electrodes, So at each electrode it splits the water molecule, so why wouldn't I get both [itex] O_2 [/itex] and [itex] H_2 [/itex]
bubbles at both ends. And when you say the reaction happens because of charge transfer, is the water molecule transferring an electron to one of the electrodes and then it becomes unstable and separates into Hydrogen and Oxygen.
Thanks for your response by the way.
 
  • #4
All chemical reactions are some kind of electron transfer. The most subtle ones are some kind of rearrangement of where the electrons in a molecule are. But electrolysis is a particularly obvious kind of electron transfer.

H2O dissociates into H+ and OH- (a small fraction of these is present in any aqueous solution). So to which electrode can you imagine either of these being attracted and what could it do in the way of giving up/acquiring an electron in what chemical reaction?
 
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  • #5
If there is a potential difference between electrodes it means that they are charged differently, doesn't it? In other words - there is an excess of electrons on one, and a lack on another. Both gases are produced in different reactions - one consumes electrons, other gives them away. The reaction that consumes electrons goes only on the electrode with excess electrons, while the one that produces them goes on the other electrode.

(This is not contradicting what epeneguin wrote, this is just another part of the full explanation).
 
  • #6
ok thanks for your posts, I think I am starting to understand a little better.
 
  • #7
So far we have an image of H20 turning into H (which bubbles up at one electrode) then an OH migrating through the liquid to the other electrode where (?) it gets the remaining H torn off (but this one doesn't bubble up) and the O goes up as a bubble here.

Not a very nice picture yet.
 
  • #8
Perhaps the best (even if not necessarily correct) way of dealing with the problem is to write two reaction equations:

2H+ + 2e- -> H2(g)

4OH- -> 2H2O + 1O2(g) + 4e-

As you see it is not necessary that hydrogen "gets torn off but doesn't bubble up".

That being said I am not sure what the exact mechanism of the electrolysis is, could be it changes depending on the pH. While it is easy to write reactions involving H+ and OH-, and while it is obvious these ions are attracted to cathode and anode, in low or high pH solutions their concentrations are very low, but we don't observe any slowing of electrolysis. Still it is solution conductivity that is the bottleneck. As concentration of these ions changes by 14 orders of magnitude, could be their presence doesn't matter much, and it is just water molecules that react. It can also be that water autodissociation is so fast, even these 14 orders of magnitude don't matter.
 

What is the purpose of electrolysis of water?

The purpose of electrolysis of water is to separate the molecules of water (H2O) into its constituent elements, hydrogen (H2) and oxygen (O2). This process involves passing an electric current through a water solution, causing a chemical reaction that splits the water molecules into their respective ions.

How does electrolysis of water work?

Electrolysis of water works by using an electric current to break the bonds between the hydrogen and oxygen atoms in a water molecule. This process occurs in a special apparatus called an electrolytic cell, which contains two electrodes (an anode and a cathode) and a conductive solution of water and an electrolyte. When an electric current is passed through the solution, the water molecules are broken down into positively charged hydrogen ions (H+) at the cathode and negatively charged oxygen ions (O2-) at the anode.

What are the products of electrolysis of water?

The products of electrolysis of water are hydrogen gas (H2) and oxygen gas (O2). These gases are released separately at the cathode and anode, respectively. The amount of each gas produced is directly proportional to the amount of electric current passed through the solution and the duration of the electrolysis process.

What are some applications of electrolysis of water?

Electrolysis of water has several important applications. The production of hydrogen gas through electrolysis is a key step in the production of clean, renewable energy. Hydrogen gas can be used as a fuel for vehicles or to generate electricity through fuel cells. Additionally, electrolysis of water is used in industrial processes to produce chemicals such as chlorine and sodium hydroxide.

Is electrolysis of water an efficient process?

Electrolysis of water is considered to be a relatively inefficient process, as it requires a significant amount of energy to produce a relatively small amount of hydrogen and oxygen gases. However, advancements in technology and the use of renewable energy sources have made electrolysis of water a more viable option for clean energy production.

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