# Could we seed Earth's atmosphere with hydrogen?

Suppose the chemical reaction: $$3CO_2+2H_2\rightarrow 2H_2O+2O_2+3C$$ This reaction could be used to filter out $CO_2$ from the atmosphere, slowing down or reversing climate change. The solar system is rich in hydrogen.

There's a problem though, for this reaction to take place requires the catalyst of iron in the form of an aerosol.

Though this might work on a planet without life, it would most certainly kill off all life on earth.

What kind of future technology could make this a possible method taking $CO_2$ out of the atmosphere at a global scale with or without iron aerosol?

Or is there another realistic way of taking $CO_2$ out of the atmosphere with technology within the span of a few decades? Assuming carbon neutral energy generation of no more than an order of magnitude higher than earth currently has.

This question asks for hard science. All answers to this question should be backed up by equations, empirical evidence, scientific papers, other citations, etc. Answers that do not satisfy this requirement might be removed. See the tag description for more information.

• Don't you think $$O_2+2H_2\rightarrow 2H_2O$$ would be more probable? Or Hidrogen just floating to the upper atmosphera and end in space. BTW, chemical elements should start in uppercase. – SJuan76 Nov 9 '16 at 12:47
• @SJuan76 I'm not sure I understand, where does the carbon come into it in your equation? – Feyre Nov 9 '16 at 12:55
• What I point is that if you just add H2 to the atmosphera, there are other (many, since hidrogen is highly reactive) possible reactions for the hidrogen to take part of (another example, combining with nitrogen to form ammonia or nitrates), specially since CO2 is a tiny fraction of the gas volume. Why are you sure that the reaction you posted is the one that will happen? – SJuan76 Nov 9 '16 at 13:00
• @SJuan76 As far as I understand it, iron aerosol is not a catalyst for other reactions. However, it would be acceptable for a certain amount of oxygen to be reacted on, as electrolysis of water is simple. Chemistry is not my forté, hence me asking this question. :) – Feyre Nov 9 '16 at 13:05

# Hydrogen floats and escapes

Hydrogen cannot be contained in the atmosphere, because it will float to the top, and then escape the Earth.

http://www.livescience.com/28466-hydrogen.html

Already today we can break up carbon dioxide. There are several ways of doing it. For instance we can pewpew it with a laser to mention one of the more exotic examples.

But the major problem with breaking up carbon dioxide is that all of these processes require energy. And the excess $CO_2$ that we have a problem with now was created when we were generating energy. So in order to split $CO_2$, we need to generate at least as much energy as was gained when the $CO_2$ was formed in the first place, and this time without having any $CO_2$ as a waste product.

This of course means that we should just skip the $CO_2$-generating step all-together and just use the carbon dioxide free energy directly instead.

So to answer your question: what (future) technology can be used to break up carbon dioxide? Well you have a buffet to choose from already.

The break-through you are looking for is a method of generating carbon dioxide free energy in such abundance that we can cover all our energy consumption needs, and have enough left over to start breaking up carbon dioxide too.

EDIT: The one technology that would be really cool and futuristic in this context — that would break up carbondioxide using sunlight as its source of energy — is one that emulates photosynthesis, in other words: artificial photosynthesis. If humanity can get artificial photosynthesis to work, then we will have a very cool technology indeed, a cool technology that will open the door to many solutions to woes that we face today.

EDIT by OP: This technology could be used as an decentralized energy source. For it to work it requires further advances in "light harvesting, charge separation, catalysis, semiconductors, nanotechnology, modelling from synthetic biology and genetic engineering, photochemistry and photophysics, photoelectrochemistry, catalysis, reaction mechanisms and device engineering."

• Laser separation is slow and insanely energy intensive though. I already rejected it as an efficient global solution. I take it as a given that carbon neutral energy exists. Escape wouldn't be instantaneous, so would there not be enough time (potentially through some artificial means) for reaction? – Feyre Nov 9 '16 at 13:12
• @Feyre It was but an example, and I stated that it was exotic (which implies it is also not very effective nor suited for large scale use). :) The main problem remains the same though: you need to put in (at least) as much energy as was gained when carbon and hydrogen was fused to form carbon dioxide. There is no way around that, which simply makes using CO2-generating energy pointless unless you find a CO2-beaking process that operates by waste heat or sunlight. There is one well known such process: en.wikipedia.org/wiki/Photosynthesis – MichaelK Nov 9 '16 at 13:23
• Feyre is right in that specific fact that "is it possible to fill our atmosphere with hydrogen?" is not answered. I see that Michael has answered the feasability of the act. I support the latter, but to fulfill the hard rules, I suggest Michael to expand the answer with this somewhat trivial detail...or Feyre to edit the question not emphasizing on the material transfer but on the CO2 issue and possible solutions. – Sonic Nov 9 '16 at 13:43
• Your second to last comment I think contains a more fitting answer than your answer so far. If you could link artificial photosynthesis with a reliable source that'd be awesome. Thank you for your attention. – Feyre Nov 9 '16 at 14:09
• @MichaelKarnerfors I agree with that. – Feyre Nov 9 '16 at 14:26

Your equation is not thermodynamically plausible. It will actually operate in the reverse direction.

One tool for determining if a reaction works is to use the Standard Gibbs Free Energy of Formation, which is a measure of how much energy it takes to create a particular molecule from its raw components in their lowest energy form. You can sum these to see if a reaction will create or consume free energy. Reactions that create free energy (by releasing it from the bonds of their molecules) will occur naturally in the forward direction. Reactions that consume it will not (mostly... there's a few details that I don't believe matter here). A table of values for your compounds would be:

• $CO_2$ : -394 kJ/mol
• $H_2$ : 0 kJ/mol
• $H_2O_{(g)}$ : -237 kJ/mol
• $O_2$ : 0 kJ/mol
• $C$ : 0 kJ/mol

For an example of how this works, consider a reaction we know occurs ferociously: $2H_2+O_2\rightarrow 2H_2O + \Delta E$, where E is energy released. If we plug in those Gibbs free energy numbers we get $2\cdot0 + 0 \rightarrow 2\cdot-237 + \Delta E$ which shows $\Delta E=474kJ$ per mole of oxygen burned.

In your equation, we can do the same: $$3CO_2+2H_2\rightarrow 2H_2O+2O_2+3C$$ $$3\cdot -394+2\cdot 0\rightarrow 2\cdot-237+2\cdot 0+3\cdot 0 + \Delta E$$ $$-1182\rightarrow -474 + \Delta E$$ $$\Delta E = -708$$

Your reaction is highly endothermic, and will not occur without a very large amount of energy from an outside source.

The issue, of course, is that $CO_2$ is a very stable compound, hence its very negative free energy of formation. Once you've got it, there's not many reasons it will let go. This is related to Oxygen's ability to... well.. oxidize. $C+O_2$ is quite energetic compared to $CO_2$.

• Is it possible that there's a more efficient reaction, or is Birch just full of manure on this one? – Feyre Nov 9 '16 at 15:21
• You might want to include a line phrasing that more simply: his equation is pretty much something burning backwards, expecting C02 to just turn into charcoal and oxygen . – Murphy Nov 9 '16 at 17:57
• @Feyre It is provable that, with those reactants and resultants, there is no way it could work. To make it work, you would need to have something on the right hand side of the equation which is more stable (larger negative free energy), so that we can release energy from the CO2 molecules. You could scan the free energy table to see what is possible. However, in general CO2 is a very stable molecule. It's generally hard to make it react unless you use a very highly reactive species to react with it, or provide energy (as photosynthesis does). – Cort Ammon Nov 9 '16 at 19:09
• Excellent answer to (yet another) hydrogen-oxygen atmosphere question... – Serban Tanasa Nov 9 '16 at 19:34