|WikiProject Chemistry||(Rated Start-class, Mid-importance)|
This is an important page and needs to be expanded upon. Currently, the Sabatier Reaction seems to be only used in discussions of how to create rocket fuel from the lunar surface or the martian surface. However, this reaction is potentially interesting for discussions of a hydrogen economy. In particular, methane would appear to be an existing method for transporting hydrogen; it transports 25% hydrogen by weight (compare to carbon nanotubes, glass beads, or metal hydrides); it has better volume properties than pure hydrogen; and there exist fuel cells that will directly consume methane.
Discussions of cost information for synthesizing methane from water and carbon dioxide are hard to come by. Other discussions of how practical it might be to expand the existing methane economy for transportation purposes while recycling carbon dioxide would be interesting. —Preceding unsigned comment added by 220.127.116.11 (talk • contribs) 15:56, 18 March 2005
- Currently the reaction goes in the other direction. Most hydrogen is produced from methane. To make the Sabatier reaction go, it requires much cheaper hydrogen, or much more expensive fossil fuels. pstudier 00:40, 2005 Jun 10 (UTC)
- The most important thing is the energy balance, even if the prices of hidrogen generation or fuel don't move. But this is a hard work, and the way to do the study can change the results. So, I think that a comparison of a few works is needed. --Proximo.xv 12:07, 12 December 2006 (UTC)
I plan on including more details of the reaction process and how a reactor would work (in a new section entitled "Process"), however I'm not a chemist and finding detailed information on this that I can understand is apparently not very easy. So far I've got a ceramic (alumina) foam catalyst cooking at around 400-700 degrees F; the reaction is exothermic meaning the exhaust (methane and steam) comes out hotter than the intake. Apparently the reaction occurs spontaneously in these conditions, so a pump to keep the CO2 and 4H2 moving is all that is required. Using a ruthenium catalyst can reduce the starting temperature significantly, nickel has a higher starting temperature. Below are some links that have some more information on the process: http://pubs.acs.org/doi/abs/10.1021/i260051a007 http://www.owlnet.rice.edu/~ceng301/34.html
There are also numerous advantages to manufactured methane over fossil fuels and I believe this should be explained in the article as well - including carbon neutrality, existing pipeline infrastructure, ease of compression and storage etc; however finding people who want to burn methane (instead of going backwards and turning it into hydrogen) to cite as references is also a pain.---Puff (talk) 16:13, 30 July 2009 (UTC)
An exothermic reaction
Rocket propellant on Mars surface
Why would it be that important to make Methane on Mars surface when we now know there are vast quantities of water available there, from which the more efficient rocket propelant Hydrogen+Oxygen could be easily produced ?
Who's to say it's more efficient? It's high performance but that isn't the most important thing on mars. Practicality is, and Hydrogen is hard to store (extremely low temps), and the water needed would have to be mined from martian soil. If you want to fuel your return ship before you get to mars (highly recommended!) then you will need to do this roboticly which is going to be fraught with problems. Not impossible, but there's easier ways. If you simply bring your hydrogen from earth, which doesn't weigh much, then all you need to do is run an air compressor and power up the synthesis plant when you land. You use up the small amount of hydrogen right away so you only have to endure boil-off during the 6 month trip out to mars. You don't need to store a much larger volume of H2 for years, in very large tanks attached to your return ship etc. A methane powered mission would be cheaper and safer in this way. Later, when there is a human presence, a base, we would certainly be mining for water and then it may make sense to use H2 as fuel. But then again, we may stick to methane because it still very easy to store at martian temps and still a very good performing fuel. 18.104.22.168 (talk) 22:54, 18 May 2010 (UTC)
I am confused by the line "The stoichiometric ratio of oxidizer and fuel is 3.5:1, for an oxygen:methane engine, however one pass through the Sabatier reactor produces a ratio of only 2:1." Where does the 3.5:1 figure come from? For diatomic oxygen and methane reacting to carbon dioxide and water, the ratio is 2:1; with monatomic oxygen, the ratio is 4:1. Other values (such as the 2:1 figure in this line) seem to refer to the monatomic case. If this 3.5:1 ratio is accurate for some reaction, it would be helpful to show the reaction it describes or provide a link to another article which describes it. It might also be useful to note in the line above that the oxygen produced from a "pass through the Sabatier reactor" assumes electrolysis of the water. -- 22.214.171.124 (talk) 17:21, 1 November 2010 (UTC)
- I believe this is still a correct criticism, since one CH4 combusts to one CO2 and two H2O with the addition of 2 O2... rewriting that, it is
CH4 + 2 (O2) -> CO2 + 2 (H2O)
- or a stoichiometric ratio of 2:1 ... now it is true that engines are often run fuel rich or oxidizer rich for various reasons. If expressed using O rather than O2, a 3.5:1 ratio would be somewhat fuel rich but not outside the realm of possibility (oxidizer rich tends to be corrosive, which is bad for reusable engines). But that's not what it says. Correction seems warranted. ++Lar: t/c 20:36, 9 April 2013 (UTC)