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Topic: Methane Decomposition  (Read 1919 times)

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Offline uzairqidwai1

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Methane Decomposition
« on: May 18, 2016, 01:10:42 AM »
Hi,
I wanted to know if it is possible to decompose methane(CH4). If yes then how?
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Offline mikasaur

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Re: Methane Decomposition
« Reply #1 on: May 18, 2016, 01:12:29 AM »
Yes it is possible. A quick search on Google yields many results on how and why decomposition occurs. Are you looking for some specific application or example?
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Or you could, you know, Google it.

Offline Enthalpy

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Re: Methane Decomposition
« Reply #2 on: May 18, 2016, 02:51:44 AM »
It's even the main industrial process to obtain hydrogen.
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Offline Burner

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Re: Methane Decomposition
« Reply #3 on: May 18, 2016, 03:53:55 AM »
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Year 1 science student in HKUST and a Chemistry geek.
If I make any mistakes in the forum, please don't hesitate to correct me as I want to learn.

Offline Enthalpy

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Re: Methane Decomposition
« Reply #4 on: May 30, 2016, 09:14:46 AM »
As things happen, I had to look for the heat stability of methane yesterday (for a rocket engine cycle of course)
http://www.scienceforums.net/topic/83156-exotic-pumping-cycles-for-rocket-engines/#entry922521
and I found kinetic data at Nist, where else:
http://kinetics.nist.gov/kinetics/Detail?id=1956SHA/PAV811:1

Unexpectedly, methane would be in equilibrium with graphite (and hydrogen, ethane) even at room temperature, in amounts small but perceivable for a clean duct. Only the slow reaction makes this unobservable. Nist displays the results of several (hence inconsistent) kinetic studies. According to the data I chose, 16kg methane would deposit 10g "decomposition products" in 300s at 710°C.

Many more reaction kinetics (not only decompositions) are available at Nist
http://kinetics.nist.gov/kinetics/index.jsp
including for cyclopropane and spiropentane, which outperform methane at identical engine
http://kinetics.nist.gov/kinetics/Detail?id=1961FAL/HUN609-611:1
http://kinetics.nist.gov/kinetics/Detail?id=1972FLO/GIB548:1
making an evolved methane engine unnecessary.
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