Methane: Difference between revisions
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JeffEvarts (talk | contribs) (Created page with "{{Compound|name=Methane|chemf=CH4|mm=16|density=0.6556|ss=446|nfpa_h=1|nfpa_f=4|mp=-182|bp=-164|stp_p=gas|stp_q=clear, odorless|fv=47.1}} ==Uses== ===Primary=== * Definitive '...") |
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{{Compound| | {{Compound|nowa=yes|chemf=CH4|mm=16|density=0.6556|ss=446|nfpa_h=1|nfpa_f=4|mp=-182|bp=-164|stp_p=gas|stp_q=clear, odorless|fv=47.1}} | ||
==Uses== | ==Uses== | ||
===Primary=== | ===Primary=== | ||
Latest revision as of 17:55, 18 October 2023
| Chemical formula | CH4 |
|---|---|
| OTP appearance | clear, odorless gas |
| Molar Mass(g/mol) | 16 |
| Density(g/cc) | 0.6556 |
| Melting Point(°C) | -182 |
| Boiling Point(°C) | -164 |
| Fuel Value(MJ/kg) | 47.1 |
| Speed of sound 20°C, 1atm (m/s) |
446 |
| NFPA 704 |  4
1
0
|
Uses
Primary
- Definitive C1 compound
- Feedstock for chloromethane production or methanol
Other
- Fuel
- Feedstock for producing hydrogen.
Natural occurrence
- Methane occurs naturally in the presence of decaying biological materials.
- 1kg biowaste through a digester (10-40 days) produces 1m3 of methane ~= 6kWh = 21.6MJ
Hazards
- Fire and explosion
- Asphyxiant
Production
Extraction
Biologic
Anaerobic decomposition of biowaste in a digester results in the production of methane.
Synthesis
alkali degradation
- Combine sodium acetate and sodium hydroxide
- CH3COONa + NaOH{CH4 + Na2CO3heat}→
- CH3COONa + NaOH
- Combine propanone and calcium hydroxide
- C3H6O + Ca(OH)2 → 2 CH4 + CaCO3
hydrogenation
of carbon monoxide
The Sabatier reaction hydrogenates carbon monoxide as feedstock and produces water as well as methane.
- CO + 2 H2{NiCH4 + H2O1atm, 200-300°C}→
of carbon dioxide
Similar to Sabatier (above), hydrogenation of carbon dioxide produces water as well as methane
- CO2 + 4 H2{NiCH4 + 2 H2O1atm, 200-300°C}→
- Urushibara nickel is a popular choice of catalyst, at temperatures of 350°C and above atmospheric pressure
- The reaction can be carried out at OTP using Ruthenium oxide / Titanium oxide catalysts, particularly with photoexcitation.[1]
of hydrocarbons
Larger hydrocarbons can be hydrogenated (usually over a catalyst like Urushibara nickel) into methane:
- Acetylene
- HCCH + 3 H2 → 2 CH4
- Pentane
- C5H12 + 4 H2 → 5 CH4
See also
- Compost
- Lunde, Peter J.; Kester, Frank L. "KINETICS OF CARBON DIOXIDE METHANATION ON A RUTHENIUM CATALYST"
Hamilton Standard
link courtesy Argonne National Laboratory.
References
- ↑ Ravindranathan Thampi, K; Kiwi, John; Grätzel, Michael (1987) "Methanation and photo-methanation of carbon dioxide at room temperature and atmospheric pressure".
Nature 327; pp506-508.
DOI:10.1038/327506a0