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Methanol is made from methane (natural gas) in a series of three reactions: Steam reforming CH 4 + H 2 O → CO + 3 H 2 Δ r H = +206 kJ mol −1 Water shift reaction CO + H 2 O → CO 2 + H 2 Δ r H = -41 kJ mol −1 Synthesis 2 H 2 + CO → CH 3 OH Δ r H = -92 kJ mol −1. The methanol thus formed may be converted to gasoline by the Mobil ...
Steam reforming or steam methane reforming (SMR) is a method for producing syngas (hydrogen and carbon monoxide) by reaction of hydrocarbons with water. Commonly, natural gas is the feedstock. The main purpose of this technology is often hydrogen production , although syngas has multiple other uses such as production of ammonia or methanol .
Methanol (also called methyl alcohol and wood spirit, ... Methanol is more easily oxidized than is the feedstock methane, so the reactions tend not to be selective ...
Autothermal reforming (ATR) uses oxygen and carbon dioxide or steam in a reaction with methane to form syngas. The reaction takes place in a single chamber where the methane is partially oxidized. The reaction is exothermic due to the oxidation. When the ATR uses carbon dioxide the H 2:CO ratio produced is 1:1; when the ATR uses steam the H 2 ...
Steam reforming of methane is an endothermic reaction requiring 206 kJ/mol of methane: CH 4 + H 2 O → CO + 3 H 2. In principle, but rarely in practice, biomass and related hydrocarbon feedstocks could be used to generate biogas and biochar in waste-to-energy gasification facilities. [7]
Partial oxidation of methane to methanol (C H 3 O H), a more convenient, liquid fuel, is challenging because the reaction typically progresses all the way to carbon dioxide and water even with an insufficient supply of oxygen. The enzyme methane monooxygenase produces methanol from methane, but cannot be used for industrial-scale reactions. [19]
The foremost challenge in catalytic oxidation is the conversion of methane to methanol. Most methane is stranded, i.e. not located near metropolitan areas. Consequently, it is flared (converted to carbon dioxide). One challenge is that methanol is more easily oxidized than is methane. [3]
However, when applying this method to methane specifically, the gaseous nature of methane requires an appropriate solvent. Reactions with other alkanes usually have the alkane in question be the solvent itself; however, any C-H bond with a lower BDE or higher polarity than methane will react first and prevent methane functionalization.