Chloromethane production
The chloromethane production consumes methane and chlorine gas, and produces Compounds of the form CHxCly where x + y = 4.
Process
Generally, methane and chlorine gasses are mixed at atmospheric pressure, and catalyzed in some way that the chlorine gas disassociates into a Cl+ and a Cl-. The negative chlorine combines with one of the hydrogens on the methane, producing hydrochloric acid. The (now slightly negative) methane remnant attracts the positive chlorine ion and bonds with it. This process can occur multiple times, producing variably chlorinated carbon atoms, resulting in chloromethane, dichloromethane, trichloromethane, and carbon tetrachloride.
The process can be catalyzed by simple heat (at over 400°C the reaction proceeeds at speed) or via exposure to ultraviolet light, which dissociates the chlorine by photonic cleavage.
The products are separated by fractional distillation:
| Compound | Boiling point (°C) |
|---|---|
| CH3Cl | -23.8 |
| CH2Cl2 | 39.6 |
| CHCl3 | 61.15 |
| CCl4 | 76.72 |