# How does a combustion process produce carbon monoxide?

My question is in the context of combustion heater safety- I want to identify the mechanism by which CO is produced, and hopefully have additional understanding, and clues to the warning signs, to identify unsafe stoves or installations. The primary safety measures will always be CO detectors and good ventilation.

The worst horror stories usually concern charcoal barbecues in confined spaces- solid carbon burning at about 900 °C. Is it a safe educated guess that the main combustion product here is CO, which fails to burn fully to CO2 in depleted oxygen levels? Or is a more complex process at work?

How does the yellow combustion of an oil or gas flame produce CO? Is it a simple matter of poor gas flow in the flue, and depleted oxygen in the feed air?

Thanks for any help

• That's right, it is ultimately a matter of incomplete combustion due to the lack of oxygen. – Ivan Neretin Oct 17 '17 at 14:18
• CO2+C->2CO, kind of a comproportionation reaction. – Ariana Oct 17 '17 at 16:25
• Since your question is in "the context of heater safety", you might get a more specific and relevant answer if you briefly described the nature of the heater of interest and the environment in which it operates. – airhuff Oct 17 '17 at 20:37
• @airhuff Good point. A bit more context- my primary interest is in outdoor burners, with a slight twist in that I burn wood to charcoal for use as biochar. On the strength of this, I'm being approached for advice from residents of an Off-Grid intentional community on installation and operation of wood-burning stoves to heat cabins- advice which I'm not really experienced to give. I don't want anyone gassed or cremated because of my advice or lack of it, so the best I can do is learn to spot installations that are really dangerous, and why, before they get lit up in the cold weather. – Brian Hughes Oct 17 '17 at 21:20

If combustion occurs in oxygen, (at least) the following reactions are relevant: $$\ce{C + O2 -> CO2}$$ $$\ce{C + 1/2 O2 -> CO}$$
You can favor the first reaction by having more oxygen in the gas phase, since it required twice $\ce{O2}$ as the first.
However, one of the most important factors is the temperature: high temperature always favors the $\ce{CO}$ product, since reaction wants to proceed fast and react with any available oxygen. You can clearly see these dependences in the Figure 6 of this article, at low temperatures the CO/CO2 ratio is low, but quickly increases by heating.