What is formed during the incomplete oxidation of methane in a limited supply of air?

When methane (CH₄) undergoes oxidation, the product formed depends on the amount of oxygen available. In a limited supply of air, oxidation does not proceed completely to carbon dioxide and water. Instead, methane is partially oxidized to methanol (CH₃OH). This process is called incomplete oxidation or partial oxidation of methane.

The chemical equation for this reaction is:
CH₄ + ½O₂ → CH₃OH

In this reaction, oxygen is not enough to completely oxidize carbon into carbon dioxide. Therefore, the oxidation stops at an intermediate stage, producing methanol. Under controlled industrial conditions, this partial oxidation is a valuable process because methanol is an important chemical used as a fuel, solvent, and raw material in various organic syntheses.

If methane were burned in an excess supply of air, it would be completely oxidized to carbon dioxide and water:
CH₄ + 2O₂ → CO₂ + 2H₂O

However, when oxygen is restricted, oxidation occurs only partially, forming CH₃OH or sometimes carbon monoxide (CO) and hydrogen gas (H₂) under different temperature and catalyst conditions.

This reaction is significant in industrial organic chemistry, where methane serves as a feedstock for methanol production through catalytic oxidation using metals like copper or molybdenum at moderate temperatures. Methanol obtained this way is a key intermediate in the production of formaldehyde, acetic acid, and other organic compounds.

Thus, during incomplete oxidation of methane in limited air, methanol (CH₃OH) is the main product formed — a controlled oxidation result important for both energy and chemical industries