Question

How does the redox reaction of burning methane work?

Answer 1

We know that combustion, or burning, is a high-temperature exothermic redox chemical reaction between a fuel and an oxidant, usually atmospheric oxygen, that produces oxidized, often gaseous products, in a mixture termed as smoke.

Complete step by step solution:
We have been asked for all the oxidation-reduction reactions for burning methane which is a combustion reaction. So, for that, Combustion is the scientific word for burning. In a combustion reaction a substance reacts with oxygen from the air and transfers energy to the surroundings as light and heat. The products of a combustion reaction are called oxides.
$C{{H}_{4}}+2{{O}_{2}}\to C{{O}_{2}}+2{{H}_{2}}O$
Methane burns in the presence of oxygen to produce carbon dioxide and water. This process of combustion releases energy. When energy is water released during the course of a chemical reaction, it is said to be an exothermic reaction. The oxidation number of elemental Carbon and oxygen are ZERO each.
The oxidation number of $C$ in is $-4,$ and that in $+4,$ So, carbon is getting oxidized, The oxidation number of $O$ in is ZERO and that in is $-2,$ So, oxygen is getting reduced. Of course, this approach would be totally impractical to do for standard combustion reactions.

Note:
Remember that redox is a type of chemical reaction in which the oxidation states of atoms are changed. Redox reactions are characterized by the actual or formal transfer of electrons between chemical species, most often with one species undergoing oxidation while another species undergoes reduction.