I am not entirely sure I understand your question, but these comments may be useful.

Equilibrium trends: At relatively low temperatures, the primary combustion products are generally the most common and well known species of each atom. In hydrocarbon combustion for example, the products are generally CO2 and H2O. As temperature increases, some species become increasingly unstable. For example, stoichiometrically balanced reactions of most hydrocarbons produce high enough temperatures that first H2O and then CO2 begin to decompose to form some H2 and CO, leaving some O2 unreacted. This leads to the nonintuitive result of having H2 and CO in equilibrium with measurable quantities of O2 at high temperatures. At higher temperatures still, O2 and N2 begin to decompose. Other compounds, such as SO2, NO2, etc. begin to decompose to smaller molecules at temperatures lower than the decomposition temperatures of H2O and CO2.

Kinetic trends: At very low temperatures, kinetics often are so slow that reactants do not reach equilibrium. Therefore, low-temperature combustion of hydrocarbons commonly produces more CO and residual hydrocarbon fuel than would exist at equilibrium, even in overall oxidizing environments, because of relatively low temperatures.

Transport and mixing rates also affect final product distributions.