In all combustion reactions (other than H2 with O2) CO2(g) and H2O(g) will be produced. CO would NOT be produced, as we are talking about COMPLETE combustion.
Why can't the products be in a form of an oxide and a compound gas?
More oxygen is used in a complete combustion.
carbon dioxide
h2o-water and co2 carbon dioxide
Complete combustion of a hydrocarbon yields carbon dioxide & water; incomplete combustion yields carbon monoxide & water. By having excess oxygen you have enough oxygen to ensure complete combustion. For example the combustion of methane (CH4):complete combustion: CH4 + 2O2 --> CO2 + 2H2Oincomplete combustion: CH4 + 1.5O2 --> CO + 2H2OAs you can see you need a 1/2 mole less of oxygen for the incomplete combustion of methane. So as long as you have twice the amount (in terms of moles) of oxygen as methane you will ensure complete combustion. So anything in excess of that will also ensure complete combustion.
Ideally, complete combustion. In practice it isn't always, which is why cars have catalytic converters.
non combustible inorganic matters
Water and carbon are byproducts of combustion. Its all good...
water vapour and carbon products of combustion.
There are two main types of combustion. These are complete, in which the reactant burns in oxygen producing a few reactions, such as carbon dioxide and water. Incomplete combustion occurs when there is not enough oxygen to complete a reaction.
More oxygen is used in a complete combustion.
carbon dioxide
carbon dioxide and water.
h2o-water and co2 carbon dioxide
Complete combustion of a hydrocarbon yields carbon dioxide & water; incomplete combustion yields carbon monoxide & water. By having excess oxygen you have enough oxygen to ensure complete combustion. For example the combustion of methane (CH4):complete combustion: CH4 + 2O2 --> CO2 + 2H2Oincomplete combustion: CH4 + 1.5O2 --> CO + 2H2OAs you can see you need a 1/2 mole less of oxygen for the incomplete combustion of methane. So as long as you have twice the amount (in terms of moles) of oxygen as methane you will ensure complete combustion. So anything in excess of that will also ensure complete combustion.
three
Ideally, complete combustion. In practice it isn't always, which is why cars have catalytic converters.
The unsaturated hydrocarbons are mor tangled up so it's harder for the oxygen to get in and break the bonds. Because of this some large sections of the hydrocarbon floats up before being broken, making the flame sooty.