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More oxygen is used in a complete combustion.
Ideally, complete combustion. In practice it isn't always, which is why cars have catalytic converters.
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.
In complete combustion, all the reactants will be converted into carbon dioxide and water. In incomplete combustion, some of the reactants will be converted to carbon dioxide, some will become carbon monoxide, and some may not react at all. Quite often incomplete combustion will result in a "sooty" flame.
If refering to hydrocarbons, complete combustion is carbon dioxide and water. Incomplete combustion may include any other compounds, e.g. carbon, carbon monoxide, aldehydes, acids, peroxides...
More oxygen is used in a complete combustion.
A complete combustion reaction will produce CO2 and H2O, while an incomplete combustion reaction produces CO and H2O.
in complete combustion the amount of oxygen is higher/more than the amount of oxygen in incomplete combustion. Heat needs oxygen.
carbon monoxide. CO is a product resulting as the definition of incomplete combustion. complete combustion yields carbon dioxide, CO2.
Ideally, complete combustion. In practice it isn't always, which is why cars have catalytic converters.
Burning of methane is:CH4 + 2 O2---------- → CO2 + 2 H2OCarbon monoxide is released after an incomplete combustion.
The formation of black soot indicates that the combustion is not receiving enough oxygen and is incomplete. Black soot is made from mainly carbon.
2C2H3OH + 5O2 --> 4CO2 + 4H2O The equation as written appears to be complete combustion, but in reality it probably would not be complete combustion. Usually combustion is incomplete, producing other products such as carbon monoxide and pure carbon (soot).
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.
In complete combustion, all the reactants will be converted into carbon dioxide and water. In incomplete combustion, some of the reactants will be converted to carbon dioxide, some will become carbon monoxide, and some may not react at all. Quite often incomplete combustion will result in a "sooty" flame.
Complete combustion produces carbon dioxide. Incomplete combustion produces carbon monoxide.
If refering to hydrocarbons, complete combustion is carbon dioxide and water. Incomplete combustion may include any other compounds, e.g. carbon, carbon monoxide, aldehydes, acids, peroxides...