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Why does excess supply of oxygen lead to complete combustion?

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.


What is the main product of complete combustion?

The main products of complete combustion are carbon dioxide (CO2) and water (H2O).


What do you call the heat released when 1 mole of a substance undergoes complete combustion?

You think probable to molar heat, expressed in J/mol.


Is more oxygen used in an incomplete combustion than a complete combustion?

Yes, more oxygen is used in incomplete combustion compared to complete combustion because incomplete combustion results in the partial burning of the fuel, leading to the formation of more byproducts like carbon monoxide and soot. This requires additional oxygen to combine with these byproducts, using up more oxygen overall.


The two by-products of complete combustion are?

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?

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Why does excess supply of oxygen lead to complete combustion?

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.


What are the products of combustion for coal and petroleum?

Complete combustion will result in the production of CO2 and H2O.


How can you tell that complete combustion has not occurred?

Complete combustion is very hard to obtain, unless you have nearly perfect conditions and little cause for error.