Assuming no change in temperature and pressure, calculate the
volume of O2 (in liters) required for the complete combustion of
14.9 L of butane (C4H10):
The problem with this question is that you did not provide any solutions, as stated, to calculate the freezing point for.
Assuming you have given a complete equation, no. It requires oxygen as a reactant and will always have CO2 and H2O as products. Plus, combustion reactions typically involve carbon based elements as reactants.
The mass of carbon dioxide is 878 g.
Out of one mole C3H8 three moles carbondioxide (CO2) are formed by complete combustion of it.So 2.13 mole C3H8 make 3*2.13 mole CO2 = 6.39 moleCO2
The complete combustion of organic compounds produces Carbon Dioxide (CO2), Water (H2O), and a residue of any impurities which were present in the coal before combustion. Complete combustion requires a great surplus of molecular Oxygen to occur.
Assuming complete combustion, the products are carbon dioxide and water.
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You would be producing carbon dioxide and water vapor, assuming that it is a complete combustion. If a partial combustion is in occurrence, carbon monoxide would also exist.
More oxygen is used in a complete combustion.
The problem with this question is that you did not provide any solutions, as stated, to calculate the freezing point for.
Assuming you have given a complete equation, no. It requires oxygen as a reactant and will always have CO2 and H2O as products. Plus, combustion reactions typically involve carbon based elements as reactants.
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.
The mass of carbon dioxide is 878 g.
Out of one mole C3H8 three moles carbondioxide (CO2) are formed by complete combustion of it.So 2.13 mole C3H8 make 3*2.13 mole CO2 = 6.39 moleCO2
Ideally, complete combustion. In practice it isn't always, which is why cars have catalytic converters.
If the combustion is complete, carbon dioxide and water.
The complete combustion of organic compounds produces Carbon Dioxide (CO2), Water (H2O), and a residue of any impurities which were present in the coal before combustion. Complete combustion requires a great surplus of molecular Oxygen to occur.