First a balanced chemical equation is needed.
CH4 + 2O2 -> CO2 + 2H2O
There is a 1:1 ratio of moles between methane and carbon dioxide so the amount of moles of methane used is the exact number of moles of carbon dioxide yielded.
To determine the number of moles of methane we take the amount used and divide by methane's mass which is about 16.04 g/mol.
100g/ 16.04g/mol=6.234moles of methane.
6.234 moles of methane are used and 6.234 moles of carbon dioxide are produced.
When methane is burned in oxygen, assuming complete combustion, the products are carbon dioxide and water.
Oxygen is NOT a PRODUCT (it is not produced) from the complete combustion of methane, it is a REACTANT (it is used in the reaction). The answer is therefore a mass of zero.
According to Lavoisier: Mass reactants [total in] = mass products [total out] x g Methane + 32 g oxygen = 22 g carbon dioxide + 18 water x + 32 = 22 + 18 = 40 x = 40 - 32 = 8 g methane
When methane undergoes complete combustion, the equation for the reaction is CH4 + 2 O2 -> CO2 + 2 H2O. This shows that the number of moles of carbon dioxide formed are the same as the number of moles of methane reacted, so that 14 moles of carbon dioxide will be formed from 14 moles of methane.
Burning methane releases only carbon dioxide and water.
The answer is 24,15 g.
Burning 2 700 g of methane produce 70406 g of carbon dioxide.
1/2 liter of carbon dioxide
When carbon is burnt, Carbon Dioxide only is produced. When methane is burnt, both carbon dioxide and water are produced.
When methane is burned in oxygen, assuming complete combustion, the products are carbon dioxide and water.
Combustion of metals forms metal oxides. Combustion of hydrocarbons, like methane, forms carbon dioxide and water.
The complete combustion of any hydrocarbon, including methane, produces one water molecule for each two atoms of hydrogen in the hydrocarbon. The formula of methane is CH4; therefore, the complete combustion of one mole of methane produces two moles of H2O.
CH4 + 2O2 → CO2 + 2H2O + Energy (Heat) Methane + Oxygen → Carbon Dioxide + Water and Energy (Heat)
A non luminous flame is produced when the air valve is opened enough to allow complete combustion of the methane gas.
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.
When an organic molecule such as methane or ethanol undergoes complete combustion (in the presence of oxygen) it produces Carbon dioxide and water.
A non luminous flame is produced when the air valve is opened enough to allow complete combustion of the methane gas.