1.28mol
MEthane or CH4 with complete combustion will turn into CO2 and H2O The formula for complete combustion of methane: CH4 + 2O2-> CO2 + 2H2O
1/2 liter of 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.
If the oxygen is not sufficient carbon monoxide is produced; this is a frequent cause of deadly intoxication.
The mass of reactants is equal to the mass of products.
The answer is 24,15 g.
A non luminous flame is produced when the air valve is opened enough to allow complete combustion of the methane gas.
A non luminous flame is produced when the air valve is opened enough to allow complete combustion of the methane gas.
A non luminous flame is produced when the air valve is opened enough to allow complete combustion of the methane gas.
A non luminous flame is produced when the air valve is opened enough to allow complete combustion of the methane gas.
Burning 2 700 g of methane produce 70406 g of carbon dioxide.
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.
what is the mass in grams of oxygen, is needed to complete combustion of 6 L of methane?
MEthane or CH4 with complete combustion will turn into CO2 and H2O The formula for complete combustion of methane: CH4 + 2O2-> CO2 + 2H2O
1/2 liter of carbon dioxide
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.
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.