The result will be 1 m3 of CO2 and 2 m3 of H2O gas (and 2 m3 of O2 will be consumed).
This is determined by the stoichiometry of the balanced reaction:
CH4 + 2O2 ---> CO2 + 2H2O
Convert this mass of methane to moles. Then set up the balanced equation for the combustion of methane. It should be easy from there to see how many moles of carbon dioxide are produced and convert back to grams.
There is one carbon atom in one molecule.So one molecule of CO2 is produced.
it look's like 950 g/kWh for gas is the CO2 figure.
o,oo6 g carbon dioxide are obtained.
about 2, (1/.5091)
approx 1.96 kg CO2/m3 methane
Approx. 1,8 kg.
23.456 g
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.
The molecule of methane has 5 atoms.
methane and oxygen react together (combustion) to give carbon dioxide + water. The reactants are methane and oxygen which react to form the products water and carbon dioxide.
Methane (CH4) is composed of one atom of carbon and four atoms of hydrogen, a total of five.
The combustion of methane can be balanced in the following manner. One molecule of CH4 plus two molecules of O2 produces one molecule of CO2 plus one molecule of H2O.
2
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.
Molecules are representative particles of a covalent (or molecular) compound. Examples: water, ammonia, methane, carbon dioxide, chlorine gas, sulfur 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.
Methane is practically the same as natural gas. When 1 molecule of methane (CH4) is burnt in oxygen it produces 1 molecule of carbon dioxide (CO2) and two molecules of water (H2O). If the methane is NOT burnt it causes twenty times more damage as a greenhouse gas than carbon dioxide. (So keep lighting those farts!)
one methane molecule plus two oxygen (gas) molecules yields one carbon dioxide molecule plus 2 water molecules.
methane + oxygen -> carbon dioxide + water 2 Methane molecules plus 4 Oxygen molecules gives 2 molecules of Carbon dioxide plus 4 Water molecules.
There are five main gases produced by greenhouses: water vapor, carbon dioxide, methane, nitrous oxide, and ozone.
When carbon is burnt, Carbon Dioxide only is produced. When methane is burnt, both carbon dioxide and water are produced.
They only affect water in a negative way. CH4 + 2O2 → CO2 + 2H2O For methane there are two molecules of water produced for every molecule of carbon dioxide. Methane affects water since methane attracts microbes that consumes Oxygen. So the methane and microbe level rise and can create a situation where there is so little oxygen that hardly anything can survive.
water
There have been learned people who have asserted this is not possible. There have been others who assert that it is. I am one of the later. Please consider this: Suppose you build a generating plant that burns methane gas leaking from a landfill to produce electricity. It burns methane against atmospheric oxygen to produce carbon dioxide and water. For each molecule of methane used, there is one molecule of carbon dioxide produced. Each molecule of methane is 37 times as powerful as carbon dioxide as a global warming gas. Therefore, the burning of methane that would otherwise be released reduces global warming, giving the process a negative carbon footprint. In fairness, I should point out that for each molecule of methane, there will be two atoms of water, in addition to the carbon dioxide, in the output. Water vapor is also a greenhouse gas. But the water produced would can be condensed immediately without any environmental effect, so I am not considering it in the calculation.