Three parts.
1. Balanced equation.
CH4 + 2O2 --> CO2 + 2H2O
2. Find moles methane with...PV = nRT ( Standard temp. = 298.15 K and standard pressure = 1.00 atmosphere )
(1.00 atm)(10.5 L) = n(0.08206 L*atm/mol*K)(298.15 K)
= 0.4292 moles CH4
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3. Run the stoichiometry.
0.4292 moles CH4 (2 moles H2O/1 mole CH4)(18.016 grams/1 mole H2O)
= 15.5 grams water produced
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The molar heat of combustion of methane (890 kJ/mol) is higher than that of water gas (525 kJ/mol)
== Methane is the simplest hydrocarbon with the molecular formula CH4. Methane could be produced from electricity of renewable energies. Methane can be stored more easily than hydrogen and the transportation, storage and combustion infrastructure are mature (pipelines, gasometers, power plants). As hydrogen and oxygen are produced in the electrolysis of water, : 2H2O → 2H2 + O2 hydrogen would then be reacted with carbon dioxide in Sabatier process, producing methane and water. : CO2 + 4H2 → CH4 + 2H2O Methane would be stored and used to produce electricity later. Produced water would be recycled back to the electrolysis stage, reducing the need for new pure water. In the electrolysis stage oxygen would also be stored for methane combustion in a pure oxygen environment in an adjacent power plant, eliminating e.g. nitrogen oxides. In the combustion of methane, carbon dioxide and water are produced. : CH4 + 2O2 → CO2 + 2H2O Produced carbon dioxide would be recycled back to boost the Sabatier process and water would be recycled back to the electrolysis stage. The carbon dioxide produced by methane combustion would be turned back to methane, thus producing no greenhouse gases. Methane production, storage and adjacent combustion would recycle all the reaction products, creating a cycle. Source www.wikipedia.com
All four C-H bonds in methane are broken during combustion.
CH4 + 2O2 → CO2 + 2H2O + Energy (Heat) Methane + Oxygen → Carbon Dioxide + Water and Energy (Heat)
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.
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 carbon is burnt, Carbon Dioxide only is produced. When methane is burnt, both carbon dioxide and water are produced.
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.
The molar heat of combustion of methane (890 kJ/mol) is higher than that of water gas (525 kJ/mol)
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.
== Methane is the simplest hydrocarbon with the molecular formula CH4. Methane could be produced from electricity of renewable energies. Methane can be stored more easily than hydrogen and the transportation, storage and combustion infrastructure are mature (pipelines, gasometers, power plants). As hydrogen and oxygen are produced in the electrolysis of water, : 2H2O → 2H2 + O2 hydrogen would then be reacted with carbon dioxide in Sabatier process, producing methane and water. : CO2 + 4H2 → CH4 + 2H2O Methane would be stored and used to produce electricity later. Produced water would be recycled back to the electrolysis stage, reducing the need for new pure water. In the electrolysis stage oxygen would also be stored for methane combustion in a pure oxygen environment in an adjacent power plant, eliminating e.g. nitrogen oxides. In the combustion of methane, carbon dioxide and water are produced. : CH4 + 2O2 → CO2 + 2H2O Produced carbon dioxide would be recycled back to boost the Sabatier process and water would be recycled back to the electrolysis stage. The carbon dioxide produced by methane combustion would be turned back to methane, thus producing no greenhouse gases. Methane production, storage and adjacent combustion would recycle all the reaction products, creating a cycle. Source www.wikipedia.com
Natural gas is mainly composed of methane. When methane undergoes combustion, it produces water and CO2 . CH4 + 2O2 -------> CO2 + 2H2O
All four C-H bonds in methane are broken during combustion.
All four C-H bonds in methane are broken during combustion.
Natural gas is mainly composed of methane. When methane undergoes combustion, it produces water and CO2 . CH4 + 2O2 -------> CO2 + 2H2O
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.