0
What else can I help you with?
What happens when Mathane burns in air?
MEthane or CH4 with complete combustion will turn into CO2 and H2O The formula for complete combustion of methane: CH4 + 2O2-> CO2 + 2H2O
Why the combined mass of CO2 and H2O produced in the combustion analysis of methane greater than mass of the methane sample being analysed?
The mass of reactants is equal to the mass of products.
What is the chemical formula for combustion of methane?
CH4 + 2O2 → CO2 + 2H2O + Energy (Heat) Methane + Oxygen → Carbon Dioxide + Water and Energy (Heat)
What does combustion have in common with cellular respiration?
It is same as combustion. O2 is involved and CO2 is produced
What type of reaction is CH4 plus O2 equals CO2 plus H2O?
Hydrocarbons such as methane burning in oxygen is an example of oxidation and also combustion.
What happens when Mathane burns in air?
MEthane or CH4 with complete combustion will turn into CO2 and H2O The formula for complete combustion of methane: CH4 + 2O2-> CO2 + 2H2O
What happens when gas undergoes combustion?
Natural gas is mainly composed of methane. When methane undergoes combustion, it produces water and CO2 . CH4 + 2O2 -------> CO2 + 2H2O
Why the combined mass of CO2 and H2O produced in the combustion analysis of methane greater than mass of the methane sample being analysed?
The mass of reactants is equal to the mass of products.
How many moles of H2O are produced by the complete combustion of methane?
For the complete combustion of methane (CH4), the balanced chemical equation is: CH4 + 2O2 -> CO2 + 2H2O This equation shows that for every mole of methane that reacts, 2 moles of water (H2O) are produced.
What would be produced in a combustion reaction a hydrocarbon hydrogen carbon dioxide oxygen?
In a combustion reaction of a hydrocarbon like methane (CH4) with oxygen, carbon dioxide (CO2) and water (H2O) would be produced. The balanced chemical equation for this reaction would be CH4 + 2O2 → CO2 + 2H2O.
What products are made from combustion of methane?
it produces co2 +2 h2o
What is the chemical equation for the complete and incomplete combustion of methane?
Burning of methane is:CH4 + 2 O2---------- → CO2 + 2 H2OCarbon monoxide is released after an incomplete combustion.
What is the amount of water produced by the combustion of 32grams of methane?
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
What are theses compounds CO2 CO CH4?
These compounds are all gases at room temperature. CO2 is carbon dioxide, a greenhouse gas produced by combustion. CO is carbon monoxide, a toxic gas formed by incomplete combustion. CH4 is methane, a greenhouse gas emitted during natural gas production and livestock digestion.
When methane and oxygen react in a combustion reaction what produces?
When methane and oxygen react in a combustion reaction, carbon dioxide and water are produced, along with heat and light as energy is released. The balanced chemical equation for this reaction is: CH4 + 2O2 → CO2 + 2H2O.
Giving balance equation state how you will convert methane to carbon dioxide?
The balanced equation for the conversion of methane (CH4) to carbon dioxide (CO2) is: CH4 + 2O2 -> CO2 + 2H2O To convert methane to carbon dioxide, you would need to combust methane in the presence of oxygen, which will produce carbon dioxide and water as products.
How many moles of carbon dioxide are produced from the complete combustion of 100.0 grams of methane?
To determine the moles of carbon dioxide produced from the combustion of methane, we first need to balance the chemical equation for the combustion of methane: CH4 + 2O2 → CO2 + 2H2O. From the balanced equation, we see that 1 mole of methane produces 1 mole of carbon dioxide. The molar mass of methane (CH4) is 16.05 g/mol, and the molar mass of carbon dioxide (CO2) is 44.01 g/mol. Therefore, 100.0 grams of methane is equivalent to 100.0 g / 16.05 g/mol = 6.23 moles of methane, which would produce 6.23 moles of carbon dioxide.
