Methane is CH4. Combustion is CH4 + 2O2 ==> CO2 + 2H2O1 mole CH4 produces 2 moles H2O
moles CH4 used = 1.1x10^-3 g x 1 mole/16 g = 6.875x10^-5 moles
moles H2O produced = 6.875x10^-5 moles CH4 x 2 moles H2O/mole CH4 = 1.375x10^-4 moles
mass H2O produced = 1.375x10^-4 moles x 18 g/mole = 2.475x10^-3 g = 2.48 mg (3 sig.figs)
9.98 * 10^(-3)
hell if i know
The answer is 11,7 g.
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
The standard enthalpy of combustion for methane is -890 kJ/mol.
When methane is burned in oxygen, assuming complete combustion, the products are carbon dioxide and water.
First a balanced chemical equation is needed.CH4 + 2O2 -> CO2 + 2H2OThere 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.
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.
1.28mol