64g of oxygen reacts completely with methane gas to form 44g of carbon dioxide gas and 36 g of water vapour. Calculate the amount of methane that takes part in the reaction .
CH4+ 2O2 >>> 2H2O + CO2
so for each two moles of Oxyen, you use one mole of CH4 and it yields 2moles H2O + one mole of CO2
YOu got 44 grams of CO2, which is one mole.
You got 36 grams of H2O, which is 2 moles
So you needed two moles of oxygen, or 64 grams, which you used.
So you must have used one mole of CH4, which is 16 grams.
To calculate the amount of methane that takes part in the reaction, we need to use the concept of stoichiometry, which relates the amounts of substances in a chemical reaction.
First, let's write the balanced chemical equation for the reaction:
CH4 + 2O2 -> CO2 + 2H2O
According to the balanced equation, 1 molecule of methane (CH4) reacts with 2 molecules of oxygen (O2) to produce 1 molecule of carbon dioxide (CO2) and 2 molecules of water (H2O).
Next, let's calculate the number of moles for each substance involved using the given masses:
Mass of oxygen (O2) = 64g
Mass of carbon dioxide (CO2) = 44g
Mass of water (H2O) = 36g
To calculate the number of moles, we divide the mass of each substance by its molar mass:
Molar mass of oxygen (O2) = 32g/mol (16g/mol x 2)
Molar mass of carbon dioxide (CO2) = 44g/mol
Molar mass of water (H2O) = 18g/mol (2g/mol x 2 + 16g/mol)
Number of moles of oxygen (O2) = Mass / Molar mass = 64g / 32g/mol = 2 moles
Number of moles of carbon dioxide (CO2) = Mass / Molar mass = 44g / 44g/mol = 1 mole
Number of moles of water (H2O) = Mass / Molar mass = 36g / 18g/mol = 2 moles
Since methane (CH4) is the limiting reactant, we can use the stoichiometric ratio to determine the number of moles of methane:
From the balanced equation, 1 mole of methane reacts with 2 moles of oxygen (O2) to produce 1 mole of carbon dioxide (CO2) and 2 moles of water (H2O).
Thus, to produce 1 mole of carbon dioxide (CO2), we need 1 mole of methane.
Therefore, the amount of methane that takes part in the reaction is 1 mole.
Note: This assumes that the reaction proceeds with complete conversion and no other reactants or side reactions occur.