What mass of Carbon dioxide is produced from the complete combustion of 4.60x10^-3g of methane?
What’s the answer?
To find the mass of carbon dioxide produced from the complete combustion of methane, we need to use the balanced chemical equation for the combustion of methane.
The balanced equation is:
CH4 + 2O2 -> CO2 + 2H2O
From the equation, we can see that one mole of methane (CH4) reacts with two moles of oxygen (O2) to produce one mole of carbon dioxide (CO2) and two moles of water (H2O).
The molar mass of methane (CH4) is 16.04 g/mol, and the molar mass of carbon dioxide (CO2) is 44.01 g/mol.
To solve the problem, we will follow these steps:
Step 1: Convert the mass of methane given (4.60x10^-3g) to moles.
Number of moles = Mass / Molar mass
= 4.60x10^-3g / 16.04 g/mol
Step 2: Use the stoichiometry of the balanced equation to determine the moles of carbon dioxide produced.
From the balanced equation, we can see that the ratio of moles of methane to moles of carbon dioxide is 1:1. Therefore, the moles of carbon dioxide produced will be equal to the moles of methane.
Step 3: Convert the moles of carbon dioxide to mass.
Mass = moles of carbon dioxide x Molar mass
= moles of methane x 44.01 g/mol
Let's calculate it:
Step 1: Convert the mass of methane to moles.
Number of moles = 4.60x10^-3g / 16.04 g/mol
= 2.867x10^-4 mol
Step 2: The moles of carbon dioxide produced will be equal to the moles of methane.
Moles of carbon dioxide = 2.867x10^-4 mol
Step 3: Convert the moles of carbon dioxide to mass.
Mass = 2.867x10^-4 mol x 44.01 g/mol
= 0.0126 g
Therefore, the mass of carbon dioxide produced from the complete combustion of 4.60x10^-3g of methane is 0.0126 grams.
CH4 + 2O2 ==> CO2 + 2H2O
mols CH4 = grams/molar mass
Using the coefficients in the balanced equation, convert mols CH4 to mols CO2.
Now convert mols CO2 to grams. g = mols x molar mass.