How many grams of carbon dioxide will be made when 100 grams of methane burn in an excess of oxygen
Here is an example of a stoichiometry problem. Just follow the steps.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To calculate the number of grams of carbon dioxide produced when methane (CH4) burns in an excess of oxygen (O2), we need to follow these steps:
1. Write and balance the chemical equation for the combustion reaction of methane:
CH4 + 2O2 → CO2 + 2H2O
The balanced equation shows that one mole of methane reacts with two moles of oxygen to produce one mole of carbon dioxide and two moles of water.
2. Calculate the molar mass of methane (CH4):
C = 12.01 g/mol
H = 1.01 g/mol
Molar mass of methane (CH4) = (12.01 g/mol × 1) + (1.01 g/mol × 4) = 16.05 g/mol
3. Determine the number of moles of methane (CH4) in 100 grams:
Number of moles = Mass in grams / Molar mass
Number of moles of CH4 = 100 g / 16.05 g/mol ≈ 6.22 mol
4. Since methane and carbon dioxide are in a 1:1 molar ratio, the number of moles of carbon dioxide produced will be the same as the number of moles of methane burnt. Therefore, 6.22 moles of carbon dioxide will be produced.
5. To calculate the mass of carbon dioxide produced, we need to multiply the number of moles of CO2 by its molar mass. The molar mass of carbon dioxide (CO2) is as follows:
C = 12.01 g/mol
O = 16.00 g/mol
Molar mass of carbon dioxide (CO2) = (12.01 g/mol × 1) + (16.00 g/mol × 2) = 44.01 g/mol
Mass of carbon dioxide = Number of moles × Molar mass = 6.22 mol × 44.01 g/mol ≈ 274.13 grams
Therefore, approximately 274.13 grams of carbon dioxide will be produced when 100 grams of methane burn in an excess of oxygen.