What is the mass of carbon dioxide if 100 grams of methane is oxidized to carbon dioxide and water?
Follow the steps of this example.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To determine the mass of carbon dioxide produced when 100 grams of methane is oxidized, we need to understand the chemical equation for the reaction and the molar masses of the compounds involved.
The balanced chemical equation for the reaction is:
CH4 + 2O2 → CO2 + 2H2O
From the equation, we see that one mole of methane (CH4) reacts to form one mole of carbon dioxide (CO2).
The molar mass of methane (CH4) is approximately 16 g/mol, and the molar mass of carbon dioxide (CO2) is approximately 44 g/mol.
Now, we can calculate the mass of carbon dioxide produced:
1. Calculate the number of moles of methane:
moles of CH4 = mass of CH4 / molar mass of CH4
mass of CH4 = 100 grams
molar mass of CH4 = 16 g/mol
moles of CH4 = 100 / 16 ≈ 6.25 moles
2. Since one mole of methane produces one mole of carbon dioxide, the number of moles of carbon dioxide formed will be the same:
moles of CO2 = moles of CH4 = 6.25 moles
3. Calculate the mass of carbon dioxide using the number of moles and the molar mass of CO2:
mass of CO2 = moles of CO2 * molar mass of CO2
moles of CO2 = 6.25 moles
molar mass of CO2 = 44 g/mol
mass of CO2 = 6.25 * 44 = 275 grams
Therefore, the mass of carbon dioxide produced when 100 grams of methane is oxidized is 275 grams.