What mass of carbon dioxide is produced from the complete combustion of 8.20×10−3 g of methane?
To find the mass of carbon dioxide produced from the combustion of methane, we need to use the stoichiometry of the balanced chemical equation.
The balanced equation for the combustion of methane (CH4) is:
CH4 + 2O2 → CO2 + 2H2O
From this equation, we can see that 1 mole of methane produces 1 mole of carbon dioxide.
First, let's determine the molar mass of methane (CH4). Carbon has a molar mass of 12.01 g/mol, and hydrogen has a molar mass of 1.01 g/mol. Adding these up, we have:
(12.01 g/mol) + 4(1.01 g/mol) = 16.05 g/mol
Now, we can calculate the number of moles of methane:
moles of CH4 = mass of CH4 / molar mass of CH4
= 8.20×10^-3 g / 16.05 g/mol
Next, using the stoichiometry of the balanced equation, we can determine the number of moles of carbon dioxide produced. Since the stoichiometric coefficient of CH4 for CO2 is 1:1, the moles of carbon dioxide produced will be the same as the moles of methane.
moles of CO2 = moles of CH4
Finally, we can calculate the mass of carbon dioxide produced:
mass of CO2 = moles of CO2 x molar mass of CO2
The molar mass of carbon dioxide (CO2) is:
(12.01 g/mol) + 2(16.00 g/mol) = 44.01 g/mol
Therefore:
mass of CO2 = moles of CO2 x molar mass of CO2
= moles of CH4 x molar mass of CO2
= (8.20×10^-3 g / 16.05 g/mol) x 44.01 g/mol
Calculate this expression to find the mass of carbon dioxide produced from the combustion of 8.20×10^-3 g of methane.
Here is a sample problem I posted for simple stoichiometry problems.
http://www.jiskha.com/science/chemistry/stoichiometry.html