What mass of carbon dioxide is produced from the complete combustion of 2.50×10−3 of methane?
To determine 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 for every mole of methane (CH4) combusted, we get one mole of carbon dioxide (CO2) as the product.
Step 1: Convert the given quantity of methane to moles.
Given: 2.50×10^−3 moles of methane
Step 2: Multiply the moles of methane by the mole ratio of methane to carbon dioxide, which is 1:1, as indicated by the balanced equation. This will give us the moles of carbon dioxide.
Moles of carbon dioxide = Moles of methane
Step 3: Calculate the molar mass of carbon dioxide (CO2).
Carbon has a molar mass of 12.01 g/mol, and oxygen has a molar mass of 16.00 g/mol. Adding these together gives us a molar mass of 12.01 + (16.00 x 2) = 44.01 g/mol for carbon dioxide.
Step 4: Multiply the moles of carbon dioxide by the molar mass to get the mass of carbon dioxide.
Mass of carbon dioxide = Moles of carbon dioxide x Molar mass of carbon dioxide
Let's plug in the given values and calculate the answer.
Moles of methane = 2.50×10^−3 moles
Moles of carbon dioxide = 2.50×10^−3 moles
Molar mass of carbon dioxide = 44.01 g/mol
Mass of carbon dioxide = (2.50×10^−3 moles) x (44.01 g/mol)
Mass of carbon dioxide = 0.1100 g
Therefore, the mass of carbon dioxide produced from the complete combustion of 2.50×10^−3 moles of methane is 0.1100 grams.
This is a simple (as opposed to a limiting reagent) stoichiometry problem. Here is a worked example of a stoichiometry problem. Just follow the steps.
http://www.jiskha.com/science/chemistry/stoichiometry.html
Post your work if you run into trouble.