If 100g of Methane are burned in this reaction to cook my dinner, How many moles of Carbon dioxide are produced?
6.25 mol
To determine the number of moles of carbon dioxide produced when 100 grams of methane (CH4) are burned, we need to use the molar mass of methane and the stoichiometry of the reaction.
Step 1: Find the molar mass of methane (CH4).
- Carbon (C) has a molar mass of approximately 12.01 g/mol.
- Hydrogen (H) has a molar mass of approximately 1.01 g/mol.
The molar mass of methane (CH4) is:
(1 mol of C) + (4 mol of H) = 12.01 g/mol + (4 * 1.01 g/mol) = 16.05 g/mol.
Step 2: Calculate the number of moles of methane.
Using the formula:
Number of moles = Mass / Molar mass.
We divide the mass (100 g) by the molar mass of methane (16.05 g/mol):
Number of moles of methane = 100 g / 16.05 g/mol = 6.22 mol (rounded to two decimal places).
Step 3: Determine the stoichiometry of the reaction.
The balanced chemical equation for the combustion of methane is:
CH4 + 2O2 -> CO2 + 2H2O.
From this equation, we can see that 1 mole of methane produces 1 mole of carbon dioxide (CO2).
Step 4: Calculate the number of moles of carbon dioxide produced.
Since 1 mole of methane produces 1 mole of carbon dioxide, the number of moles of carbon dioxide will be the same as the number of moles of methane:
Number of moles of carbon dioxide = 6.22 mol.
Therefore, when 100 grams of methane are burned, 6.22 moles of carbon dioxide are produced.