What is the mass of carbon dioxide if 100 grams of methane is oxidized to carbon dioxide and water?

Follow the steps in this worked example.

http://www.jiskha.com/science/chemistry/stoichiometry.html

To calculate the mass of carbon dioxide produced when 100 grams of methane is oxidized, we need to know the balanced chemical equation for the reaction between methane (CH4) and oxygen (O2).

The balanced chemical equation is:

CH4 + 2O2 → CO2 + 2H2O

From the balanced equation, we can see that for every 1 mole of CH4, we obtain 1 mole of CO2. The molecular mass of carbon dioxide (CO2) is approximately 44 grams/mol.

To calculate the mass of carbon dioxide produced, we can use the following steps:

Step 1: Convert the given mass of methane (CH4) to moles.

The molar mass of methane is approximately 16 grams/mol (1 carbon atom + 4 hydrogen atoms).

Moles of CH4 = Mass of CH4 / Molar mass of CH4
Moles of CH4 = 100 g / 16 g/mol
Moles of CH4 ≈ 6.25 mol

Step 2: Calculate the moles of carbon dioxide produced.

Since the balanced equation shows a 1:1 ratio between CH4 and CO2, the moles of CO2 will be equal to the moles of CH4.

Moles of CO2 ≈ 6.25 mol

Step 3: Convert moles of carbon dioxide to mass.

Mass of CO2 = Moles of CO2 × Molar mass of CO2
Mass of CO2 = 6.25 mol × 44 g/mol
Mass of CO2 ≈ 275 g

Therefore, the mass of carbon dioxide produced when 100 grams of methane is oxidized is approximately 275 grams.