1. Write the balanced chemical equation:

CH₄ + 2O₂ → CO₂ + 2H₂O

2. Calculate the molar mass of each compound:

* CH₄: (12.01 g/mol) + (4 * 1.01 g/mol) = 16.05 g/mol

* O₂: (2 * 16.00 g/mol) = 32.00 g/mol

* CO₂: (12.01 g/mol) + (2 * 16.00 g/mol) = 44.01 g/mol

* H₂O: (2 * 1.01 g/mol) + (16.00 g/mol) = 18.02 g/mol

3. Determine the moles of CH₄:

* Moles of CH₄ = (32 g) / (16.05 g/mol) = 2 mol

4. Use the mole ratio from the balanced equation to find the moles of O₂ consumed:

* From the balanced equation, 1 mole of CH₄ reacts with 2 moles of O₂.

* Moles of O₂ = 2 mol CH₄ * (2 mol O₂ / 1 mol CH₄) = 4 mol O₂

5. Calculate the mass of O₂ consumed:

* Mass of O₂ = (4 mol) * (32.00 g/mol) = 128 g

Therefore, 128 grams of O₂ were consumed in the reaction.