A mixture of methane \(\left(\mathrm{CH}_{4}\right)\) and ethane \(\left(\mathrm{C}_{2} \mathrm{H}_{6}\right)\) is \(25.6 \%\) methane by mass. When \(1.50 \mathrm{~g}\) of this mixture is burned, what is the mass of carbon dioxide produced?

The mass of CO₂ produced when 1.50 g of a mixture containing 25.6% methane by mass and the rest ethane is burned can be found by following these steps: 1. Calculate the mass of each component in the mixture: Mass of CH₄ = \((25.6/100) \times 1.50 \mathrm{~g}\) and Mass of C₂H₆ = \(1.50 \mathrm{~g}\) - Mass of CH₄ 2. Convert the mass of each component to moles: Moles of CH₄ = \(\dfrac{\text{Mass of CH₄}}{16.04 \mathrm{ g/mol}}\) and Moles of C₂H₆ = \(\dfrac{\text{Mass of C₂H₆}}{30.07 \mathrm{ g/mol}}\) 3. Determine the moles of CO₂ produced from both CH₄ and C₂H₆: Moles of CO₂ from CH₄ = Moles of CH₄, Moles of CO₂ from C₂H₆ = 2 × Moles of C₂H₆ 4. Calculate the mass of CO₂ produced: Mass of CO₂ = Total moles of CO₂ × 44.01 g/mol, where Total moles of CO₂ = Moles of CO₂ from CH₄ + Moles of CO₂ from C₂H₆