Final answer:
The maximum mass of carbon dioxide that could be produced is 1.76 grams, with the answer rounded to two significant digits to reflect the precision of the given masses.
Step-by-step explanation:
To calculate the maximum mass of carbon dioxide (CO₂) that could be produced from the combustion of butane (C₄H₁₀), we first need to write the balanced chemical equation for the reaction:
C₄H₁₀(g) + 13/2 O₂(g) → 4CO₂(g) + 5H₂O(g)
Next, we convert the masses of butane and oxygen to moles:
- For butane (molar mass = 58.12 g/mol): moles of C₄H₁₀ = 0.581 g / 58.12 g/mol = 0.01 moles
- For oxygen (molar mass = 32.00 g/mol for O₂): moles of O₂ = 1.1 g / 32.00 g/mol = 0.034375 moles
The stoichiometry of the reaction shows that 1 mole of butane reacts with 6.5 moles of oxygen to produce 4 moles of carbon dioxide. Therefore, butane is the limiting reactant here, because it will run out before oxygen.
We can now calculate the moles of CO₂ produced:
Moles of CO₂ = 4 moles CO₂ / 1 mole C₄H₁₀ × 0.01 moles C₄H₁₀ = 0.04 moles CO₂
We then convert moles of CO₂ to grams:
Mass of CO₂ = 0.04 moles × 44.01 g/mol = 1.76 g