Final answer:
To find the mass of CO₂ produced from 37.5 g of C₂H₆, we calculate moles of C₂H₆, use the molar ratio from the balanced equation to find moles of CO₂.
Step-by-step explanation:
We first need the balanced chemical equation for the combustion of ethane: 2C₂H₆ + 7O₂ → 4CO₂ + 6H₂O. From the equation, it is clear that 2 moles of ethane produce 4 moles of carbon dioxide. To find the mass of CO₂, we need to determine the number of moles of C₂H₆ first.
The molar mass of C₂H₆ is approximately 30.07 g/mol. Thus, the number of moles of C₂H₆ in 37.5 g is: moles C₂H₆ = 37.5 g / 30.07 g/mol ≈ 1.247 moles C₂H₆. According to the balanced equation, the molar ratio is 2 moles C₂H₆ to 4 moles CO₂. So, the moles of CO₂ produced is: moles CO₂ = 1.247 moles C₂H₆ × (4 moles CO₂ / 2 moles C₂H₆) ≈ 2.494 moles CO₂
Now, with the molar mass of CO₂ being approximately 44.01 g/mol, we can find the mass: mass of CO₂ = 2.494 moles CO₂ × 44.01 g/mol ≈ 109.7 g CO₂. Therefore, the mass of CO₂ produced from the combustion of 37.5 g of C₂H₆ will be approximately 109.7 g.