b. How many liters of CO2 would be produced from the reaction of 3.50 L of C4H10O and 2.00 L of O2 at 1.00 atm and 25 °C?

Question

Answer 1

Since neither the temperature nor pressure changes during the reaction, we can simply use the ratio of volumes with no need to convert to moles.

C₄H₁₀O + 6O₂ ==> 4CO₂ + 5H₂O ... balanced equation for complete combustion of C₄H₁₀O

Which reactant is limiting?

3.50 L C₄H₁₀O x 6 L O₂/1 L C₄H₁₀O = 21 L O₂ required. Clearly not enough O₂ present.

Volume of CO₂ will be dependent on O₂ as O₂ is limiting.

2.00 L O₂ x 4 L CO₂ / 6 L O₂ = 1.33 L CO₂ formed