Question

Acetylene gas (C₂H₂) undergoes combustion to produce carbon dioxide and water vapor. a. how many liters of C₂H₂ are required to produce 75.0 l of CO₂? b. what volume of H₂O is produced?

what volume of O₂ is required?

Answer 1

To produce 75.0 liters of CO2 through the combustion of acetylene, 37.5 liters of C2H2 are required, which also produces 37.5 liters of H2O vapor. The reaction requires 93.75 liters of O2.

Step-by-step explanation:

The balanced chemical equation for the combustion of acetylene (C2H2) is 2 C2H2 (g) + 5 O2 (g) → 4 CO2 (g) + 2 H2O (g). From this equation, we deduce that 2 volumes of C2H2 produce 4 volumes of CO2. Therefore, to produce 75.0 liters of CO2, 37.5 liters of C2H2 are required since the ratio is 1:2. For water vapor, for every 2 liters of C2H2, 2 liters of H2O are produced, so the volume of H2O produced is the same as the amount of C2H2 burned, which amounts to 37.5 liters.

Lastly, for the volume of O2 required, the equation shows that 5 volumes of O2 are needed for every 2 volumes of C2H2, thus to combust 37.5 liters of C2H2, we require 93.75 liters of O2.