Question

100 mL of a gaseous mixture contains 38% of CH₄, 35% of H₂ and 12% of C₂H₄ and 15% of СО. This mixture was mixed with 200 mL of oxygen and was exploded. Calculate the volume and the composition of the resulting mixture when cooled to room temperature and pressure.

Answer 1

Given:

CH₄ = 38 mL, H₂ = 35 mL, C₂H₄ = 12 mL, CO = 15 mL

Total O₂ added = 200 mL

Oxygen consumed:

For CH₄ = 38 × 2 = 76 mL

For H₂ = `35/2` = 17.5 mL

For C₂H₄ = 12 × 3 = 36 mL

For CO = `15/2` = 7.5 mL

Total O₂ used = 76 + 17.5 + 36 + 7.5 = 137 mL

CO₂ produced:

From CH₄ = 38 mL

From C₂H₄ = 12 × 2 = 24 mL

From CO = 15 mL

Total CO₂ = 38 + 24 + 15 = 77 mL

Final Mixture (at room temperature):

Remaining O₂ = 200 − 137 = 63 mL

CO₂ produced = 77 mL

Total Volume = 63 + 77 = 140 mL