Assuming no change in temperature or pressure, how many liters of O2 would be needed to completely combust 4.0 liters of C4H6? 2 C4H6(g) + 11 O2(g) → 8 CO2(g) + 6 H2O(g)

Question

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Assuming no change in temperature or pressure, how many liters of O2 would be needed to completely combust 4.0 liters of C4H6?
2 C4H6(g) + 11 O2(g) → 8 CO2(g) + 6 H2O(g)

Answer 1

2C₄H₆(g) + 11O₂(g) ==> 8CO₂(g) + 6H²O(g) ... balanced equation

Since there is no change in temperature or pressure, the coefficients in the balanced equation can be taken as moles or liters, it doesn't matter. Using dimensional analysis, we have...

4.0 L C₄H₆ x 11 L O₂/ 2 L C₄H₆ = 22 L O₂ needed