Exercise on Mass Produced from Burning Butane: Solutions

Butane (C4H10) burns in air according to the following equation:
2C4H10 + 13O2 → 8CO2 + 10H2O

Question: What is the mass of CO2 produced from burning of 0.75 g of butane?

Solution:
C4H10(g) + 13/ 2 O2(g) → 4CO2(g) + 5H2O (l)
5.16 × 10− 2 moles of CO2 are produced and the details are as follows:

Moles of butane = (0.75 g) / (58.12 · g· mol− 1) = 1.29 × 10− 2 mol.
Each mole of butane gives 4 moles of CO2 upon complete combustion.
Therefore, moles of CO2 = 4 × 1.29 × 10− 2 mol = 5.16 × 10− 2 mol
This is equivalent mass of 5.16 × 10− 2 mol × 44.01 · g · mol− 1 ≅ 2.28 g


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Date of last modification: Summer , 2019