Question

Naproxen (C14H14O3) is a common pain reliever. When solid naproxen was combusted in the presence of oxygen gas, gaseous carbon dioxide and gaseous water were produced.

Write a complete, balanced chemical equation for this reaction.

How much oxygen gas (in grams) is required to completely combust 250. grams

of naproxen?

[556 g O2]

What is the theoretical yield of carbon dioxide gas upon complete combustion of

250. grams of naproxen?

[669 g CO2]

Answer 1

1)

The balanced combustion chemical reaction is

C₁₄H₁₄O₃ + 16 O₂ 14 CO₂ + 7 H₂O

2) From the balanced chemical equation

1 mole of Naproxen requires 16 moles of Oxygen for combustion.

Molar mass of Naproxen = 230

230 g of Naproxen requires 16x 32 = 512g of Oxygen for combustion

mass of oxygen required for combustion of 250 g of Naproxen = (512 / 230) x 250 = 556.52 g = 556 g

3)  From the balanced chemical equation

1 mole of Naproxen yields 14 moles of carbondioxide after combustion.

so, mass of CO₂ produced = 14 x molar mass of CO₂ = 14 x 44 = 616 g

Molar mass of Naproxen = 230

230 g of Naproxen produced 616 g of CO₂ on combustion

mass of CO₂ produced on combustion of 250 g of Naproxen  = (616 / 230) x 250 = 669.56 g = 669 g