A sample with a mass of 15.6 g, consisting of oxide and calcium carbonate, was calcined
A sample with a mass of 15.6 g, consisting of oxide and calcium carbonate, was calcined, as a result of which a gas with a volume of 2.24 liters was released. Determine the mass fraction in% of calcium oxide in the sample.
When calcined, calcium oxide does not change, and calcium carbonate decomposes into calcium oxide and carbon dioxide:
CaCO3 = CaO + CO2.
The volume of 1 mol of gas under normal conditions is 22.4 liters, which means that 2.24 / 22.4 = 0.1 mol of CO2 was released as a result of the reaction.
This means that there was 0.1 mol of CaCO3 in the sample.
Molar mass М (CaCO3) = 40 + 12 + 16 × 3 = 100 g / mol, so the mass of CaCO3 is 10 g.
Calcium oxide mass: 15.6 – 10 = 5.6 g, which corresponds to a mass fraction of 5.6 / 15.6 × 100% = 35.9%.