In the reaction, CaCO3(s)⟶CaO(s)+CO2(g) how many liters of carbon dioxide, CO2, measured at STP, would be produced from the decomposition of 325 g of calcium carbonate, CaCO3?

Answer 1

Find moles of CO₂ and then convert to liters using conversion of 1 mol @ STP = 22.4 liters.

To find moles CO₂, use stoichiometry (mole ratio) of balanced equation and dimensional analysis

molar mass CaCO₃ = 100 g / mol

molar mass CO₂ = 44 g / mole

CaCO₃ ==> CaO + CO₂ .. balanced equation

moles CaCO₃ present = 325 g x 1 mol / 100 g = 3.25 mols

moles CO₂ produced = 3.25 mols CaCO₃ x 1 mol CO₂ / mol CaCO₃ = 3.25 mols CO₂ produced

Liters CO₂ = 3.25 mols x 22.4 L / mol = 72.8 L