The chemical equation for the decomposition of calcium carbonate (CaCO3) into calcium oxide (CaO) and carbon dioxide (CO2) is as follows:
CaCO3 → CaO + CO2
To determine the amount of carbon dioxide produced, we need to compare the molar ratio of calcium carbonate to carbon dioxide. According to the balanced equation, 1 mole of calcium carbonate produces 1 mole of carbon dioxide.
The molar mass of calcium carbonate (CaCO3) is: 40.08 g/mol (Ca) + 12.01 g/mol (C) + (3 * 16.00 g/mol) (O) = 100.09 g/mol
To find the number of moles of calcium carbonate in 80 g, we divide the mass by the molar mass:
Number of moles of CaCO3 = 80 g / 100.09 g/mol ≈ 0.7996 mol
Since the molar ratio of CaCO3 to CO2 is 1:1, the number of moles of carbon dioxide produced is also approximately 0.7996 mol.
To determine the mass of carbon dioxide, we multiply the number of moles by its molar mass:
Mass of CO2 = 0.7996 mol * 44.01 g/mol (molar mass of CO2) ≈ 35.19 g
Therefore, approximately 35.19 grams of carbon dioxide would be produced when 80 grams of calcium oxide is formed by the decomposition of calcium carbonate.