What mass of CO₂ would be produced by heating a 200.-kg sample of limestone that is 49.1% CaCO₃? Assume complete reaction and no other source of carbon dioxide.

Question

Quizplus · Accepted Answer

The mass of CaCO3 in the sample is 200 kg * 49.1% = 98.2 kg. The molar mass of CaCO3 is 100.09 g/mol, and CO2 is 44.01 g/mol. The reaction CaCO3 → CaO + CO2 shows a 1:1 molar ratio. Thus, 98.2 kg of CaCO3 produces (98.2 kg * 44.01 g/mol) / 100.09 g/mol = 43.2 kg of CO2.

What Mass of CO2 Would Be Produced by Heating a 200.-Kg

What Mass of CO₂ Would Be Produced by Heating a 200.-Kg