What mass of CO₂ would be produced by heating a 600.-kg sample of limestone that is 68.9% CaCO₃? Assume complete reaction and no other source of carbon dioxide. A) 182 kg B) 413 kg C) 264 kg D) 30.3 kg E) 600 kg

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Quizplus · Accepted Answer

The mass of $ \text{CaCO}_3 $ in the limestone is $ 600 \, \text{kg} \times 0.689 = 413.4 \, \text{kg} $. The molar mass of $ \text{CaCO}_3 $ is approximately $ 100.09 \, \text{g/mol} $, and the molar mass of $ \text{CaO} $ is about $ 56.08 \, \text{g/mol} $. The reaction is $ \text{CaCO}_3 \rightarrow \text{CaO} + \text{CO}_2 $. For every mole of $ \text{CaCO}_3 $, one mole of $ \text{CaO} $ is produced. Therefore, the mass of $ \text{CaO} $ produced can be calculated by the ratio of their molar masses and the mass of $ \text{CaCO}_3 $ used. $ 413.4 \, \text{kg} \times \frac{56.08}{100.09} \approx 232.5 \, \text{kg} $ of $ \text{CaO} $. However, the question asks for the mass of $ \text{CO}_2 $ produced, not $ \text{CaO} $. The molar mass of $ \text{CO}_2 $ is about $ 44.01 \, \text{g/mol} $, so using the same initial mass of $ \text{CaCO}_3 $, $ 413.4 \, \text{kg} \times \frac{44.01}{100.09} \approx 182 \, \text{kg} $ of $ \text{CO}_2 $ is produced.

What Mass of CO2 Would Be Produced by Heating a 600.-Kg

What Mass of CO₂ Would Be Produced by Heating a 600.-Kg