A mixture of CaCO3 and CaO weighing 0.635 g was heated to produce gaseous CO2. A

Question

A mixture of CaCO3 and CaO weighing 0.635 g was heated to produce gaseous CO2. After heating, the remaining solid weighed 0.427 g. Assuming all the CaCO3 broke down to CaO and CO2, calculate the mass percent of CaCO3 in the original mixture.

Explanation / Answer

CaCO3 --> upon heating --> CaO(s) & Co2 (g) 0.635 g = 0.427 g = 0.208 grams of CO2 released use molar masses to find the original amount of CaCO3 present, knowing that 1 mole of CaCO3 released 1 mole of CO2): (0.208 grams of CO2) (100.1 g/mol CaCO3) / (44.01 g/mol CO2) = 0.4721 grams of CaCO3 calculate the mass percent of CaCO3 in the original mixture. 0.4721 grams of CaCO3 / 0.635 g sample = 74.34% CaCO3

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