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A mixture of CaCO₃ and CaO weighing 0.693 g was heated to produce gaseous CO₂. After heating, the remaining solid weighed 0.508 g. Assuming all the CaCO₃ broke down to CaO and CO₂, calculate the mass percent of CaCO₃ in the original mixture.



Answer :

CaCO3(s) -----> CO2(g) + CaO(s)

We deduct the mass of the residue from the mass of the mixture to obtain the mass of oxygen.

amount of CO2 is the sum of the mass of the mixture and the mass of the residue.

Moles of CO2 equal 0.185 g CO2 = 1 mol O2/44.01 g CO2 = 4.204 x 103 mol CaCO3

Moles of CaCO3 = (4.204 x 103 mol CO2) = (1 mol CaCO3/1 mol CO2) = 4.204 x 10-3 mol CaCO3 are the amount of moles.

CaCO3's mass is equal to 4.204 x 10 mol CaCO3 (100.00 g CaCO3/1 mol CaCO3), which equals 0.4208 g CaCO3.

CaCO's mass percentage is 60.72% (mass percent = 0.4208 g CaCO3/0.693 g mixture*100).

The mass percent of CaCO3 is 60.72%

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