Question

You are given a crushed sample containing limestone, lime, and sand. After heating, the sample weighs 3.9865 g (final weight). What is the percentage of calcium carbonate in the original mixture? (MW of calcium carbonate = 100.1 g/mol)

Answer 1

Without additional data such as the initial mass of the mixture and the weight changes during heating, the percentage of calcium carbonate in the original mixture cannot be calculated. The question seems to require an understanding of stoichiometry and the law of conservation of mass.

Step-by-step explanation:

To calculate the percentage of calcium carbonate in the original mixture, more information is needed such as the mass of the mixture before heating and the relevant chemical equations and stoichiometric calculations. Without this specific data, the calculation cannot be made. The law of conservation of mass and stoichiometry are typically used in these calculations.

For instance, if heating calcium carbonate (CaCO3) produces calcium oxide (CaO) and carbon dioxide (CO2), and the initial and final weights of the sample are known, the percentage of CaCO3 can be determined using stoichiometry. However, the final weight alone is insufficient. An example of a stoichiometric calculation is shown where calcium carbonate when heated produces equal weights in carbon dioxide and calcium oxide, adhering to the law of conservation of mass.