Question

A sample of CaCO3 and FeCO3 contains equal portions of each by weight. Strong ignition produces CaO and Fe2O3. What is the weight of a 1.000 g sample after thorough ignition?

Answer 1

Answer:

0.6246g

Explanation:

You need balanced equations first: (don't mind the equal sign)

CaCO3 = CaO + CO2

4FeCO3 = 2Fe2O3 + 4CO2

Because they are equal in mass we have 0.5g of both carbonates.

0.5g of ferrous carbonate is 0.004316 moles so we get 0.002158 moles of ferric oxide, which is 0.3446g.

0.5g of calcium carbonate is 0.005 moles so we get 0.005 moles of calcium oxide, which is 0.28g.

So the total mass is 0.28 + 0.3446g = 0.6246g