500g of zinc carbonate was heated to constant mass.A.state what was observed? write an ionic equation that took place? calculate the apparent loss in mass?
Your post isn't quite clear. What DID YOU OBSERVE? I don't know what you saw.
ZnCO3 ==> ZnO + CO2
What do you mean by APPARENT loss in mass. It either lost mass or didn't lose mass. There is nothing apparent about it.
A White Precipitate Of Zinc Oxide Was Formed
When 500g of zinc carbonate is heated to constant mass, the following observations can be made:
1. The solid zinc carbonate will decompose upon heating, releasing carbon dioxide gas (CO2) and leaving behind a solid residue.
The balanced chemical equation for the decomposition of zinc carbonate is:
ZnCO3(s) → ZnO(s) + CO2(g)
In this reaction, zinc carbonate decomposes into zinc oxide (ZnO) and carbon dioxide (CO2).
To calculate the apparent loss in mass, we need to compare the initial mass of zinc carbonate (500g) with the final mass of the residue after heating. The residue should consist of only zinc oxide.
Assuming that all the zinc carbonate decomposed completely and the residue is purely zinc oxide, we calculate the mass of zinc oxide by subtracting the mass of carbon dioxide released from the initial mass of zinc carbonate.
The molar mass of CO2 is approximately 44 g/mol. The balanced equation shows that one mole of zinc carbonate produces one mole of CO2. The molar mass of zinc carbonate (ZnCO3) is approximately 125 g/mol.
Using these values, we can calculate the moles of CO2 produced:
Moles of CO2 = Mass of CO2 / Molar mass of CO2
= Mass of CO2 / (44 g/mol)
Since the balanced equation shows a 1:1 mole ratio between CO2 and zinc carbonate, the moles of CO2 released are also equal to the moles of zinc carbonate decomposed.
Therefore, the mass of zinc carbonate decomposed is:
Mass of ZnCO3 decomposed = Moles of CO2 x Molar mass of ZnCO3
Finally, to find the apparent loss in mass:
Apparent loss in mass = Initial mass of ZnCO3 - Mass of ZnCO3 decomposed