Initial: CaCl •2H O (g)Initial: CaCl •2H O (mol)Initial: CaCl (mol)Initial: Na CO (mol)Initial: Na CO (g)Theoretical: CaCO (g)Mass of Filter paper (g)Mass of Filter Paper + CaCO (g)Actual: CaCO (g)% Yield:2 2 1.0 g2 2 0.0068 mol2 0.0068 mol2 3 0.0068 mol2 3 0.8 g3 0.68g0.9 g3 1.5 g3 0.6 g86% 1. Given that a theoretical yield for isolating Calcium Carbonate in this experiment would be 100%. From that information and based on the results you obtained in this experiment, describe your success in the recovery of calcium carbonate and suggest two possible sources of error that would have caused you to not obtain 100% yield. Excess product of CaCO3 would be produced because there wouldn't be enough CaCl2 to react with Na2CO3. The purpose of stoichiometric quantities is to know the correct amount or close to the correct amount of each reactant in order to produce a product that is close to the theoretical amount and therefore have a higher percent yield.
2. What impact would adding twice as much Na CO than required for stoichiometric quantit ies have on the quantity of product produced?
3. Determine the quantity (g) of pure CaCl in 7.5 g of CaCl •9H.
4. Determine the quantity (g) of pure MgSO in 2.4 g of MgSO •7H O.
5. Conservation of mass was discussed in the background. Describe how conservation of mass (actual, not theoretical) could be checked in the experiment performed.