Post Lab Questions: A perfect percent yield would be 100%. Based on your results, describe your degree...

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Chemistry

Post Lab Questions:
A perfect percent yield would be 100%. Based on your results,describe your degree of accuracy and suggest possible sources oferror.
What impact would adding twice as muchNa₂CO₃ than required for stoichiometricquantities have on the quantity of product produced?
Determine the quantity (g) of pure CaCl₂ in 7.5 g ofCaCl₂â€¢9H₂O.
Determine the quantity (g) of pure MgSO₄ in 2.4 g ofMgSO₄â€¢7H₂O.
Conservation of mass was discussed in the background. Describehow conservation of mass (actual, not theoretical) could be checkedin the experiment performed.
Based on these findings:
Data Table 1. Stoichiometry Values
Initial: CaCl₂â€¢2H₂O(g)
.68
Initial: CaCl₂â€¢2H₂O(moles)
.0068
Initial: CaCl₂ (moles)
.00368
Initial: Na₂CO₃(moles)
.0012
Initial: Na₂CO₃ (g)
.12
Theoretical: CaCO₃ (g)
.68
Mass of Filter paper (g)
1g
Mass of Filter Paper + CaCO₃ (g)
1.7g
Actual: CaCO₃ (g)
.72g
% Yield:
103

Answer & Explanation Solved by verified expert

4.3 Ratings (951 Votes)

A perfect percent yield would be 100 Based on your results describe your degree of accuracy and suggest possible sources of error Solution If the reaction is not gone for the completion then it will not form the complete precipitate and some of the reactant may lost in the solution while the filtration this will give the lower percent yield If the precipitate is not dried well and See Answer

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Initial: CaCl₂â€¢2H₂O(g)	.68
Initial: CaCl₂â€¢2H₂O(moles)	.0068
Initial: CaCl₂ (moles)	.00368
Initial: Na₂CO₃(moles)	.0012
Initial: Na₂CO₃ (g)	.12
Theoretical: CaCO₃ (g)	.68
Mass of Filter paper (g)	1g
Mass of Filter Paper + CaCO₃ (g)	1.7g
Actual: CaCO₃ (g)	.72g
% Yield:	103