Experiment 1 Data Table 1: Stoichiometry Values Initial: 1.50g CaCl2.2H₂O (g) Initial: 0.0102 mol CaCl2.2H₂O (mol) Initial: CaCl2 0.0102 mol (mol) Initial: Na2CO3 0.0102 mol (mol) Initial: Na2CO3 1.0816g (g) Theoretical: 1.02g CaCO3 (g) Mass of Filter 0.81 paper (g) Mass of Filter 0.93 Paper + CaCO3 (g) Actual: CaCO3 0.99g (g) % Yield: 97.06% Data Table 1
Experiment 1 Data Table 1: Stoichiometry Values Initial: 1.50g CaCl2.2H₂O (g) Initial: 0.0102 mol CaCl2.2H₂O (mol) Initial: CaCl2 0.0102 mol (mol) Initial: Na2CO3 0.0102 mol (mol) Initial: Na2CO3 1.0816g (g) Theoretical: 1.02g CaCO3 (g) Mass of Filter 0.81 paper (g) Mass of Filter 0.93 Paper + CaCO3 (g) Actual: CaCO3 0.99g (g) % Yield: 97.06% Data Table 1
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
Related questions
Question
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.
Results are attached form experiment
Transcribed Image Text:Experiment 1
Data Table 1: Stoichiometry Values
Initial:
1.50g
CaCl2.2H₂O
(g)
Initial:
0.0102 mol
CaCl2.2H₂O
(mol)
Initial: CaCl2
0.0102 mol
(mol)
Initial: Na2CO3
0.0102 mol
(mol)
Initial: Na2CO3
1.0816g
(g)
Theoretical:
1.02g
CaCO3 (g)
Mass of Filter
0.81
paper (g)
Mass of Filter
0.93
Paper + CaCO3
(g)
Actual: CaCO3
0.99g
(g)
% Yield:
97.06%
Data Table 1
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