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Using stoichiometry, calculate the limiting reactant, and the theoretical yield (the mass of CaCO3 product) for the reaction.

Using stoichiometry, calculate the limiting reactant, and the theoretical yield (the mass of CaCO3 product) for the reaction.

Chemistry
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...
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1. A 10.0 mL graduated cylinder to measure 10.0 mL of a 1.00 M CaCl2 solution into an initially empty 50.0 mL beaker. 2. A 50.0 mL graduated cylinder was then used to measure out 25.0 mL of 0.500 M K,CO3. This K2CO3 solution was then added to the beaker containing the CaCl2 solution. The solution became cloudy, and the student concluded that a precipitate must have formed. Write a balanced chemical reaction below, including phases, and identify the chemical formula of the precipitate: CaCl2(aq)+K2CO3(aq)→2KCI(aq)+CaCO3(s) 3. The student then collected the precipitate by filtering it using the gravity filtration apparatus below: funnel, with filter paper clamp stand conical flask Figure 3.1 - Gravity Filtration Apparatus (Conical Flask = Erlenmeyer Flask) c BY Unless otherwise noted, content of University of York is licensed under CC BY 4.0 After the solid was collected, it was dried on a hot plate three times. The following data was collected: Mass of solid product after first heating (g) 1.0250 g Mass of solid product after second heating (g) 0.9723g Mass of solid product after third heating (g) 0.9719 g
Transcribed Image Text:1. A 10.0 mL graduated cylinder to measure 10.0 mL of a 1.00 M CaCl2 solution into an initially empty 50.0 mL beaker. 2. A 50.0 mL graduated cylinder was then used to measure out 25.0 mL of 0.500 M K,CO3. This K2CO3 solution was then added to the beaker containing the CaCl2 solution. The solution became cloudy, and the student concluded that a precipitate must have formed. Write a balanced chemical reaction below, including phases, and identify the chemical formula of the precipitate: CaCl2(aq)+K2CO3(aq)→2KCI(aq)+CaCO3(s) 3. The student then collected the precipitate by filtering it using the gravity filtration apparatus below: funnel, with filter paper clamp stand conical flask Figure 3.1 - Gravity Filtration Apparatus (Conical Flask = Erlenmeyer Flask) c BY Unless otherwise noted, content of University of York is licensed under CC BY 4.0 After the solid was collected, it was dried on a hot plate three times. The following data was collected: Mass of solid product after first heating (g) 1.0250 g Mass of solid product after second heating (g) 0.9723g Mass of solid product after third heating (g) 0.9719 g
3. Using stoichiometry, calculate the limiting reactant, and the theoretical yield (the mass of CaCO3 product) for the reaction.
Transcribed Image Text:3. Using stoichiometry, calculate the limiting reactant, and the theoretical yield (the mass of CaCO3 product) for the reaction.
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