Part 1 – Preparation of CaCO3(s) The following is a procedure that was theoretically performed by a student. Read through the procedure and answer the questions below.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.A 50.0 mL graduated cylinder was then used to measure out 25.0 mL of 0.500 M K2CO3. This K2CO3 solution was then added to the beaker containing the CaCl2 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: Answer the questions below as part of Data Analysis. 1. What is the actual yield of the product?2. Using stoichiometry, calculate the limiting reactant, and the theoretical yield (the mass of CaCO3 product) for the reaction.3. Determine the percent yield of the reaction.

Given: Volume of CaCl2 = 10 mL concentration of CaCl2 = 1.0 M Volume of K2CO3 = 25 mL concentration of K2CO3 = 0.5 M Balanced chemical reaction is given by, CaCl2(aq)+K2CO3(aq)→CaCO3(s)+2KCl(aq)Calculation for moles of CaCl2: moles=molarity×volumemoles of CaCl2=1.0 mol/L×10×10-3 Lmoles of CaCl2=0.01 mol Calculation for moles of K2CO3: moles=molarity×volumemoles of K2CO3=0.5 mol/L×25×10-3 Lmoles of K2CO3=0.0125 molIdentifying limiting reactant: moles of CaCl2 : 0.01/1 = 0.01 mol moles of K2CO3 : 0.0125/1 = 0.0125 mol moles of CaCl2 < moles of K2CO3 Therefore, CaCl2 is the limiting reactant. Calculation for mass of CaCO3 (theoretical yield): 1 mole of CaCl2 produces 1 mole of CaCO3. 0.01 mole of CaCl2 produces 0.01 mole of CaCO3. mass=moles×molar massmass of CaCO3=0.01 mol×100.087 g/molmass of CaCO3=1.0 g Calculation for percent yield: percent yield=actual mass of CaCO3(precipitate)theoretical mass of CaCO3×100 Note: actual mass CaCO3 (mass of precipitate) is not given in the question.

Answered: Part 1 – Preparation of CaCO3(s) The…

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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Part 1 – Preparation of CaCO₃(s)

The following is a procedure that was theoretically performed by a student. Read through the procedure and answer the questions below.

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.
A 50.0 mL graduated cylinder was then used to measure out 25.0 mL of 0.500 M K₂CO₃. This K₂CO₃ solution was then added to the beaker containing the CaCl₂ 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:

Answer the questions below as part of Data Analysis.

1. What is the actual yield of the product?

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

3. Determine the percent yield of the reaction.

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