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1)What is the theoretical yield (in grams) of CaCO3 in the precipitation reaction that occurs when when a solution prepared by dissolving 1.004 g of solid CaCl2 in 30 mL of water is mixed with a solution prepared by dissolving 0.997 g of Na2CO3 in 30 mL of water? Include the appropriate number of significant figures in your answer.   2)Suppose that 0.814 g of CaCO3 is actually isolated in the precipitation reaction described in Question 1.  What is the percent yield of this reaction? Report your answer to the correct number of significant figures.

1)What is the theoretical yield (in grams) of CaCO3 in the precipitation reaction that occurs when when a solution prepared by dissolving 1.004 g of solid CaCl2 in 30 mL of water is mixed with a solution prepared by dissolving 0.997 g of Na2CO3 in 30 mL of water? Include the appropriate number of significant figures in your answer.   2)Suppose that 0.814 g of CaCO3 is actually isolated in the precipitation reaction described in Question 1.  What is the percent yield of this reaction? Report your answer to the correct number of significant figures.

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter4: Stoichiometry
Section: Chapter Questions
Problem 4.68PAE: 4.68 The pictures below show a molecular-scale view of a chemical reaction between the compounds AB2...
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1)What is the theoretical yield (in grams) of CaCO3 in the precipitation reaction that occurs when when a solution prepared by dissolving 1.004 g of solid CaCl2 in 30 mL of water is mixed with a solution prepared by dissolving 0.997 g of Na2CO3 in 30 mL of water?
Include the appropriate number of significant figures in your answer.
 
2)Suppose that 0.814 g of CaCO3 is actually isolated in the precipitation reaction described in Question 1.  What is the percent yield of this reaction?
Report your answer to the correct number of significant figures.
 
3)A solution of Na2CO3 is prepared by dissolving 0.511 g of the solid in approximately 30 mL of water.  How many moles of Na2CO3 does this solution contain?
Express your answer to the correct number of significant figures.  
 
4)Suppose the Na2CO3  solution described in Question 13 is added to a solution that contains excess CaCl2?  What is the maximum number of moles of solid CaCO3 that can form in the resulting precipitation reaction?  
 
5)What is the maximum mass (in grams) of CaCO3 that could form in the precipitation reaction described in Question 4?
Include the correct number of significant figures in your answer.
 
 
 
Expert Solution
Step 1
If one mole of calcium carbonate is formed in the reaction then the theoretical yield will be 100 gram. 
How to Find/Calculate Theoretical Yield
  1. Step 1: Check to see if your chemical equations are balanced. 
  2. Step 2: Calculate the mole ratios of the reactants and products. 
  3. Step 3: Find the theoretical yield of the reaction. ...
  4. Solution: .
  5. Percent Yield = Mass of Actual Yield / Mass of Theoretical Yield x 100 percent.
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