B. Stoichiometry and Percent YieldDATA1. Mass of sodium carbonate2. Mass of filter paper3. Mass of dry filter paper and calcium carbonate productCALCULATIONS AND QUESTIONS (show all of your work)1. Mass of dried product (actual yield)(Mass of dry filter paper and calcium carbonate product - mass of filter paper)1.0 g1.2g2.692. Write the balanced chemical equation for the reaction of sodium carbonate and calciumchloride. (Ignore the hydrate in this equation)2.893. Use stoichiometry to calculate the theoretical yield of calcium carbonate product basedon the starting mass of sodium carbonate.4. Calculate the percent yield of the reaction based on the actual yield of dried calciumcarbonate product and the theoretical yield of calcium carbonate product.<5. Why is it necessary to write the balanced chemical equation for the reaction beforecompleting any stoichiometry problems?11 /13 >11

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B. Stoichiometry and Percent Yield DATA 1. Mass of sodium carbonate 2. Mass of filter paper 3. Mass of dry filter paper and calcium carbonate product 1.0 g -1.28 2.08 CALCULATIONS AND QUESTIONS (show all of your work) 1. Mass of dried product (actual yield) (Mass of dry filter paper and calcium carbonate product-mass of filter paper) RB J 2. Write the balanced chemical equation for the reaction of sodium carbonate and calcium chloride. (Ignore the hydrate in this equation) 3. Use stoichiometry to calculate the theoretical yield of calcium carbonate product based on the starting mass of sodium carbonate. 4. Calculate the percent yield of the reaction based on the actual yield of dried calcium carbonate product and the theoretical yield of calcium carbonate product.

B. Stoichiometry and Percent Yield DATA 1. Mass of sodium carbonate 2. Mass of filter paper 3. Mass of dry filter paper and calcium carbonate product 1.0 g -1.28 2.08 CALCULATIONS AND QUESTIONS (show all of your work) 1. Mass of dried product (actual yield) (Mass of dry filter paper and calcium carbonate product-mass of filter paper) RB J 2. Write the balanced chemical equation for the reaction of sodium carbonate and calcium chloride. (Ignore the hydrate in this equation) 3. Use stoichiometry to calculate the theoretical yield of calcium carbonate product based on the starting mass of sodium carbonate. 4. Calculate the percent yield of the reaction based on the actual yield of dried calcium carbonate product and the theoretical yield of calcium carbonate product.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 98AP

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On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
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