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4. Compare the total mass of the reactants with the total mass of the products: Total Mass of the Reactants vs. Total Mass of the Products ATAC

4. Compare the total mass of the reactants with the total mass of the products: Total Mass of the Reactants vs. Total Mass of the Products ATAC

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter3: Chemical Reactions
Section: Chapter Questions
Problem 141QRT
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Name Stoichiometry: Mass-Mass Experimentation has shown that there is usually a definite relationship between the number of moles of reactant and the number of moles of product in a chemical reaction. If one mole of A reacts with two moles of B, then it is reasonable to assume that one molecule of A can react with two molecules of B. The quantitative study of chemical reactions has led to the development of many important theories about the nature of matter. Mass-Mass experiments involve the mass relationships which accompany a chemical reaction. This experiment can yield very accurate results if care is taken in weighing, decanting, and filtering both reactants and products. The reaction involves: K2CrO4 (aq) PB(NO3 (aq) > 2KNO3(aq) PbCrO4 (s) Potassium Chromate Lead Nitrate Potassium Nitrate Lead Chromatefst 91samo The PbCrO4 (s) is a yellow precipitate that can be collected on a filter paper and weighed. DATA = 33ul0s 1. First calculate the mass of exactly 0.005 moles of Potassium Chromate and Lead Nitrate not bads ow fedh 29 c Show work here: O.v05 194.19-0.971 0.00Sa 321.cs grams K,CrOa/calculated (this is what needs to be weighed)O,97|a grams Pb(NO3)>/calculated (this is what needs to be weighed)aG539 Mass of 250 ml beaker0.06 g Mass of 250 ml flask 02g Mass of filter Paper_ Mass of filter paper and collected PbCrO4 (yellow stuff)_ Mass of flask with evaporated KNO3 solution 973 Calculations (show the work): L.679g 1. Mass of PbCrO4 (yellow stuff, this will require some subtraction)o o71g /14– 110.006=3.94 1,679
Transcribed Image Text:Name Stoichiometry: Mass-Mass Experimentation has shown that there is usually a definite relationship between the number of moles of reactant and the number of moles of product in a chemical reaction. If one mole of A reacts with two moles of B, then it is reasonable to assume that one molecule of A can react with two molecules of B. The quantitative study of chemical reactions has led to the development of many important theories about the nature of matter. Mass-Mass experiments involve the mass relationships which accompany a chemical reaction. This experiment can yield very accurate results if care is taken in weighing, decanting, and filtering both reactants and products. The reaction involves: K2CrO4 (aq) PB(NO3 (aq) > 2KNO3(aq) PbCrO4 (s) Potassium Chromate Lead Nitrate Potassium Nitrate Lead Chromatefst 91samo The PbCrO4 (s) is a yellow precipitate that can be collected on a filter paper and weighed. DATA = 33ul0s 1. First calculate the mass of exactly 0.005 moles of Potassium Chromate and Lead Nitrate not bads ow fedh 29 c Show work here: O.v05 194.19-0.971 0.00Sa 321.cs grams K,CrOa/calculated (this is what needs to be weighed)O,97|a grams Pb(NO3)>/calculated (this is what needs to be weighed)aG539 Mass of 250 ml beaker0.06 g Mass of 250 ml flask 02g Mass of filter Paper_ Mass of filter paper and collected PbCrO4 (yellow stuff)_ Mass of flask with evaporated KNO3 solution 973 Calculations (show the work): L.679g 1. Mass of PbCrO4 (yellow stuff, this will require some subtraction)o o71g /14– 110.006=3.94 1,679
2. Mass of KNO3 (this will require some subtraction) 0.953 111.973-111.02- 0:953 3. Calculate the moles of each product you obtained (use the masses you obtained): 114-261g-110.0bg=1.679 1.679 303.1932 Moles of PbCrO4 5.195 A103 0953 - 9.426 ad0 5.195 x 10-3 lo1.1032 Moles of KNO3 9.426~10-3 4. Compare the total mass of the reactants with the total mass of the products: Total Mass of the Reactants vs. Total Mass of the Products Using Stoichiometry (show work) calculate the Theoretical Yield for both products starting with the masses that you weighed for the reagents. 5. Using Reagent K,CrO .005mol L2CrOul Tma 0.01 mol kWbz (eT Imut 00S mol PoCrb>( 3222g Boro2. L,6165 .0US mol kaCrou Lmal Theoretical Yield (g) of PbCrO4_ Theoretical Yield (g) of KNO3 011 Using Reagent Pb(NO3) wol enohslusie Theoretical Yield (g) of PbCrO4 Theoretical Yield (g) of KNO3 6. How does the theoretical yield (g) compare to the actual mass values you got???
Transcribed Image Text:2. Mass of KNO3 (this will require some subtraction) 0.953 111.973-111.02- 0:953 3. Calculate the moles of each product you obtained (use the masses you obtained): 114-261g-110.0bg=1.679 1.679 303.1932 Moles of PbCrO4 5.195 A103 0953 - 9.426 ad0 5.195 x 10-3 lo1.1032 Moles of KNO3 9.426~10-3 4. Compare the total mass of the reactants with the total mass of the products: Total Mass of the Reactants vs. Total Mass of the Products Using Stoichiometry (show work) calculate the Theoretical Yield for both products starting with the masses that you weighed for the reagents. 5. Using Reagent K,CrO .005mol L2CrOul Tma 0.01 mol kWbz (eT Imut 00S mol PoCrb>( 3222g Boro2. L,6165 .0US mol kaCrou Lmal Theoretical Yield (g) of PbCrO4_ Theoretical Yield (g) of KNO3 011 Using Reagent Pb(NO3) wol enohslusie Theoretical Yield (g) of PbCrO4 Theoretical Yield (g) of KNO3 6. How does the theoretical yield (g) compare to the actual mass values you got???
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