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3 Aluminum reacts with an aqueous solution containing excess copper (II) sulfate. If 1.85 g Al reacts and the percentage yield of Cu is 56.6%, what mass of Cu is produced? Al +3CUSO4 →_Cu +_Al2(SO4)3

3 Aluminum reacts with an aqueous solution containing excess copper (II) sulfate. If 1.85 g Al reacts and the percentage yield of Cu is 56.6%, what mass of Cu is produced? Al +3CUSO4 →_Cu +_Al2(SO4)3

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Percent Yield Problems Theoretical Yield - The maximun amount of product that can be formed from given reactants --Theoretical yield is the answer from the stoichiometry calculation = maximum possible amount ---Number based upon the theoretical" mathematical equation – no experiments were conducted Actual Yield --Due to a variety of factors, the actual amount will ALWAYS be less than the theoretical vield ---In real life, we never get as much as we anticipate, this "actual" amount from the lab experi The amount of product that actually forms when the reaction is carried out in the lak Percent Yield - The ratio of the actual yield to the theoretical yield expressed as a percentage, Actual Theoretical Percent Yield- x 100 EXAMPLE) How many grams of hydrofluoric acid (HF) are required to react completely with 23 8 grams of calcium hydroxide in the following reaction? 1 Ca(OH)2 +2_ HF → 1 CAF2+ 2 H20 1 mol Ca(OH)2 2 mol HF 20.01 g HF 23.68 g Ca(OH): X = 12.79 g HF| 74.10 g Ca(OH)2 1 mol Ca(OH)2 1 mol HF Based on the stoichiometry of this problem, the Theoretical Yield for this problem is 12.79 g HF But. when this experiment was conducted, an Actual Yield of only 10.41g HF was collected. Using the equation for percent yield, the Percent Yield of this experiment was 81.39%. Actual x 100 = Theoretical 10.41g HF,x 100 = 81.39% 12.79g HF Percent Yield = 1) A student adds 200.0g of C7H6O3 to an excess of C4H®O3, thịs produces C9H&O4 and C2H4O2. Calculate the percent yield if 231 g of aspirin (C9H8O4) is produced in an experiment. V C7H6O3 + CAH6O3 _C9H%O4 + 1_ C2H4O2 2) According to the following equation, Calculate the percentage yield if 550.0 g of toluene (C;H8 )added to an excess of nitric acid (HNO3) provides 305 g of the p-nitrotoluene (C7H¬NO2 ) product in a lab experiment. C7H8 + HNO3 > C7H7NO2 + H2O 3 Aluminum reacts with an aqueous solution containing excess copper (II) sulfate. If 1.85 g Al reacts and the percentage yield of Cu is 56.6%, what mass of Cu is produced? Al +3CUSO4 →_Cu +_Al2(SO4)3 4) The combustion of methane(CH4) produces carbon dioxide and water. Assume that 2.0 mc of CH4 burned in the presence of excess air. What is the percentage yield if in an experimen the reaction produces 87.0 g of CO2? 5) 15.3 grams of Lithium is dropped into a solution containing excess copper II phosphate. When the reaction is completed, 1.25 grams of copper is formed. What is the percent yield DO NOT WRITE ON THIS SHEET
Transcribed Image Text:Percent Yield Problems Theoretical Yield - The maximun amount of product that can be formed from given reactants --Theoretical yield is the answer from the stoichiometry calculation = maximum possible amount ---Number based upon the theoretical" mathematical equation – no experiments were conducted Actual Yield --Due to a variety of factors, the actual amount will ALWAYS be less than the theoretical vield ---In real life, we never get as much as we anticipate, this "actual" amount from the lab experi The amount of product that actually forms when the reaction is carried out in the lak Percent Yield - The ratio of the actual yield to the theoretical yield expressed as a percentage, Actual Theoretical Percent Yield- x 100 EXAMPLE) How many grams of hydrofluoric acid (HF) are required to react completely with 23 8 grams of calcium hydroxide in the following reaction? 1 Ca(OH)2 +2_ HF → 1 CAF2+ 2 H20 1 mol Ca(OH)2 2 mol HF 20.01 g HF 23.68 g Ca(OH): X = 12.79 g HF| 74.10 g Ca(OH)2 1 mol Ca(OH)2 1 mol HF Based on the stoichiometry of this problem, the Theoretical Yield for this problem is 12.79 g HF But. when this experiment was conducted, an Actual Yield of only 10.41g HF was collected. Using the equation for percent yield, the Percent Yield of this experiment was 81.39%. Actual x 100 = Theoretical 10.41g HF,x 100 = 81.39% 12.79g HF Percent Yield = 1) A student adds 200.0g of C7H6O3 to an excess of C4H®O3, thịs produces C9H&O4 and C2H4O2. Calculate the percent yield if 231 g of aspirin (C9H8O4) is produced in an experiment. V C7H6O3 + CAH6O3 _C9H%O4 + 1_ C2H4O2 2) According to the following equation, Calculate the percentage yield if 550.0 g of toluene (C;H8 )added to an excess of nitric acid (HNO3) provides 305 g of the p-nitrotoluene (C7H¬NO2 ) product in a lab experiment. C7H8 + HNO3 > C7H7NO2 + H2O 3 Aluminum reacts with an aqueous solution containing excess copper (II) sulfate. If 1.85 g Al reacts and the percentage yield of Cu is 56.6%, what mass of Cu is produced? Al +3CUSO4 →_Cu +_Al2(SO4)3 4) The combustion of methane(CH4) produces carbon dioxide and water. Assume that 2.0 mc of CH4 burned in the presence of excess air. What is the percentage yield if in an experimen the reaction produces 87.0 g of CO2? 5) 15.3 grams of Lithium is dropped into a solution containing excess copper II phosphate. When the reaction is completed, 1.25 grams of copper is formed. What is the percent yield DO NOT WRITE ON THIS SHEET
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