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4) The combustion of methane(CH4) produces carbon dioxide and water. Assume that 2.0 mol of CH4 burned in the presence of excess air. What is the percentage yield if in an experiment the reaction produces 87.0 g of CO2?

4) The combustion of methane(CH4) produces carbon dioxide and water. Assume that 2.0 mol of CH4 burned in the presence of excess air. What is the percentage yield if in an experiment the reaction produces 87.0 g of CO2?

Introductory Chemistry: An Active Learning Approach
Introductory Chemistry: An Active Learning Approach
6th Edition
ISBN:9781305079250
Author:Mark S. Cracolice, Ed Peters
Publisher:Mark S. Cracolice, Ed Peters
Chapter10: Quantity Relationships In Chemical Reactions
Section: Chapter Questions
Problem 70E: Classify each of the following statements as true or false: a Coefficients in a chemical equation...
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Actual Yield - The amount of product that actually forms when the reaction is carried out in the lab. -In real life, we never get as much as we anticipate, this "actual" amount from the lab experiment, Based on the stoichiometry of this problem, the Theoretical Yield for this problem is 12.79 g HF But, Percent Yield ProblemS Theoretical Yield- The maximum amount of product that can be formed from given react -Theoretical yield is the answer from the stoichiometry calculationmaximum possible amount Number based upon the heoretical" mathematical equation- no experiments were conducted Actual Yicd - The amount of product that actualty forms when the reaction is carried out ine --Due to a variety of factors, the actual amount will ALWAYS be less than the theoretical vie -In real life, we never get as much as we anticipate, this "actual" amount from the lab Percent Yield = The ratio of the actual vield 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 w grams of calcium hydroxide in the following reaction? 1 Ca(OH)2 + 2. HF >1 CaF2+_2 H;0 1 mol Ca(OH)2 2 mol HF 20.01 g HF 23.68 g Ca(OH): X X -------- 1 mol Ca(OH)2 ---- X = 12.79 gHE 74.10 g Ca(OH)2 1 mol HF Based on the stoichiometry of this problem, the Theoretical Yield for this problem is 12.79 g HE when this experiment was conducted, an Actual Yield of only 10.41 g HF was collected, UsinoB equation for percent yield, the Percent Yield of this experiment was 81.39%. 10.41g HF. 12.79g HF x 100 = 81.39% Actual Theoretical Percent Yield = x 100 = 1) A student adds 200.0g of C7H6O3 to an excess of C4H6O3, this produces CsH&O4 and C2H4O2 Calculate the percent yield if 231 g of aspirin (CoH&O4) is produced in an experiment V CzHeO3 +l CAH6O3 →_C9H8O4 + _C2H4O2 2) According to the following equation, Calculate the percentage yield if 550.0 g of toluene (C;Hg )added to an excess of nitric acid (HNO3) provides 305 g of the p-nitrotoluene (C¬H;NO, ). product in a lab experiment. C7H8 + _HNO3 →C7H7NO2 + 3 Aluminum reacts with an aqueous solution containing excess copper (II) sulfate. If 1.85 g AI reacts and the percentage yield of Cu is 56.6%, what mass of Cu is produced? 2Al +3CUSO4 Cu +_Al2(SO4)3 4) The combustion of methane(CH4) produces carbon dioxide and water. Assume that 2.0 mol of CH4 burned in the presence of excess air. What is the percentage yield if in an experiment 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:Actual Yield - The amount of product that actually forms when the reaction is carried out in the lab. -In real life, we never get as much as we anticipate, this "actual" amount from the lab experiment, Based on the stoichiometry of this problem, the Theoretical Yield for this problem is 12.79 g HF But, Percent Yield ProblemS Theoretical Yield- The maximum amount of product that can be formed from given react -Theoretical yield is the answer from the stoichiometry calculationmaximum possible amount Number based upon the heoretical" mathematical equation- no experiments were conducted Actual Yicd - The amount of product that actualty forms when the reaction is carried out ine --Due to a variety of factors, the actual amount will ALWAYS be less than the theoretical vie -In real life, we never get as much as we anticipate, this "actual" amount from the lab Percent Yield = The ratio of the actual vield 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 w grams of calcium hydroxide in the following reaction? 1 Ca(OH)2 + 2. HF >1 CaF2+_2 H;0 1 mol Ca(OH)2 2 mol HF 20.01 g HF 23.68 g Ca(OH): X X -------- 1 mol Ca(OH)2 ---- X = 12.79 gHE 74.10 g Ca(OH)2 1 mol HF Based on the stoichiometry of this problem, the Theoretical Yield for this problem is 12.79 g HE when this experiment was conducted, an Actual Yield of only 10.41 g HF was collected, UsinoB equation for percent yield, the Percent Yield of this experiment was 81.39%. 10.41g HF. 12.79g HF x 100 = 81.39% Actual Theoretical Percent Yield = x 100 = 1) A student adds 200.0g of C7H6O3 to an excess of C4H6O3, this produces CsH&O4 and C2H4O2 Calculate the percent yield if 231 g of aspirin (CoH&O4) is produced in an experiment V CzHeO3 +l CAH6O3 →_C9H8O4 + _C2H4O2 2) According to the following equation, Calculate the percentage yield if 550.0 g of toluene (C;Hg )added to an excess of nitric acid (HNO3) provides 305 g of the p-nitrotoluene (C¬H;NO, ). product in a lab experiment. C7H8 + _HNO3 →C7H7NO2 + 3 Aluminum reacts with an aqueous solution containing excess copper (II) sulfate. If 1.85 g AI reacts and the percentage yield of Cu is 56.6%, what mass of Cu is produced? 2Al +3CUSO4 Cu +_Al2(SO4)3 4) The combustion of methane(CH4) produces carbon dioxide and water. Assume that 2.0 mol of CH4 burned in the presence of excess air. What is the percentage yield if in an experiment 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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