how would you do number 3? Percent Yield ProblemsTheoretical 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 conductedActual 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 experiThe amount of product that actually forms when the reaction is carried out in the lakPercent Yield - The ratio of the actual yield to the theoretical yield expressed as a percentage,ActualTheoreticalPercent Yield-x 100EXAMPLE) How many grams of hydrofluoric acid (HF) are required to react completely with 23 8grams of calcium hydroxide in the following reaction?1 Ca(OH)2 +2_ HF → 1 CAF2+ 2 H201 mol Ca(OH)22 mol HF20.01 g HF23.68 g Ca(OH): X= 12.79 g HF|74.10 g Ca(OH)21 mol Ca(OH)21 mol HFBased 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 theequation for percent yield, the Percent Yield of this experiment was 81.39%.Actual x 100 =Theoretical10.41g HF,x 100 = 81.39%12.79g HFPercent Yield =1) A student adds 200.0g of C7H6O3 to an excess of C4H®O3, thịs produces C9H&O4 andC2H4O2. Calculate the percent yield if 231 g of aspirin (C9H8O4) is produced in an experiment.V C7H6O3 +CAH6O3 _C9H%O4 + 1_ C2H4O22) 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 +H2O3 Aluminum reacts with an aqueous solution containing excess copper (II) sulfate. If 1.85 g Alreacts and the percentage yield of Cu is 56.6%, what mass of Cu is produced?Al +3CUSO4 →_Cu +_Al2(SO4)34) The combustion of methane(CH4) produces carbon dioxide and water. Assume that 2.0 mcof CH4 burned in the presence of excess air. What is the percentage yield if in an experimenthe 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 yieldDO NOT WRITE ON THIS SHEET

3. Given :- Balanced chemical equation : 2 Al + 3 CuSO4 ---> 3 Cu + Al2(SO4)3 amount of Al =…

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

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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Classify each of the following statements as true or false: a Coefficients in a chemical equation express the molar proportions among both reactants and products. b A stoichiometry problem can be solved with an unbalanced equation. c In solving a stoichiometry problem, the change from quantity of given substance to quantity of wanted substance is based on masses. d Percentage yield is actual yield expressed as a percentage of ideal yield. e The quantity of product of any reaction can be calculated only through the moles of the limiting reactant. f rH is positive for an endothermic reaction and negative for an exothermic reaction.
Apply When a campfire begins to die down and smolder, you can rekindle the flame by fanning the fire. Explain, in terms of stoichiometry, why the fire again begins 10 flare up when fanned.
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Refer to this equation: 3SCl2 + 4NaF --> SF4 + S2Cl2 + 4NaCl 64.0 grams SCl2 is reacted with excess NaF and 12.5 grams of SF4 is formed. What is percent yield SF4? Hint: find theoretical yieldHint: percent yield =(actual yield/ theoretical yield) x 100
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My actual yield is 17.64 need thoeritcal yield and percent yield calculated help photo helps you what to do and explains what not to do
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match the folowing terms. one answer will not be used. Left Side: limiting reactant actual yield theoretical yield percent yield mole ratio Right Side (match) maximum amount of product that could produced relationship between two different components of a balanced equation the reaction component that is consumed entirely the reaction component that is present in excess the actual yield divided by the theoretical yield 100 times amount of product physically produced from a reaction