Chemical reactions in the real world don't always go exactly as planned on paper. In the course of an experiment, many thingswill contribute to the formation of less product than would be predicted. Besides spills and other experimental errors, there areusually losses due to an incomplete reaction and undesirable side reactions. Chemists need a measurement that indicates howsuccessful a reaction has been. This measurement is called the percent yield.To compute the percent yield, it is first necessary to determine how much of the product should be formed based onstoichiometry. This is called the theoretical yield, the maximum amount of product that could be formed from the givenamounts of reactants. The actual yield is the amount of product that is actually formed when the reaction is carried out in thelaboratory. The percent yield is the ratio of the actual yield to the theoretical yield, expressed as a percentage.Percent yield is very important in the manufacture of products. Much time and money is spent improving the percent yield forchemical production. When complex chemicals are synthesized by many different reactions, one step with a low percent yieldcan quickly cause a large waste of reactants and unnecessary expense.Typically, percent yields are understandably less than 100 % because of the reasons indicated earlier. However, percent yieldsgreater than 100% are possible if the measured product of the reaction contains impurities that cause its mass to be greaterthan it actually would be if the product was pure. When a chemist synthesizes a desired chemical, he or she is always careful topurify the products of the reaction. StoichiometryTheoretical, Actual, & Percent Yields1. According to the article, what is "theoretical yield"?2. According to the article, what is "actual yield"?3. According to the article, which yield isdetermined from stoichiometry calculations?●4. According to the article, why is it necessary to calculate apercent yield for each reaction?Answer these questions, using this text on Slide #1 for reference.On Slide #1, highlight the areas where you found the answers.5. According to the article, why might some reactions produce anactual yield less than the theoretical yield?6. According to the article, why might some reactions produce anactual yield greater than the theoretical yield?

The given questions have to be answered by studying the given article which is about yield of the…

Theoretical, Actual, & Percent Yields 1. According to the article, what is "theoretical yield"? 2. According to the article, what is "actual yield"? 3. According to the article, which yield is determined from stoichiometry calculations? OR Slide #1, highlight the areas where you found the answers. 4. According to the article, why is it necessary to calculate a percent yield for each reaction? 5. According to the article, why might some reactions produce an actual yield less than the theoretical yield? 6. According to the article, why might some reactions produce an actual yield greater than the theoretical yield.

Theoretical, Actual, & Percent Yields 1. According to the article, what is "theoretical yield"? 2. According to the article, what is "actual yield"? 3. According to the article, which yield is determined from stoichiometry calculations? OR Slide #1, highlight the areas where you found the answers. 4. According to the article, why is it necessary to calculate a percent yield for each reaction? 5. According to the article, why might some reactions produce an actual yield less than the theoretical yield? 6. According to the article, why might some reactions produce an actual yield greater than the theoretical yield.

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Two experimental procedures have the same reactants and the same products. Procedure A has 4 steps between reactants and products. Procedure B has 2 steps. Which procedure is likely to have a higher % yield and why? Be detailed and write in complete sentences.
QUESTION 23 Which of the following statements is false? The limiting reactant is completely consumed in a chemical reaction. O The theoretical yield is the amount of product that can be made based on the amount of limiting reagent. O The actual yield is the amount of product actually produced by a chemical reaction. O The percent yield = (actual yield/theoretical yield) x 100% O All of the above are true statements.
Aspirin can be synthesized in the lab by combining salicylic acid (C,H,0,) and acetic anhydride (C,H,0,) to form aspirin ( C,H,O,) and acetic acid (C,H,O,). The balanced equation for this reaction is C,H,O, + C,H,O, → C,H,0, + C,H,O, A student started with 3.33 mL acetic anhydride (density = 1.08 g/mL) and 2.61 g salicylic acid. The student synthesized 2.53 g of aspirin. Select the limiting reactant. salicylic acid (C, H,0,) acetic anhydride (C,H,O;) aspirin (C,H,O,) O acetic acid (C,H,O,) Calculate the theoretical yield of aspirin (C,H,O,). theoretical yield: Calculate the percent yield for aspirin (C,H,O).
Do not give handwriting solution. Determine the percent yield to two decimal places if 5.53 g of alum are synthesized using 0.43 g of aluminum. (MM Al = 26.98 g/mol; MM alum = 474.38 g/mol)
* Question Completion Status: A Moving to another question will save this response. Question 25 "How many grams of carbon dioxide will be produced by the complete combustion of 50 grams of C 5H 12? With 128.62grams of oxygen? Enter the coefficients for the balanced chemical equation (enter "" 1" for compounds without a coefficient) C5H 12+ 02 - H20 How many grams of carbon dioxide are produced from the amount of hydrocarbon? round your answer to the nearest whole number How many grams of carbon dioxide are produced from the amount ofoxygen? round your answer to the nearest whole number Which is reactant is the limiting reactant? type ""oxygen"" or ""hydrocarbon"" How many grams of carbon dioxide is produced? round your answer to the nearest whole number A Moving to another question will save this response.
Answer the question below please!!
Iron reacts with oxygen at high temperatures to form iron(III) oxide. 4 Fe(s) + 30,(g) 2 Fe,0,(s) Suppose 17.2 g of iron (Fe) is reacted with 16.6 g of oxygen (0,). Select the limiting reagent. O2 Fe O Fe,O, Calculate the theoretical yield of iron(II) oxide (Fe, O,). 3 ald
The combustion of methane produces carbon dioxide and water. Assume that 52.8 grams of methane burned in the presence of excess oxygen gas. The percent yield is __________ percent if the reaction produces 100.9 grams of carbon dioxide.
1) The Law of Conservation of Mass states that the total mass, in an open system, does not change as the result of reactions between its parts. True False 2) The deviation from the theoretical yield to the actual yield is called the percent yield. True False
Hi! I need help with these limiting reactants questions from my Chem class please
Please correct answer and don't use hand rating