What is the difference between actual yield and theoretical yield? A) Actual yield has to do only with the reactants of a reaction, and theoretical yield has to do only with the products of a reaction. B) Actual yield is how much is actually produced in a reaction (it has to be given or measured), and theoretical yield is a calculation that has to be done. C) Actual yield is how much the reaction produces, and theoretical yield is how much a reaction consumes. D) Actual yield has to do with how much you can actually get out of a reaction, and theoretical yield is how much you can get out of a reaction if you have maximum starting materials.

What is the difference between actual yield and theoretical yield? A) Actual yield has to do only with the reactants of a reaction, and theoretical yield has to do only with the products of a reaction. B) Actual yield is how much is actually produced in a reaction (it has to be given or measured), and theoretical yield is a calculation that has to be done. C) Actual yield is how much the reaction produces, and theoretical yield is how much a reaction consumes. D) Actual yield has to do with how much you can actually get out of a reaction, and theoretical yield is how much you can get out of a reaction if you have maximum starting materials.

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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Why is theoretical yield important?
The actual yield of one of the reactions in 43.5g. What was theoretical yield in the laboratory if the scientist concluded that % yield of the reaction ended up to be 77%.
Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 4.29g of magnesium co ribbon burns with 9.01g of oxygen, a bright, white light and a white, powdery product are formed. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. Incorrect What is the limiting reactant? magnesium oxygen If the percent yield for the reaction is 84.9%, how many grams of product were formed? mass of product formed tneorrect How many grams of the excess reactant remain? mass of excess reactant: g
The mass of the product formed in an experiment is theoretical yield? True or false?
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Why is it essential to use balanced chemical equations when determining the quantity of a product formed from a given quantity of a reactant?
The theoretical yield of product for a particular reaction is 37.06 g. A very careless student obtained only 35.47 g of product after carrying out this reaction. What is the percent yield that this student obtained? Enter a number only; do not spell Include the correct number of significant figures for your answer Answer: % yield
A 0.206 g piece of solid magnesium reacts with gaseous oxygen from the atmosphere to form solid magnesium oxide. In the laboratory a student weighs the mass of the magnesium oxide collected from this reaction as 0.254 g. What is the percent yield of this reaction?
Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 3.51 g of magnesium ribbon burns with 8.71 g of oxygen, a bright, white light and a white, powdery product are formed. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. equation: What is the limiting reactant? magnesium oxygen If the percent yield for the reaction is 82.3%, how many grams of product were formed? mass of product formed: How many grams of the excess reactant remain? mass of excess reactant: g 50 g
Use this table to answer the following questions below: Before reaction Before reaction Theoretical yield Theoretical yield Actual yield Yes, it is balanced. Other: Is the chemical reaction involved balanced? If not, kindly type the correct balanced equation. Please take note that subscripts cannot be written properly. What is the percentage yield in this experiment? * 96.3% 93.6% CH3OH 32.0 g 1.00 mol 36.9% 63.9% CO Excess Excess CH3COOH 0 0 1.00 mol 60.0 g 57.8 g
The percent yield for a difficult reaction to be studied was likely to be only 51%of the theoretical yield. The prelab stiichiometric calculations predict that the theoretical yield should be 66.50g. What is the actual yield likely to be?