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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TABLE 3. PERCENT YIELD Mass salicylic acid 9 Mass of synthesized aspirin g 9 Theoretical Yield (aspirin) Percent Yield % Calculations: Note: Show calculations in a separate bond paper. (For the percent yield, you must first determine the limiting reactant from the following data: molar mass of salicylic acid = 138 g; molar mass of acetic anhydride = 102 g; density of acetic anhydride = 1.08 g/mL). TABLE 4. MELTING POINT DATA Sample Melting Point Range salicylic acid synthesized aspirin
A pile of leaves is lit on fire, and then covered completely with a fire blanket so that the fire goes out. Identify the limiting reactant in this situation.
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
For the following reaction, 0.350 moles of carbon (graphite) are mixed with 0.266 moles of oxygen gas. carbon (graphite)(s) + oxygen(g) → carbon dioxide(g) What is the formula for the limiting reagent? What is the maximum amount of carbon dioxide that can be produced? moles
An excess of sodium carbonate, Na, CO2, in solution is added to a solution containing 17.03 g CaCl,. After performing the experiment, 14.51 g of calcium carbonate, CACO,, is produced. Calculate the percent yield of this reaction. 3> percent yield:
Chemicals won’t react unless you have added the right ratios. If you are trying to create a product, you must add the correct amounts of reactants; otherwise it won’t form. When you balance an equation, it will inform you about how much of the reactant you need, which will enable you to guess how much product you will make. You must establish a ratio for the reaction to occur. In your opinion, which one of these reasons is the best? Justify your response. In your opinion, which of these reasons is the worst? Justify your response. Develop a different plausible explanation and share.
DDT, which can be prepared by the reaction shown below, was an insecticide used to prevent mosquito borne diseases. Due to the harmful effects on birds and fish, it is now banned in the US. However, other countries still use it to control mosquitos. Determine the amount of DDT that can be produced and the percent yield for this reaction by constructing a BCA table, determining the maximum grams of DDT that can be produced, and calculating the percent yield. Complete Parts 1-3 before submitting your answer. 1 Before (mol) Change (mol) After (mol) 2 C₂H₂CI+ C₂HOCI → C₁H₂Cl + H₂O 3 14 9 5 2 3 NEXT > If a company in South America started with 1175 g of chlorobenzene (CH₂CI, MW 112.55 g/mol) and 538.5 g of chloral (C₂HOCI, MW 147.39 g/mol), set up the table below that represents 100% yield with the given reaction conditions. 2 C₂H₂CI + C₂HOCI CH.CI 14 9 5 + H₂O
What is the relationship between limiting reactant and theoretical yield? The limiting reactant is the reactant that runs out, so it will determine the theoretical yield of product The limiting reactant is the reactant that is put in first, so it will determine the theoretical yield of product The limiting reactant is the reactant you have the most of, so it determines the theoretical yield of product The limiting reactant is the reactant you have less of, so it determines the theoretical yield of product
Why is it essential to use balanced chemical equations when determining the quantity of a product formed from a given quantity of a reactant?
Consider the following reaction for the synthesis of acetic acid, which can occur in certain bacteria: ?CO2 + ?H2 ?CH;COOH + ?H,0 If you start with 70.7 g of CO, and 17.2 g of H2, what is the theoretical yield of acetic acid? State your answer in g (without units). Hint: equation is not balanced (note the "?" marks).
Vocabulary Assignment: Quantity Relationships in Chemical Reactions 1. Stoichiometry - 2. Give an example of a balanced equation to show how to obtain conversion factors - 3. Write a stepwise mass to mass conversion for calculating mass of desired or wanted chemical given the mass of one chemical the balanced chemical equation - 4. What is the theoretical yield and how is it calculated? - 5. What is the actual or experimental yield? - 6. Write the formula for the percent yield why is this number important?- 7. Limiting reactant - 8. Use the comparison of calculated mass method to determine limiting reactan - 9. Excess reactant - 10. energy - 11. Joule - 12. Calorie - 13. Enthalpy of reactions and its relationship to exothermic and endothermic reactions- 14. Write a stepwise mass to energy conversion using a thermochemical equation to calculate energy of a reaction - short and sweet please! thank you!