# Educational Transcript and Explanation**Title: Understanding Reaction Sequences and Percent Yields in Chemistry**### IntroductionTo successfully tackle chemistry problems involving reaction sequences, it's essential to use a methodical approach:1. **Writing the Correct Balanced Equation:** Start with the balanced chemical equation for each reaction. 2. **Stoichiometric Calculations:** Use stoichiometric coefficients to convert quantities from one species to another.3. **Theoretical Yield Calculations:** Begin with the theoretical (or 100%) yield to understand the maximum possible product yield.4. **Percent Yield Considerations:** Use the percent yield of each reaction to determine actual yields.5. **Use of Tables:** Consider structuring the data in a table for clarity.### Detailed Example Problem**Question Prompt:**Consider a series of 5 sequential reactions, each using the product of the previous reaction. The percentage yields for these reactions are as follows: 80%, 90%, 65%, 76%, and 30%. If you start with 100 molecules of the initial limiting reagent, what is the maximum number of product molecules you can obtain at the end of the final reaction?**Hint:** Remember, fractional molecules are not possible.### Step-by-Step Solution Process1. **Identify Initial Quantity:** - Start with 100 molecules of the initial reagent.2. **Apply Percent Yield of Each Reaction Sequentially:** - **First Reaction:** - Yield = 80% of 100 molecules - Product = 0.8 × 100 = 80 molecules - **Second Reaction:** - Yield = 90% of 80 molecules - Product = 0.9 × 80 = 72 molecules - **Third Reaction:** - Yield = 65% of 72 molecules - Product = 0.65 × 72 = 46.8 → round down to 46 molecules (since fractional molecules are not possible) - **Fourth Reaction:** - Yield = 76% of 46 molecules - Product = 0.76 × 46 = 34.96 → round down to 34 molecules - **Fifth Reaction:** - Yield = 30% of 34 molecules - Product = 0.3 × 34 = 10.2 → round down to 10 molecules### ConclusionThrough this systematic approach

The five sequential reactions can be represented as:A →80% B →90% C →65% D →76% E →30% FLet the…

Consider 5 sequential reactions where the product of each reaction is the reactant of the next and the 5 percent yields are 80%, 90%, 65%, 76% and 30%. If you begin with 100 molecules of the first limiting reagent, what is the maximum number of product molecules you can form at the end of the final reaction? HINT: Remember that you cannot have parts of a molecule!

Consider 5 sequential reactions where the product of each reaction is the reactant of the next and the 5 percent yields are 80%, 90%, 65%, 76% and 30%. If you begin with 100 molecules of the first limiting reagent, what is the maximum number of product molecules you can form at the end of the final reaction? HINT: Remember that you cannot have parts of a molecule!

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...

See similar textbooks

Similar questions

What is the conversion factor between two different substances in a chemical reaction? 81°F Mostly sunny Esc F1 1 {0 atomic numbers mole ratio molar mass F2 mass ratio -8- @ 2 F3 -Ő+ #M 3 FA 54 $ F5 % 5 F6 T Q F7 < 6 F8 & 7 F9 ★ * 00 8 F10 9 F11 ) F12 a P Prt Sc
In initial state before CH4 and Cl2 is shown in the figure based on the balance equation in the future what is the limiting reactant? A. CCL4 B. CH4 C. HCL D. CL2
Which of the following is NOT true about "yield"? * The percent yield is the ratio of the actual yield to the theoretical yield. The value of the actual yield must be given in order for the percent yield to be calculated. The actual yield may be different from the theoretical yield because insufficient limiting reagent was used. The actual yield may be different from the theoretical yield because reactions do not always go to completion.
calculate how many moles of products would be produced if 0.500 mole of the first reactant were to react completely.
11. An old bike is left abandoned in a shed for many years, where it begins to rust. The bike is not exposed to rain or wind that would cause the rust to fall off the bike. Is the bike gaining mass, losing mass, or maintaining the same mass as it rusts? Explain. 12. Describe 2 factors that can reduce percent yield when a scientist is trying to create a specific chemical product. Explain specifically how each factor reduces percent yield. 13. How did decomposition reactions help early chemists come to the Law of Definite Proportions?
* 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.
Insert the correct number of atoms from each element on the reactant side of the equation
I Review | Constants | Periodic Table Many home barbeques are fueled with propane gas (C3H3). Part A What mass of carbon dioxide is produced upon the complete combustion of 12.1 L of propane (the approximate contents of one 5-gallon tank)? Assume that the density of the liquid propane in the tank is 0.621 g/mL. (Hint: Begin by writing a balanced equation for the combustion reaction.) Express your answer in kilograms. View Available Hint(s)
Directions: Write T if the statement is true and F it is false. Place your answers on the blank provided in each number. 1. Chemists need a measurement called percent yield to indicate how successful a reaction has been. _2. The theoretical yield is the ratio of the actual yield to the theoretical yield, expressed as a percentage. 3. The actual yield is the amount of product that is actually formed when the reaction is carried out in the laboratory. 4. The maximum amount of product that could be formed from the given amounts of reactants is called the percent yield.
Answer the question below please!!
Hi! I need help with these limiting reactants questions from my Chem class please
A grease fire started on the stove, it was then covered completely with a fire blanket so that the fire goes out. Identify the limiting reactant in this situation