= molecule A %3D = molecule B %3D Using the above figure, answer the following questions: A) What is the balanced equation for this reaction? [ Select ] B) What are the limiting and excess reactants? Limiting reactant = [ Select ] Excess reactant = [ Select ] C) If you wanted to completely react BOTH reactants (i.e., there is no limiting or excess reactant), how many of each would you need? [ Select ] D) The above picture represents the theoretical yield. Your actual yield is 7 product molecules. What is your percent yield? [ Select ]

= molecule A %3D = molecule B %3D Using the above figure, answer the following questions: A) What is the balanced equation for this reaction? [ Select ] B) What are the limiting and excess reactants? Limiting reactant = [ Select ] Excess reactant = [ Select ] C) If you wanted to completely react BOTH reactants (i.e., there is no limiting or excess reactant), how many of each would you need? [ Select ] D) The above picture represents the theoretical yield. Your actual yield is 7 product molecules. What is your percent yield? [ Select ]

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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For the sentence below answer the following questions: Q1) Change the sentence into a chemical equation Q2) What are the reactants and products? "1 mole of aqueous Pb(NO3)2 reacts with 2 moles of aqueous KI to produce 1 mole of solid Pbl, and 2 moles of aqueous KNO3."
Please follow the instructions on the paper Also for question 3 the reaction is on the top of the paper that you have to find the percentage yield for AGAIN PLEASE FOLLOW THE INSTRUCTIONS
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