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Post Laboratory Questions 1. Based on your data and observation: a. Which of the reactants in your experiment was the limiting reagent? Briefly explain. b. Which of the reactants in your experiment was present in excess? Briefly explain. 2. You have reacted copper chloride solution with Zn metal to precipitate out all the Cu in its elemental form. a. Based on the empirical formula you determined for copper chloride, present the balanced chemical equation for this experiment. b. Based on the mass of Zn reacted and your equation in 2 a, how much Cu do you expect to produce (the theoretical yield)? Mass of Zn reacted = _____g Theoretical yield of Cu = .9 c. Determine the percent yield of Cu from your determination.

Post Laboratory Questions 1. Based on your data and observation: a. Which of the reactants in your experiment was the limiting reagent? Briefly explain. b. Which of the reactants in your experiment was present in excess? Briefly explain. 2. You have reacted copper chloride solution with Zn metal to precipitate out all the Cu in its elemental form. a. Based on the empirical formula you determined for copper chloride, present the balanced chemical equation for this experiment. b. Based on the mass of Zn reacted and your equation in 2 a, how much Cu do you expect to produce (the theoretical yield)? Mass of Zn reacted = _____g Theoretical yield of Cu = .9 c. Determine the percent yield of Cu from your determination.

Chemistry
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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Post Laboratory Questions 1. Based on your data and observation: a. Which of the reactants in your experiment was the limiting reagent? Briefly explain. b. Which of the reactants in your experiment was present in excess? Briefly explain. 2. You have reacted copper chloride solution with Zn metal to precipitate out all the Cu in its elemental form. a. Based on the empirical formula you determined for copper chloride, present the balanced chemical equation for this experiment. b. Based on the mass of Zn reacted and your equation in 2 a, how much Cu do you expect to produce (the theoretical yield)? Mass of Zn reacted = Theoretical yield of Cu = g g c. Determine the percent yield of Cu from your determination.
Transcribed Image Text:Post Laboratory Questions 1. Based on your data and observation: a. Which of the reactants in your experiment was the limiting reagent? Briefly explain. b. Which of the reactants in your experiment was present in excess? Briefly explain. 2. You have reacted copper chloride solution with Zn metal to precipitate out all the Cu in its elemental form. a. Based on the empirical formula you determined for copper chloride, present the balanced chemical equation for this experiment. b. Based on the mass of Zn reacted and your equation in 2 a, how much Cu do you expect to produce (the theoretical yield)? Mass of Zn reacted = Theoretical yield of Cu = g g c. Determine the percent yield of Cu from your determination.
Data mass of copper chloride in 25.0 mL of solution, g initial mass of Zn, g mass of Zn after reaction, g mass of Zn reacted, g filter mass of wax paper, g mass of wax paper + Cu, g after 5 min. on 51.686Büchner funnel, g 51.684 after additional 5 min. on bench, g 51.674 after another 5 min. on bench, g mass of Cu produced, g mass of Cl in copper chloride, g moles of Cu in copper chloride, mol moles of Cl in copper chloride, mol empirical formula of copper chloride 2.021 g 1.636 9 g 0.6859 0.298 Glass dish : 50.572 0.816 0.814 0.804 0.804ą 1.2119 0.0127 0.0343 CuClz Section Calculation: Mass of Cu: Chem 1083-07 0.814-0.804=0.01 20.05 Mass of CI: 0.804 + (mass of (1) = 2.021g 2.021=0.804 = 1.217g Moles of Cu: class ? poper 0.804 x 63.546 -39- =0.0127 Moles of Cl: 1.217 g * 35.453 = 0.0343 mol c Empirical Formula: 0.0127 0.0127 = 1 (v: 2.7CI = ICU: 3C1 mol Cv 0.0343 mol Cv 0.0127 mol =CUC13
Transcribed Image Text:Data mass of copper chloride in 25.0 mL of solution, g initial mass of Zn, g mass of Zn after reaction, g mass of Zn reacted, g filter mass of wax paper, g mass of wax paper + Cu, g after 5 min. on 51.686Büchner funnel, g 51.684 after additional 5 min. on bench, g 51.674 after another 5 min. on bench, g mass of Cu produced, g mass of Cl in copper chloride, g moles of Cu in copper chloride, mol moles of Cl in copper chloride, mol empirical formula of copper chloride 2.021 g 1.636 9 g 0.6859 0.298 Glass dish : 50.572 0.816 0.814 0.804 0.804ą 1.2119 0.0127 0.0343 CuClz Section Calculation: Mass of Cu: Chem 1083-07 0.814-0.804=0.01 20.05 Mass of CI: 0.804 + (mass of (1) = 2.021g 2.021=0.804 = 1.217g Moles of Cu: class ? poper 0.804 x 63.546 -39- =0.0127 Moles of Cl: 1.217 g * 35.453 = 0.0343 mol c Empirical Formula: 0.0127 0.0127 = 1 (v: 2.7CI = ICU: 3C1 mol Cv 0.0343 mol Cv 0.0127 mol =CUC13
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