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.
Introductory Chemistry: An Active Learning Approach
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Chapter10: Quantity Relationships In Chemical Reactions
Section: Chapter Questions
Problem 41E: Ammonia can be formed from a combination reaction of its elements. A small fraction of an unreacted...
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Question
#2 please of post laboratory question.
![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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1b897147-dac4-49d3-a0b7-87acbe9c344d%2F724a2d6c-40a0-4ef9-872d-7d3f05c7aa3f%2Fge7xq8_processed.jpeg&w=3840&q=75)
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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1b897147-dac4-49d3-a0b7-87acbe9c344d%2F724a2d6c-40a0-4ef9-872d-7d3f05c7aa3f%2Fewc63tj_processed.jpeg&w=3840&q=75)
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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