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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Calculate the theoretical yield of the product. The recorded weight of the product was 3.48grams. Use this information and the UV-vis data to calculate the theoretical yield of the product.
Transcribed Image Text:Serial Number:
ROM Version:
Sample Name:
Date:
Operator:
3.000
U-2800 Spectrophotometer
1720024
11
0
02/06/24 16:45
ABS
0.000
Peak
250.0
Wavelength Scan
Data Mode:
Start WL (nm):
Stop WL (nm):
Scan Speed (nm/min):
Sample Interval (nm):
Baseline:
Response:
Slit Width (nm):
Path Length (mm):
Lamp Change Mode:
Lamp Change WL (nm):
ID WL (nm)
1
684.0
ABS
0.203
ABS
750.0
250.0
400
0.5
1
User1
Medium
1.5
10.0
Auto
340.0
ID
2
WL (nm)
586.5
A
ABS
0.125
ID
3
WL (nm)
253.5
(
750.0 nm
ABS
0.991
![The tetrahedral tetrachlorocobaltate(II) salts are an excellent contrast to the
octahedral Werner complexes of cobalt(III). Their preparation utilizes large
counter-cations to crystallize the complex from a weakly coordinating solvent.¹
The synthesis of tetrachlorocobaltate(II) salts again begins with CoCl2-6H₂O:
2 NEt4Cl + CoCl2 6H2O (NEt4)2COCI4+ 6H₂O
[eq. 1]
Dissolve 2.6 g NEt4CI-H₂O in 30 mL absolute ethanol. Add a solution of
1.78 g CoCl2-6H₂O in 35 mL absolute ethanol. The desired compound crystallizes
at this stage as a blue precipitate. Heat the solution to 75 °C, adding more
ethanol if necessary to obtain a clear solution. Slowly cool to crystallize the
compound as deep blue crystals. Collect the crystals with a sintered glass filter (a
Buchner funnel is ok but use two pieces of filter paper). Analyze the product by
FTIR (use separate spatulas for sample and KBr) and UV-Vis spectroscopy
(accurately measure 7 mg sample in precisely 25 mL of acetonitrile; plastic
cuvettes are ok to use). Calculate the extinction coefficient of the complex and the
percent yield.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd6957468-6fb1-4659-9083-987b06676d6d%2Fde5e9871-745a-46fe-8e1c-20b7816b53e8%2Fpfgffo_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The tetrahedral tetrachlorocobaltate(II) salts are an excellent contrast to the
octahedral Werner complexes of cobalt(III). Their preparation utilizes large
counter-cations to crystallize the complex from a weakly coordinating solvent.¹
The synthesis of tetrachlorocobaltate(II) salts again begins with CoCl2-6H₂O:
2 NEt4Cl + CoCl2 6H2O (NEt4)2COCI4+ 6H₂O
[eq. 1]
Dissolve 2.6 g NEt4CI-H₂O in 30 mL absolute ethanol. Add a solution of
1.78 g CoCl2-6H₂O in 35 mL absolute ethanol. The desired compound crystallizes
at this stage as a blue precipitate. Heat the solution to 75 °C, adding more
ethanol if necessary to obtain a clear solution. Slowly cool to crystallize the
compound as deep blue crystals. Collect the crystals with a sintered glass filter (a
Buchner funnel is ok but use two pieces of filter paper). Analyze the product by
FTIR (use separate spatulas for sample and KBr) and UV-Vis spectroscopy
(accurately measure 7 mg sample in precisely 25 mL of acetonitrile; plastic
cuvettes are ok to use). Calculate the extinction coefficient of the complex and the
percent yield.
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Step 1: Given data and required constants
VIEWStep 2: The balanced chemical equation.
VIEWStep 3: Determination of the number of moles
VIEWStep 4: Determining the limiting reagent
VIEWStep 5: Determination of theoretical yield
VIEWStep 6: Percentage yield
VIEWStep 7: IR spectrum of the compound
VIEWStep 8: Determination of concentration of the sample for UV-visible studies
VIEWStep 9: Determination of extinction coefficient
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