Experiment:
Experiment: Date:
Simple and Fractional Distillation11/10/25
NamePartnersDrawer No.Course / Section
Katheryn SotoN/A#21CHEM 315/204
Purpose:
The purpose of this experiment is to determine the relative effectiveness of simple and fractional distillation in separating mixtures of organic compounds based on differences in boiling points.
Approach:
Perform Simple and fractional distillation using a Vigreux Fractionation Column on a mixture of Ethyl acetate and Butyl acetate with an unknown mole %. Compute the total volume recovered and percent volume recovered relative to the starting volume. Construct a bar graph comparing the two methods of distillation. Compute the masses of Ethyl acetate and Butly acetate. Compute the moles of Ethyl acetate and Butyl acetate. Calculate the total moles present in the mixture. Calculate the mole fractions of each component in the mixture. Calculate the mole percentage for each component of the mixture. Using the gas chromatograph, run a chromatogram of a standard equimolar mixture of the two compounds. From the chromatograph, compute the peak areas, total peak area, mole fraction and mole percents of distillates. Measure the refractive indexes of the isolated Ethyl acetate and Butyl acetate using the Abbe refractometer. Adjust raw refractive index values using the temperature correction factor.
References
Text
Pavia, D.L., Lampman, G.M., Kriz, G.S., Engel, .G.R., 2011, Introduction to Organic Laboratory Techniques, A Small Scale Approach, GMU Edition, Chem 315/318, Cengage Learning: pp. 729-740 Slayden, S., Stalick, W., Roth, R, 2014, Organic Chemistry Laboratory Manual, 2nd Edition: Pearson Custom Publishing: pp. 55-59
Web Site URL Dr Schornicks Website: http:/mason.gmu.edu/~jschorni/simple&fractionaldist
Unknown or Synthesized Compound
Ethyl acetate, 141-78-6, CRC Handbook of Chemistry & Physics, 84th Edition, Lide, D.R., Editor-in-chief, 2003-2004, CRC Press, p 3-250, 4871.
Butyl acetate, 123-86-4, CRC Handbook of Chemistry & Physics, 84th Edition, Lide, D.R., Editor-in-chief, 2003-2004, CRC Press, p 3-80, 1487.
Proc # 1Simple and Fractional DistillationResultsUnk No.A
MaterialsEquipmentSimple and Fractional Distillation
Volume (mL)
Temp (oC)SimpleFractional0-65
0065-70
0070-75
0.5075-80
3.1080-85
1.2085-90
3.1090-95
2.60.7Vol Vial 1:
10.50.7Vial 1 = distillate up to 95oC (Mostly EtAc B.P.=77.1oC)
Temp (oC)Simple
Fractional
95-100
2.01.0100-105
0.84.2Vol Vial 2:
2.85.2Vial 2 = distillate from 95-105oC
Temp (oC)Simple
Fractional
105-110
0.54.1110-115
0.30.2115-120
1.90.5120-125
1.60.2125-130
1.60.1Pot Residue
06.0Vol Vial 3:
5.911.1Vial 3 =distillate above 105oC (Mostly BuAc B.P.=126.0oC)
Observations Pot residue that remained after simple distillation was negligible (less than 1mL)
Unknown molarity ethyl acetate/butyl acetate mixture A Heating Block
Heating Plate
50 mL Distillation Flask Aluminum plate
Sand bath Teflon boiling chip Distillation Head
Thermometer
Thermometer Adapter
Water Jacket Condenser
2 10 mL graduated cylinders
3 labeled vials with sealing caps
Desc:
Place 20 mL of mixture in 50 mL round bottom flask Heat the mixture gently on a hot plate
Collect distillate in a 10 mL graduated cylinder until the temperature rises to 65oC. Record volume of distillate. Collect volumes of distillate in 5oC increments, until temperature reaches 95oC recording the volume of distillate collected for each increment. Record the total volume collected.
Transfer the volume collected from 0oC-95oC to the first labeled vial. Continue to collect distillate in 5 degree increments from 95oC to 105oC.
Record the total volume collected. Transfer to the second labeled vial. Increase the temperature of the hotplate Continue to collect distillate in 5oC increments until 1mL of solution remains in the distillation flask Allow solution remaining in the distillation head and column to cool and drain back into the distillation flask. Transfer this pot residue to a 10mL graduated cylinder. Record volume and transfer to the third labeled vial. Repeat procedure adding the Vigreux column between the distillation flask and the distillation head to perform fractional distillation with the solution.
Do not distill to dryness (1mL should remain in the flask when distillation is complete)
Equation Setup:
Proc # 2Total Volume RecoveredResults
MaterialsEquipmentTotal Volume RecoveredSimple
Fractional
Vol Vial 1
10.5 mL0.7mLVol Vial 2
2.8 mL5.2 mLVol Vial 3
5.9 mL11.1 mLTotal 19.2 mL17.0 mLInitial 20.0 mL
20.0 mL
Lost
0.8 mL3.0 mL Simple
Total (mL) = 10.5 + 2.8 + 5.9 = 19.2Lost = 20.0 19.2 = 0.8
Fractional
Total (mL) =0.7 + 5.2 + 11.1 = 17.0Lost = 20.0 -17.0 = 3.0
Calculator
Desc:
Compute the total volume recovered by adding.
Equation Setup:
Total Volume Recovered (mL) = Vol Vial 1 + Vol Vial 2 + Vol Vial 3
Proc #5Percent Volume RecoveredResults
MaterialsEquipmentPercent Volume Recovered
Simple
Fractional
Vol (mL)%Vol (mL)%Vial 1
10.554.70.74.1Vial 2
2.814.65.230.6Vial 3
5.930.711.165.3Total19.217.0Simple
Vial 1
(10.5 / 19.2) * 100 = 54.7%Vial 2
(2.8 / 19.2) * 100 = 14.6%Vial 3
(5.9 / 19.2) * 100 = 30.7%FractionalVial 1
(0.7 / 17) * 100 = 4.1%Vial 2
(5.2 / 17) * 100 = 30.6%Vial 3
(11.1 / 17) * 100 = 65.3%
Calculator
Desc:
Compute percent volume recovered for each of the fractional volumes collected for the simple and fractional distillations of the mixture.
Equation Setup:
Proc #6Total Volume RecoveredResults
MaterialsEquipmentTotal Volume Recovered:SimpleTemperature (Co)Volume (mL)0-95
10.595-105
2.8105-130
5.9Total
19.2Total Volume Recovered:Fractional
Temperature (Co)
Volume (mL)
0-95
0.795-105
5.2105-130
11.1Total
17.0Simple0-95oC
0.5 + 3.1 + 1.2 + 3.1 + 2.6 = 10.5mL95-105 oC
2.0 + 0.8 = 2.8mL105-130 oC
0.5 + 0.3 + 1.9 + 1.6 + 1.6 = 5.9mLFractional0-95oC
0.7 = 0.7mL95-105 oC
1.0 + 4.2 = 5.2mL
105-130 oC4.1 + 0.2 + 0.5 + 0.2 + 0.1 + 6.0 = 11.1mL
Calculator
Desc:
Determine total volumes recovered for specified temperature ranges by computing the sum of the fractional volumes.
Equation Setup:
Proc # 2Bar GraphResults
MaterialsEquipment
Calculator
Desc:
Plot results of simple and fractional distillations in a bar graph with temperature increments on the x-axis and volume increments on the y-axis
Equation Setup:
Proc #7 Mass of CompoundsResults
MaterialsEquipmentMass of Compounds
Simple
Fractional
Density (g/mL)Vol (mL)
Mass (g)
Vol (mL)
Mass (g)
EtAc0.900613.311.985.95.31BuAc0.88255.95.2111.19.80SimpleVol EtAc = 10.5 + 2.8 = 13.3mLVol BuAc = 5.9mLMass EtAc = 0.9006 * 13.3 = 11.98g
Mass BuAc = 0.8825 * 5.9 = 5.21gFractional
Vol EtAc = 0.7 + 5.2 = 5.9mLVol BuAc = 11.1mLMass EtAc = 0.9006 * 5.9 = 5.31gMass BuAc = 0.8825 * 11.1 = 9.80g
Calculator
Desc:
Assume vials 1 and 2 represent Ethyl acetate.
Assume vial 3 represents Butyl acetate
Calculate the mass of each compound collected from the respective volumes and densities of each compound
Equation Setup:
Vol EtAc = Vial 1 (mL) + Vial 2 (mL)
Vol BuAc = Vial 3 (mL)
Proc #8 Moles of CompoundsResults
MaterialsEquipmentMoles of Compounds
Simple
Fractional
M.W. (g/mol)Mass (g)
Mol
Mass (g)
Mol
EtAc
88.1111.980.1365.310.062BuAc
116.165.210.0459.800.084Simple
Mol EtAc = 11.98 / 88.11 = 0.136molMol BuAc = 5.21 / 116.16 = 0.045molFractionalMol EtAc = 5.31 / 88.11 = 0.062molMol BuAc = 9.80 / 116.16 = 0.084mol
Calculator
Desc:
Compute the moles of each compound using their masses and molecular weights
Equation Setup:
Proc #9 Total MolesResults
MaterialsEquipmentTotal Moles
Simple
FractionalEtAc (mol)0.1360.062BuAc (mol)0.0450.084Total
0.1810.146SimpleTotal = 0.136 + 0.45 = 0.181molFractionalTotal = 0.062 + 0.084 = 0.146mol
Calculator
Desc:
Compute the total moles in the two fractions
Equation Setup:
Proc #10 Mole FractionResults
MaterialsEquipmentMole Fraction
Simple
Fractional
EtAc (mol)
0.1360.062BuAc (mol)
0.0450.084Total Mol
0.1810.146Fract. EtAc0.7510.425Fract. BuAc0.2490.575Simple
Mol Fraction EtAc = 0.136 / 0.181 = 0.751Mol Fraction BuAc = 0.045 / 0.181 = 0.249Fractional
Mol Fraction EtAc = 0.062 / 0.146 = 0.425Mol Fraction BuAc = 0.084 / 0.146 = 0.575
Calculator
Desc:
Computed by dividing the total moles for each compound respectively by the total combined moles for each distillation. Fractional representation of the number of moles of each compound that resulted from each distillation
Equation Setup:
Proc #11 Mole PercentResults
MaterialsEquipmentMole Percent
Simple
Fractional
EtAc
0.7510.425BuAc
0.2490.575Mol % EtAc75.142.5Mol % BuAc24.957.5SimpleMole % EtAc = 0.751 * 100 = 75.1%Mole % BuAc = 0.249 * 100 = 24.9%FractionalMole % EtAc = 0.425 * 100 = 42.5%Mole % BuAc = 0.575 * 100 = 57.5%
Calculator
Desc:
Compute by multiplying the mole fraction for each compound by 100 for each distillation
Equation Setup:
Proc #12 Gas ChromatographyResults
MaterialsEquipmentInstrument ReadingsInjection port temp.
120oC
Column temp.
120oC
Detector temp.
120oC
Chart Speed25.0mm/minGas flow rate
10 mL/min (He @ 7PSI)Moving liquid phase
Supelco Carbowax 20m, 6 ft
2L Standard ether sample
2L Of each vial collected for simple and fractional distillations Gas chromatography
Microsyringe
Desc:
Begin a new chromatogram.
Rinse the microsyringe several times with the sample solution.
Insert the syringe into the sample solution and raise and depress the plunger several times to remove any air bubbles from the syringe.
Load the microsyringe with a small amount of sample (2L).
Insert the syringe into the chromatograph port through the rubber septum.
Quickly inject the sample and withdraw the syringe from the port
Wait approximately 5 minutes to allow the sample to be analyzed.
Print resulting chromatogram. Rinse the syringe with the sample solution several times.
Repeat steps with additional samples.
Equation Setup:
Proc #13 Peak AreasResults
MaterialsEquipmentPeak Areas-Standard Soln.Peak
Height (mm)
(mm)
Peak Area (mm2)
C2
176
5
88
C4
149
7
104
AreaC4 = 149 * 7= 104
AreaC2 = 176 * 5 = 880
Peak Areas
SamplePeak
Height (mm)
(mm)
Peak Area (mm2)
A
C290.05.0450.0C469.06.0414.0SimpleS1C2
57.53.0172.5C4
9.02.522.5S2C2
117.06.0702.0C4
49.59.0445.5S3C2
20.04.590.0C4
124.56.0747.0Fractional
F1C2
000C4
000F2C2
123.56.0741.0C4
9.07.063.0F3C2
93.04.0372.0C4
128.05.5704.0Sample A
AreaC2 = 90.0 * 5.0 = 450.0mm2AreaC4 = 69.0 * 6.0 = 414.0mm2Simple S1AreaC2 = 57.5 * 3.0 = 172.5mm2AreaC4 = 9.0 * 2.5 = 22.5mm2Simple S2
AreaC2 = 117.0 * 6.0 = 702.0mm2AreaC4 = 49.5 * 9.0 = 445.5mm2Simple S3
AreaC2 = 20.0 * 4.5 = 90.0mm2AreaC4 = 124.5 * 6.0 = 747.0mm2Fractional F1
Evaporated Fractional F2
AreaC2 = 123.5 * 6.0 = 741.0mm2AreaC4 = 9.0 * 7.0 = 63.0mm2Fractional F3
AreaC2 = 93.0 * 4.0 = 372.0mm2AreaC4 = 128.0 * 5.5 = 704.0mm2
Chromatograms for standard solution, sample solution A, and simple and fractional vials. Calculator
Desc:
Measure the height of the peak (in mm.) from the baseline
Measure the width of the peak at half the height
Multiply the two measurements to determine the peak areas.
Equation Setup:
Where h = peak height from baseline and = width of peak at the peak height:
S1, S2, S3 = Samples for Simple DistillationF1, F2, F3 = Samples for Fractional Distillation
C2 = EtAc
C4 = BuAc
Proc #14 Adjusted Peak AreasResults
MaterialsEquipmentAdjusted Peak Areas
C2
C4
Standard
Peak Area (mm2)
88
104
TRs/TRi=As/Ai (s=C2 )
1.00.85A
Peak Area (mm2)
450.0
414.0
A1/As
(s=C2)
450.0351.9Simple
S1
Peak Area (mm2)
172.522.5A1/As
(s=C2)
172.519.1S2
Peak Area (mm2)
702.0445.5A1/As(s=C2)
702.0378.7S3
Peak Area (mm2)
90.0747.0A1/As(s=C2)
90.0635.0Fractional
F1Peak Area (mm2)
00A1/As(s=C2)
00F2Peak Area (mm2)
741.063.0A1/As(s=C2)
741.053.6F3Peak Area (mm2)
372.0704.0A1/As(s=C2)
372.0598.4Standard Solution (Gas Chromatography of Acetates Experiment):TR2 = AreaC2 / AreaC2 = 88 / 88 = 1.0mm2TR4 = AreaC2 / AreaC4 = 88 / 104 = 0.85mm2Sample A:
AreaC2(adj) = AreaC2 * TR2 = 450.0 * 1.0 = 450.0mm2
AreaC4(adj) = AreaC4 * TR4 = 414.0 * 0.85 = 351.9mm2S1:
AreaC2(adj) = AreaC2 * TR2 = 172.5 * 1.0 = 172.5mm2AreaC4(adj) = AreaC4 * TR4 = 22.5 * 0.85 = 19.1mm2S2:
AreaC2(adj) = AreaC2 * TR2 = 702.0 * 1.0 = 702.0mm2AreaC4(adj) = AreaC4 * TR4 = 445.5 * 0.85 = 378.7mm2S3:AreaC2(adj) = AreaC2 * TR2 = 90.0 * 1.0 = 90.0mm2AreaC4(adj) = AreaC4 * TR4 = 747.0 * 0.85 = 635.0mm2F2:AreaC2(adj) = AreaC2 * TR2 = 741.0 * 1.0 = 741.0mm2AreaC4(adj) = AreaC4 * TR4 = 63.0 * 0.85 = 53.6mm2F3:AreaC2(adj) = AreaC2 * TR2 = 372.0 *1.0 = 372.0mm2AreaC4(adj) = AreaC4 * TR4 = 704.0 * 0.85 = 598.4mm2
Calculator
Desc:
Thermal response factors (TR) are computed as ratios of the areas of one peak in the known mixture (base peak) to the area of each of the other peaks in the mixture
There must be at least two similar compounds in the known and unknown mixtures
TR values will be calculated from the areas under the peaks in the standard equimolar mixture.
Equation Setup:
Thermal Response Factor
TR2 = AreaC2 / AreaC2Where TR2 represents the Thermal Response factor for Ethyl acetate and AreaC2 represents the peak area for Ethyl acetate for the standard equimolar solution. TR4 = AreaC2 / AreaC4
Where TR4 represents the Thermal Response factor for Butyl acetate, AreaC2 represent the peak area for Ethyl acetate for the standard equimolar solution, and AreaC4 represents the peak area for Butyl acetate for the standard equimolar solution.Adjusted Peak Areas
AreaC2(adj) = AreaC2 * TR2Where AreaC2(adj) represents the adjusted peak area for Ethyl acetate, AreaC2 represents the peak area for Ethyl acetate with respect to the chromatogram specified, and TR2 represents the Thermal Response factor calculated for Ethyl acetate from the standard equimolar solution.AreaC4(adj) = AreaC4 * TR4Where AreaC4(adj) represents the adjusted peak area for Butyl acetate, AreaC4 represents the peak area for Butyl acetate with respect to the chromatogram specified, and TR4 represents the Thermal Response factor calculated for Butyl acetate from the standard equimolar solution.
Proc # 15Total Peak Area Results
MaterialsEquipmentTotal Peak Areas
SampleC2
C4
A450.0351.9801.9Simple
S1
172.519.1191.6S2
702.0378.71080.7S3
90.0635.0725.0Fractional
F1
000F2
741.053.6794.6F3
372.0598.4970.4A = 450.0 + 351.9 = 801.9S1 = 172.5 + 19.1 = 191.6S2 = 702.0 + 378.7 = 1080.7S3 = 90.0 + 635.0 = 725.0F1 = 0F2 = 741.0 + 53.6 = 794.6F3 = 372.0 + 598.4 = 970.4
Calculator
Desc:
The areas of gas chromatogram peaks are proportional to the molarity of the compound.
Varying thermal conductivity based on the structure and substituent groups of different compound causes deviations in this relationship
Determined from the adjusted peak areas and add them to determine the total peak area
Equation Setup:
Add adjusted peak area values calculated for each of the components of the solution to determine the total peak area.
Proc#16Mole FractionResults
MaterialsEquipmentMole Fractions
C2 (mol)
C4 (mol)
Total (mol)
Fraction C2
Fraction C4
A450.0351.9801.90.56120.4388Simple
S1
172.519.1191.60.9003
0.0997
S2
702.0378.71080.70.64960.3504S3
90.063.5725.00.1241
0.0875Fractional
F1
00000F2
741.053.6794.60.93250.0662F3
372.0598.4970.40.38340.6166Sample A:
Fraction C2 = 450.0 / 801.9 = 0.5612Fraction C4 = 351.9 / 801.9 = 0.4388S1:Fraction C2 = 172.5 / 191.6 = 0.9003Fraction C4 = 19.1 / 191.6 = 0.0997S2:
Fraction C2 = 702.0 / 1080.7 = 0.6496Fraction C4 = 378.7 / 1080.7 = 0.3504S3:
Fraction C2 = 90.0 / 725.0 = 0.1241Fraction C4 = 63.5/ 725.0 = 0.0875F1:
Fraction C2 = 0Fraction C4 = 0F2:
Fraction C2 -= 741.0 / 794.6 = 0.9325Fraction C4 = 52.6 / 794.6 = 0.0662F3:Fraction C2 = 372.0 / 970.4 = 0.3834Fraction C4 = 598.4 / 970.4 = 0.6166
Calculator
Desc:
Computed by dividing the individual adjusted peak areas by the sum of the adjusted peak areas in the chromatogram.
Equation Setup:
Mole Fraction:
Where areai represents a component of the mixture and represents the adjusted total peak areaFraction C2 = C2/ Total
Fraction C4 = C4/Total
C2 = Ethyl acetate
C4 = Butyl acetate
Proc # 17Mole PercentResults
MaterialsEquipmentMole Percent
Mole Fraction
Mole %
A
EtAc
0.5612x 100 =
56BuAc
0.4388x 100 =
44Simple
S1
EtAc
0.9003x 100 =
90BuAc
0.0997x 100 =
10S2
EtAc
0.6496x 100 =
65BuAc
0.3504x 100 =
35S3
EtAc
0.1241x 100 =
12BuAc
0.0875x 100 =
9Fractional
F1
EtAc
0x 100 =
0BuAc
0x 100 =
0F2
EtAc
0.9325x 100 =
93BuAc
0.0662x 100 =
7F3
EtAc
0.3834x 100 =
38BuAc
0.6166x 100 =
62
Calculator
Desc:
Computed by multiplying the Mole fraction values by 100.
Represents the percentage of moles of a component that is present in a compound.
Equation Setup:
Summary of Results:
The total recovered volumes for simple and fractional distillation were 19.2mL and 17.0 mL respectively. The percent volumes recovered for simple distillation were as follows: 54.7% for vial 1, 14.6% for vial 2, and 30.7% for vial 3. The percent volumes recovered for fractional distillation were as follows: 4.1% for vial 1, 30.6% for vial 2, and 65.3% for vial 3. The volumes recovered for simple distillation by temperature range were as follows: 10.5mL from 0-95oC, 2.8mL from 95-105oC, and 5.9mL from 105-130oC. The volumes recovered for fractional distillation by temperature range were as follows: 0.7mL from 0-95oC, 5.2mL from 95-105oC, and 11.1mL from 105-130oC. The masses of Ethyl acetate computed from the density and the volumes recovered for simple distillation and fractional distillation were 11.98g and 5.31g respectively. The masses of Butyl acetate computed from the density and the volumes recovered for simple distillation and fractional distillation were 5.21g and 9.80g respectively. The moles of Ethyl acetate computed from the masses recovered for simple and fractional distillation were 0.136mol and 0.062mol respectively. The moles of Butyl acetate computed from the masses recovered for simple and fractional distillation were 0.045mol and 0.084mol respectively. The total moles recovered for simple and fractional distillation were 0.181mol and 0.146mol respectively. The mole fractions for Ethyl acetate recovered from simple and fractional distillation were 0.751 and 0.425 respectively. The mole fractions for Butyl acetate recovered from simple and fractional distillation were 0.249 and 0.575 respectively. The mole percents for Ethyl acetate for simple and fractional distillation were 75.1% and 42.5% respectively. The mole percents for Butyl acetate for simple and fractional distillation were 24.9% and 57.5% respectively. The peak areas calculated for sample A were as follows: C2=450.0mm and C4=414.0mm. The peak areas calculated for S1 were as follows: C2=172.5mm and C4=22.5mm. The peak areas calculated for S2 were as follows: C2=702.0mm and C4=445.5mm. The peak areas calculated for S3 were as follows: C2=90.0mm and C4=747.0mm. The peak areas calculated for F2 were as follows: C2=741.0mm and C4=63.0mm. The peak areas calculated for F3 were as follows: C2=372.00mm and C4=704.0mm. The thermal adjustment factors calculated from the standard equimolar mixture were as follows: TRC2=1.0 and TRC4=0.85. The adjusted peak areas for sample A were as follows: C2=450.0 and C4=351.9. The adjusted peak areas for S1 were as follows: C2=172.5 and C4=19.1. The adjusted peak areas for S2 were as follows: C2=702.0 and C4=378.7. The adjusted peak areas for S3 were as follows: C2=90.0 and C4=635.0. The adjusted peak areas for F2 were as follows: C2=741.0 and C4=53.6. The adjusted peak areas for F3 were as follows: C2=372.0 and C4=598.4. The total peak areas calculated were as follows: Sample A=801.9, S1=191.6, S2=1080.7, S3=725.0, F2=794.6, F3=970.4. The Mole fractions for Ethyl acetate calculated from the adjusted peak areas were as follows: Sample A=0.5612, S1=0.9003, S2=0.6496, S3=0.1241, F2=0.9325, and F3=0.3834. The Mole fractions for Butyl acetate calculated from the adjusted peak areas were as follows: Sample A=0.0997, S1=, S2=0.3504, S3=0.0875, F2=0.0662, and F3=0.6166.The mole percents for Ethyl Acetate were as follows: Sample A=56%, S1=90%, S2=65%, S3=12%, F2=93%, and F3=38%. The mole percents for Butyl Acetate were as follows: Sample A=44%, S1=10%, S2=35%, S3=9%, F2=7%, and F3=62%.
Analysis & Conclusions:
Simple distillation involves a single cycle of vaporization and condensation, thus producing an impure product due to incomplete separation of the components of the mixture unless the boiling points of the components differ by a minimum of 100oC. To produce relatively pure separation would require multiple distillations and is an impractical approach. Because the boiling points of Ethyl Acetate and Butyl acetate only differ by 48.9oC (EtAc B.P.=77.1oC; BuAc B.P. =126.0oC) thus it is expected simple distillation is not likely an effective method for separating these compounds and that fractional distillation will produce the most accurate results.Fractional Distillation is similar to simple distillation, but requires the use of a Vigreux Column, which achieves the same result as performing multiple vaporization/condensation cycles with multiple simple distillations. This produces a more clean separation of the components in a mixture when the boiling points of its components are less than 100oC apart.The quantity of distillate collected in the second fraction (95-105oC) although well above the boiling point of Ethyl acetate was considered to consist mostly of ethyl acetate. This fraction collected via simple distillation was substantially smaller (2.8mL) and according to gas chromatography consisted of 65% Ethyl acetate and 35% Butyl acetate, whereas the composition of the same fraction collected via fractional distillation was 93% Ethyl acetate and 7% Butyl acetate and was substantially larger in volume (5.2mL). The bar graph of temperature vs time for the simple distillation shows many peaks, suggesting that both compounds were distilled arbitrarily throughout the distillation process across many temperatures. This is characteristic of simple distillation with a mixture consisting compounds with boiling points that are