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