Fractional Distillations
Sample Lab Report
Simple and Fractional Distillation
Unknown # 2
Purpose
In this experiment we aim to demonstrate that we can separate two volatile compounds from a mixture due to the different chemical properties of each compound. We will accomplish this by a separation procedure known as distillation, which relies on each compound having a distinct and separate boiling point. Our pure products will be analyzed with gas chromatography to determine the success of the distillation.
Procedures
The experiment was performed as stated in the course textbook:
Pavia, D. L., Lampman, G. M., Kriz, G. S., Engel, R. G. Introduction to Organic Laboratory Techniques: A Microscale Approach. 2007, 4th Ed. Pp 51—57. .
Data
The distillation curves for our simple and fractional distillation (See page 3) clearly demonstrate that fractional distillation separates the two compounds more completely. The boiling point (bp) of our unknown compounds was taken from the flat regions of the fractional distillation curve. Our unknown mixture contained hexane (bp 69 ºC) and toluene (bp 110.6 ºC).
Analysis via gas chromatography allowed us to determine the relative percentage of hexane and toluene at fractions near the beginning and end of our distillations. Relative percentages have been recorded in the table below, and our calculations are shown on page 5.
Simple Distillation Retention time (s)
Fractional Distillation
Retention time (s)
Cyclohexane
Retention time (s)
Toluene
Retention time (s)
Cyclohexane
Retention time (s)
Toluene
Retention time (s)
Fraction 1 (4th mL)
15
25
14
24
Fraction 2
(17th mL)
14
26
16
25
Simple Distillation
Area (s)
Fractional Distillation
Area
Cyclohexane
Retention time (s)
Toluene
Retention time (s)
Cyclohexane
Retention time (s)
Toluene
Retention time (s)
Fraction 1 (4th mL)
15551
400
14444
248
Fraction 2
(17th mL)
222
16558
166
25995
A figure of the gas
Simple and Fractional Distillation
Unknown # 2
Purpose
In this experiment we aim to demonstrate that we can separate two volatile compounds from a mixture due to the different chemical properties of each compound. We will accomplish this by a separation procedure known as distillation, which relies on each compound having a distinct and separate boiling point. Our pure products will be analyzed with gas chromatography to determine the success of the distillation.
Procedures
The experiment was performed as stated in the course textbook:
Pavia, D. L., Lampman, G. M., Kriz, G. S., Engel, R. G. Introduction to Organic Laboratory Techniques: A Microscale Approach. 2007, 4th Ed. Pp 51—57. .
Data
The distillation curves for our simple and fractional distillation (See page 3) clearly demonstrate that fractional distillation separates the two compounds more completely. The boiling point (bp) of our unknown compounds was taken from the flat regions of the fractional distillation curve. Our unknown mixture contained hexane (bp 69 ºC) and toluene (bp 110.6 ºC).
Analysis via gas chromatography allowed us to determine the relative percentage of hexane and toluene at fractions near the beginning and end of our distillations. Relative percentages have been recorded in the table below, and our calculations are shown on page 5.
Simple Distillation Retention time (s)
Fractional Distillation
Retention time (s)
Cyclohexane
Retention time (s)
Toluene
Retention time (s)
Cyclohexane
Retention time (s)
Toluene
Retention time (s)
Fraction 1 (4th mL)
15
25
14
24
Fraction 2
(17th mL)
14
26
16
25
Simple Distillation
Area (s)
Fractional Distillation
Area
Cyclohexane
Retention time (s)
Toluene
Retention time (s)
Cyclohexane
Retention time (s)
Toluene
Retention time (s)
Fraction 1 (4th mL)
15551
400
14444
248
Fraction 2
(17th mL)
222
16558
166
25995
A figure of the gas