Nick Taylor
Chem. 211, Dr. Oxy
Section 20303
Date of experiment: 10/03/2017
Post-lab: Synthesis of Isopentyl acetate (banana oil)
CALCULATIONS:
143.56°C-143=0.56°C difference between the boiling points of actual and theoretical values percent yield: (actual/theoretical)times 100 = (143/143.56)times 100=99.61%
Mass of 25ml round flask: 29.85g
Flask + solution= 36.28g
36.28-29.85= 6.43g
Weight of Isoamyl acetate (experimental)= 6.43g
Weight of Isoamyl acetate (theoretical)= 4.01g
Percent yield= (expetimental/theoretical)times 100
(6.43g/4.01g)times 100=160.3%
RESULTS:
Boiling point expected:
130°C-143°C
Boiling point collected in degrees=
143.56°C Initial Isoamyl acetate=
6.43g
Isoamyl acetate recorded=
4.01g
Percent yield =
99.61%
Percent yield=
160.3%
DISCUSSION:
The drips started forming at around 143.56 °C and the distillation procedures mentioned that they would form at some point between 130°C and 143°C.
The reagents that were used in this experiment were: isopentyl alcohol, glacial acetic acid, anhydrous MgSO4, saturated NaCl (aq), concentrated H2SO4, 10% Na2CO3.…show more content… The catalyst that I used to do the direct esterification of acetic acid along with isopentyl alcohol was sulfuric acid. It’s important to note that I also used the mechanism of isolation to achieve a purified form of isopentyl acetate. I used sodium bicarbonate to achieve this purified form. I received 4.01g of isopentyl acetate. Isopentyl alcohol is the limiting reagent here. It’s safe to say that I had a successful experiment since I achieved the small of bananas in my solution. I tried as best as I could to only use very clean flasks and beakers and other glassware but there may have been a source of error in my experiment due to dirty glassware. Another source of error might have occurred in the distillation process because in some cases, water has trouble circulating through the
