Acid-Catalyzed Hydration of 1-Hexene
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Acid-Catalyzed Hydration of 1-Hexene
Objective:
The purpose of this experiment is to understand the process of acid-catalyzed hydration
by reacting 1-Hexene with water in the presence of an acid catalyst. Converting
1-Hexene into 2-Hexanol by the acid catalyst. While analyzing the product by gas
chromatography, IR spectroscopy, and or NMR spectroscopy.
Introduction:
The goal of this experiment being performed was to have an alkene reaction using
1-hexene for our main material. In order to have a hydration reaction, the alkene
compound must be hydrated with water in the presence of an acid as the catalyst. The
reason for this experiment to be performed, sulphuric acid was used as our catalyst
compound, which donates as a hydrogen. We as well try to accomplish preparing an
alcohol using alkene as the key material and lastly, determine the major alcohol
component, 2-hexanol. The alcohol compounds are synthesized through hydration of
alkenes. This involves net addition to break the bonds of the alkene compound. This
creates a carbocation located on carbon number two. Following Markovnikov's rule,the
water molecule then attacks the carbocation, causing the oxygen in the water molecule
to be electron-deficient. Deprotonation of the oxygen then results in an alcohol on
carbon number two. The resulting product is a racemic mixture of 2-hexanol.
Procedure:
1.
Place 1.0 mL of H2SO4 in a 3mL and adding 0.5 mL of 1-hexene and a magnetic
stir bar
2.
Place on a stir plate and turn it on for the stirring magnet to stir smoothly at the
highest setting for 20 min
3.
Add 0.5 mL of 1-hexene to the same solution letting it stir for another 20 min
4.
Transfer the solution to a 10 mL Erlenmeyer flask letting it sit to cool down and
placing it in an ice bath
5.
Measure 4 mL of 9M NaOH in a graduated cylinder and using a pasteur pipet
transfer 1mL of 9M NaOH to the vial letting it mix and swirl with the solution
placing it in the ice bath right after putting each drop
-
The solution should have some color change as the time goes by from orange- to
pink to light yellow as the NaOH is being added and there should be a solid
formed at the bottom
6.
Once done with that we will collect the liquid product in the reaction and using the
buchner funnel and filter paper we will vacuum it
7.
We will measure the mass of a empty 50 mL beaker recording it down and then
we will pour the liquid we got after vacuuming and then we will measure the new
mass and record it down again
8.
Calculate and record the mass of the liquid product.
Data sheet:
72.093g
(Mass of Crystals and filter paper)
-
62.669g
(Mass of filter paper)
9.424 g = Actual yield
Mass for 1 mole ( 1- Hexene ) = 6 x 12 + 12 = 84 g
Mass for 1 mole (hexanol-1)
= 6 x 12 + 14 + 16 = 102g
10mL 85% / H2SO4 mass
= 85 x 10 / 98.079 = 8.66g
Total Reactants used =
8.66 g + 5.00 g = 13.66 g
102 x 5 / 84 = 6.07142857 = 6.07 g hexanol
%
Theoretical yield =
( 6.07 g / 13.66g) x100 = 44.4 %
Theoretical yield = ( actual yield / percentage yield) x 100
21.225 g = (9.424 g / 44.4) x 100
Percent yield = ( actual yield / theoretical yield) x 100
44.400471= 9.424 g /21.225 g
44.4%
Mechanism:
CH3-CH2-CH2-CH2-CH=CH2—--↑H2SO4↓NaOH-→CH3-CH2-CH2-CH2-CH2-CH2-OH
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Results and Discussion:
During the experiment there were some mistakes that were made in the beginning. The
solution was to be set in the stirring plate but what we didn't realize was that the stirring
plate had the heat on which caused it to have a fast reaction. The solution in it turned
black dark brown and we spilled it out but didn’t clean the flask being used, making
some impurities in the solution we worked with after pouring that one out. That is why
the percentage that we got has a high percentage showing the error in our experiment.
After the vacuuming as well there was still a lot of solid so we had to do the process all
over again to get a better number.
Conclusion:
Throughout the experiment we were able to work with 1-hexene and 2-hexanol which
helped us understand the process of acid-catalyzed hydration. The percentage that we
ended up with was 44.4% which shows us that our experiment has a lot of errors along
the way or impurities that decreased our chances to get better results. The reason for
that was how our first mistake might have contaminated the flask that we didn’t do after
burning the solution we had first done. Also a lot of impurities went through which were
the solids whenever the vacuuming process was done. Which resulted in having to
vacuuming it all over again.
7. Conclusion: Summarize your findings. Was the product what you expected? Were
the results good or bad? Explain why. Remember, this is just a general guide. Your
actual report will depend on the specific details of your experiment.
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