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U14A4 Learning aim D: Investigate organic chemistry reactions in order to gain skills in preparative organic chemistry
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Assignment BriefLab Report
Date: Monday 26th March 2021
Experiment 1: Preparation of Ethyl Ethanoate
Introduction:
An explanation of each of the three chemical reactions, including the balanced chemical equation,
the functional groups involved and an appropriate reaction mechanism.
Functional group
CH3COOH + CH3CH2OH CH3COOCH2CH3 + H2O
Ethanoic + Ethanol Ethyl Ethanoate + Water
Acid
(Carboxylic (Alcohol) Ester Acid)
CH3CH2OH + CH3COOH
CH3COOCH2CH3 + H2O
The group is that its in the Ester group
Esterification reaction (reaction type condensation reaction)
The mechanism for the hydrolysis of the ethyl ethanoate where the ethyl ethanoate will be heated that is
under the reflux with the dilute acid that is the hydrochloric acid/sulfuric acid, as such the ester will then
react with the water to produce the ethanoic acid and the ethanol mentioned (Clark, 2020).
The functional group of the ethanol is the alcohol the OH group.
The functional group for ethanoic acid is the COOH carboxylic acid.
For the water that is produced tends to be removed by the distillation that the techinques tend to involve
with the preparation of this ester. However, for the condensation reaction forming the two polymers or of
the products that tend to be instead of the polymer molecule tend to be formed and the smaller molecule
such that tends to be more water and there is at least one water molecule that tends to be formed for each
of the ester of the molecule that tends to be made. As such the concentrated sulphuric acid that tend to
increase the completion of the reaction that tends to speed up since the catalyst tend to increase the rate
of reaction. Also, since more of this was added to the protonate the butan-1-ol. The reflux will then in the
reaction condition tend to be important for helping with the purification for the esters that tend to be
produced and for the reflux that tend to be used at a specific time and for the higher ratio of the reflux
that the more product that to be available as such that the liquid tend to be produced in the column this
occurs due to the vapour contact that tend to happen. For this the ratio of the reflux tend to be higher as
such the purity of the product or of the distillate tend to be high and accurate because the temperature
and the pressure of the two steps that tend to be kept for this at the equilibrium as such that the vapour
and for the liquid will not change and for that the evaporation tend to occur at the condensation of the
molecules tend to be equal rate for this as such that this results of having at a higher rate of the reflux as
such this means for it to have at high purity. Then for the distillation this tends to allow for the unwanted
products to then be separated for the desired product that tend to be produced. As such for this the
sulphuric acid as such this isn’t needed so much for the final products. Moreover, this tends to be
essential for purifying and separating the products and this then tends to get the final product of this
Unit 14: Applications of Organic Chemistry Page 1 of 26
,without the impurities of the other products for this. Also, the distillation tends to be used at the end to
then purify the product and then it’s the condition that tends to be useful for more than the ones. This
happens to ensure accuracy and reliable and this makes it pure to the results and for that the product tend
to be separated this is due to unwanted products. For the functional group tends to be of the ethyl acetate
that shows to be the acetic ester that tend to be the organic compound and that of the carboxylic acid
esters for this and the carboxylic group that is the carbon from this of the carbonyl group that tends to be
attached to that of the alkyl group then will be done through the oxygen that forms the ester. That when
the esters are produced of the carboxylic acid tends to be heated with the alcohol for due to the acid
catalyst – the sulphuric acid. For the hydrogen chloride in the gas tend to be used in the experiment that
tends to be used for the sulphuric acid because it increases the catalyst that is used to increase the rate of
reaction as such then works as a dehydrating agent. Also, the mechanism for this is that of the
esterification that is used in for the carbonyl oxygen that tends to then attack the sulfuric acid and then
this will then deprotonating of the OH group. For this reason of the dry hydrogen chloride gas tend to be
used in the aromatic ester and that the carboxylic acid will then have the benzene ring in it. As such by
heating the reaction under the reflux will then prevent the lose of the volatile reactants and that of the
products. Furthermore, the increase of ester of the yield and the hot vapours tend to rise from the
condenser and cold water removes the hot vapours from it and then cools it down and then will condense
inside of it.
A health and safety assessment
Using chemicals like ethanol, which is flammable, glacial ethanoic acid which tends to be corrosive and
flammable, concentrated sulphuric acid that is corrosive, sodium carbonate that is the irritant, and finally
the anhydrous calcium chloride. Ensuring to wear lab coats, goggle, and gloves used during the duration of
the experiment. The lab coat to protect from the spillages of the acids, googles for the eyes protection as
the acid tend to be dangerous as for the contact, gloves tend to be worn for the hand protection that to be
product from the acid irritation that tend to cause the serious damage, and when disposing for the waste for
avoiding that tend to damage for the environment. The lab coat must be worn and for this is the health and
safety measure to protecting from the spillages of acids. For this is the goggle be worn eyes that must ne
protected that for the acid is dangerous that if had contact with the eye irritation. For this reason the gloves
needs to be worn and for the hand must be protected from the acid irritation for the causing of serious
damage if there is contact with the skin. As such that when disposing of the waste in for the appropriate
area this to due to avoiding damage to the environment.
Method:
• Your proposed, detailed method with the reactants and predicted products, quantities used,
and diagrams of apparatus
• The actual reaction conditions to be used, including reagents, temperatures and times
Reaction
1) 5cm3 of ethanol and 5cm3 of glacial ethanoic acid were mixed thoroughly in a 50cm 3 roundbottomed
flask.
2) 1cm3 of concentrated sulphuric acid was slowly added to the mixture with cooling and shaking.
3) Then the flask was fitted with a reflux water-condenser and the mixture was boiled gently for 10
Unit 14: Applications of Organic Chemistry Page 2 of 26
, minutes.
Separation of the product
4) The position of the condenser was rearranged for distillation, and about two-thirds of the mixture
was distilled off.
5) The distillate was transferred to a separating funnel and about 3cm 3 of 30% sodium carbonate
solution was added to it. The funnel was stoppered and was shaken, opening the tap from time to
time.
6) The two layers were allowed to separate and carefully run off and was rejected the lower layer,
ensuring that the sodium carbonate was removed as completely as possible.
Purification of the Product
7) 2.5g of anhydrous calcium chloride was dissolved in 2.5cm 3 of distilled water and was added to the
ethyl ethanoate in the funnel, and was shaken well, and the lower aqueous layer was removed.
8) The ethyl ethanoate was poured into a beaker, a few lumps of solid anhydrous calcium chloride was
added and was shaken well. The ethyl ethanoate was decanted into a clean dry round 50cm 3 bottom
flask.
9) Some anti-bumping granules were added, and was arranged for distillation including a 0-100 oC
thermometer in the apparatus. The ether that was always formed in this reaction was distilled off at
35-40oC, and was discarded. The mixture was continued to heat, and the fraction that boils between
74o and 79oC was collected.
When preparing the compound its essential to keep it in the right storage with name. date, and
compound stated.
Testing the purity of the ethyl ethanoate sample that has been prepared
Measure the boiling point of the sample prepared
Run an IR spectrum for the organic compound made
Photographs of different stages of the method
Results and calculation:
• Records of any tests of purity and quantities of product made
• Percentage yield calculations
The boiling point of Ethyl ethanoate: 74.8 °C
The IR spectroscopy of Ethyl ethanol
Molar mass of ethanol = 46 gmol-1
Unit 14: Applications of Organic Chemistry Page 3 of 26
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