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Summary Unit 14 - Applications of Organic Chemistry BTEC Unit 14 Assignment 4 all criteria
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Unit 14 - Applications of Organic Chemistry BTEC Unit 14 Assignment 4 all criteria / distinction received
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Moreen Mero / U14A4Lab Report
Date:
Experiment 1: Preparation of Ethyl Ethanoate
Introduction:
Ethanol + ethanoic acid → ethyl ethanoate + water
CH3CH2OH + CH3COOH → CH3COOCH2CH3 + H2O
The functional group of ethanol is alcohol (-OH).
The functional group for ethanoic acid is (COOH) carboxylic acid.
The water that is produced will be removed by distillation, which is one of the techniques
involved with the preparation of this ester. However, in the condensation reaction form two
polymers, or products, instead of one: a polymer molecule will be formed, and a smaller
molecule as well, which is mostly water. as one water molecule will be formed for each ester
molecule that is made.
Justifying the reaction conditions used:
- The concentrated sulphuric acid : using sulphuric acid it increases the completion of the reaction → speeds up
the reaction as a catalyst to increase the rate of the reaction. And more was added to protonate the butan-1-ol.
- Reflux : this reaction condition is very important as it help with purifying the esters that are been produced.
And reflux was used for a specific time, as the higher ratio of the reflux, the more product will be available (the
liquid produced in the column due to the vapour contact that occurs) as the ratio of the reflux is higher, therefore
the purity of the product or the distillate will be also high and more accurate → when having the temperature
and the pressure of the two phases they are kept at the equilibrium→ therefore the vapour and the liquid will not
change and the evaporation, as well as the condensation of the molecules, will be at an equal rate, as result of
having higher rate of reflux, meaning higher purity.
- Distillation : this is used to allow the unwanted products to be separated for the desired product that are
produced. Such as the sulphuric acid, that is not needed for the final product. This is important to purify and
separate the products → to get the final product without impurities of other products. Distillation was used at the
end to also purify the product, in which it is a condition has been used more than ones, for more accuracy, and
more purity, means more reliability to the results and the product will be fully separated from any unwanted
products.
A health and safety assessment
- lab coat must be worn → as health and safety measure, to protect from spillages of acids.
- Googles must be worn → eyes must be protected, the acid is dangerous if it had contact with the eye →
irritation.
- Gloves must be worn → hand must be protected from acid irritation as it causes serious damage if contact with
skin.
- Disposing the waste in the appropriate area → avoiding damages to the environment
Method:
Reaction
1) 5cm3 of ethanol and 5cm3 of glacial ethanoic acid were mixed thoroughly in a 50cm 3 round-bottomed 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 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.
Unit 14: Applications of Organic Chemistry Page 1 of 12
, Moreen Mero / U14A4
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 0-100oC 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 74 o and 79oC was collected.
Photographs of different stages of the method
Results and calculation:
The boiling point of Ethyl ethanoate: .....74... °C
The IR spectroscopy of Ethyl ethanoate:
Calculation:
Molar mass of ethanol = 46 gmol-1
Molar mass of ethanoic acid = 60 gmol-1
Molar mass of ethyl ethanoate = 88 gmol-1
% Atom economy = (molar mass of desired product) x 100
(molar mass of ALL reactants)
% Atom economy = 88 x 100 = 83.0%
(46 + 60)
Theoretical Yield = mass of ethanol x 88.0 g of ethyl ethanoate
46.0 g of ethanol
Theoretical Yield = 3.90 g x 88.0 g
46.0 g
Theoretical Yield = 7.46 g
Actual Yield = …4.23… g
Percentage Yield = actual yield x 100
Theoretical yield
Percentage Yield = 4.23 x 100
7.46
Percentage Yield = …57….%
Unit 14: Applications of Organic Chemistry Page 2 of 12
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