The Distillation of Ethanol from 20ml Gin Through Simple and Fractional Distillation
Autor: Joshua • January 18, 2018 • 2,099 Words (9 Pages) • 505 Views
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Table No. 2 Results of Simple Distillation
Test Tube Number
Volume (mL)
Temperature (°C)
Flammability
1
0.5
78.0
Flammable
2
0.5
80.2
Flammable
3
0.5
82.1
Flammable
4
0.5
82.3
Flammable
5
0.5
83.0
Flammable
6
0.5
82.7
Flammable
7
0.5
82.5
Flammable
8
0.5
82.9
Flammable
9
0.5
83.9
Flammable
10
0.5
85.0
Flammable
11
0.5
85.7
Flammable
12
0.5
87.0
Flammable
13
0.5
88.0
Flammable
14
0.5
89.1
Flammable
15
0.5
91.0
Non-Flammable
16
0.5
93.0
Non-Flammable
17
0.5
96.3
Non-Flammable
18
0.5
97.6
Non-Flammable
19
0.5
99.1
Non-Flammable
20
0.5
99.4
Non-Flammable
Table No. 3 Computations for Percentage of Fractional Distillation
% EtOH
35%
% Lost
33.5%
% Error
12.5%
Table No. 4 Computations for Percentage of Simple Distillation
% EtOH
35%
% Lost
25%
% Error
12.5%
Boiling chips, which were put in the distilling flask with the gin, have pores inside which provide cavities both to trap air and to provide spaces where bubbles of solvent vapor can form. These bubbles ensure even boiling and prevent bumping and boiling over and loss of the solution. The joints of the setups were greased to ensure that the parts of the quickfit setup would stick together. The flask was heated by constantly revolving the Bunsen flame to make sure the heat is equally distributed. Flammability test was conducted to see which samples contained ethanol.
One principle that affects the distillation process is Equilibrium Vapor Pressure. It is when the pressure in the space above the liquid will rise and finally reach some constant value, due entirely to the vapor of the liquid.
The equilibrium vapor increases with temperature as shown in the equation:
[pic 1]
The existence of vapor pressure is explained by molecules of liquid escaping into the empty space above the liquid. As the number of molecules in the vapor space above the liquid becomes larger, the rate of return of molecules in the vapor space to the liquid increases until the rate of return has risen to equal the constant rate of escape.
Another principle is the principle of Partial Pressure, which is the hypothetical pressure of that gas if it alone occupied the volume of the mixture at the same temperature. The total pressure of an ideal gas mixture is the sum of the partial pressures of each individual gas in the mixture. If there are other molecules present, the equilibrium vapor pressure will not be equal to the total pressure. The total pressure will be the sum of the equilibrium vapor pressure of the liquid
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