Thermodynamics lab experiment

1. Koya University
Faculty Of Engineering
Chemical Engineering Department – 2nd stage
Supervised by:
Mr. Ribwar and Mr. Hassan
Prepared by:
Safeen Yaseen Jafar
Ramazan Shkur Kakl
Rivan Dler Ali
Lab Report
Experiment Name
Boyle's law
Part 1 - Expansion
Experiment Date
14/10/2020
Submit Date
21/10/2020

2. Table of Content
Subject Pages
Aim of Experiment………………......………………………………………. 1
Theory/Introduction...…….........…………………………………………….. 2
Methology of Tools...………......…………………………………………… 3
Procedure…..…………………......…………………………………………. 4
Table of Reading.…………………...……………………………………….. 5
Discussion………………………....………………………………………… 6
Reference list…………………….....………………………………………. 7

3. 1
Aim of This Experiment
The purpose of Boyle's law is to set up a relationship between the pressure and the volume of
a gas. The law states that as the pressure of a gas increases, its volume decreases, and vice-
versa.

4. 2
Introduction/Theory
The Boyle’s Law was named after chemist and physicist Robert Boyle, who published
the original law in 1662. Boyle showed that the volume of air trapped by a liquid in the
closed short limb of a J-shaped tube decreased in exact proportion to the pressure produced
by the liquid in the long part of the tube. (1)
Robert Boyle and others formulated a law relating the pressure and volume of a constant
quantity of gas at constant temperature. The basis of the law was first published by Boyle in
1662. Boyle's Law states that at constant temperature the pressure p of the gas times its
volume V will remain constant:
P V = Constant
The above relation is only approximately true. This experiment will allow you to explore this
relation of pressure and volume for a fixed quantity of dry air. (2)

5. 3
Methology of Tools 7 8 9
10
1. Vessel 1 for isothermal change of state.
2. Digital displays.
3. Digital display’s way valve for switching between compression and expansion.
4. Heating controller.
5. Digital Displays.
6. Vessel 2 for isochoric change of state.
7. Volume Sensor.
8. Temperature Sensor.
9. Pressure Sensor.
10. Main Switch
OTHERS:
Two 3-way valves

6. 4
Procedure
1. Turn on main switch.
2. Open vent valve.
3. We take two directions to a number one.
4. Turn on compressor until the liquid reach the half of the vessel.
5. Turn off the compressor.
6. Close the vent valve.
7. Inverse the Direction.
8. Record the volume and pressure as we see on the digital displays, also calculate the
temperature from digital display and write as constant.

7. 5
Table of Reading
Pressure (bar) Volume (L) T (o
C) T (K) PV = Constant
0.91 bar 1.8 L 28.1 o
C 301.1 K ≅ 1.6
0.85 bar 1.93 L 28.1 o
C 301.1 K ≅ 1.6
0.79 bar 2.08 L 28.1 o
C 301.1 K ≅ 1.6
0.73 bar 2.25 L 28.1 o
C 301.1 K ≅ 1.6
0.68 bar 2.45 L 28.1 o
C 301.1 K ≅ 1.6

8. 6
Discussion
The pressure would be a third of what it was before in Boyle's Law, Why does this
change?
The motion of gases also causes them to expand and fill their container, giving them a
volume equal to that of their container. If they did not strike the sides of the container, they
would continue on in a straight path.
Why are pressure and volume related then? Aren't they just two unique properties of
gases?
The link comes in how pressure is defined, and how volume affects the pressure.
Pressure is a derived unit. Pressure is force divided by a two-dimensional surface
measurement. Force is often measured in newtons (N), a unit derived from a kilogram-meter
(kg-m). Surface area is often measured in square meters or square centimeters. A pressure
unit would then be a newton per square meter (N/m?), the Pascal (Pa). Because a Pascal is
relatively small, force is often measured more conveniently in kiloPascals (kPa).
With a gas, the pressure is exerted on the sides of the container. If there is a greater surface
area, the force will remain the same, so the pressure will go down. For ex ample, if a ten
newton force is exerted over ten square meters, the pressure is 1 kPa. If the surface area
increases to twenty square meters, the pressure is reduced to 0.5 kPa. If the surface area
decreases to five square meters, the pressure is increased to 2 kPa.
The volume of the container dictates its internal surface area for the gas. If the volume of a
gas decreases, because a gas expands to fill its container, the container's volume must have
decreased. Therefore, there is a smaller surface area, and the pressure increases. If the volume
of the gas expands, meaning a larger container, the pressure would go down. This type of
relationship is called an inverse relationship.
That's most of Boyle's law! Mathematically, this is represented as PV. Boyle's law produces a
constant, K, so extended, the formula is PV=K. However, because the con stant stays the
same, additional pressures and volumes can be equated and solutions can be found for
unknowns. This equation can be a powerful tool in solving for or converting pressures and
volumes.

9. 7
Reference list
1. David M. 2013. Boyle’s Law. [online] faraday.physics.utoronto.ca. Available at:
https://faraday.physics.utoronto.ca/IYearLab/Intros/BoylesLaw/BoylesLaw.html#:~:te
xt=Robert%20Boyle%20and%20others%20formulated,published%20by%20Boyle%2
0in%201662.&text=This%20experiment%20will%20allow%20you,fixed%20quantity
%20of%20dry%20air. [Accessed 17 OCT 2020].
2. Wiktionary, 2019. Boyle’s Law: Volume and Pressure. [online] Available at:
https://courses.lumenlearning.com/introchem/chapter/boyles-law-volume-and-
pressure/ [Accessed 17 OCT 2020].