Confirm Gas Laws
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Oxford Brookes *
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Subject
Law
Date
Nov 24, 2024
Type
docx
Pages
7
Uploaded by muenbridgit32
Confirm Gas Laws
Name
May 26, 2023
Introduction
Boyle’s law relates pressure and volume. The number of particles and temperature in Boyle’s law
is assumed to be constant. Boyle’s law states that pressure and volume have an inverse
relationship. As the volume increases, pressure decreases and vice versa. Gay-Lussac’s law
examines the relationship between pressure and temperature while keeping volume and mass
constant. This law states that pressure has a direct relationship with the absolute temperature of a
gas. Charles’ law states that volume and absolute temperature have a direct relationship. The
purpose of this lab is to confirm Boyle’s law, Charles’ law, and Gay-Lussac’s Law.
Experimental details
The PhET website was used to complete the lab.
The ideal section of the simulation was used.
After clicking the ideal section, the controls on the top of the simulation were noted. The
experiment was controlled by clicking on pressure, temperature, and velocity. The measurement
of the experimental chamber was taken by clicking on width. Particles were added to the
chamber and temperature was controlled by moving the scale on the bucket.
The first experiment involved manipulating volume while measuring pressure. Temperature had
been held constant at 300K. The second experiment involved manipulating temperature while
keeping pressure constant and measuring the volume. The third experiment involved keeping the
volume constant and manipulating temperature to measure pressure. Temperature was
manipulated by heating the container.
Results
First experiment (constant temperature 300K)
Volume (mm
3
)
Pressure (atm)
5
23.2
6
19.5
7
16.4
8
14.3
9
13.2
10
11.7
11
10.1
13
8.8
15
7.8
4
6
8
10
12
14
16
0
5
10
15
20
25
Pressure vs volume (constant temperature
volume (mm3)
Pressure (atm)
Second experiment (constant pressure (11 atm)
Volume (mm
3
)
Temp (K)
5
151
5.4
161
5.7
171
6
181
6.4
191
6.7
201
7.0
211
7.4
221
7.7
231
8.0
241
8.4
251
8.7
261
9.0
271
Volume vs temperature graph
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140
160
180
200
220
240
260
280
0
1
2
3
4
5
6
7
8
9
10
volume vs temperature(constant pressure)
temp(K)
volume (mm3)
Third experiment (temperature and pressure, volume constant)
Temp (K)
Pressure (atm)
300
12.1
320
13.2
340
13.9
360
14.5
370
15.1
430
17.5
440
17.9
450
18.5
500
20
Pressure vs temperature graph
11.5
12.5
13.5
14.5
15.5
16.5
17.5
18.5
19.5
20.5
0
100
200
300
400
500
600
temp vs pressure (constant volume)
Pressure (atm)
Temp (K)
Theoretical calculations
The following equations were used to perform calculations:
P
1
V
1
=
P
2
V
2
V
1
T
1
=
V
2
T
2
P
1
T
1
=
P
2
T
2
5
(
24
)=
P
2
(
6
)
P
2
=
20
atm
The combined gas law equation was used to perform the calculations of various values. The
values were recorded in the table below:
Volume (mm
3
)
Pressure
(atm)
Volume
(mm
3
)
Temp (K)
Temp (K)
Pressure
(atm)
5
24
5
150
300
12
6
20
5.4
165
320
13
7
17
5.7
175
340
14
8
15
6
184
360
15
9
13
6.4
192
370
16
10
12
6.7
204
430
17
11
10
7.0
214
440
18
13
8
7.4
224
450
19
15
7
7.7
235
500
22
There were differences in the values of pressure and temperature.
Discussion
The experiment showed that volume and temperature are directly proportional, and volume and
pressure are inversely proportional. It also showed that temperature and pressure have a direct
relationship. As temperature increases, pressure increases when the volume is held constant. At
constant temperature, pressure decreases as volume increases. This experiment was able to
demonstrate the relationship between temperature, volume, and pressure in the ideal gas law
equation.
A possible source of errors in this laboratory was rounding the decimals. The decimals might
have been rounded off leading to errors in the final values of the theoretical values. Another
source of error might have taking incorrect readings of various pressure and temperature values.
Conclusions and Summary
This experiment verified Boyle’s Law, Gay-Lussac’s Law, and Charles’ Law. It showed that
pressure and volume are inversely proportional while volume and temperature, and temperature
and pressure are directly proportional. The ideal gas law is a combination of all gas laws. This
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law was confirmed in the experiment by the relationship between various variables such as
pressure and volume.
REFERENCES
Laugier, A., & Garai, J. (2020). Derivation of the ideal gas law.
Journal of Chemical
Education
,
84
(11), 1832.
Silbey, R. J., Alberty, R. A., Papadantonakis, G. A., & Bawendi, M. G. (2022).
Physical
chemistry
. John Wiley & Sons.