family law is responsible in protecting Indian familiesFull description
for your reading of criminal law from ecpress
Source of Hindu Law. Who is Hindu 1. ConcepT of Hindu Marrige. 2. Theroy of divorce. 3. Ground of Maintenance. 4. Hindu Succession Act. HINDU MARRIAGE IS A SACRAMENT AND NOT A CONTRACTFull description
partnershipFull description
international law and municipal law differenceFull description
This Is The Recto Law (Installment Sales Law)
Civil Law Common Law DiferenciasDescripción completa
These days consumers are showing keen interest in the way food is produced, processed, and marketed. The increasing globalization of the food supply chain has resulted in unprecedented interest in the development of food standards and regulations. In
The paper focuses on the systems of the English legal system
building law
media law
thinkiit hcverma hindi
Full description
Negotiable Instruments quizzer
Full description
Mercantile Law ReviewerFull description
1.0 TITLE Experiment of Relationship between Pressure and Volume in Gas
2.0 OBJECTIVE -
To understand the application concept of Boyle’s Law.
-
To study the relationship between the pressure and volume of a confined gas.
-
To understand the planning of a measurement series, the reading of measurement result and the conversion of measurements into a statement of theoretical principle.
3.0 THEORY Boyle's law (sometimes known as the Boyle Mariotte law) is one of the gas laws. Boyle fixed the amount of gas and its temperature during his investigation. He found that when he manipulated the pressure that the volume responded in the opposite direction. For example, when Boyle increased the pressure on a gas sample the volume would decrease. Mathematically, PV = constant value if the gas is behaving as an Ideal Gas. A practical math expression of Boyle's findings is as follows:
Where: •
V is volume of the gas.
•
P is the pressure of the gas.
•
k is a constant (see Note 1).
where the variables with the 1 subscript mean initial values before the manipulation and the variables with the 2 subscript mean final values after the manipulation.
4.0 PROCEDURE AND APPARATUS WL100 Apparatus for Demonstrating Boyle’s Law
Figure 3 - Schematic Diagram For Boyle’s Law Apparatus Compression Operation (1.0L-0.3L) 1. Both the hose side and atmosphere side valves at the compression side are closed.
2. Hose side closed and atmosphere side opened at the suction side. 3. The pump is turned on. 4. The compression valve (hose side) is slowly opened and closed firmly when the test point reached (volume air 0.9L). 5. Quantities of pressure is read and recorded into the table when the level of water remains steady. 6. Steps 3 to 5 repeated for the test point 0.7, 0.5 and 0.3. 7. The pump is turned off. 8. Dual valve compression side and suction side are opened.
Vacuum Operation (1.0L-2.0L) 1. Hose side closed and atmosphere side opened at the compression side. 2. Both the hose side and atmosphere side valves at the suction side are closed. 3. The pump is turned on. 4. The compression valve (hose side) is slowly opened and closed firmly when the test point reached (volume air 1.1L). 5. Quantities of pressure is read and recorded into the table when the level of water remains steady. 6. Steps 3 to 5 repeated for the test point 1.3, 1.5, 1.7 and 1.9. 7. The pump is turned off. 8. Dual valve compression side and suction side are opened. 9. Main switch is switched off.
5.0 DATA AND ANALYSIS V (litre)
(bar)
xV (litre.bar) [X]
Absolute deviance from mean [X – Y] (litre.bar)
Relative deviance from mean (%) [ x 100]
0.3
3.20
3.18
3.18
3.19
0.957
0.040
4.01
0.5
2.00
1.98
1.98
1.99
0.995
0.002
0.20
0.7
1.48
1.46
1.44
1.46
1.022
0.025
2.51
0.9
1.10
1.10
1.08
1.09
0.981
0.016
1.60
1.1
0.90
0.90
0.91
0.90
0.990
0.007
0.70
1.3
0.78
0.77
0.78
0.78
1.014
0.017
1.71
1.5
0.70
0.68
0.67
0.68
1.020
0.023
2.31
1.7
0.60
0.59
0.59
0.59
1.003
0.006
0.60
1.9
0.52
0.52
0.52
0.52
0.988 Mean [Y]
0.009
0.90 Mean = 1.62
= 0.997
Graph of Pressure vs Volume 3.50 3.00
Pressure (bar)
2.50 2.00 1.50 1.00 0.50 0.00 0
0.2
0.4
0.6
0.8
1 Volume (L)
1.2
1.4
1.6
1.8
2
Pressure (bar)
1/V (1/L)
3.19 1.99 1.46 1.09 0.9 0.78 0.68
3.33 2.00 1.43 1.11 0.91 0.77 0.67
Graph of Pressure vs 1/V 3.50 3.00
Pressure (bar)
2.50 2.00 1.50 1.00 0.50 0.00 0
0.5
1
1.5
2 1/V (1/L)
2.5
3
3.5
6.0 CALCULATION
=
= = 3.19 X
=
xV
= 3.19 x 0.3 = 0.957 litre.bar Absolute deviance from mean = [X – Y] = 0.957 – 0.997 = 0.40 litre.bar
Relative deviance from mean (%)
=[
x 100]
= = 4.01
7.0 DISCUSSION 1. From the graph that plotted, the P versus 1/V is a straight line graph and passes through the origin. This graph shows that P is directly proportional to 1/V. While for the graph P versus V, we get a hyperbolic curve graph. The pattern that we can see is when the volume increasing, the pressure decreasing which mean that in this experiment Boyle’s Law is valid. 2. The gas will not apply Boyle’s Law when the temperature of gas is not fixed while doing the experiment. This is because Boyle’s Law allows us to find out the relationship between pressure and volume under condition where temperature is fixed. Besides that, if the gas is not an ideal gas it does not apply Boyle’s Law because according to Boyle’s Law, PV= constant value just when the gas behaving like an ideal gas. Real gas will disobey the boyle’s Law 3. There is some error which occurs in this experiment such as error we made when reading the scale of pressure gauge. The scale of the pressure gauge is too big so we just take the approximate reading which causes the error in reading. Parallax error also occurs in this experiment. This error occurs when we take the reading from graduated cylinder.
8.0 CONCLUSION Conclusion, from this experiment we have proved that the volume of a fixed mass of an ideal gas is inversely proportional to its pressure which is same with what stated in Boyle’s Law. When we increase the volume inside the cylinder, the pressure inside the pressure cylinder will also decreases correspondingly. To apply Boyle’s Law in this experiment, we had to assume that the temperature was fixed and the gas we used is an ideal gas before we start the experiment.
