What does Boyle’s Law state? .....................................................2 An outline of what this project is about....................................2 Title.....................................................................................................2 Investigative question.....................................................................3 Hypothesis.........................................................................................3 Variables.............................................................................................3 Materials needed for experiment and procedure....................4 Diagram of set-up............................................................................5 Results and questions and answers..........................................6-8 Conclusion...........................................................................................9

Investigating Boyle’s Law

1. What does Boyle’s Law state?
Boyle's law states that the absolute pressure and volume of a given mass of confined gas are inversely proportional, if the temperature remains unchanged within a closed system.

2. An outline of what this project is about.

In this project I will be testing to see if pressure and volume are inversely proportional to one another. I will use Boyle’s apparatus and a pump to test this. When the pump is pumped it will raise the pressure in the tube. The oil level will then rise therefore decreasing the volume of air in the tube. Results will be taken and if the products of the pressures and the volumes are constant then we can conclude that pressure and volume are inversely proportional.

3. Title
Investigating the relationship between pressure and volume.

4. Investigative question
Will the increase in pressure decrease the volume of air in the apparatus?

5. Hypothesis
If the amount of pressure in the apparatus is...

...Chihwei Liu
2012/11/28
Boyle’sLaw
Purpose: Define the effect of air dense to pressure.
Variables:
Independent Variables: Milliliters of air
Dependent Variables: Pressure
Controlled Variables: Milliliters of air, room temperature, same syringe.
Materials: Syringe, pressure senser.
Procedure: On the paper
Data:
ml ±0.5 Room Temperature kpa1 ±0.01 kpa2 ±0.01 kpa3 ±0.01 kpa4 ±0.01 kpa5 ±0.01 Averages kpa ±0.05
20 24.6℃ 102.840 102.950 102.780 102.780 102.940 102.858
19 24.6℃ 108.810 108.550 108.470 108.470 109.140 108.688
18 24.6℃ 114.580 114.130 114.430 114.110 114.900 114.430
17 24.6℃ 121.320 120.830 121.310 120.560 121.310 121.066
16 24.6℃ 128.010 128.150 128.440 128.320 128.520 128.288
15 24.6℃ 136.750 136.130 137.820 136.750 137.240 136.938
14 24.6℃ 146.250 145.780 146.750 145.230 146.260 146.054
13 24.6℃ 156.790 156.750 157.040 156.310 157.030 156.784
12 24.6℃ 167.350 169.280 168.650 169.640 169.410 168.866
11 24.6℃ 184.870 184.030 182.390 183.640 184.410 183.868
10 24.6℃ 202.300 200.000 200.040 199.820 201.020 200.636
Not a linear function, so I will inverse the X axis values to make it into a linear function.
Conclusion:
Looking at the graph above, we can tell there is a linear increase, which is the inverse value of volume increase the pressure increase which also means that when the volume decrease, the pressure decrease....

...Boyle'sLaw Experiment
Aim
To show that Pressure is proportional to the inverse to volume
Method
A gas syringe was attached to a pressure sensor. The pressure sensor was calibrated, assuming the atmospheric pressure at the time of the experiment was 100kPa. Differing volumes of gas were created in the gas syringe and they were recorded as were the corresponding values of pressure at that particular volume. The volume was varied between 20cm3 and 75cm3.
Results
A set of readings was obtained and the results were plotted on two graphs, one showing pressure against volume and the other showing pressure against the inverse volume.
Conclusion
The graph plotted showing pressure against volume does not show any obvious connection, as the graph takes the shape of an exponential decay. However the graph showing pressure against the inverse volume produces a straight line intercepting the pressure axis at approximately 8kPa. As a straight line graph is produced by plotting pressure against the inverse of volume we have shown that pressure is indeed proportional to the inverse of volume. However we have yet to explain the intercept produced.
For an ideal gas P 1/V, thus creating a straight line graph passing through the origin proving no other parameters i.e. mass or temperature of gas are changed.
As a straight line graph is produced that does not pass through the origin we can say that the most likely cause of the non-zero pressure intercept...

...Boyle’sLaw
5-1: Boyle’sLaw: Pressure and Volume
Robert Boyle, a philosopher and theologian, studied the properties of gases in the 17th century. He noticed that gases behave similarly to springs; when compressed or expanded, they tend to ‘spring’ back to their original volume. He published his findings in 1662 in a monograph entitled The Spring of the Air and Its Effects. You will make observations similar to those of Robert Boyle and learn about the relationship between the pressure and volume of an ideal gas.
1. Start Virtual ChemLab and select Boyle’sLaw: Pressure and Volume from the list of assignments. The lab will open in the Gases laboratory.
2. Note that the balloon in the chamber is filled with 0.300 moles of an ideal gas (MW = 4 g/mol) at a temperature of 298 K, a pressure of 1.00 atm, and a volume of 7.336 L. To the left of the Pressure LCD controller is a lever that will decrease and increase the pressure as it is moved up or down; the digit changes depending on how far the lever is moved. Digits may also be clicked directly to type in the desired number. You may want to practice adjusting the lever so that you can decrease and increase the pressure accurately. Make sure the moles, temperature, and pressure are returned to their original values before proceeding.
3. Click on the Lab Book to open it. Back in the laboratory, click on the Save button to start...

...Gas Laws
Gases exhibit many qualities that are very different from those of liquids or solids. Gases have particles that are farther apart when compared to liquids and solids. The particles in gases move at different speeds in random directions and they are constantly moving. These particles collide with each other and with whatever container or area they are in. Gases are also very easy to compress. They expand to fill their containers and they occupy far more space than the liquids and solids from which they form.
An ideal gas follows all of the gas laws. The conditions that allow real gases to behave like ideal ones are high temperatures, low pressure, and weak intermolecular forces. Gases may be measured in newtons/square meter (N/m2), pascals (Pa), atmospheres (atm), millimeters of mercury (mmHg), torrs, and pounds per in2 (PSI). When these units are all equal, they end up being 1.01 x 105 N/m2, 1.01 x 105 Pa, 1.00 atm, 760. mmHg, 760. torr, and 14.7 PSI. Gasses at STP, or standard conditions of pressure, are at 1 atm and 0°C.
Gases have certain law formulas that they tend to follow. For these formulas, P=pressure,
V=volume, n=moles, and T=temperature. According to Boyle’slaw, P1V1=P2V2, and any unit of
pressure and volume may be used. This is successful because pressure and volume are inversely
related, meaning as one goes up the other goes down, and vise versa. Charles’s...

...gas given the temperature and # of molecules remained constant. Using the Boyle'slaw apparatus, and textbooks to demonstrate pressure it was concluded that there was a relationship between pressure and volume. However, the relationship was not a direct relationship, and it was determined that the pressure and volume of a gas are inversely proportioned. Thus,proving Boyle's theory correct.
Introduction
Objectives: The main objective of this lab was to determine the relationship between the volume and pressure when the temperature and number of molecules remains the same throughout. Other minor objectives of this lab were to determine any possible source of error, so there is more awareness of these errors when conducting another experiment.
Theory: Gases are matter with no definite volume or shape. They will take on the volume and shape of whatever they are being contained in. There are three gas laws. The first is Boyle'sLaw. Boyle'slaw states that at a maintained temperature, and number of molecules, the volume and pressure of a gas are inversely proportional to each other. Which simply means that the higher the pressure is on a gas, the lower the volume of the gas will be, and vice-versa. The formula for this law is: P¹V¹=P²V². V¹ is the old volume, and P¹ is the old pressure. V² is the new volume and P² is the old...

...BOYLE’SLAW AND THE EMPTY SPACE IN AIR
Laboratory Report 1:
Chemistry 1502ENG
Date of Experiment: 17/08/2010
Due Date: 31/08/2010
Introduction:
In comparison to solids and liquids, gases have many distinctive characteristics such as, it’s compressibility and it’s ability to obtain the volume (shape) of its container. Such properties of gases are vital to society and industries for essential science based theory. Boyle’sLaw sometimes referred as the Boyle-Mariotte Law is one of several gas laws as well as a special case of the Ideal Gas Law. Generally, Boyle’slaws explain the inversely comparative relationship among the complete pressure and capacity of gas, if the temperature is reserved in stable within a closed system. The mathematical expression for Boyles Law is:
V=K(1/P) or PV=K (Constant T and n)
Where, P and V are the pressure and volume of the gas sample respectively. K is a constant and dependent of the temperature (T) and the amount of gas (n, moles).
The Graph below successfully indicates Boyle’sLaw visually:
A: Volume Verses Pressure
B: Volume Verses 1/P
Part I of this experiment was specifically designed to validate Boyle’sLaw, through the use of a homemade barometer. The open-end tube of the barometer, when moved to different...

...Name: _____________________________________ Block: _________ Date: _______________
Lab #14: Boyle’sLaw
Objective: To determine the relationship between the pressure and volume of a gas at constant temperature.
Introduction:
The relationship of pressure to volume for a gas in a rigid container was first described in 1662 by the Irishborn
scientist Sir Robert Boyle (16271691), and is known as Boyle'sLaw. As long as the temperature of the gas
remains constant, the pressure of a gas has a predictable relationship with the volume of the gas.
The pressure of a gas is a measure of the force the gas exerts on the walls of its container. Recall that the
particles (atoms or molecules) of the gas are in constant motion, colliding with each other and with the walls of
their container. The net effect of these collisions is pressure. Even if a gas is not contained, the force of
collisions results in pressure. For example, the air around us exerts a force on every object it touches, and we can
measure this atmospheric pressure with a barometer.
In this activity, you will use a datalogger (called a SPARK) and a Pressure Sensor connected to a syringe full of
air to investigate the relationship between the volume and pressure of a gas.
Procedure:
Part A. Measuring Air Pressure ...

...Ideal Gas Law:
The ideal gas law is the equation of state of a hypothetical ideal gas. It obeys Boyle'sLaw and Charles Law.
Ideal Gas Law Formula :
General Gas Equation: PV = nRT
Pressure(P) = nRT / V
Volume(V) = nRT / P
Temperature(T) = PV / nR
Moles of Gas(n) = PV / RT
where,
P = pressure,
V = volume,
n = moles of gas,
T = temperature,
R = 8.314 J K-1 mol-1, ideal gas constant.
Ideal Gas Law Example:
Case 1: Find the volume from the 0.250 moles gas at 200kpa and 300K temperature.
P = 200 kPa, n = 0.250 mol, T = 300K, R = 8.314 J K-1 mol-1
Step 1: Substitute the values in the below volume equation:
Volume(V) = nRT / P
= (0.250 x 8.314 x 300) / 200
= 623.55 / 200
Volume(V) = 3.12 L
This example will guide you to calculate the volume manually.
Case 2: Find the temperature from the 250ml cylinder contaning 0.50 moles gas at 153kpa.
V = 250ml -> 250 / 1000 = 0.250 L, n = 0.50 mol, P = 153 kPa, R = 8.314 J K-1 mol-1
Step 1: Substitute the values in the below temperature equation:
Temperature(T) = PV / nR
= (153 x 0.250) / (0.50 x 8.314)
= 38.25 / 4.16
Temperature(T) = 9.2 K
This example will guide you to calculate the temperature manually.
Gay-Lussac's Law:
Gay-Lussac's Law states that the pressure...