In the 1700's a number of people investigated gas behavior in the laboratory. Robert Boyle investigated the relationship between the volume of a dry ideal gas and its pressure. Since there are four variables that can be altered in a gas sample, in order to investigate how one variable will affect another, all other variables must be held constant or fixed. 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:

P1V1 = P2V2

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.

Charles's Law

Jacques Charles investigated the relationship between the Volume of a gas and how it changes with temperature. He noted that the volume of a gas increased with the temperature. Charles's Law states that the volume of a given amount of dry ideal gas is directly proportional to the Kelvin Temperature provided the amount of gas and the pressure remain fixed. When we plot the Volume of a gas against the Kelvin temperature it forms a straight line. The mathematical statement is that the V / T = a constant. For two sets of conditions the following is a math statement of Charles's Law:

V1 / T1 = V2 / T2

Gay-Lussac Law

Gay-Lussac investigated the relationship between the Pressure of a gas and its temperature. At constant Volume, the pressure of a gas sample is directly proportional to the Kelvin Temperature. The relationship is similar to the Volume-Temperature relationship (Charles's Law). The mathematical statement is as follows:

...Boyle’s Law - Solutions
1) If I have 5.6 liters of gas in a piston at a pressure of 1.5 atm and compress the gas until its volume is 4.8 L, what will the new pressure inside the piston be?
P1V1 = P2V2
(1.5 atm)(5.6 L) = (x)(4.8 L)
x = 1.8 atm
2) I have added 15 L of air to a balloon at sea level (1.0 atm). If I take the balloon with me to Denver, where the air pressure is 0.85 atm, what will the new volume of the balloon be?
P1V1 =...

...Ideal GasLaw Lab
1. Procedure: First, we used a balance to weigh the canister of gas, and recorded that mass as the original weight.
Then, we filled a large bucket with water and recorded the temperature. We then filled a small test tube with water at the same temperature and poured that water into a graduated cylinder to measure the original volume of water in the tube.
We then poured the water back into the test tube and placed the tube into...

...BOYLE’S LAW 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’s Law sometimes referred as the...

...between pressure, volume and temperature of gas
Date of experiment: 12/11/2008
Aim of experiment:
The objective of this experiment is:
1. To study the relationship between pressure and volume of a gas at constant temperature.
2. To study the relationship between the volume and temperature of a gas at constant pressure.
Principles involved:
When gases are compared, their volumes, temperatures and pressure are always involved. The volume...

...GasLaws
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...

...23rd, 2013
Generation of Hydrogen Gas
Abstract
Hydrogen gas was produced from a reaction in a eudiometer between a weighted amount of magnesium ribbon and 5ml of diluted 6M hydrochloric acid. The partial pressure of the hydrogen gas produced was calculated using Dalton’s Law of partial pressure. With this partial pressure value along with known values in the experiment the number of moles of hydrogen gas produced could...

...of the GasLaw Constant
Objectives In this experiment, we will determine the Ideal Gas Constant, R, which relates the number of moles of gas present to its volume, pressure and absolute temperature. Background To see how "R" was derived, we must look at the proportionalities defined by the other fundamental gaslaws. For example, Charles' Law showed us that the volume of a gas...

...objective of the experiment was to verify the molar volume of a gas and gas constant.¹ The method in which was used to determine the volume of H2 gas at standard temperature and pressure and the gas constant was to measure a strip of magnesium and place it inside the gas buret which contained hydrochloric acid, blue dye and distilled water and allow the reaction to occur. Once the reaction was complete and there were no...

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