Title: PROP0332 Evaluation of the Gas Law Constant

Abstract: The result of the change in volume was approximately 22 CC or 0.00084 mol. This translates into the average for the R constant being 83.8L*atm/K*mol. The four determinations ensured that the results were accurate because more than one trial helps somewhat prevent error. Approximately 0.20g of the Mg ribbon was used for these determinations.

Introduction:
1. Theory
If the temperature of a gas sample was held constant, its volume varied inversely with its pressure. The Kelvin scale is known as the absolute scale. Charles’ law states that volume of a given mass varies directly with its absolute temperature if the pressure remains constant. Ideal gases are those whose behavior is exactly described by Boyle’s and Charles’ laws. Avagadro’s principle says that the volume of a gas sample at a given temperature and pressure is proportional to the mass or number of moles of the gas. 2. Reference citations

Grover W. Everett, East Carolina University, Signature Lab Series, Prop 0332, p. 141 3. Important Equations
V α 1/P
V=K1/P
V=K2*T
V α T
P1V1T1P2VxT1P2V2T2
Vx=V1(P1/P2)
V2=Vx(T2/T1)
V2=V1(P1*T1/P2*T2)
P2*V2/T2=P1*V1/T1
PV/T=K
PV=nRT
Mg(s)+2HCl(aq)MgCl2(aq)+H2(g)
PV/nT=R
PV/nT=atmosphere-millileter/mole-degree=R
Corrected pressure, atm= ((recorded barometric pressure, torr - vapor pressure of water, torr)/760 torr atm^-1)

4. Objective
In the experiment, one must determine the volume of a known mass of a gas at a measured temperature and pressure. One must use data to evaluate the universal gas law constant, R.

Experimental:
1. The procedure for this experiment appears in the lab manual1. Everett, G.W.; Everett G.W. Jr. Classifying Matter by Properties; Cengage Learning: Manson, OH, 1997, pp 143-149. Results:
Mass Mg, g0.021g0.021g0.022g0.020g
# of moles Mg
Initial syringe vol, mL4.5 CC5.0 CC19.0 CC10.0 CC
Final syrine vol, mL26.5 CC27.3 CC43.3 CC...

...CHEMISTRY 130 Laboratory Section: ________
Page 1
Name ______________________
Evaluation of the GasLawConstant
Objectives In this experiment, we will determine the Ideal GasConstant, 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 sample is proportional to its absolute temperature at constant pressure. Thus V ∝ T abs . In addition, Boyle's Law states that the volume of a gas sample is proportional to the inverse of 1 its pressure at constant temperature. That is, V ∝ P . If we include the fact that Avogadro's Law states in effect that the volume of a gas sample is proportional to the number of moles of gas, n, at constant temperature and pressure we have V∝n . Combining these three proportionalities into one produces the following: V∝
nT P
where T is the absolute temperature. Note that any proportionality can be made into an equality if we derive the proper 'proportionality constant'. In this case we will use the symbol "R" to represent this...

...Vanessa Gale
Formal Lab:
Evaluation of the GasLawConstant
Dr. Monzyk
Due 06/25/2012
Purpose:
The purpose of this lab is to evaluate the gaslawconstant. The ideal gaslaw is represented as PV=nRT, where R represents the gaslawconstant. To determine R, we must find the other parameters, P, V, n and T through the experiment.
Equipment and Materials:
Large beaker
Ring stand
Clamp
Copper wire
100 mL eudiometer tube
Magnesium (Mg) ribbon
M6 H2SO4 (Sulfuric Acid)
Wash bottle filled with distilled water
Procedure:
First I cut a piece of Mg ribbon and used steel wool to rub off the MgO (magnesium oxide). I then used the scale to determine when I had approximately 0.0440g of Mg. I then wrapped the Mg with copper wire so that none was showing, but left a tail of copper wire.
In the fume hood, I added 8 mL of M6 H2SO4 to the eudiometer tube. I used the wash bottle to carefully and completely fill the tube with water, being sure not to mix the water with the sulfuric acid. Then I placed the copper covered Mg into the tube and left the tail end hanging over the edge. I placed the rubber stopper into the end. I held my finger over the hole in the stopper, gently flipped over the tube and place the stopped end into the water. I removed my fingers and then...

...GasLawsLab
Introduction:
The four basic physical properties of a gas sample are pressure, volume, temperature, and number of moles. The volume simply indicates the volume of the container since a gas will take up all space available to it. The temperature indicates the average kinetic energy of the gas particles. For gases, the temperature must be converted to the Kelvin unit. The pressure of thegas indicates the number of collisions with each other and the wall of the container. The number of moles indicates the amount of gas particles.
Gases do not have a definite shape of volume. Gases spread out into their container and occupy the entire volume available, which means they are free to move around and have large amounts of empty space. In many chemical reactions, gases are produced; for example, reactions involving metal carbonates that react with an acid produce gaseous carbon dioxide.
Objective:
To determine the volume of gas produced from a reaction between a metal carbonate and acid and to determine the identity of an unknown carbonate salt.
Pre-Lab Questions:
1. If you increase the temperature what happens to the speed of the particles? Explain.
2. What is the formula to convert Celsius temperature to Kelvin?
a. °C+273.15=K
3. What are the standard conditions for a gas? Are you at...

...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 = P2V2
(1.0 atm)(15 L) = (0.85 atm)(x)
x = 18 L
3) I’ve got a car with an internal volume of 12,000 L. If I drive my car into the river and it implodes, what will be the volume of the gas when the pressure goes from 1.0 atm to 1.4 atm?
P1V1 = P2V2
(1.0 atm)(12,000 L) = (1.4 atm)(x)
x = 8600 L
Charles’s Law – Solutions
1) If I have 45 liters of helium in a balloon at 250 C and increase the temperature of the balloon to 550 C, what will the new volume of the balloon be?
[pic]
2) Calcium carbonate decomposes at 12000 C to form carbon dioxide and calcium oxide. If 25 liters of carbon dioxide are collected at 12000 C, what will the volume of this gas be after it cools to 250 C?
[pic]
3) I have 130 liters of gas in a piston at a temperature of 2500 C. If I cool the gas until the volume decreases to 85 liters, what will temperature of the gas be?
[pic]...

...Ideal GasLawLab
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 the bucket with the opening upwards, turning the open end downwards after the tube was fully submerged beneath the surface. We then placed the canister directly below the opening of the test tube, and released the gas so that the bubbles rose into the test tube.
Next, we used a cork whose head was larger than the opening of the test tube to block off the opening (without changing the pressure inside of the tube), so that we could transport the remaining water to a graduated cylinder. When doing this, it was very important that the water level inside of the tube was equal to that of the surrounding water in the bucket, because that ensured that since the water pressure in the tube was the same as that of the surrounding water, the pressure of the gas would be the same as that of the surrounding air. Thus, we recorded the gas pressure to be the same as the pressure in the room, which was calculated to be 763.0 mmHg.
We poured the...

...Introduction
A gas is the state of matter that is characterized by having neither a fixed shape nor a fixed volume. Gases exert pressure, are compressible, have low densities and diffuse rapidly when mixed with other gases. On a microscopic level, the molecules (or atoms) in a gas are separated by large distances and are in constant, random motion. When dealing with gases, the Ideal GasLaw equation is the most famous equation used to relate all the factors in dealing and solving the problem. The four factors or variables for gas are: pressure (P), volume (V), number of mole of gas (n), and temperature (T), and the constant in the equation is R, known as the gasconstant.
The Ideal Gaslaw equation which is pV=nRT is obtained by combining the three GasLaws: Boyle’s Law, Charles’s Law and Avogadro’s Law. Boyle’s Law describes the inverse proportional relationship between pressure and volume at a constant temperature and a fixed amount of gas. Charles's Law describes the directly proportional relationship between the volume and temperature (in Kelvin) of a fixed amount of gas, when the pressure is held constant. Avogadro’s Law describes...

...GASLAWS
GROUP 1
Sheena Mae Agustin
Hans Alcantara
Renzo Bren Ado
Miguel Afable
Ron J Advincula
De La Salle University - Dasmariñas
Dasmariñas, Cavite Philippines
ABSTRACT
Gases behave in a similar way over a wide variety of conditions because to a good approximationthey all have molecules which are widely spaced, and nowadays the equation of state for an ideal gas isderived from kinetic theory. The combinedgaslaw or general gas equation is formed by the combination of the three laws, and shows the relationship between the pressure, volume, and temperature for a fixed mass of gas. The GasLaws that have been subject to testing were Combined GasLaw and Graham’s Law.
INTRODUCTION
The combined gaslaws a gaslaw which combines Charles's law, Boyle's law, and Gay-Lussac's law. These laws each relate one thermodynamic variable to another mathematically whileholding everything else constant. Charles's law states that volume and temperature are directlyproportional to each other as long as pressure is held constant. Boyle's law asserts that pressure andvolume are inversely proportional to each other...

...GasLaws
Name
Institution
The 3 GasLaws
Introduction
The three gaslaws include: Gay-Lussac’s law, Boyle’s law and Charles’ law. When combined with Avogadro’s law the three laws can be generalized by the ideal gaslaw. Gases possess observable properties which include, mass, pressure (P), thermodynamic temperature (T) and volume (V). These properties are related to each other and the state of a gas is determined by their values. The three laws are derived from these properties.
Discussion
Boyle’s gaslaw
Boyle’s law relates the volume and pressure of an ideal gas. It states that when the temperature of a given mass of a confined gas is held constant, its pressure and volume are inversely proportional. In other words, the product of absolute pressure and volume is nearly constant and exactly a constant for an ideal gas (Stoker, 2013).
The mathematical equation for Boyle's law is:
PV = k
Where:
P denotes the pressure of the system.
V denotes the volume of the gas.
K is a constant value representative of the pressure and volume of the system.
Explanation
Provided a fixed quantity of...

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