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]

Combined Gas Law Worksheet - Solutions

1)If I initially have 4.0 L of a gas at a pressure of 1.1 atm, what will the volume be if I increase the pressure to 3.4 atm?

(1.1 atm)(4.0 L) = (3.4 atm)(x L)
x = 1.29 L

2)A toy balloon has an internal pressure of 1.05 atm and a volume of 5.0 L. If the temperature where the balloon is released is 200 C, what will happen to the volume when the balloon rises to an altitude where the pressure is 0.65 atm and the temperature is –150 C?

(1.05 atm)(5.0 L)/(293 K) = (0.65 atm)(x L)/(258 K)
x = 7.11 L

3)A small research submarine with a volume of 1.2 x 105 L has an internal...

...Gaslaws have an impact on several aspects of our lives. The S.T.E.M I decided to explore deals a great deal in thermodynamics in the gaslaw I chose chemistry. First off I have to explain what is the broad practice of chemistry. Chemistry, a branch of physical science, is the study of the composition, properties and behavior of matter. Chemistry is concerned with atoms and their interactions with other atoms, and particularly with the properties of chemical bonds. Chemistry is also concerned with the interactions between atoms and various forms of energy Chemistry is sometimes called "the central science" because it bridges other natural sciences like physics, geology and biology with each other. Chemistry is a branch of physical science but distinct from physics. The origin of the word chemistry has been much disputed. The origin of chemistry can be traced to certain practices, known as alchemy, The scientific discipline that intersects the areas of chemistry and physic is commonly known as physical chemistry, and it is in that area that a thorough study of thermodynamics takes place. Physics concerns itself heavily with the mechanics of events in nature. Certainly changes in energy however measured, whether it be heat, light, work are clearly physical events that also have a chemical nature to them. Thermodynamics is the study of energy changes accompanying physical and chemical changes. From temperature, meaning...

...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 at fixed temperature....

...valency of magnesium
Date :29/6/2011
Lecturer :Dr Ha Sie Tiong
Title: Determination of the Valency of Magnesium
Objective
To study the quantitative relationship between the amount of reactants and products of a reaction. A known starting mass of magnesium and the measured collection of hydrogen gas will be used to determine the reaction stoichiometry and the valency of magnesium.
Introduction
Stoichiometry is a measure of relative amount of reactants to products in an experiment. In this experiment, a known mass of magnesium and volume of hydrogen gas collected is used to determine stoichiometry in this experiment.
A known mass of magnesium ribbon is mixed with hydrochloric acid to produce magnesium chloride and hydrogen gas.
Mg(s) + xHCl (l) MgClx (aq) + (x/2)H2(g)
Magnesium will be the limiting factor in this experiment, excess of hydrochloric acid will react completely with magnesium to give hydrogen gas and magnesium chloride. The yield of hydrogen gas is depend on the amount of magnesium used, thus the volume of hydrogen gas collected can be used to determine the x number.
Methodology
1. Burette is used upside down to collect hydrogen gas produced in the experiment. There’s an unknown volume between unmarked space and the tap of burette, the volume is determined by pipette 25.00cm3 of water into the vertically clamped burette
right...

...Ideal GasLaw:
The ideal gaslaw is the equation of state of a hypothetical ideal gas. It obeys Boyle's Law and Charles Law.
Ideal GasLaw 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 ofgas,
T = temperature,
R = 8.314 J K-1 mol-1, ideal gas constant.
Ideal GasLaw 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...

...
Ideal Gas Behavior
Author: VanessaStoll
Lab Partners: Janelle Vallejo
Instructor: Nieves Montano
Chem 151, Section 002G
Date Work Performed: February 12, 2014
Date Report Submitted: February 20, 2014
Abstract:
This paper reports a lab experiment done on the ideal gaslaw to determine differences in gas based upon their “R” constant difference to 0.082057. A total of seven gases were tested, which included, Ethanol, Hexane, Cyclohexane, Pentane, Ethyl Acetate, Butane and Acetone. These gases were each heated and then condensed to liquid gas to find specific values and determined Ethanol as the gas closest to ideal behavior in this experiment.
Introduction:
The Ideal GasLaw demonstrates the relationship of the properties of gases. This relationship is specific to the gases that are considered “ideal”. For a gas to be considered “ideal,” it will have no interactions with other molecules and the molecules that make up the gas won’t take up any space.
The Ideal GasLaw equation is PV=nRT. “P” stands for pressure, “V” is for volume, “n” gives the number of moles, “R” is the gas constant and “T” is for temperature. The ideal gas constant value is 0.082057 (L x atm)÷(mol x K). The purpose of the experiment was to be able to measure the temperature and...

...EXPERIMENT NO. 6
DETERMINATION OF THE MOLAR VOLUME OF A GAS
AND THE UNIVERSAL GAS CONSTANT
Salve, Ryan Angelo TAB3, Group 6, Mr. John Kevin Paulo Biadomang
Tabor, Frances Hermilyn March 8, 2013
-------------------------------------------------
I. Abstract
This experiment is working with the ideal gaslaw, which is the summation of Boyle’s Law, where pressure is inversely proportional to volume, Charles’Law, where the volume is directly proportional to temperature and Avogadro’s Law, where the volume is directly proportional to moles. In this experiment, the volume occupied by one mole of H2 was determined. By measuring the volume of H2 gas generated, its molar volume can also be calculated. The universal gas constant can be determined using the ideal gaslaw.
The experiment was done by inverting a graduated cylinder containing HCl and water with the cork assembly that was placed in its mouth into a beaker of ¾ full. The cork assembly was done by using a paper clip with a small piece of Mg ribbon attached to it. Using the equations of gaslaw, the universal gas constant and the molar volume were calculated. The experiment results lead us into a conclusion that there are possible errors happened during the experiment that made it different from the desired...

...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 gas constant.
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 that volume of a gas is directly proportional to 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 visible gas bubbles, the volume was obtained and recorded. This procedure was completed three times. After gathering all the information needed, and using the ideal gaslaw to find the gas constant for each trial, the average of the three results were then calculated and turned out to be 0.0841L atm/k mol. The approximation error turned out to be 0.00404 L atm/k mol. Finding the molar volume at STP was done by multiplying the number of moles of the gas by the value of the gas constant found in the experiment.
Introduction:
The purpose of this experiment is to discover how the molar volume of a gas and the gas constant is found. The molar volume can be found by the equation:
MV = V/n = RT/P
where it is either dependent on a given volume (V) and a number (n) of moles or a constant temperature (T), pressure (P) and the gas constant. In Avogadro’s Law it is stated that when the pressure and...