“If we assume that the last breath of, say, Julius Caesar has by now become thoroughly scattered through the atmosphere, then the chances are that each of us inhales one molecule of it with every breath we take.”
― James Jeans, An Introduction To The Kinetic Theory Of Gases
This law defines the behaviour of gases and it consist of various assumptions are-
It is defined for the energy produced from the motion of the particles which is proportional to the absolute temperature of the gas.
It depends on quantity like Temperature , mass of a gas molecule . average velocity and other certain conditions.
P – pressure as force exerted on the walls of the container during collision
N – No. of the particles
When the number of particles increases, The frequency of collisions with the walls also increases.
Hence, pressure increases with increase in gas molecules.
The kinetic molecular theory of gas followed by the laws are defined for the ideal gas , whose molecules have no interionic interactions.
PV=nRT , R is a gas constant
CHARLES LAW (V,T)
Keeping constant the pressure of a gas , the volume becomes proportional to the temperature of the gas. This is based on the fact that as mass of the particles is constant , this thereby increases and balances the pressure applied by the gas particles on the surface of the wall . Hence , the volume of gas becomes larger as temperature increases.
Keeping temperature constant, The pressure applied by the gas molecules is inversely proportional to the volume.
I based on the constant Temperature conditions , which results in the same kinetic energy. Hence during collisions of high number , pressure of the gas also increases , but the volume decreases because now frequency of collision is high.
Keeping temperature and pressure, The volume of the gas is proportional to the number of gas molecules.
This law states that the total pressure of a mixture of gases must be the sum of partial pressure of each gas present in the mixture. These gases must be non-reactive with each other.
By joseph Louis GAY-LUSSAC
It is based on the assumption that keeping constant the volume and temperature of the gas.
The pressure applied is proportional to the temperature.
The 0K or -273.15°C is called absolute zero temperature. It can be represented in the V/T curve after extra plotting of the curve to zero. At this temperature, all molecular motions would cease.
The behaviour of real gases behaves differently as of ideal gases and deviates the laws because-
Real gas molecules both attract and repel due to interionic force of interaction.
True gas molecules have an infinite volume
But at high temperature and low pressure all the real gases behave ideally.
Q 1. In a closed vessel , If total pressure is 6Atm by the mixtures of gases consisting of Hydrogen , oxygen and nitrogen with the partial pressure of 3atm , 2.5 . Then what will be the partial pressure exerted by nitrogen gas ?
Total pressure = 6 atm
Applying DALTON LAW
Total pressure = PH2 + PO2 + PN2
6= 3+ 2.5 + PN2
0.5 atm = PN2
Answer: PN2 = 0.5 atm
Q 2. Which law obeys only at constant volume conditions?
Gay lussac law
Dalton theory of partial pressure
Ans: Boyle law
Q3 Which of the conditions are necessarily for Real gas to behave ideally?
Constant Temperature and pressure
High pressure and low temperature
Low pressure and high temperature
Low pressure and low temperature
Ans: Low pressure and high temperature
Do you need help to understand the molecular origins of average kinetic energy? We’re here to help if you need to go down that road and complete your chemistry assignment without any stress. Whether you need help to understand how gas particles behave and respond to changes, let us help you in revising general conception of matter.
Besides we’ll assist you to apply the theory to predict and explain gas laws by covering major concepts in detail. Be it a College research paper where you need to assess, analyze and demonstrate the relationship between kinetic energy and molecular speed- we’ll leave no track uncovered.
Right from covering the postulates to understanding the main points- we provide self-explanatory notes or written material to help you grasp those elusive concepts. With the help of diagrams and in-depth explanations covering tricky topics, our top solvers ensure your academic success.
Get exam help from dependable homework solvers who will help you understand gas particles, molecules and cite enough examples to meet high writing standards.
Whether you are in high school or in college- our highly qualified dedicated project managers who will provide well structured solutions elaborating on theory to explain observable properties - get ready to cover formulas in detail.
Our team understands the importance of timely delivery and quality assistance, hence experts are available 24/7 as a quick aid to solve urgent queries. Right from covering “what is an ideal gas?” or working on “average kinetic energy formula”- let us reassure you that your work is in good hands.
Not only do we ensure quick delivery but also maintain an unbeatable track record of maintaining quality standards.
Hire academic experts at reasonable price by following these few simple steps:
Step 1: Fill out our quick help homework form by uploading worksheets and assignment instructions
Step 2: Reach an agreement with the hired helper on budgetary considerations and set a timeline
Step 3: Review your assignment before releasing payment for delivered draft from escrow
At TutorEye, we provide 100% authentic and unique assignments within set deadlines. Our quality assessment team checks each and every draft for plagiarism and ensures there are no copyright issues. We adhere to Money Refund policy to maintain trust and satisfaction of our students.
Gas laws (Boyle’s law, Avogadro’s law, Dalton’s law and Charles’s law) can be explained using kinetic molecular theory. The increase in pressure of a gas on decreasing the surface area of a container is due to increased molecular strikes per unit of time. Volume must be increased to keep the pressure constant. Increase in temperature of gas results in increased kinetic energy of the molecules. The gas expands to keep the pressure constant.
Kinetic molecular theory explains different properties of gases and different gas laws. Boyle’s law can be explained by kinetic molecular theory. The pressure of a gas depends on the number of times the molecules strike the surface of the container. On compressing the gas to a smaller volume, the surface area is smaller but the number of molecules is the same. In other words the number of molecules striking against the surface is now more. Hence, pressure will increase. To keep the pressure constant, the volume must increase, which explains Avogadro's law.
Charles’s law can also be explained using kinetic molecular theory. According to kinetic molecular theory the increase in temperature increases average kinetic energy of the molecules. If the molecules are moving with more speed but the pressure remains the same, then the molecules must stay apart, so that the increase in the rate of molecular collisions with the surface of the container is compensated for by the increased surface area.
Kinetic molecular theory is very useful in understanding both microscopic and macroscopic properties of gases. All gas laws including Boyle’s law, Avogadro's law, Charles’s law can be explained using kinetic molecular theory of gases.