Topics in ChemistryPostulate of the kinetic theory of gases
Academic Questions in Chemistry
The _____ spectrometry experiment conducted on isotopic elements gave a confirmation for the existence of isotopes.
D. Number of moles
F. Amount of substance
John Dalton's first atomic theory was modified based on a discovery made by _____.
A. Sir Isaac Newton
B. Albert Einstein
E. Boyle and Charles
F. Gay Lussac
Which of the following isn't an element of the periodic table.
An understanding on the concept of the kinetic theory of gases is considered a vital part of chemistry. This is true because chemistry involves the study of matter and the changes they undergo. In this regard, gaseous particles are always in motion (moving). In fact, the word kinetic means 'in motion'.
Take for instance, when a perfume is released into a room, the gaseous particles of the perfume will diffuse around the room. By diffusion, I mean that the gaseous particles of the perfume will move from the region of higher concentration to that of lower concentration around the room. As a result, the entire room will become filed with the scents of the perfume, and this is a function of the random motion exhibited by gaseous particles.
It is noteworthy to state that gases are comprised of a large number of separated submicroscopic particles at the atomic and molecular levels. According to the kinetic theory of gases, these extremely small gaseous particles are always in a constant, rapid and random motion which occurs in a straight line. While in motion, the gaseous particles will constantly collide with one another and the walls of its container.
In the 19th century, the kinetic theory of gases was established by the great works of British scientist - James Clerk Maxwell and Austrian physicist - Ludwig Boltzmann, in an attempt to study their behaviors.
The kinetic theory of gases further explains how properties like pressure, temperature, viscosity, thermal conductivity and volume impact on the movement of various gaseous molecules.
The basic principles of kinetic theory of gases may also be termed as the postulate of the kinetic theory of gases. They are listed and explained below:
Gaseous molecules present in a container are not static. They are in constant motion. In fact, if the container is opened, the gases will escape (or move out) from it. For this reason, we see why released gases escape into an open space. This random movement in a straight line is a major characteristic of gases since their comprising atoms or molecules are extremely small and widely separated.
Also, the forces that tend to attract the gaseous particles are very small or neglible. In summary, gas molecules are constantly and randomly moving in a straight line. This is in support of Newton's first law of motion.
With regards to gaseous molecules as material bodies, they obey Newton's laws of motion. This means that the molecules of an ideal gas will move randomly in straight lines until they collide with each other or with the walls of the container. This is shown in the image below:
Whenever gas molecules collide or come into contact with one another, they do so in an elastic manner. This implies that the colliding gaseous molecules bounce off one another, changing their directions and kinetic energies in the process.
Meanwhile, understand that gas molecules do not adhere to each other when they collide. This is also true whenever they collide with the walls of the container. In a similar fashion, they bounce off the container and do not stick to it.
Collisions are perfectly elastic with gaseous molecules. Whenever two gas particles collide, they change their directions and kinetic energies, but the total kinetic energy is conserved. Collisions are not sticky.
Each particle or atom that make up a gas is very small (microscopic). Also, they are widely separated from other gaseous particles.
Focusing on this particle, the actual volume it occupies in the container is extremely small (or even neglible). For this reason, the particles can freely move and collide since there exist a massive space within the container.
It is noteworthy to state that gas particles are separated by a large distance in relation to their particulate size. In this regard, if the container was opened, the gaseous particles will escape completely because of the massive space in the atmosphere.
In summary, the average distances of the gaseous particles are much greater than the sizes of the particles themselves.
As explained earlier, gas molecules are constantly in motion and will always collide with themselves and the walls of the container. However, there is no interactive force (that is, force of attraction or repulsion) between the gaseous particles.
Recall that solids have their particles adhering closely to one another. In fact, this is why solids have definite shapes and fixed sizes with static particles. In other words, the cohesive forces in solids are great. This is not the case in gases.
With regards to gases, the particles are widely spaced apart and are also constantly moving. Based of this fact, gases have no definite shape since there is no cohesive or binding forces between its particles.
The term 'average' is very significant in this theory. Now, let's imagine a gas is present inside a sealed metallic container. Based on our previous kinetic theories, the gaseous molecules will be in constant motion within the container, giving rise to an average kinetic energy of the overall gas molecules. Meanwhile, recall that the word 'kinetic' means moving or in motion.
Now, let's imagine that heat is applied to this container. When this happens, the gases will move at an increased speed (motion) and collision will be consequently increased. In short, a higher temperature will imply a higher speed and collision between the gas molecules themselves, alongside the gas molecules and the container's walls. The reverse will happen if temperature is decreased by putting the container in a refrigerator. In fact, at an absolute zero temperature, the gaseous particles will cease moving.
With regards to the explanations thus far, gaseous molecules can be summarized to exhibit the following behaviors:
All gases are made up of tiny molecules that are constantly, randomly and persistently moving in straight lines.
All the molecules in an ideal gas obey Newton's laws of motion.
Please read on motion and speed here.
The separation (distance) between the gaseous molecules are overwhelmingly greater than the size of each molecule.
Collisions between the gas molecules themselves and the walls of the container are considered to be perfectly elastic.
Compared to the space present inside the container, the size of the gas molecules are very small or neglible.
If a gas sample is kept in a container, the molecules making up the gas will not exert any force on the walls of the container during collision.
The time interval of a collision between two molecules, and between a molecule and the walls of the container is considered to be neglible.
If a gas sample is left for a sufficient time, it will eventually come to a steady state. In this case, the density of molecules and their distributions are independent of position, distance and time.
The average kinetic energy of the gaseous molecules is temperature dependent and will always be in proportion to it.
Kindly share this article via the links below:
Alfred Ajibola is a Medical Biochemist, a passionate Academician with over 7 years of experience, a Versatile Writer, a Web Developer, a Cisco Certified Network Associate and a Cisco CyberOps Associate.
Amazing facts in Chemistry
Plastic and Glass can decompose, but not in our lifetimes. It takes an average time of 450 years for plastics to decompose. As for the decomposition of glasses, it takes about 4,000 years
The only letters that failed to appear on the periodic table are letters:
Gold and copper are the only two non-silvery colored metals.
Copper is the only metal that is naturally antibacterial. For this reason, some children utilize 'copper water bottles' in schools
NOTABLE POINTS IN Chemistry
In chemistry, hydrocarbons can be classified as either aliphatic or aromatic. Recently, both classifications of hydrocarbon were based on their structure rather than their origin.
Aliphatic hydrocarbons are put into three main groups according to the types of bonds they possess. These are:
They are shown in the image below:
It's important to note the followings:
Alkanes have single bonds (only) in their structures.
Alkenes always have a carbon-carbon double bond present in their structure.
Alkynes always have a carbon-carbon triple bond present in their structure.
Aromatic hydrocarbons are classified into:
Organic chemistry is the study of carbon and it's compounds.
Carbon is the focus of organic chemistry because it has a wide chemical diversity in the sense that it can combine with other carbon atoms to form a long chain of carbon molecule. This ability and process whereby carbon can form a long chain of itself is called catenation.