Kinetic Theory of Gases
Gases are an exciting subject to study, which can be easily understood by taking into consideration the action of individual molecules. You can also understand more about gases by taking into consideration the gases’ large scale action. However, to further study how molecules act in different situations, you need a theoretical model. This is where the Kinetic theory of gases comes into the picture. Now, the most obvious question is, what do you mean by the kinetic theory of gases? It is the conceptual model that assumes that the size of molecules is very small when compared to the distance between these molecules. These molecules are constantly moving, and since the distance between them is less, they collide with each other.
Basics of Kinetic Theory of Gases
As per the basics of the kinetic theory of gases, the molecules move in random motion and keep on colliding with each other as well as the walls of the container they are kept in. Since these collisions remain elastic in nature, both the total momentum as well as total kinetic energy are conserved easily. Thus, you will find that neither the energy is preserved nor lost during this collision of molecules.
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(In the image above, you can see the kinetic theory of gases formula. The different aspects of the formula are P = pressure of gas; V = volume of gas; T = temperature; N = moles of gas which are present; and R is the constant, which is known as the universal gas constant)
Here: PV = nRT;
P is the pressure of gas;
V is the volume of the gas;
T is the temperature which is measured in kelvin;
N is regarded as the moles of gas which are present;
R is the constant, which is known as the universal gas constant.
Postulates of Kinetic Theory of Gases
The theory related to gases based on the molecular motion is known as the kinetic theory of gases. However, like any other theory, there are some postulates of the kinetic theory of gases as well. Let us read in detail about these postulates of the kinetic theory of gases:
During the collision process, the molecules cannot lose any kind of kinetic energy. Thus, it can be easily said that these said collisions are perfectly elastic.
You can find ample space between these moving molecules, which leads to continuous motion between them.
The molecules present in a gas are actually very minute and distanced from each other. This implies that the volume occupied by a particular gas is just empty space and nothing else.
The collision occurs between molecules among each and with the walls of the container they are kept in. This collision is responsible for the gas pressure.
Assumptions of Kinetic Theory of Gases
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(the image represents the assumptions of the kinetic theory of gases. There are 5 main assumptions as mentioned below)
These gas molecules move in constant random motion, and most of these molecules are moving in one single direction than other molecules.
During the process, these said molecules present in the gas are not exerting any kind of attractive or repulsive forces on each other. During the collision, they do exert pressure on each other. However, when they are not colliding, they keep on moving in straight lines.
The division between these molecules is much more in size than the molecules’ actual size.
All kinds of collisions occurring between these molecules, as well as between the molecules and the wall, are elastic in nature.
All these molecules present in the said gas diligently obey Newton's law of motion.
These assumptions of the kinetic theory of gases make sure that the gas characteristics lie within the range of mathematical calculations.
More About Kinetic Theory of Gases
It was in the 19th century that scientists, by the name of James Clark Maxwell, Clausius, and Rudolph, worked upon the development of the kinetic theory of gases to explain the concerned gases’ behaviour. As per the theory, gas is considered to be a complete collection of minute, hard spheres that can interact with each other as well as the container in which the gas is contained.
As per the kinetic theory, the pressure exerted by the gas is the result of collisions taking place between the gas molecules as well as the container walls where they exist. Further, the temperature of the gas is in relation to the gas molecules’ average moving speed. However, remember that at a constant temperature, the molecules’ speed actually remains constant. Now, if anyone reduces the container’s volume, the molecules will enjoy less distance for travelling, and thus, they would be hitting the container’s wall causing higher pressure. On the other hand, if the container’s volume increases, the molecules will hit the walls of the container with less speed, resulting in lower pressure.
1. What do you Understand by Three Main Components of the Kinetic Theory Of Gases?
The Kinetic Theory of Gases actually makes an attempt to explain the complete properties of gases. These properties are based on pressure, volume, temperature, etc of the gases, and these are calculated by considering the molecular composition of the gas as well as the motion of the gases. The kinetic theory is also known by the name of collision theory or kinetic-molecular theory. The three main components of the kinetic theory of gases are:
The molecules move in a linear as well as constant motion;
During the collision of the molecules, no energy is lost or gained;
The space is taken up by the molecules present in gas in relation to the container they are kept in almost negligible.
2. How can you Explain the Kinetic Theory of Gases?
The kinetic theory of gases explains the fact of how the molecules present in a gas move around freely as well as rapidly along the straight lines. However, while moving, these molecules actually collide causing many variations both in thor directions and velocity. As per the theory, the pressure can be interpreted as coming from the influence of these particles on the container’s walls.