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The kinetic theory of gases is a mathematical representation of the thermodynamic behaviour of gases in a closed system. This model represents a gas that contains a huge number of submicroscopic particles that are in rapid, random motion and regularly clash with one another as well as with the walls of any container in which they are contained. The larger the temperature difference between them, the greater the likelihood of them colliding.
Kinetic energy
Kinetic energy is the energy generated by motion or movement of a thing.The amount of kinetic energy produced by the molecules is proportional to the speed of the molecules. Increases in the overall kinetic energy of the colliding molecules are proportional to increases in the speed of the colliding molecules.
Because their size is smaller than the average distance between the particles, it is thought that they are closer together. Known as the kinetic theory of gases, it is responsible for explaining the macroscopic properties of gases such as volume, pressure, and temperature, as well as microstructural features such as viscosity and thermal conductivity. This model also provides information on Brownian motion.
Fundamental principles of the kinetic theory of gases
- Gases are made up of rigid molecules having a spherical shape.
- When compared to the volume of gas [the volume of the container], the volume of the molecule is insignificant.
- There are no intermolecular forces in the absence of an external force.
- Molecules are continually in random motion, attempting to collide in a completely plastic manner.
- When these molecules collide with the walls of the container, they exert pressure on the contents.
- There is no effect of gravity on the molecule of gas that can be contained.
- Gas kinetics is a branch of physics that studies the behaviour of gases.
Fortunately, the Kinetic Theory of Gases is useful and can be employed in this case; with its guidance, the real qualities of any gas may be characterised in terms of three quantifiable attributes, which is a common occurrence. The pressure, volume, and temperature of the compartment in which the gas is stored or is present are all measured and recorded.
The kinetic theory of gases describes the random movement of molecules in a gas and provides an explanation for this movement. The kinetic theory of gases describes how gases behave by assuming that the gas is made up of fast moving particles or atoms and that these particles or atoms are in motion.
The kinetic theory of gases consists of a number of general terms.
- When it comes to pressure, it is defined as the amount of force applied per unit area.
Volume: The quantity of 3D space occupied by a substance or object is referred to as its volume.
- Temperature: Temperature is a feature of matter that represents the amount of energy expended by the particles that make up the substance in motion. It is a measure of how hot or cold a material is in comparison to another.
- The gas constant is as follows: In the equation of state of gases, a gas constant is defined as the product of the pressure and volume of one mole divided by the absolute temperature, which in the case of an ideal gas is equal to one mole divided by the absolute temperature. R = 8.314Jmol-1 K-1
Molecular Speed
The pace at which atoms are gathered is standard for this process. It is impossible for particles in a perfect gas to come into contact with one another. There are three types of molecular speeds: RMS velocity, Average velocity, and Most probable velocity. RMS velocity is the mean of the three types of molecular speeds. Here are the formulas for the various speeds in the appropriate order.
- For speed, the root-mean-square (RMS) speed is the sum of the squares in the stacking speed values divided by the number of features.
Vrms = √(3RT)/(M) or √(3P)/(d)
vrms = Root-mean-square velocity
M = Molar mass of the gas (Kg/mole)
R= Molar gas constant
T = Temperature in Kelvin.
- Molecular average speed is defined as the arithmetic mean of the speeds of all the molecules in a system.
Vavg= √(8RT)/(πM) or (√8P)/(πd)
- In the case of a curve, the most probable velocity is defined as the speed that corresponds to the curve’s maximum point of intersection.
Vmp= √(2RT)/(M) or √(2P)/(d )
Conclusion
The amount of kinetic energy produced by the molecules is proportional to the speed of the molecules. Increases in the overall kinetic energy of the colliding molecules are proportional to increases in the speed of the colliding molecules.
Because their size is smaller than the average distance between the particles, it is thought that they are closer together.
The pace at which atoms are gathered is standard for this process. It is impossible for particles in a perfect gas to come into contact with one another.
