Kinetic theory of gases এর সম্পর্কে তথ্য যা পরীক্ষা তে দেবে সফলতা। скачать в хорошем качестве

Kinetic theory of gases এর সম্পর্কে তথ্য যা পরীক্ষা তে দেবে সফলতা।

The Kinetic Theory of Gases explains the behavior of gases in terms of the motion of their individual molecules. It is a fundamental theory in thermodynamics that provides a microscopic explanation for the macroscopic properties of gases such as pressure, temperature, and volume. Key Assumptions of the Kinetic Theory of Gases: Gas molecules are in constant, random motion. The molecules move in straight lines until they collide with another molecule or the walls of the container. The volume of individual gas molecules is negligible. Gas molecules themselves have very little volume compared to the volume of the gas as a whole. Collisions between gas molecules and with the container walls are perfectly elastic. This means that during collisions, the total kinetic energy of the system is conserved. There are no attractive or repulsive forces between gas molecules. This assumption simplifies the interactions between molecules to only include collisions, not forces like gravity or electrostatic attraction. The gas molecules are assumed to be identical. All molecules of a particular gas are assumed to have the same mass and size. Key Concepts Derived from the Kinetic Theory: Pressure of a Gas: The pressure exerted by a gas on the walls of its container is the result of countless collisions between the gas molecules and the wall. Each collision exerts a small force, and the cumulative effect of all these collisions is the observed pressure. Temperature and Average Kinetic Energy: Temperature is directly related to the average kinetic energy of the gas molecules. The higher the temperature, the faster the molecules move, leading to greater kinetic energy. The average kinetic energy of gas molecules is given by the equation: Boyle’s Law, Charles’s Law, and Ideal Gas Law: The Kinetic Theory of Gases helps explain the relationship between pressure, volume, and temperature of gases, which are summarized in the Ideal Gas Law: P = pressure V = volume n= number of moles of gas R = universal gas constant T = temperature in Kelvin Applications: Diffusion: The kinetic theory explains how gas molecules move and spread out to fill a container, a process known as diffusion. The rate of diffusion depends on the temperature and mass of the molecules. Effusion: The kinetic theory also accounts for how gases escape through tiny holes (effusion). Lighter gases tend to effuse faster than heavier ones. In essence, the Kinetic Theory of Gases offers a molecular-level explanation for many of the macroscopic properties of gases that we observe in daily life, helping us understand how temperature, pressure, and volume are related.