(Kinetic Energy of Gases in chemistry bio tech bsc

in this you will get the info about the kinetic energy of gasees

1. Title: kinetic theory of gases By: MARIUM ZAKIR Bsc . Biotech 1 st Year

2. WHAT IS KINETIC THEORY OF GASES? GAS : A state of matter in which particles are in constant random motion with negligible intermolecular forces. Kinetic Theory Of Gases : - A theory that connects the macroscopic properties of gases (pressure, temperature, volume) to the microscopic motion of molecules. - The Theory forms the basis of gas laws (Boyle’s law, Charles’ law etc.) and helps in understanding thermodynamics and the behavior of real gases

3. ASSUMPTIONS OF KINETIC THEORY- 1. Gas molecules are perfectly rigid and elastic. They are identical in all respect for a . . given gas and for different gas. 2. The size of molecules is negligible as compared to the average distance between them. 3. The molecules are in state of continuous random motion moving in all possible direction. 4. During random motion molecules collide with one another and with the walls of container. 5. The collisions are perfectly elastic and there are no force of attraction or repulsion . . between them. 6. Between two collisions molecules move in a straight line. 7. Despite collision density remains same.

4. PRESSURE OF GAS When gas molecules move and hit the container walls, they exert a force on the walls. The continuous bombardment of billions of molecules creates gas pressure. Using kinetic theory , pressure can be derived as:- P = 1 Nm 3 V (v^2 ) Where :- N = number of molecules M = mass of each molecule V = volume of container (v^2)= mean square speed This shows that gas pressure depends on molecular motion . Faster molecules (higher temperature)| = Higher pressure. x

5. KINETIC ENERGY AND TEMPERATURE RELATION From kinetic theory, the average kinetic en ergy of gas molecules is directly related to its temperatures. FORMULA: 1 2 m (v^2) = 3 2 K b T Where:- m = mass of molecule (v^2) = mean square speed Kb = Boltzmann constant (1.3806 x 10^-23 J/K ) T = absolute temperature (Kelvin) Temperature is basically a measure of the average kinetic energy of molecules. If temperature increases  molecules moves faster  more energy. This explains why hating a gas increases its pressure and why temperature is not just “heat” but a measure of microscopic motion.

6. CONCLUSION The kinetic theory gives us a microscopic picture o matter, that shows gases are made up of very large number of tiny molecules moving randomly in all directions. The pressure of gas is explained as a result of these molecules colliding continuously with the walls of container and transferring momentum. The temperature of the gas is not just a physical quantity , we measure with a thermometer , but it actually represents the kinetic energy of the molecule inside the gas. Thus , higher temperature means molecules move faster and carry more energy