9.12: Kinetic Theory of Gases: Postulates of the Kinetic Theory
- 1 The molecules in a gas are small and very far apart.
- 2 Gas molecules are in constant random motion.
- 3 Molecules can collide with each other and with the walls of the container.
- 4 When collisions occur, the molecules lose no kinetic energy; that is, the collisions are said to be perfectly elastic.
Keeping this in view, who proposed the kinetic molecular theory?
Unlike Lavoisier and Dalton, the 19th century German physicist Rudolf Clausius rejected caloric theory. Instead of regarding heat as a substance that surrounds molecules, Clausius proposed that heat is a form of energy that affects the temperature of matter by changing the motion of molecules in matter.
What are the four basic assumptions of the kinetic theory?
The simplest kinetic model is based on the assumptions that: (1) the gas is composed of a large number of identical molecules moving in random directions, separated by distances that are large compared with their size; (2) the molecules undergo perfectly elastic collisions (no energy loss) with each other and with the
What are the four assumptions of the kinetic molecular theory?
- GASES CONSIST OF LARGE NUMBERS OF PARTICLES THAT ARE FAR APART RELATIVE TO THEIR SIZE.
- COLLISIONS BETWEEN GAS PARTICLES ARE ELASTIC COLLISIONS.
- GAS PARTICLES ARE IN CONSTANT, RAPID, RANDOM MOTION.
- THERE ARE NO FORCES OF ATTRACTION OR REPULSION BETWEEN GAS PARTICLES.