what is the main postulates of kinetic molecular theory of gases ? explain boyles law on the basis of kinetic molecular theory?
what is the main postulates of kinetic molecular theory of gases ? explain boyles law on the basis of kinetic molecular theory?
Robert Boyle reached to the conclusion that at constant temperature, the pressure of a fixed amount (i.e., number of moles n) of gas varies inversely with its volume. This is known as Boyle’s law. Mathematically, it can be written as
⇒P ∝ 1/V ( at constant T and n)
⇒ p = k1 (1/V)
Assumptions or postulates of the kinetic molecular theory of gases are given below :
⇒Gases consist of large number of identical particles (atoms or molecules) that are so small and so far apart on the average that the actual volume of the molecules is negligible in comparison to the empty space between them.
⇒ There is no force of attraction between the particles of a gas at ordinary temperature and pressure.
⇒ Particles of a gas are always in constant and random motion.
⇒ Particles of a gas move in all possible directions in straight lines.
⇒ Collisions of gas molecules are perfectly elastic.
⇒ At any particular time, different particles in the gas have different speeds and hence different kinetic energies.
⇒ If a molecule has variable speed, then it must have a variable kinetic energy.
Robert Boyle reached to the conclusion that at constant temperature, the pressure of a fixed amount (i.e., number of moles n) of gas varies inversely with its volume. This is known as Boyle’s law. Mathematically, it can be written as
⇒P ∝ 1/V ( at constant T and n)
⇒ p = k1 (1/V)
Assumptions or postulates of the kinetic molecular theory of gases are given below :
⇒Gases consist of large number of identical particles (atoms or molecules) that are so small and so far apart on the average that the actual volume of the molecules is negligible in comparison to the empty space between them.
⇒ There is no force of attraction between the particles of a gas at ordinary temperature and pressure.
⇒ Particles of a gas are always in constant and random motion.
⇒ Particles of a gas move in all possible directions in straight lines.
⇒ Collisions of gas molecules are perfectly elastic.
⇒ At any particular time, different particles in the gas have different speeds and hence different kinetic energies.
⇒ If a molecule has variable speed, then it must have a variable kinetic energy.
