Kinetic Theory of Gases

Easily liquefiable gases show larger deviations from gas laws. Comment on this statement on the basis of kinetic molecular theory.

Two gases A and B which do not chemically react, are taken in two $1 \mathrm{L}$ containers. They are found to exert pressures ${\mathrm{P}}_1$ and ${\mathrm{P}}_2$, respectively. When the mixture of the gases A and B is taken in another $1 \mathrm{L}$ container, the pressure exerted is found to be $\left({\mathrm{P}}_1+{\mathrm{P}}_2\right)$. How can you justify this on the basis of kinetic molecular theory?

Arrange the following relevant points in a proper sequence to explain why gases exert pressure.

$\left(1\right)$ Gas molecules are in random motion.

$\left(2\right)$ Kinetic energy of gas molecules is proportional to absolute temperature.

$\left(3\right)$ A gas is made up of tiny particles called molecules.

$\left(4\right)$ Intermolecular forces of attraction are negligible in gases.

$\left(5\right)$ During random motion, the gas molecules collide with each other.

$\left(6\right)$ During random motion, the gas molecules collide with the walls of a container.

What is kinetic theory of gases?

The kinetic energy of a mole of ideal gas in calories is approximately equal to 

The molecular speeds of gaseous molecules analogous to those of rifle bullets. Then why is odour of a gas not detected so fast ?

Which is wrong according to Kinetic theory?

According to Kinetic theory of gases, there are 

State the kinetic molecular theory of gases. What are the postulates of kinetic molecular theory of gases?

List the postulates of kinetic molecular theory of gases.