Kinetic Theory of an Ideal Gas

$600 \mathrm{c}.\mathrm{c}.$ of a gas at a pressure of $750 \mathrm{mm}$ is compressed to $500 \mathrm{c}.\mathrm{c}$. Taking the temperature to remain constant, the increase in pressure, is

What is Boyle''s law ?

If volume occupied by ${\mathrm{CO}}_2$ Molecules are negligible, then what will be the pressure $\left(\frac{\mathrm{P}}{5.227}\right)$Exerted by one mole of ${\mathrm{CO}}_2$ Gas at $300\mathrm{K} ?$$(\mathrm{a}=3.592\mathrm{atm}-{\mathrm{L}}^2{\mathrm{mol}}^{-1})$

If $\beta$ is the pressure coefficient at constant volume then which of the following is true.

For all gases, the experimental value of the pressure coefficient at constant volume$\left(\beta \right)$  is 

If $\alpha$ is the volume coefficient at constant pressure then which of the following indicates Charles law mathematically.

For all gases, the experimental value of the volume coefficient at constant pressure is 

Derive the formula for time for successive collision between the walls of the container with the molecule.

For a gas with $n$ number of molecules per unit volume, Suppose the molecules of a gas are spheres of diameter $d$  the average speed of each molecule is $v$. The time between two successive collisions is on the average $\Gamma =\frac{1}{n{\mathrm{\pi vd}}^2}$

State the assumption regarding the volume of gas molecules to consider the gas as an ideal gas.

For gas to be ideal gas, it is assumed that the _____ of the molecules is negligibly small compared to the volume occupied by the gas.

Consider the number of molecules of an ideal gas present per unit volume to be ${10}^{30}$ and their average velocity to be $2\times {10}^4 \mathrm{m}/\mathrm{s}$. Calculate the rate of collisions of its molecule if its diameter is $7\times {10}^{-10} \mathrm{m}$.

Calculate the time taken between two successive collisions for a helium molecule having a diameter $7\times {10}^{-10} \mathrm{m}$ and an average velocity of ${10}^3 \mathrm{m}/\mathrm{s}$, consider ${10}^{30}$ molecules present per unit volume.

Derive the formula of the time interval between two successive collisions of molecules.

Calculate the rate of collisions of a hydrogen molecule having a diameter $200 \mathrm{pm}$ and an average velocity of ${10}^6 \mathrm{m}/\mathrm{s}$, consider ${10}^{15}$ molecules present per unit volume.

Derive the formula for the rate of collisions of a molecule with other nearby molecules.

Boyle's law states that when the temperature of a gas is kept constant, the volume of a fixed mass of gas is inversely proportional to its pressure. 

For a molecule of an ideal gas, the number density is $2\sqrt{2}\times {10}^8 {\mathrm{cm}}^{-3}$ and the mean free path is $\frac{{10}^{-2}}{\pi } \mathrm{cm}$. The diameter of the gas molecule is

Collision in which the laws of conservation of momentum and kinetic energy hold true, is known as elastic collision.

The average intermolecular distance is considerably small as compared to the diameter of the molecule.