How does the mean free path `lamda` and the number of collisions of each molecule per unit time `v` depend on the absolute temperature of an ideal gas undergoing
(a) an isochoric process ,
(b) an isobaric process ?

As a result of some process the pressure of an ideal gas increases n-fold . How many times have the mean free path lamda and the number of collisions of each molecule per unit time v changed and how, if the process is (a) isochoric , (b) isothermal ?

How does the mean free path depend on the number density of molecules?

An ideal gas consisting of rigid diatimic molecules goes through an adiabatic process process. How do the mean free path lamda and the number of collisions of each molecule per second v depend in this process on (a) the volume V , (b) the pressure p , ( c) the temperature T ?

How does an average kinetic energy of gas molecules depends on the absolute temperature ?

An ideal gas goes through a polytropic process with exponent n . Find the mean free path lamda and the number of collisions of each molecule per second v as a function of (a) the volume V , (b) the pressure p , ( c) the temperature T .

How does mean free path depend on the diameter (size) of the molecule?

How can the number of molecular collisions per unit time in a gas be increased ?

If the temperature of a gas is increased at constant volume,how will the number of collisions of the molecules per unit time change?

On which other factor does the pressure of a gas depend,besides the number of molecules per unit volume and the temperature of the gas?

The expression for mean free path (lamda) of molecules is given by [where n is no of molecules per unit volume and d molecular diameter of the gas]