In a dilute gas at pressure P and temperature T, the mean time between successive collisions of a molecule varies with T as :

An ideal gas is enclosed in a cylinder at pressure of 2atm and temperature, 300K. The mean time between two successive collisions is 6xx10^(-8) s. If the pressure is doubled and temperature is increased to 500K, the mean time between two successive collisions will be close to:

An ideal gas is enclosed in a cylinder at pressure of 2 atm and temperature, 300 K.The men time between two successive collosions is 6xx10^(-8) s. If the pressure to 500K , the mean time between two successive collisions will be close to :

A molecule of a perrfect gas travels, between two successive collisions along a

Find the mean free path and the mean time interval between successive collisions of gaseous nitrogen molecules (a) under standard conditions , (b) at temperature t = 0 ^@C and pressure p = 1.0 nPa (such a pressure can be reached by means of contemporary vacuum pumps).

The pressure P , volume V and temperature T of a gas in the jqar A and other gas in the jar B as at pressure 2P , volume V//4 and temperature 2T , then the ratio of the number of molecules in the jar A and B will be

The average distance travelled by a molecule of gas at temperature T between two successive collisions is called its mean free path which can be expressed by (P is pressure of gas, K is Boltzmann cosntant, d diameter of molecule)

Consider an ideal gas at pressure p, volume V and temperature T. The mean free path for molecules of the gas is L. If the radius of gas molecules, as well as pressure, volume and temperature of the gas are doubled, then the mean free path will be

The pressure P, Volume V and temperature T of a gas in the jar A and the other gas in the jar B at pressure 2P , volume V//4 and temperature 2 T , then the ratio of the number of molecules in the jar A and B will be