Given that the pressure of the nitrogen molecule cylinder is 2.0 atm, the temperature is 17 °C and the radius of nitrogen molecule is 1 A 0 .
Let P be the pressure inside the cylinder, V be the volume, R be the universal gas constant and T be the temperature, then for 1 mole, the gas equation is,
PV=RT V= RT P
Substitute the values in the above expression.
V= 8.31×( 273+17 ) 2.026× 10 5 = 8.31×( 290 ) 2.026× 10 5 =1.19× 10 −2 m 3
Let n be the number of molecules per unit volume, then
n= N V
Here, N is the Avogadro number.
Substitute the values in the above expression.
n= 6.022× 10 23 1.19× 10 −2 ≈5× 10 25 m −3
Let λ be the mean free path, then
λ= 1 2 πn d 2 = 1 2 πn ( 2r ) 2
Here, r is the radius of nitrogen molecule.
Substitute the values in the above expression.
λ= 1 2 ×3.14×5× 10 25 × ( 2× 10 −10 ) 2 =1× 10 −7 m
Let v rms be the root mean square velocity of nitrogen atom, then
v rms = 3RT M
Here, M is the molecular mass of nitrogen which is 28 g and R is the universal gas constant.
Substitute the values in the above expression.
v rms = 3×8.314×( 290 ) 28× 10 −3 =5.08× 10 2 m/s
Let f be the collision frequency, then
f= v rms λ
Substitute the values in the above expression.
f= 5.08× 10 2 1× 10 −7 ≈5.1× 10 9 s −1
Let t be the time between the successive collisions between molecules, then
t= 1 f
Substitute the value in the above expression.
t= 1 5.1× 10 9 ≈2× 10 −10 s
Let T be the collision time, then
T= d v rms = 2r v rms
Substitute the values in the above expression.
T= 2× 10 −10 5.08× 10 2 ≈4× 10 −13 s
Let T ′ be the time taken between successive collisions, then
T ′ = t T
Substitute the values in the above expression.
T ′ = 2× 10 −10 4× 10 −13 =500
Hence, the value of mean free path is 1× 10 −7 m, the value of collision frequency is 5.1× 10 9 s −1 and the time taken between two successive collisions is 500 times the time taken for a collision.