The mean free path of nitrogen molecules at 27^(@)C is 3xx10^(-7)m//s . If the average speed of nitrogen molecules at the same temperature is 600 m/s then the collision frequency will be
find the rms speed of oxygen molecules in a gas at 300K.
A temperature at which rms speed of SO_(2) molecule is half of that of helium molecules at 300 K
If the rms speed of nitrogen molecules is 490 m s^(-1) at 273 K, find the rms speed of hydrogem molecules at the same temperature.
For a given gas at 1 atm pressure, rms speed of the molecules is 200 m/s at 127^(@)C . At 2 atm pressure and at 227^(@)C , the rms speed of the molecules will be:
For a given gas at 1 atm pressure, rms speed of the molecule is 300m/sec at 27°C. At 2 atm pressure and at 127°C the rms speed of the molecules will be (A) 300m/sec (B) 400m/sec (C)346.4m sec (D)743m/ sec
The root mean square velocity of the molecules of a gas is 200m//s . What will be the rms velocity of the molecules if the atomic weight is doubled and the absolute temperature is halved?
If the rms speed of oxygen molecules at 0^(@)C is 160 m/s, find the rms speed of hydrogen molecules at 0^(@)C.
Two gaseous molecules A and B are traveling towards each other. Let the mean free path of the molecule be sigma and Z be the collision number with other molecules at pressure 1 atm . Answer the following questions If the collision frequency of a gas at 1 atm pressure is Z , then its collision frequency at 0.5 atm is
