What is mean free path for oxygen molecule at room temperature (300K)and at atmospheric pressure of 1atm? (given diameter of oxygen molecule is 2.9times10^(-10)m)

Estimate the mean free path of a molecule of air at 27^(@)C and one atmospheric pressure. Given average radius of each air molecule is 2.0 xx 10^(-10)m .

For oxygen at 25^(@)C , the collision diameter is 0.361 nm. What is the mean free path (in m) for oxygen molecules at (a) 1 atm pressure and (b) 0.1 Pa pressure ? In scientific notation, if your answer is x xx 10^(y) then fill y in OMR.

The mass of an oxygen molecule is about 16 times that of a hydrogen molecule. At room temperature the 'rms' speed of oxygen molecules is v. The 'rms' speed of oxygen molecules is v. the 'rms' speed of the hydrogen molecules at the same temperature will be

Calculate the value of mean free path (lambda) for oxygen molecules at temperature 27^(@)C and pressure 1.01 xx 10^(5) Pa. Assume the molecular diameter 0.3 nm and the gas is ideal. (k=1.38xx10^(-23)JK^(-1))

The number of molecules in one litre of an ideal gas at 300 K and 2 atmospheric pressure with mean kinetic energy 2xx10^(-9) J per molecules is :

A person's lungs might holds 6.0 L of air at body temperature (310K) and atmospheric pressure (101 kPa). Given that the air contains 21% oxygen, find the number of oxygen molecules in the lungs.

Calculate the mean free path of molecule of a gas having number density (number of molecules per cm^3 ) 2xx10^(8) and the diameter of the molecule is 10^(-5) cm.

A sample of helium gas is at a temperature of 300 K and a pressure of 0.5 atm . What is the average kinetic energy of a molecule of a gas ?