At 1 atm and 273 K the volume of nitrogen gas required to cover a sample of silica gel, assuming Langmuir monolayer adsorption , is found to be `1.30 cm^(3)g^(-1)` of the gel. The area occupoied by a nitrogen molecule os `0.16nm^(2)`. Find out the no. of surface sites occupied per molecule of `N_(2)`.
For nitrogen a = 1.4 L^(2) atm, mol^(-2) , b = 0.04 L mol^(-1) . Find out the diameter of nitrogen molecule.
20% surface sites have adsorbed N_2 . On heating N_2 gas is evolved from sites and were collected at 25^@C and 0.001 atm in a container of volume 2.46cm^(3) . Density of surface sites is 6 xx 10^(4) cm^(-2) and surface area is 10^(3) cm^(2) .Find the number of surface sites occupied per molecule of N_2 .
The surface are of activated charcoal is 10^(3)m^(3)g^(-1) .If effective surface area of ammonia molecule is 0.129nm^(2) and complete monolayer coverage is assumed. how much ammonia at STP could be adsorbed on 10g of charcoal?
Estimate the mean free path and collision frequency of a nitrogen molecule in a cylinder containing nitrogen at 2.0 atm and temperature 17^(@)C . Take the radius of a nitrogen molecule to be roughly 1.0 Å. Compare the collision time with the time the molecule moves freely between two successive collisions (Molecular mass of N_(2) = 28.0 u).
Ideal gas equation is represented as PV=nRT . Gases present in the universe were found ideal n the Boyle's temperature range only. The compressibility factor for an ideal gas, Z= (PV)/(nRT) . The main cause to show deviations were due to wrong assumptions made bout forces of attractions (which becomes significant at high pressure). olume occupied by molecules V, in PV = nRT, is supposed to be volume of as or, the volume of container in which gas is placed by assuming that aseous molecules do not have appreciable volume. Actual volume of the as is that volume in which each molecule of a gas can move freely. If olume occupied by gaseous molecule is not negligible, then the term V hould be replaced by the ideal volume which is available for free motion of ach molecule of gas. Similarly for n moles of gas V_("actual") = V-nb The excluded volume can be calculated by considering bimolecular collisions. The excluded volume is the volume occupied by the sphere of 2r for each pair of molecule. Thus, excluded volume for one pair of molecules = 4/3 pi (2r)^3 = (4 xx 8 pi r^3)/3 The excluded volume for 1 molecule = 2/3 xx 8 pi r^3 = 4 xx (4/3 pi r^3) = 4V The excluded volume for N molecules = 4NV = b (where N is Avogadro's No.) The compressibility factor for N_2 at -50^@C and 800 atm pressure is 1.95. Number of moles of N_2 required to fill a balloon of 100 L capacity is :
NARENDRA AWASTHI-SURFACE CHEMISTRY-Level 3 - Assertion - Reason Type Questions
