Estimate the total number of air molecules (inclusive of oxygen, nitrogen, water vapour and other constituents) in a room of capacity `25.0 m^3` at a temperature of `27 ^@C` and 1 atm pressure.

Total number of moles of oxygen atoms in 3 litre O_3 (g) at 27^@ C and 8.21 atm are :

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 1.0overset@ A . Compare the collision time with the time the molecule moves freely between two successive collisions (Molecular mass of N_2 = 28.0 u).

The air is a mixture of number of gases. The major components are oxygen and nitrogen with approximate proportion of 20% is to 79% by volume at 298K. The water is in equilibrium with air at a pressure of 10 atm. Henry's law constants for oxygen and nitrogen at 298 K are 3.30xx10^7mm and 6.51xx10^7mm respectively. calculate the composition of these gases in water.

Which one of the folloiwng statement about the composition of the vapour over an ideal 1:1 molar mixture of benzene and toluene is correct? Assume that the temperature of constant at 25^@C . (given ,vapour pressure data at 25^@C , benzene=12.8kPa, toulent=3.85kPa)

Stearic acid [CH_(3)(CH_(2))_(16)CO_(2)H] is a fatty acid the part of fat that stores most of the energy .1.0 g of Stearic acid was burnt in a bomb calorimeter . The bomb had capacity of 652 J//^(@)C . If the temperature of 500 g water rose from 25.0 to 39.3^(@)C how much heat is released when the stearic acid was burned? ["Given "C_(p)(H_(2)O)=4.18J//g^(@)c]

At 760 torr pressure and 20^(@)C tempreature , 1 L of water dissolves 0.04 gm of pure oxygen or 0.02 gm of pure nitrogen. Assuming that dry air is compound of 20% oxygen and 80% nitrogen (by volume), the masses (in g/L) of oxygen and nitrogen dissolved by 1 L of water at 20^(@)C exposed to air at a total pressure of 706 torr are respectively :

The total vapour pressure of a 4 mole % solution of NH_(3) in water at 293 K is 50.0 torr. The vapour pressure of pure water is 17.0 torr at this temperature . Applying Henry's and Raoult's laws, calcilate the total vapour pressure for a 5 mole % solution:

A small bubble rises from the bottom of a lake, where the temperature and pressure are 8^(@)C and 6.0 atm , to the water's surface, where the temperature is 25^(@)C and pressure is 1.0 atm . Calculate the final volume of the bubble if its initial volume was 2mL .

What is the pressure inside the drop of mercury of radius 3.00 mm at room temperature ? Surface tension of mercury at that temperature ( 20^@C ) is 4.65xx10^-1 N m^-1 The atmospheric pressure is 1.01xx 10^5Pa . Also give the excess pressure inside the drop.