A Box of `1.00 m^3` is filled with nitrogen at 1.50 atm at 300 K. The box has a hole of an area 0.010 `mm^2`. How much time is required for the pressure to reduce by 0.10 atm. If the pressure outside is 1 atm.

Which has the lowest boiling point at 1 atm pressure ?

One mole of H_2 gas is contained in a box of volume V = 1.00 m^3 at T = 300 K . The gas is heated to a temperature of T = 3000K and the gas gets converted to a gas of hydrogen atoms. The final pressure would be (considering all gases of be ideal)

A certain sample of gas has a volume of 0.2 litre measured at 1 atm pressure and 0^(@)C . At the same pressure but at 273^(@)C , its volume will be

10 g of a gas at 1 atm and 273 K occupies 5 litres. The temperature at which the volume becomes double for the same mass of gas at the same pressure is:

At 300 K the half-life of a sample of a gaseous compound initially at 1 atm is 100 sec. When the pressure is 0.5 atm the half-life is 50 sec. The order of reaction is :

Henry's law constant of oxygen 1.4xx10^-3 molL^-1 atm^-1 at 298K. How much of oxygen is dissolved in 100 mL at 298K when partial pressure of oxygen is 0.5 atm?

A 2.24L cylinder of oxygen at 1 atm and 273 K is found to develop a leakage. When the leakage was plugged the pressure dropped to 570 mm of Hg. The number of moles of gas that escaped will be :

One mole of an ideal gas (C_(v,m)=(5)/(2)R) at 300 K and 5 atm is expanded adiabatically to a final pressure of 2 atm against a constant pressure of 2 atm. Final temperature of the gas is :

A heating coil is immersed in a 100 g sample of H_(2)O (l) at a 1 atm and 100^(@) C in a closed vessel. In this heating process , 60% of the liquid is converted to the gaseous form at constant pressure of 1 atm . The densities of liquid and gas under these conditions are 1000 kg//m^(3) and 0.60 kg//m^(3) respectively . Magnitude of the work done forthe process is : (Take : 1L-atm= 100J)

The rate of a reaction is expressed as : 3.65 xx 10^-3 atm^-1 s^-1 . The order of reaction