A tyre pumped to a pressure of `3.375` atmosphere and at `27^@C` suddenly bursts . Calculate the temperature of escaping air . (y = 1.5)

Air is filled in a motor tube at 27^@C and at a pressure of 8 atmosphere . The tube suddenly bursts, then temperature of air is

The solubility of nitrogen gas at 2 atm pressure at 25^(@)C " is " 13.6xx10^(-4) mol dm^(-3) calculate the solubility of N_(2) gas from atmosphere at 25^(@)C, of atmospgeric pressure is 2 atmosphere and partial pressure of N_(2) gas at this temperature and pressure is 1.53 atm.

Oen litre of oxygen at a pressure of one atmosphere and two litres of nitrogen at a pressure of 0.5 atmosphere are introduced into a vessel of 1 litre capacity , with out any change in the temperature. The total pressure would be

The density of a gas at 27^@C and 1 bar pressure is 2.56 gL^-1 .Calculate the molar mass.

Half a mole of helium at 27 °C and at a pressure of 2 atmosphere is mixed with 1.5 mole of N_2 at 77 °C and at a pressure of 5 atmosphere so that the volume of the mixture is equal to the sum of their initial volumes. If the temperature of the mixture is 69 °C, then its pressure, in atmospheres, is

A steel tyre of 1.2 m inner diameter at 20^@C is to be fitted on a cartwheel of 120.33 cm diameter of the tyre. Calculate the temperature to which the steel tyre is to be raised so that it will just slip on the wheel. (alpha_(Steel) = 11 xx 10^-6//^@C)

A cylinder containing one gram molecule of the gas compressed adiabatic ally until its temperature from 27^@C to 97^@C . Calculate the work done and heat produced in the gas. (y = 1.5)

A steel tank holds 0.2 m^3 of air at a pressure of 5 atm. The volante of air that would occupy at the same temperature but at a pressure l atom is

The solubility of nitrogen gas at1bar pressure at 25^@C is 6.8 xx 10^(-4) moldnr^(-3 . Calculate the solubility of N_2 gasfrom atmosphere at 25^@C if atmospheric pressure is 1 bar and partial pressure of N_2 gas at this temperature and pressure is 0.78 bar.