An oxygen cylinder of volume 30 litres has an initial gauge pressure of 15 atm and a temperature of `27 ^@C`. After some oxygen is withdrawn from the cylinder, the gauge pressure drops to 11 atm and its temperature drops to `17 ^@C`. Estimate the mass of oxygen taken out of the cylinder (`R= 8.31 J mol^-1 K^-1 ’, molecular mass of `O_2` = 32 u)

0.32 g of oxygen is kept in a rigid container and is heated .Find the heat energy needed to raise the temperature from 25^@C to 35^@C .The molar heat capacity of oxygen at constant volume is 20 J mol^(-1) K^(-1) .

The work done in adiabatic compression of 2 mole of an ideal monoatomic gas by constant external pressure of 2 atm starting from initial pressure of 1 atm and initial temperature of 30 K(R=2 cal//"mol-degree")

What amount of heat must be supplied to 2.0 xx 10^-2 kg of nitrogen (at room temperature) to raise its temperature by 45 ^@C at constant pressure ? (Molecular mass of N_2 = 28, R = 8.3 J mol^-1 K^-1. )

A compressed cylinder of gas contains 1.50xx10^(3) g of N_(2) gas at a pressure of 2.0xx10^(7) Pa and a temperature of 17.1^(@)C . What volume of gas has been released into the atmosphere if the final pressure in the cylinder is 1.80xx10^(5) Pa ? Assume ideal behaviour and that the gas temperature is unchanged.

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).

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 :

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.

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 .

11.6g of an organic compound having formula C_n H_(2n+2) is burnt in excess of O_2(g) initially taken in a 22.41 litre steel vessel. Before reactio0n the gaseous mixture was at 273K with pressure reading 2 atm. Aftercomplete combustion and loss of considerable amount of heat, the mixture of product and excess of O_2 had a temperature of 546K and 4.6 atm pressure. The formula of organic compound is :