A flask of volume 1 litre contains vapour of `CH_3OH` at a pressure of 1 atm and `25^@C`. The flask was then evacuated till the final pressure drop to `10^(-1)` mm. Find the number of molecules of `CH_3OH` left in the flask.

Oxygen gas is present in a 1L flask ata pressure 7.6xx10^(-10)mm Hg at 0^(@)C . Calculate the number of O_(2) molecules in the flask.

Two flasks of equal volumes have been joined by a narrow tube of negligible volume. Initially both flasks are at 300 K containing 0.60 mol of O_2 gas at 0.5 atm pressure. One of the flasks is then placed in a thermostat at 600 K. Calculate number of moles of _2 2 gas in each flask.

Oxygen gas is present,in a 1.0 L flask at a pressure of 7.6 xx 10^(-10)mm Hg at 27^@C . Calculate the number of oxygen atoms in the "flask

The initial volume of a gas is 1 L and the pressure is 16 atm. Due to adiabatic expansion, the final pressure of the gas becomes 2 atm. Find out the final volume of the gas [gamma = 3/2] .

When 2 g of a gas 'M' is introduced into an empty flask at 30^(@)C , its pressure becomes 1 atm. Now, if 3g of another gas 'N' is introduced in the same flask at the same temperature, the total pressure becomes 1.5 atm. Find the ratio of the molar masses of the two gases.

The number of molecules 67.2 L of a gas at 0^@C and 1 atm pressure is:

One litre flask contains air, water vapour and a small amount of liquid water at a pressure of 200 mmHg. If this is connected to another one litre evacuated flask, what will be the final pressure of the gas mixture at equilibrium? Assume the temperature to be 50^@C . Aqueous tension at 50^@C=93 mmHg