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

In a 10 litre volumetric flask contains 1 gram He and 6.4 and gram O_2 at 27^@C temperature If that total pressure of the mixture is 1.107 atmosphere then what is the partial pressure of He and O_2 ?

One mole of H_2 , 2 moles of I_2 and 3 moles of HI are injected in a one litre of flask. What will be the concentration of H_2, I_2 and HI at equilibrium when K_c is 45.9 ?

At 100^(@)C a 2 litre flask contains 0.4 g of O_(2) and 0.6 g of H_(2) . What is the total pressure of this gas mixture in the flask?

A vessel has nitrogen gas and water vapour in equilibrium with liquid water at a total pressure of 1 atm. The partial pressure of water vapours is 0.3 atm. The volume of this vessel is reduced to one third of the original volume, at the same temperature, then total pressure of the system is: (Neglect volume occupied by liquid water)

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.

Two bulbs of equal volume are connected by a narrow tube of negligible volume and filled with a gas at STP. IF one of the bulbs is kept in melting ice and the other in the water bath at 62^@C ,what will be the new pressure of the gas?

A 15.0 L vessel containing 5.6g of N_(2) is connected to a 5.0 L vessel containing 8.0g of O_(2) by means of a valve. After the valve is opened and the gases are allowed to mix, what will be the partial pressure of each gas in the mixture at 27^(@)C ?

A 15.0 L vessel containing 5.6g of N_(2) is connected to a 5.0 L vessel containing 8.0g of O_(2) by means of a valve. After the valve is opened and the gases are allowed to mix, what will be the partial pressure of each gas in the mixture at 27^(@)C ?

Air inside a closed container is saturated with water vapour . The air pressure is p and the saturated vapour pressure of water is oversetto p . If the mixture is compressed to one half of its volume by maintaining temperature constant, the pressure becomes

A container of fixed volume 0.4 L contains 0.56 g of a gas at 27^(@)C . The pressure of the gas at this temperature is 936 mmHg. If the amount of the gas is increased to 2.1g and its temperature is decreased to 17^(@)C , then what will be the pressure of the gas? Assuming gas behaves ideally.