Pressure of 1kg of an ideal gas at `27^@C` is found to be 2 bar . When 2 g of another ideal gas B is introduceed in the same flask at same temperature the pressure becomes 3 bar Find a realationship between their molecular masses.

At same temperature and pressure of an ideal gas

3.4g of a gas at 17^@C occupied sam e volume as 0.16 gram of H_2 at the same temperature and pressure Molecular mass of the gas is

1 litre of an ideal gas at 27 °C is heated at a constant pressure to 297 °C. The final volume is approximately

A vessel contains 2 gm of gas and the pressure is 40 cm of Hg. Under the same conditions , if 1 gm of gas is introduced into the vessel , the pressure will be

At pressure P and absolute temperature T a mass M of an ideal gas fills a closed container of volume V. An additional mass 2M of the same gas is added into the container and the volume is then reduced to V/3 and the temperature to T/3 . The pressure of the gas will now be:

The number of moles in a sample of ideal gas whose volume is 6 lit. at 27^@C and 1.6 atmosphere pressure is

2.9g of a gas at 95^@C occupied the same volume as 0.184 g of dihydrogen at 17^@C, at the same pressure. What is the molar mass of the gas?

One mole of a gas at pressure 2 Pa and temperature 27 °C is heated till both pressure and volume are tripled. What is the temperature of the gas?

The volume of a given mass of a gas at 0^@C is 2 dm^3. Calculate the new volume of the gas at constant pressure when :The temperature is decreased by 10^@C.

The work done when two mole of an ideal gas is compressed form a volume of 5 m^(3) to 1 dm^(3) at 300 K , under a pressure of 100 kPa is