Gaseous State T...

At which of the following temperature would the molecules of a gas have twice the average kinetic energy they have at 20°C?

A vessel contains a mixture of one mole of oxygen and two moles of nitrogen at 300 K. The ratio of the average rotational kinetic energy per O₂ molecule to that per N₂ molecule is:

The average translational energy and the rms speed of molecules in a sample of oxygen gas at 300K are 6.12×10^–21J and 484m/s respectively. The corresponding values at 600K are nearly: (assuming ideal gas behaviour)

The temperature at which RMS velocity of SO₂ molecules is half that of He molecules at 300K is:

The rms speed of N₂ molecules in a gas is u. If the temperature is doubled and the nitrogen molecules dissociate into nitrogen atoms, the rms speed becomes:

A gas at 27°C has a volume V and pressure P. On heating its pressure is doubled and volume becomes three times. The resulting temperature of the gas will be:

A flask is filled with 13 gm of an ideal gas at 27°C and its temperature is raised to 52°C. The mass of the gas that has to be released to maintain the temperature of the gas in the flask at 52°C and the pressure remaining the same is:

If the value of molar gas constant is 8.3 J/mole-K, the n specific gas constant for hydrogen in J/mole-K will be:

At constant temperature on increasing the pressure of a gas by 5% will decrease its volume by:

On 0°C pressure measured by barometer is 760 mm. What will be pressure on 100°C?