Kinetic Theory ...

The speeds of 5 molecules of a gas (in arbitrary units) are as follws: 2, 3, 4, 5, 6, The root mean squre speed for these molecules is

To what temperature should the hydrogen at room temperature (27^o C) be heated at constant pressuse so that the rms velocity of its molecule becomes double of its previous value

The rms speed of gas molecules is given by

A sample of gas is at O^o C. To what temperature it must be raised in order to double the rms speed of molecule.

The molecules of a given mass of a gas have a rms velocity of 200m s at 27^o C and 1.0 × 10⁵ Nm^–2 pressure when the temperature is 127^o C and pressure is 0.5 × 10⁵ Nm^–2, the rms velocity in m/s will be

If the molecular weight of two gases are M₁ and M₂ , then at a given temperature the ratio of root mean square velocity v₁ and v₂ will be

The root mean square velocity of the molecules in a sample of helium is 5/7 th that of the molecules in a sample of hydrogen. If the temperature of hydorgen sample is 0^oC, then the temperature of the helium sample is about

At room temperature ( 27^o C), the rms speed of the molecules of certain diatomic gas is found to be 1930 m/s. The gas is

If three molecules have velocities 0.5, 1 and 2 the ratio of rms speed and average speed is (The velocities are in km/s)

At what temperature pressure remaining constant will the rms speed of a gas molecules increase by 10% of the rms speed at NTP?