To what temperature should the hydrogen at `327^(@)C` be cooled at constant pressure, so that the root mean square velocity of its molecules become half of its previous value?

To what temperature should the oxygem at 27^(@)C be heated at constant pressure, so that the root mean square velocity of its molecules becomes thrice of its previous value.

To what temperature should the hydrogen at room temperature (27^(@)C) be heahted at constant perssure so that the RMS velocity of iths molecules becomes double its previous value?

Calculate for hydrogen at 27^(@)C root mean square velocity of the molecules.

The temperature at which the root mean square velocity of the gas molecules would becomes twice of its value at 0^(@)C is

The temperature at which the root mean square velocity of the gas molecules would become twice of its value at 0^(@)C is

At constant pressure, calculate the root mean square velocity of a gas molecule at temperature 27^(@)C if its rms speed at 0^(@)C is 4km/s

At constant pressure, calculate the root mean square velocity of a gas molecule at temperature 27^@ C if its rms speed at 0^@ C . Is 4 km/s.

At constant pressure, calculate the root mean square velocity of a gas molecule at temperature 27^(@)C if its rms speed at 0^(@)C is 4km/s

At constant pressure, calculate the root mean square velocity of a gas molecule at temperature 27^@ C if its rms speed at 0^@ C . Is 4 km/s.

At what temperature will the root mean square velocity of methane become double of its value at N.T.P.?