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

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

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

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.