Which of the following statements is incorrect about `H_(2)` and `CO_(2)` gas considering them as ideal gases?

Options

A. The average kinetic energies of `H_(2)` and `CO_(2)` molecules are the same at a given temperature.
B. The root mean square velocities of `H_(2)` and `CO_(2)` molecules are the same at a given temperature
C. The fraction of `H_(2)` and `CO_(2)` molecules with the most probable:velocity decreases with increase in temperature.
D. The density of `H_(2)` is less that `CO_(2)` at a given temperature and pressure

Answer

B

Explanation

Average kinetic energy per mole is equal to kinetic energy per molecule multiplied by Avogadro number `E_("avg") = N_(A) xx (3)/(2) kT = (3)/(2) RT`
Since , for any ideal gas average kinetic energy depends only on the temperature , so at a given temperature as well as on molar mass , so , for two different ideal gases , it is different at a given temperature .
`V_(rms) = sqrt((3RT)/(M)) or V_(rms) prop sqrt((T)/(M))`
Maxwell.s distribution curve of velocity graph flatters on increasing temperature , so the most probably velocity fraction is decreased . Since density is directly proportional to the molar mass , and molar mass of hydrogen is lower than carbon dioxide , so , density of hydrogen is less than carbon dioxide