For $1 \ mol$ of a gas,the average kinetic energy is $E$. Then the root mean square velocity $U_{rms}$ of the gas is:

The volumes of ozone and chlorine gas diffusing in the same time are $35 \ mL$ and $29 \ mL$ respectively. If the molar mass of chlorine is $71$,calculate the molar mass of ozone. (in $.7$)

The root mean square (rms) speed of $X_2$ gas is $x \ m/s$ at a given temperature. When the temperature is doubled, the $X_2$ molecules dissociate completely into atoms. The root mean square speed of the sample of gas then becomes (in $m/s$):

At temperature $T$ (in Kelvin),the $rms$ velocity of $CO_2$ is $x \ cm/sec$. At what temperature (in Kelvin) will the $rms$ velocity of nitrous oxide $(N_2O)$ be $4x \ cm/sec$ (in $T$)?

The increasing order of the rate of diffusion for the gases $H_2$,$O_2$,$NH_3$,and $CO_2$ is:

$A$ gas bulb of $1 \ L$ capacity contains $2.0 \times 10^{21}$ molecules of nitrogen gas at a pressure of $7.57 \times 10^3 \ N \ m^{-2}$. Calculate the root mean square speed in $cm \ sec^{-1}$. (in $.5$)