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 $m/s$):
- A$x / 2$
- B$x$
- C$2x$
- D$4x$
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Which of the following equations does not represent the root mean square velocity $(u_{rms})$?
Easy
View SolutionCase $-1:$ An ideal gas of molecular weight $M$ at temperature $T$.
Case $-2:$ Another ideal gas of molecular weight $2M$ at temperature $T/2$.
Identify the correct statement in the context of the above two cases.
Case $-2:$ Another ideal gas of molecular weight $2M$ at temperature $T/2$.
Identify the correct statement in the context of the above two cases.
MediumWBJEE 2023
View SolutionThe ratio between the $RMS$ velocity of $N_2$ at $200 \ K$ and that of $CO$ at $800 \ K$ is (molecular mass of $N_2 = 28 \ g \ mol^{-1}$, molecular mass of $CO = 28 \ g \ mol^{-1}$)
Initially,the root mean square $(rms)$ velocity of $N_2$ molecules at a certain temperature is $u$. If this temperature is doubled and all the nitrogen molecules dissociate into nitrogen atoms,then the new $rms$ velocity will be:
At $T$ $(K)$,the $P$,$V$ and $u_{rms}$ of $1$ mole of an ideal gas were measured. The following graph is obtained. What is its slope $(m)$? ($x$-axis $= PV$; $y$-axis $= u_{rms}^2$,$M =$ Molar mass)
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