The molecular weight of a gas that diffuses twice as rapidly as the gas with molecular weight $64$ is:

When the temperature of a gas is increased from $30^{\circ} C$ to $930^{\circ} C$,the root mean square speed of the gas would

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:

Which of the following changes can be made in order to double the root mean square speed,$(V_{rms})$,of a gas kept in a rigid container?

Case $-1:$ 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.

What change occurs in the velocity distribution graph when the temperature is increased?